Chemistry - Test #1 Study Guide

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The science that deals with the materials of the universe and the changes that these materials undergo.

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1. Chemistry

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The process that lies at the center of scientific inquiry. The steps are: (a) State the problem and collect data (make observations); (b) Formulate hypotheses; (c) Perform experiments.

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2. Scientific Method

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A set of tested hypotheses that gives an overall explanation of some part of nature.

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3. Theory (Model)

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Generally observed behavior which shows that the same observation applies to many different systems in order to explain how something happens.

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4. Natural Law

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1. Chemistry is the science that deals with the materials of the universe and the _______ these materials undergo. It is the _______ science; understanding most other fields of science requires an understanding of chemistry.

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Chemistry is the science that deals with the materials of the universe and the (CHANGES) these materials undergo. It is the (CENTRAL) science; understanding most other fields of science requires an understanding of chemistry.

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2. Formulating a __________ – propose possible solutions to the problem or possible explanations for the observation.

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Formulating a (HYPOTHESIS) – propose possible solutions to the problem or possible explanations for the observation.

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3. Making an ___________ – recognize the problem and state it clearly.

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Making an (OBSERVATION) – recognize the problem and state it clearly.

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4. Performing an __________ – decide which of the solutions is the best or decide whether the explanation proposed is reasonable.

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Performing an (EXPERIMENT) – decide which of the solutions is the best or decide whether the explanation proposed is reasonable.

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5. _______ is a framework for gaining and organizing knowledge.

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(SCIENCE) is a framework for gaining and organizing knowledge.

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6. Science is a ____ __ ______ – a procedure for processing and understanding certain types of information.

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Science is a (PLAN OF ACTION) – a procedure for processing and understanding certain types of information.

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7. Scientists are always ___________ our current beliefs about science, asking questions, and experimenting to gain new knowledge (scientific method is needed).

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Scientists are always (CHALLENGING) our current beliefs about science, asking questions, and experimenting to gain new knowledge (scientific method is needed).

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8. The scientific method yields two outcomes: (1) ______ – which is based on your hypothesis yet is not proven; and (2) ___ – gather the observations and formulate a law.

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The scientific method yields two outcomes: (1) (THEORY) – which is based on your hypothesis yet is not proven; and (2) (LAW) – gather the observations and formulate a law.

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9. The __________ ______ is the process that lies at the center of scientific inquiry. Observation -> Hypothesis -> Experiment (repeat as many times as needed, going back to Observation after Experiment), (A) which then leads to Theory (Model) -> Prediction -> Experiment -> Theory (______ as needed) (which is also repeated as many times as needed), OR becomes (B) Law

Back 13

The (SCIENTIFIC METHOD) is the process that lies at the center of scientific inquiry. Observation -> Hypothesis -> Experiment (repeat as many times as needed, going back to Observation after Experiment), (A) which then leads to Theory (Model) -> Prediction -> Experiment -> Theory ([MODIFY] as needed) (which is also repeated as many times as needed), OR becomes (B) Law

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10. Outcomes of the scientific method – Law. A summary statement describing the ____________ associated with a particular phenomenon. The law of conservation of matter: matter is neither created nor destroyed by chemical reactions. Murphy’s law: the probability of the toast landing butter side down is directly proportional to the price of the carpet.

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Outcomes of the scientific method – Law. A summary statement describing the (OBSERVATIONS) associated with a particular phenomenon. The law of conservation of matter: matter is neither created nor destroyed by chemical reactions. Murphy’s law: the probability of the toast landing butter side down is directly proportional to the price of the carpet.

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11. Outcomes of the scientific method – Theory (Model). Set of tested hypotheses that gives an overall ___________ of some natural phenomenon including the ability to predict what might happen next (Atomic Theory).

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Outcomes of the scientific method – Theory (Model). Set of tested hypotheses that gives an overall (EXPLANATION) of some natural phenomenon including the ability to predict what might happen next (Atomic Theory).

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1. Steps in the Scientific Method
a. State the _______ – Observation
b. Propose a possible ___________ for the problem – Hypothesis 1
c. Perform an __________ – Observation
d. Formulate a new or modified ___________ – Hypothesis 2
e. Repeat the process

Back 16

Steps in the Scientific Method
a. State the (PROBLEM) – Observation
b. Propose a possible (EXPLANATION) for the problem – Hypothesis 1
c. Perform an (EXPERIMENT) – Observation
d. Formulate a new or modified (EXPLANATION) – Hypothesis 2
e. Repeat the process

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2. Outcomes: Law
a. A Summary statement describing the ____________ associated with a particular phenomenon
b. The Law of Conservation of Matter: Matter is neither created nor destroyed by ________ reactions
c. The probability of the toast landing butter side down is directly proportional to the price of the carpet

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Outcomes: Law
a. A Summary statement describing the (OBSERVATIONS) associated with a particular phenomenon
b. The Law of Conservation of Matter: Matter is neither created nor destroyed by (CHEMICAL) reactions
c. The probability of the toast landing butter side down is directly proportional to the price of the carpet

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3. Outcomes: Theory (Model)
a. Set of tested __________ that gives an overall explanation of some natural phenomenon including the ability to predict what might happen next
b. Atomic Theory

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Outcomes: Theory (Model)
a. Set of tested (HYPOTHESES) that gives an overall explanation of some natural phenomenon including the ability to predict what might happen next
b. Atomic Theory

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4. The Scientific Method Yields 2 Outcomes:

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Theory or Law

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5. Concept Check

Which of the steps in the scientific method is missing from the following situation?
“Your instructor is holding a balloon and quickly inhales some of the gas inside the balloon. He then speaks and his voice changes to a high-pitched sound (and sounds quite funny!). He then asks you to determine what gas was inside the balloon that he inhaled. Based on your observations, you conclude that the gas must be helium.”
a) State the problem.
b) Make observations.
c) Formulate a hypothesis.
d) Perform experiments.

Back 20

1. Concept Check

Which of the steps in the scientific method is missing from the following situation?
“Your instructor is holding a balloon and quickly inhales some of the gas inside the balloon. He then speaks and his voice changes to a high-pitched sound (and sounds quite funny!). (MAKE OBSERVATION) He then asks you to determine what gas was inside the balloon that he inhaled. (STATE THE PROBLEM) Based on your observations, you conclude that the gas must be helium. (FORMULATE A HYPOTHESIS) ”.”
d) Perform experiments.

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6. Concept Check

Which are the observations, hypotheses, experiments, theories described in the following situation?

A woman notices a lump in her breast. Her doctor orders a mammogram which shows two additional masses in her breast. The doctor has all three suspect areas biopsied and only the lump shows cancer. The woman has a lumpectomy. Two years later the cancer recurs.
a) What are the observations.
b) The Hypothesis
c) The Experiments
d) The Theory
e) Is the Theory Correct

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6. Concept Check

Which are the observations, hypotheses, experiments, theories described in the following situation?

A woman notices a lump in her breast (OBSERVATION). Her doctor orders a mammogram (EXPERIMENT) which shows two additional masses in her breast.(OBSERVATION) The doctor has all three suspect areas biopsied (HYPOTHESIS) and only the lump shows cancer. (THEORY) The woman has a lumpectomy. (EXPERIMENT) Two years later the cancer recurs. (THEORY INCORRECT)
a) What are the observations.
b) The Hypothesis
c) The Experiments
d) The Theory
e) Is the Theory Correct

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1. Which of the following statements is false?
1. A knowledge of chemistry is useful to almost everyone.
2. The principles of chemistry are inherently neither good nor bad – it’s what we do with this knowledge that really matters.
3. A major by-product of studying chemistry is that you will become a better problem solver.
4. Chemical industries are the ones responsible for all our environmental problems today.

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Choice #4 is false. Although chemical industries have contributed to some environmental problems, they are not responsible for all of them. The industries that apply the chemical sciences are now determined to be part of the solution to our environmental ills rather than part of the problem.

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2. Chemistry can be defined as the science that deals with the materials of the universe and the ____________ that these materials undergo.
1. synthesizing
2. decomposing
3. changes
4. observations

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Choice #3 is the correct answer. Most of the phenomena that occur in the world around us involve chemical changes, changes where one or more substances become different substances.

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3. One of the steps in the scientific method is to state the problem and collect data (make observations). Which of the following is an example of stating the problem?
1. What is my friend’s illness?
2. I think my friend has the flu.
3. My friend is lethargic and will not eat.
4. My friend has a fever of 102.3°F.

Back 24

Choice #1 is the correct answer. This is the problem in which you will have to apply the rest of the scientific method in order to come up with a reasonable answer.

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4. One of the steps in the scientific method is to state the problem and collect data (make observations). Which of the following is an example of a quantitative observation?
1. What is my friend’s illness?
2. I think my friend has the flu.
3. My friend is lethargic and will not eat.
4. My friend has a fever of 102.3°F.

Back 25

Choice #4 is the correct answer. A quantitative observation is called a measurement and involves a number and a unit.

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5. One of the steps in the scientific method is to state the problem and collect data (make observations). Which of the following is an example of a qualitative observation?
1. What is my friend’s illness?
2. I think my friend has the flu.
3. My friend is lethargic and will not eat.
4. My friend has a fever of 102.3°F.

Back 26

Choice #3 is the correct answer. A qualititative observation does not involve a number.

Front 27

6. Another step in the scientific method is to formulate hypotheses. Which of the following is an example of formulating a hypothesis?
1. What is my friend’s illness?
2. I think my friend has the flu.
3. My friend is lethargic and will not eat.
4. My friend has a fever of 102.3°F.

Back 27

Choice #2 is the correct answer. A hypothesis is a possible explanation for the observation(s).

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7. Which of the following statements is false?
1. Science is a framework for gaining and organizing knowledge.
2. Science is not simply a set of facts but also a plan of action – a procedure for processing and understanding certain types of information.
3. To explain the behavior of a given part of nature, we repeat the steps of the scientific method many times.
4. A theory and a model are two separate (and different) ideas.

Back 28

Choice #4 is false. A theory is often called a model.

Front 29

8. Which of the steps in the scientific method is missing from the following situation?
“Your instructor is holding a balloon and quickly inhales some of the gas inside the balloon. He then speaks and his voice changes to a high-pitched sound (and sounds quite funny!). He then asks you to determine what gas was inside the balloon that he inhaled. Based on your observations, you conclude that the gas must be helium.”
1. State the problem.
2. Make observations.
3. Formulate a hypothesis.
4. Perform experiments.

Back 29

Choice #4 is missing. Experiments must be performed to test and see if the gas is in fact helium. For example, a good test to perform would be a flammability test. This would produce new observations that could support or contradict your hypothesis.

Your instructor is holding a balloon and quickly inhales some of the gas inside the balloon. He then speaks and his voice changes to a high-pitched sound (and sounds quite funny!). (MAKE OBSERVATION) He then asks you to determine what gas was inside the balloon that he inhaled. (STATE THE PROBLEM) Based on your observations, you conclude that the gas must be helium. (FORMULATE A HYPOTHESIS) ”

Front 30

9. Which of the following statements is false?
1. A law is a summary of observed behavior. For example, studies of innumerable chemical changes have shown that the total mass of the materials involved is the same before and after the change.
2. A theory is an explanation of behavior – why nature behaves in a particular way.
3. If a theory is disproven, then all of the observations that support that theory must also be disproven.
4. A law tells what happens.

Back 30

Choice #3 is false. A theory can be wrong in its attempt to explain why a behavior occurs but that does not mean that the observed behavior in itself is also wrong.

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10. To be successful in chemistry, you must:
1. know the vocabulary and memorize certain pieces of information.
2. make an attempt to solve a problem and then analyze the feedback (learn from your mistakes).
3. practice solving problems and ask for help when confused or really frustrated.
4. All of the above.

Back 31

Choice #4 is correct!

Front 32

A quantitative observation.

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1. Measurement

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Expresses a number as a product of a number between 1 and 10 and the appropriate power of 10; which is figured by how many places the decimal moves.

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2. Scientific Notation

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Tells what scale or standard is being used to represent the results of the measurement.

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3. Units

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A common unit of measurement which is used in the United States to measure quantities such as mass, length, time, and temperature.

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4. English System

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A common unit of measurement which is used in most of the industrialized world (besides the U.S.) to measure quantities such as mass, length, time, and temperature.

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5. Metric System

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A comprehensive system of units which is based on the metric system and units derived from the metric system, which was set up in 1960 in an international agreement.

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6. SI Units (International System)

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The amount of three-dimensional space occupied by a substance.

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7. Volume

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The quantity of matter present in an object.

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8. Mass

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The numbers recorded in a measurement (all the certain numbers plus the first uncertain number).

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9. Significant Figures

Front 41

When we perform a calculation and the number of digits is greater than the number of significant figures needed, we do this to reduce the amount of digits to make it conform to the number of digits that is needed for the answer.

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10. Rounding Off

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A ratio of the two parts of the statement that relates the two units.

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11. Conversion Factor

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In the English and metric systems, such as for distance, when 2.54 cm = 1 in., the respective numbers are different because they refer to different scales (units) of distance; though they are exactly the same in length.

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12. Equivalence Statement

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Changing from one unit to another via conversion factors (based on the equivalence statements between the units).

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13. Dimensional Analysis

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The temperature scale that is widely used in the U.S. and Great Britain, and is the scale employed in most of the engineering sciences.

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14. Fahrenheit Scale

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The temperature scale that is used in Canada and Europe and in the physical and life sciences in most countries, and follows the metric system which is based on the powers of 10.

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15. Celsius Scale

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Another temperature scale which is used in the sciences, though this one is used the least.

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16. Kelvin (Absolute) Scale

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The amount of matter present in a given volume of substance.

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17. Density

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The ratio of the density of a given liquid to the density of water at 4˚C; because it is a ratio of densities, it has no units.

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18. Specific Gravity

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1. A ____________ observation is called a measurement and always consists of a number and a unit.

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A (QUANTITATIVE) observation is called a measurement and always consists of a number and a unit.

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2. We can conveniently express very large or very small numbers using __________ ________, which represents the number as a number between 1 and 10 multiplied by 10 raised to a power.

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We can conveniently express very large or very small numbers using (SCIENTIFIC NOTATION), which represents the number as a number between 1 and 10 multiplied by 10 raised to a power.

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3. _____ give a scale on which to represent the results of a measurement. The three systems discussed are the English, metric, and SI systems. The metric and SI systems use ________ to change the size of the units.

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(UNITS) give a scale on which to represent the results of a measurement. The three systems discussed are the English, metric, and SI systems. The metric and SI systems use (PREFIXES) to change the size of the units.

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4. The ____ of an object represents the quantity of matter in that object.

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The (MASS) of an object represents the quantity of matter in that object.

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5. All measurements have a degree of ___________, which is reflected in the number of significant figures used to express them. Various rules are used to round off to the correct number of significant figures in a calculated result.

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All measurements have a degree of (UNCERTAINTY), which is reflected in the number of significant figures used to express them. Various rules are used to round off to the correct number of significant figures in a calculated result.

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6. We can convert from one system of units to another by a method called ___________ ________, in which conversion factors are used.

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We can convert from one system of units to another by a method called (DIMENSIONAL ANALYSIS), in which conversion factors are used.

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7. ___________ can be measured on three different scales: Fahrenheit, Celsius, and Kelvin. We can readily convert among these scales.

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(TEMPERATURE) can be measured on three different scales: Fahrenheit, Celsius, and Kelvin. We can readily convert among these scales.

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8. _______ is the amount of matter present in a given volume (mass per unit volume).

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(DENSITY) is the amount of matter present in a given volume (mass per unit volume).

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1. ___________ – having to do with the quality of something (definition, color, texture, shape).

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(QUALITATIVE) – having to do with the quality of something (definition, color, texture, shape).

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2. ____________ – Having to do with the quantity of something, can assign a number to it (how many, how much). Has 2 parts, number and ____, number tells comparison, ____ tells scale.

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(QUANTITATIVE) – Having to do with the quantity of something, can assign a number to it (how many, how much). Has 2 parts, number and (UNIT), number tells comparison, (UNIT) tells scale.

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3. The purpose of the __________ ________ is to make things easier, as it is a technique used to express very large or very small numbers. Expresses a number as a _______ of a number between 1 and 10 and the appropriate power of 10.

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The purpose of the (SCIENTIFIC NOTATION) is to make things easier, as it is a technique used to express very large or very small numbers. Expresses a number as a (PRODUCT) of a number between 1 and 10 and the appropriate power of 10.

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4. Scientific Notation – Any number can be represented as the product of a number between 1 and 10 and a power of 10 (either ________ or ________). 93,000,000 = 9.3 X 10,000,000 = 9.3 X 10⁷ (OR) 0.00000093 = 9.3 / 10,000,000 = 9.3 X 10⁻⁷ The power of 10 depends on the number of places the _______ _____ is moved and in which direction.

Back 61

Scientific Notation – Any number can be represented as the product of a number between 1 and 10 and a power of 10 (either [POSITIVE] or [NEGATIVE]). 93,000,000 = 9.3 X 10,000,000 = 9.3 X 10⁷ (OR) 0.00000093 = 9.3 / 10,000,000 = 9.3 X 10⁻⁷ The power of 10 depends on the number of places the (DECIMAL POINT) is moved and in which direction.

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5. Scientific Notation – The number of places the decimal point is moved determines the power of 10. The direction of the move determines whether the power of 10 is positive or negative. If the decimal point is moved to the ____, the power of 10 is positive; if the decimal point is moved to the _____, the power of 10 is negative.

Back 62

Scientific Notation – The number of places the decimal point is moved determines the power of 10. The direction of the move determines whether the power of 10 is positive or negative. If the decimal point is moved to the (LEFT), the power of 10 is positive; if the decimal point is moved to the (RIGHT), the power of 10 is negative.

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6. ___________ – quantitative observation consisting of two parts; number, scale (unit).

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(MEASUREMENT) – quantitative observation consisting of two parts; number, scale (unit).

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7. Units – ________ are used to change the size of the unit in the SI System.

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Units – (PREFIXES) are used to change the size of the unit in the SI System.

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8. Length – Fundamental SI unit of length is the _____.

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Length – Fundamental SI unit of length is the (METER).

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9. ______ – measure of the amount of 3-D space occupied by a substance. SI unit = cubic meter (m³). Commonly measure solid ______ in cm³ (1 mL = 1 cm³, 1 L = 1dm³).

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(VOLUME) – measure of the amount of 3-D space occupied by a substance. SI unit = cubic meter (m³). Commonly measure solid (VOLUME) in cm³ (1 mL = 1 cm³, 1 L = 1dm³).

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10. Mass – Measure of the amount of ______ present in an object. SI unit = kilogram (kg); 1 kg = 2.2046 lbs., 1 lb. = 453.59 g.

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Mass – Measure of the amount of (MATTER) present in an object. SI unit = kilogram (kg); 1 kg = 2.2046 lbs., 1 lb. = 453.59 g.

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11. A _____ (a number between 1 and 10 with no decimals) that must be estimated is called uncertain. A measurement always has some degree of uncertainty. Record the certain ______ and the first uncertain _____ (the estimated number).

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A (DIGIT) (a number between 1 and 10 with no decimals) that must be estimated is called uncertain. A measurement always has some degree of uncertainty. Record the certain (DIGITS) and the first uncertain (DIGIT) (the estimated number).

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12. Using a ruler the length of a pin occurs at about 2.85 cm; the _______ digits are 2.8, and the _________ digit is 5.

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Using a ruler the length of a pin occurs at about 2.85 cm; the (CERTAIN) digits are 2.8, and the (UNCERTAIN) digit is 5.

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13. Nonzero ________ always count as significant figures (3456 has 4 significant figures).

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Nonzero (INTEGERS) always count as significant figures (3456 has 4 significant figures).

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14. There are three classes of zeros: _______ zeros are zeros that precede all the nonzero digits, these do not count as significant figures (0.048 has two significant figures). _______ zeros are zeros between nonzero digits; these always count as significant figures (16.07 has four significant figures). ________ zeros are zeros at the right end of the number, they are significant only if the number contains a decimal point (9.300 has four significant figures; 150 has 2 significant figures).

Back 71

There are three classes of zeros: (LEADING) zeros are zeros that precede all the nonzero digits, these do not count as significant figures (0.048 has two significant figures). (CAPTIVE) zeros are zeros between nonzero digits; these always count as significant figures (16.07 has four significant figures). (TRAILING) zeros are zeros at the right end of the number, they are significant only if the number contains a decimal point (9.300 has four significant figures; 150 has 2 significant figures).

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15. Exact numbers have an ________ number of significant figures (1 inch = 2.54 cm, exactly), so regardless of how many digits are there, if the number is exact, all the figures in the number are significant.

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Exact numbers have an (INFINITE) number of significant figures (1 inch = 2.54 cm, exactly), so regardless of how many digits are there, if the number is exact, all the figures in the number are significant.

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16. Significant figures using ___________ ________ have two advantages, (1) the number of significant figures can be easily indicated, and (2) fewer zeros are needed to write a very large or very small number (300 written as 3.00 X 10², this contains three significant numbers).

Back 73

Significant figures using (EXPONENTIAL NOTATION) have two advantages, (1) the number of significant figures can be easily indicated, and (2) fewer zeros are needed to write a very large or very small number (300 written as 3.00 X 10², this contains three significant numbers).

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17. Rules for ________ ___ – is why we have significant figures (1) (if the digit to be removed is less than 5 [is the number to be rounded], the preceding digit stays the same; 5.64, if the answer requires 2 significant figures, will then round to 5.6). If the digit to be removed is equal to or greater than 5, the preceding digit is increased by 1 (if the final result is to be 2 figures, the next two answers will be as follows: 5.68 rounds to 5.7; and 3.861 rounds to 3.9). (2) In a series of calculations, carry the extra digits through to the final result and then round off (this means that you should carry all of the digits that show on your calculator until you arrive at the final number [the answer] and then round off, using the procedures in Rule 1).

Back 74

Rules for (ROUNDING OFF) – is why we have significant figures (1) (if the digit to be removed is less than 5 [is the number to be rounded], the preceding digit stays the same; 5.64, if the answer requires 2 significant figures, will then round to 5.6). If the digit to be removed is equal to or greater than 5, the preceding digit is increased by 1 (if the final result is to be 2 figures, the next two answers will be as follows: 5.68 rounds to 5.7; and 3.861 rounds to 3.9). (2) In a series of calculations, carry the extra digits through to the final result and then round off (this means that you should carry all of the digits that show on your calculator until you arrive at the final number [the answer] and then round off, using the procedures in Rule 1).

Front 75

18. Significant Figures in Mathematical Operations – (1) For multiplication or division, the number of significant figures in the result is the same as that in the measurement with the ________ number of significant figures (1.342 X 5.5 = 7.381 -> 7.4). (2) For addition or subtraction, the ________ ____ is the one with the smallest number of decimal places (23.445 + 7.83 = 31.275 – Corrected by rounding up to the lowest number of significant figures).

Back 75

Significant Figures in Mathematical Operations – (1) For multiplication or division, the number of significant figures in the result is the same as that in the measurement with the (SMALLEST) number of significant figures (1.342 X 5.5 = 7.381 -> 7.4). (2) For addition or subtraction, the (LIMITING TERM) is the one with the smallest number of decimal places (23.445 + 7.83 = 31.275 – Corrected by rounding up to the lowest number of significant figures).

Front 76

19. Significant Figures (Concept Check) – You have water in each graduated cylinder shown. You then add both samples to a beaker (assume that all of the liquid is transferred). How would you write the number describing the total volume? =_._ mL= What limits the precision of the total volume? =___ _________ ________=

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Significant Figures (Concept Check) – You have water in each graduated cylinder shown. You then add both samples to a beaker (assume that all of the liquid is transferred). How would you write the number describing the total volume? =(3.1) mL= What limits the precision of the total volume? =(1ST GRADUATED CYLINDER)=

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20. Problem Solving and Dimensional Analysis – Use when converting a given result from one system of units to another. (1) To convert from one unit to another, use the ___________ statement that relates the two units. (2) Choose the appropriate __________ factor by looking at the direction of the required change (make sure the unwanted units cancel). (3) Multiply the quantity to be _________ by the conversion factor to give the quantity with the desired units. (4) Check that you have the correct number of ___________ _______. (5) Does my answer make sense?

Back 77

Problem Solving and Dimensional Analysis – Use when converting a given result from one system of units to another. (1) To convert from one unit to another, use the (EQUIVALENCE) statement that relates the two units. (2) Choose the appropriate (CONVERSION) factor by looking at the direction of the required change (make sure the unwanted units cancel). (3) Multiply the quantity to be (CONVERTED) by the conversion factor to give the quantity with the desired units. (4) Check that you have the correct number of (SIGNIFICANT FIGURES). (5) Does my answer make sense?

Front 78

21. Problem Solving and Dimensional Analysis – Example #1a – A golfer putted a golf ball 6.8 ft. across a green. How many inches does this represent? To convert from one unit to another, use the ___________ statement that relates the two units.
(1 ft. = 12 in. The two unit factors are: 1 ft./12 in. and 12 in./1 ft.)

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Problem Solving and Dimensional Analysis – Example #1a – A golfer putted a golf ball 6.8 ft. across a green. How many inches does this represent? To convert from one unit to another, use the (EQUIVALENCE) statement that relates the two units.
(1 ft. = 12 in. The two unit factors are: 1 ft./12 in. and 12 in./1 ft.)

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22. Problem Solving and Dimensional Analysis – Example #1b – A golfer putted a golf ball 6.8 ft. across a green. How many inches does this represent? Choose the appropriate __________ factor by looking at the direction of the required change (make sure the unwanted units cancel). ft x in/ft = ?

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Problem Solving and Dimensional Analysis – Example #1b – A golfer putted a golf ball 6.8 ft. across a green. How many inches does this represent? Choose the appropriate (CONVERSION) factor by looking at the direction of the required change (make sure the unwanted units cancel). 6.8 ft. X 12 in./1 ft. = in. [the ft. cancel each other]).

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23. Problem Solving and Dimensional Analysis – Example #1c – A golfer putted a golf ball 6.8 ft. across a green. How many inches does this represent? Multiply the quantity to be _________ by the conversion factor to give the quantity with the desired units. 6.8 ft. X 12 in./1 ft. = __ in [the ft. cancel each other]). Correct significant figures? Does this answer make sense?

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Problem Solving and Dimensional Analysis – Example #1c – A golfer putted a golf ball 6.8 ft. across a green. How many inches does this represent? Multiply the quantity to be (CONVERTED) by the conversion factor to give the quantity with the desired units. 6.8 ft. X 12 in./1 ft. = (82) in [the ft. cancel each other]). Correct significant figures? Does this answer make sense?

Front 81

24. Problem Solving and Dimensional Analysis – Example #2 – An iron sample has a mass of 4.50 lbs. What is the mass of this sample in grams? (1 lb = 0.453592 kg; 1 kg. = 1000 g.)

Back 81

Problem Solving and Dimensional Analysis – Example #2 – An iron sample has a mass of 4.50 lbs. What is the mass of this sample in grams? (1kg = 2.2046 lbs.; 1 kg. = 1000 g.) 4.50 lbs. X 1kg./2.2046 lbs. X 1000 g/1kg. = 2.04 X 10³ g.

Front 82

25. Problem Solving and Dimensional Analysis – Concept Check – What data would you need to estimate the money you would spend on gasoline to drive your car from New York to Los Angeles? Provide estimates of values and a sample calculation.

Back 82

Problem Solving and Dimensional Analysis – Concept Check – What data would you need to estimate the money you would spend on gasoline to drive your car from New York to Los Angeles? Provide estimates of values and a sample calculation.
SAMPLE ANSWER: Distance between New York and Los Angeles: 2500 miles. Average gas mileage: 25 miles per gallon. Average cost of gasoline: $3.25 per gallon. 2500 mi X 1 gal/25 mi X $3.25/1 gal = $325

Front 83

26. Three Systems for Measuring Temperature – Fahrenheit, Celsius, and Kelvin. _______ Point of Water: 212˚ F, 100˚ C, and 373˚ K; ________ Point of Water: 32˚ F, 0˚ C, and 273˚ K; 0˚F is -18˚ C, and 255˚ K; ________ ____ is 0˚ K, which is -460˚ F, and -273˚ C.

Back 83

Three Systems for Measuring Temperature – Fahrenheit, Celsius, and Kelvin. (BOILING) Point of Water: 212˚ F, 100˚ C, and 373˚ K; (FREEZING) Point of Water: 32˚ F, 0˚ C, and 273˚ K; 0˚F is -18˚ C, and 255˚ K; (ABSOLUTE ZERO) is 0˚ K, which is -460˚ F, and -273˚ C.

Front 84

27. _______ – Mass of substance per unit volume of the substance; common units are g/cm³ or g/mL.

Back 84

(DENSITY) – Mass of substance per unit volume of the substance; common units are g/cm³ or g/mL.

Front 85

28. Density – Example #1 – A certain mineral has a mass of 17.8 g and a volume of 2.35 cm³. What is the density of this mineral? Density = ____/______

Back 85

Density – Example #1 – A certain mineral has a mass of 17.8 g and a volume of 2.35 cm³. What is the density of this mineral? Density = (MASS)/(VOLUME) (D=M/V)
Density = 17.8 g/2.35 cm³; Density = 7.57 g/cm³

Front 86

29. Density – Example #2 – What is the mass of a 49.6 mL sample of a liquid, which has a density of 0.85 g/mL? D=M/V

Back 86

Density – Example #2 – What is the mass of a 49.6 mL sample of a liquid, which has a density of 0.85 g/mL? Density = mass/volume
0.85 g/mL = x/49.6 mL; mass =
x = 42 g

Front 87

30. Density – Exercise – If an object has a mass of 243.8 g and occupies a volume of 0.125 L, what is the density of this object in g/cm³?
D=M/V; 1 liter = 1000 milliliter

Back 87

Density – Exercise – If an object has a mass of 243.8 g and occupies a volume of 0.125 L, what is the density of this object in g/cm³?
=1.95 g/cm³=

Front 88

31. Density – Concept Check – Copper has a density of 8.96 g/cm³. If 75.0 g of copper is added to 50.0 mL of water in a graduated cylinder, to what volume reading will the water level in the cylinder rise?
D=M/V

Back 88

Density – Concept Check – Copper has a density of 8.96 g/cm³. If 75.0 g of copper is added to 50.0 mL of water in a graduated cylinder, to what volume reading will the water level in the cylinder rise?
=58.4 mL=

Front 89

1. Scientific Notation
a) Technique used to express very large or very small numbers.
b) Expresses a number as a _______ of a number between 1 and 10 and the appropriate power of 10.

Back 89

Scientific Notation
a) Technique used to express very large or very small numbers.
b) Expresses a number as a (PRODUCT) of a number between 1 and 10 and the appropriate power of 10.

Front 90

2. Using Scientific Notation
• Any number can be represented as the product of a number between 1 and 10 and a power of 10 (either positive or negative).
regular notation scientific notation
• 93,000,000 = 9.3 x 10,000,000 = 9.3 x 10⁷
• 0.00000093 = 9.3 / 10,000,000 = 9.3 x 10⁻⁷
• The power of 10 depends on the number of places the _______ _____ is moved and in which direction.

Back 90

Using Scientific Notation
• Any number can be represented as the product of a number between 1 and 10 and a power of 10 (either positive or negative).
regular notation scientific notation
• 93,000,000 = 9.3 x 10,000,000 = 9.3 x 10⁷
• 0.00000093 = 9.3 / 10,000,000 = 9.3 x 10⁻⁷
The power of 10 depends on the number of places the (DECIMAL POINT) is moved and in which direction.

Front 91

3. Using Scientific Notation
• If the decimal point is moved to the left, the power of 10 is ________.
• If the decimal point is moved to the right, the power of 10 is ________.

Back 91

Using Scientific Notation
• If the decimal point is moved to the left, the power of 10 is (POSITIVE).
345 = 3.45 × 10²
• If the decimal point is moved to the right, the power of 10 is (NEGATIVE).
0.0671 = 6.71 × 10⁻²

Front 92

4. Concept Check
Which of the following correctly expresses 7,882 in scientific notation?
a) 7.882 × 10⁴
b) 788.2 × 10³
c) 7.882 × 10³
d) 7.882 × 10⁻³

Back 92

c) 7.882 × 10³

Front 93

5. Concept Check
Which of the following correctly expresses 0.0000496 in scientific notation?
a) 4.96 × 10⁻⁵
b) 4.96 × 10⁻⁶
c) 4.96 × 10⁻⁷
d) 496 × 10⁷

Back 93

a) 4.96 × 10⁻⁵

Front 94

6. Capacity vs. # of Decimal Places

• Maximum Capacity 150 g
• This flask has a mass of 82.2863 g
• 4 decimal places

Back 94

Capacity vs. # of Decimal Places

Maximum capacity 34,000 pounds
This truck weighs 10,050 pounds
No decimal places

Front 95

7. Uncertainty of Measurement
a) A digit that must be _________ is called uncertain.
b) A measurement always has some degree of uncertainty.
c) Record the certain digits and the _____ uncertain digit (the _________ number).

Back 95

Uncertainty of Measurement
a) A digit that must be (ESTIMATED) is called uncertain.
b) A measurement always has some degree of uncertainty.
c) Record the certain digits and the (FIRST) uncertain digit (the [ESTIMATED] number).

Front 96

8. Measurement of Length Using a Ruler
a) The length of the pin occurs at about _.__ cm.
b) Certain digits: _.__
c) Uncertain digit: _.__
d) Estimate between _._-_._

Back 96

Measurement of Length Using a Ruler
a) The length of the pin occurs at about (2.85) cm.
b) Certain digits: (2.8)
c) Uncertain digit: (0.05)
d) Estimate between (2.8-2.9)

Front 97

9. Rules for Rounding Off
If the digit to be removed is equal to or greater than 5, the preceding digit is increased by 1.
 5.68 rounds to _._ (if final result to 2 sig figs)
 3.861 rounds to _._ (if final result to 2 sig figs)

Back 97

Rules for Rounding Off
If the digit to be removed is equal to or greater than 5, the preceding digit is increased by 1.
 5.68 rounds to (5.7) (if final result to 2 sig figs)
 3.861 rounds to (3.9) (if final result to 2 sig figs)

Front 98

10. Significant Figures in Mathematical Operations
a. For multiplication or division, the number of significant figures in the result is the same as that in the measurement with the smallest number of ___________ _______.
b. For addition or subtraction, the limiting term is the one with the smallest number of _______ ______.

Back 98

Significant Figures in Mathematical Operations
a. For multiplication or division, the number of significant figures in the result is the same as that in the measurement with the smallest number of (SIGNIFICANT FIGURES).
1.342 × 5.5 = 7.381  7.4
b. For addition or subtraction, the limiting term is the one with the smallest number of (DECIMAL PLACES).

Front 99

11. Concept Check
You have water in each graduated cylinder shown. You then add both samples to a beaker (assume that all of the liquid is transferred).
How would you write the number describing the total volume?
What limits the precision of the total volume?

Back 99

11. Concept Check
You have water in each graduated cylinder shown. You then add both samples to a beaker (assume that all of the liquid is transferred).
How would you write the number describing the total volume?
3.1 mL
What limits the precision of the total volume?
1st graduated cylinder

Front 100

12. Example #1
A golfer putted a golf ball 6.8 ft across a green. How many inches does this represent?
• Choose the appropriate conversion factor by looking at the direction of the required change (make sure the unwanted units cancel).
ft x in/ft = in

Back 100

12. Example #1
A golfer putted a golf ball 6.8 ft across a green. How many inches does this represent?
• Choose the appropriate conversion factor by looking at the direction of the required change (make sure the unwanted units cancel).

Front 101

13. Example #1
A golfer putted a golf ball 6.8 ft across a green. How many inches does this represent?
• Multiply the quantity to be converted by the conversion factor to give the quantity with the desired units.
ft x in/ft = in

Back 101

13. Example #1
A golfer putted a golf ball 6.8 ft across a green. How many inches does this represent?
• Multiply the quantity to be converted by the conversion factor to give the quantity with the desired units.
• Correct sig figs? Does my answer make sense?

Front 102

14. Example #2
An iron sample has a mass of 4.50 lb. What is the mass of this sample in grams?
(1 kg = 2.2046 lbs; 1 kg = 1000 g)

Back 102

14. Example #2
An iron sample has a mass of 4.50 lb. What is the mass of this sample in grams?
(1 kg = 2.2046 lbs; 1 kg = 1000 g)

Front 103

15. Concept Check
What data would you need to estimate the money you would spend on gasoline to drive your car from New York to Los Angeles? Provide estimates of values and a sample calculation.

Back 103

15. Concept Check
What data would you need to estimate the money you would spend on gasoline to drive your car from New York to Los Angeles? Provide estimates of values and a sample calculation.
Sample Answer:
Distance between New York and Los Angeles: 2500 miles
Average gas mileage: 25 miles per gallon
Average cost of gasoline: $3.25 per gallon

Front 104

16. The Three Major Temperature Scales

Back 104

Converting Between Scales

Front 105

17. Exercise
The normal body temperature for a dog is approximately 102°F. What is this equivalent to on the Kelvin temperature scale?
a) 373 K
b) 312 K
c) 289 K
d) 202 K

Back 105

1. Exercise
The normal body temperature for a dog is approximately 102°F. What is this equivalent to on the Kelvin temperature scale?
b) 312 K

Front 106

18. Exercise
At what temperature does °C = °F?
• Since °C equals °F, they both should be the same value (designated as variable x).
• Use one of the conversion equations such as:
• Substitute in the value of x for both T°C and T°F. Solve for x.

Back 106

If °C = -40
°F = 1.80 (°C) +32 = 1.80 (-40) +32 = -72 + 32 = -40

Front 107

19. Mass of substance per unit volume of the substance.
Common units are g/cm³ or g/mL.

Back 107

Front 108

20. Example #1
A certain mineral has a mass of 17.8 g and a volume of 2.35 cm³. What is the density of this mineral?

Back 108

Front 109

21. Example #2
What is the mass of a 49.6 mL sample of a liquid, which has a density of 0.85 g/mL?

Back 109

Front 110

22. Exercise
If an object has a mass of 243.8 g and occupies a volume of 0.125 L, what is the density of this object in g/cm³?
(1 L = 0.001 kL; D=M/V)
a) 0.513
b) 1.95
c) 30.5
d) 1950

Back 110

1. Exercise
If an object has a mass of 243.8 g and occupies a volume of 0.125 L, what is the density of this object in g/cm³?
b) 1.95

Front 111

23. Concept Check
Copper has a density of 8.96 g/cm3. If 75.0 g of copper is added to 50.0 mL of water in a graduated cylinder, to what volume reading will the water level in the cylinder rise?
(D=M/V)
a) 8.4 mL
b) 41.6 mL
c) 58.4 mL
d) 83.7 mL

Back 111

1. Concept Check
Copper has a density of 8.96 g/cm3. If 75.0 g of copper is added to 50.0 mL of water in a graduated cylinder, to what volume reading will the water level in the cylinder rise?
c) 58.4 mL

Front 112

1. Many scientific measurements involve very small or very large numbers, which can be quite bulky. For example, radioactive disintegrations are measured in units of curies. One curie is approximately equal to 37,000,000,000 disintegrations per second. What is this number expressed in scientific notation?
1) 3.7 × 10¹⁰
2) 37 × 10¹⁰
3) 3.7 × 10⁻¹⁰
4) 0.37 × 10¹⁰

Back 112

Choice #1 is the correct answer. We move the decimal point to the left ten times in order to get 3.7 (a number between 1 and 10) to yield the answer 3.7 × 10¹⁰.

Front 113

2. In recent years, many substances have been found to be harmful to human health, even if present in very low concentrations. For example, dioxin, which has been classified by the World Health Organization as a known human carcinogen, has been found to be lethal to monkeys at an oral dose of less than 0.000070 grams per kilogram of body weight. What is this number expressed in scientific notation?
1) 0.70 × 10⁴
2) 7.0 × 10⁻⁴
3) 7.0 × 10⁻⁵
4) 70 × 10⁴

Back 113

Choice #3 is the correct answer. Because we have to move the decimal point five places to the right in order to obtain 7.0 (a number between 1 and 10), we arrive at the answer 7.0 × 10⁻⁵.

Front 114

3. Which of the following correctly expresses 7,882 in scientific notation?
1. 7.882 × 10⁴
2. 788.2 × 10³
3. 7.882 × 10³
4. 7.882 × 10⁻³

Back 114

Choice #3 is the correct answer. The decimal point should be moved three places to the left to be correctly expressed in scientific notation.

Front 115

4. Which of the following correctly expresses 0.0000496 in scientific notation?
1. 4.96 × 10⁻⁵
2. 4.96 × 10⁻⁶
3. 4.96 × 10⁻⁷
4. 496 × 10⁷

Back 115

Choice #1 is the correct answer. The decimal point should be moved five places to the right to be correctly expressed in scientific notation.

Front 116

5. In 1999 the Mars Climate Orbiter (worth $125 million) was destroyed due to confusion over units. The scientists at NASA assumed data was in metric units when actually it was in English units, and as a result the Orbiter dipped 100 kilometers deeper into the Mars’ atmosphere than was anticipated and the craft burned up due to atmospheric friction. Convert 100 kilometers into units of meters. (1km = 1000m)
1) 1 × 10² m
2) 1 × 10⁻² m
3) 1 × 10⁴ m
4) 1 × 10⁵ m

Back 116

Choice #4 is the correct answer. Multiply the value by an appropriate conversion factor to change 100 km to m. We can use 1000 m in the numerator (equal to 1 km) as the conversion factor:
100 × 1000 m/1 km = 1 × 10⁵ m

Front 117

6. How many nickels are equal to the value of the lost Mars Climate Orbiter (valued at $125 million)?
(20 nickels = 1 dollar)
1) 5.00 × 10⁵
2) 1.25 × 10⁶
3) 2.50 × 10⁹
4) 1.00 × 10¹⁰

Back 117

Choice #3 correctly expresses the number of nickels.
(20 nickels = 1 dollar)
125 million × 20 = 2.50 × 10⁹ nickels

Front 118

7. Choose the statement that contains an improper use of a commonly used unit (doesn’t make sense)?
1. A gallon of milk is equal to about 4 L of milk.
2. A 200-lb man has a mass of about 90 kg.
3. A basketball player has a height of 7 m tall.
4. A nickel is 2 mm thick.

Back 118

Choice #3 doesn’t make sense. A basketball player cannot be 7 m tall (but rather 7 feet tall). There are about 3 feet in a meter so it’s more likely that the player has a height of 2.3 m.

Front 119

8. If the graduated cylinder pictured here were used to measure a volume of liquid, which value below is most likely to represent a value recorded correctly, considering the uncertainty in the measurement?
1) 10 mL
2) 61 mL
3) 72.5 mL
4) 81.45 mL

Back 119

Choice #3 correctly represents a measurement likely to be made. Note that the first 2 figures would be measured and the third figure would be estimated.

Front 120

9. Using zero as your reference point, how much liquid has left the buret?
1) 20 mL
2) 22 mL
3) 22.0 mL
4) 38 mL

Back 120

Choice #3 is the correct answer. Note that the first 2 figures can be exactly measured and the third figure has to be estimated.

Front 121

10. A forensic chemist in a crime lab weighs a shard of colored thread removed from a suspicious vehicle and records the weight as 0.002500 g. This number contains how many significant figures?
1. 2
2. 4
3. 6
4. 7

Back 121

Choice #2 is the correct answer. The first three zeroes are insignificant because they are “leading zeroes,” which can be thought of as “place holders.” The last two zeroes would not be recorded unless they were significant. Remember that you should always assume that you are looking at a measured number in which the last digit recorded is estimated and is therefore significant.

Front 122

11. If a geochemist has measured the concentration of lead in the sediments of a polluted waterway to be 2.446 ppm (parts per million), how would this number be reported correctly if rounded off to 2 significant figures?
1) 2.45 ppm
2) 2.4 ppm
3) 2.5 ppm
4) 2.46 ppm

Back 122

Choice #2 is correct. Note that we do not round the 4 to a 5 because there is a 4 to the right of it.

Front 123

12. What is the length of the nail reported to the correct number of significant figures ?

1. 4.4 cm
2. 4.40 cm
3. 4.44 cm
4. 5 cm

Back 123

Choice #1 is the correct answer. The first digit is certain since the nail clearly lies between the 4 and 5 cm graduations. The second digit is estimated since you’re estimating between the graduations.

Front 124

13. Upon adding together the numbers below
5.88
+ 5.12
The answer is correctly expressed as
1) 11
2) 11.0
3) 11.00
4) 11.000

Back 124

Choice #3 is the correct answer. Note that when adding numbers together, it is possible to generate an answer with a greater number of significant figures than is present in the individual numbers.

Front 125

14. You take 20.0 mL of water from a graduated cylinder and add it to the beaker of water shown. What is the new volume of water in the beaker?

1. 40. mL
2. 35 mL
3. 35.0 mL
4. 25.0 mL

Back 125

Choice #2 is the correct answer. The original volume of water in the beaker is 15 mL (with “5” as the estimated digit). When 20.0 mL of water is added, you must report the added volumes to the least number of decimal places (which is to the ones place).

Front 126

15. How many centimeters long is this arrow? (1 inch = 2.54 cm)?
1. 11.68 cm
2. 11.9 cm
3. 12.446 cm
4. 12 cm

Back 126

Choice #4 is the correct answer. The arrow is estimated at 4.7 inches. This measurement then has to be converted to cm using the conversion factor 2.54 cm = 1 inch.
4.7 in × 2.54 cm/1in = 12 cm
The final answer is to 2 significant figures since the original measurement is to 2 significant figures.

Front 127

16. While driving in London you encounter a speed limit sign that reads 80 km/hr. How fast can you legally travel in miles/hr?
(1 km = 0.621371 mph)
1. 80
2. 70
3. 60
4. 50

Back 127

Choice #4 is the correct answer. If you use the conversion factors given in the chapter, your setup might look like this:
80 km/hr × 1000m/km × 1.094 yd/m × 1 mile/1760 yd = 50 mph
If you had available the conversion 0.62 miles = 1 km, you could have done the problem in one step:
80 km/hr × 0.62 miles/km = 50 miles/hr

Front 128

17. Mercury is the only metal known to exist as a liquid at room temperature and pressure. It has a very high density of 13.6 g/mL. Convert the density of mercury into units of lbs/in³.
(1 g/mL = 0.036127298147753 lb/in³)
1. 0.00183
2. 0.0762
3. 0.193
4. 0.491

Back 128

Choice #4 is the correct answer. Using dimensional analysis, we employ conversion factors that cancel out the units we want eliminated and yield the desired units.
13.6 g/mL × 1.00 lb/453.6 g × 1 mL/1 cm³ × (2.54 cm/1.00 in.)³ = 0.491 lb/in³

Front 129

18. The normal body temperature for a dog is approximately 102°F.
What is this equivalent to on the Kelvin temperature scale?
1. 373 K
2. 312 K
3. 289 K
4. 202 K

Back 129

Choice #2 is correct.
(102 – 32) / 1.80 = 39°C
39 + 273 = 312 K

Front 130

19. If an object has a mass of 243.8 g and occupies a volume of 0.125 L, what is the density of this object in g/cm³?
(1 L = 1000 cm³; D=M/V)
1. 0.513
2. 1.95
3. 30.5
4. 1950

Back 130

Choice #2 is correct. Density = mass/volume. First convert 0.125 L to cm³.
0.125 L × 1000 mL/1 L × 1 cm³/1mL = 125 cm³
Density = 243.8 g / 125 cm³ = 1.95 g/cm³

Front 131

20. Copper has a density of 8.96 g/cm³. If 75.0 g of copper is added to 50.0 mL of water in a graduated cylinder, to what volume reading will the water level in the cylinder rise?
1. 8.4 mL
2. 41.6 mL
3. 58.4 mL
4. 83.7 mL

Back 131

Choice #3 is the correct answer. Using the density and mass of copper, determine the volume of metal present.
75.0 g × cm³/8.96 g = 8.37 cm³
Since the density of water is 1 g/1 mL, the volume of the metal can be determined by displacement. Therefore, the water level will rise to 58.4 mL (50.0 + 8.37 mL).

Front 132

The “stuff” of which the universe is composed, which has two characteristics: it has mass and it occupies space.

Back 132

1. Matter

Front 133

This takes the form of solid, liquid, and gas. The state of a given form of these depends on the strength of the forces among the particles contained.

Back 133

2. States of Matter

Front 134

Rigid, has a fixed shape and volume.

Back 134

3. Solid

Front 135

Has a definite volume but takes the shape of its container.

Back 135

4. Liquid

Front 136

Has no fixed volume or shape; takes the shape and volume of its container.

Back 136

5. Gas

Front 137

The unique characteristics of substances, which include: odor, color, volume, state (gas, liquid, or solid), density, melting point, and boiling point.

Back 137

6. Physical Properties

Front 138

Refers to a substances ability to form new substances (burning wood turning to ash, rusting of steel on our cars, the digestion of food in our stomachs, and grass growing in our yards); a given substance changes to a fundamentally different substance or substances.

Back 138

7. Chemical Properties

Front 139

A change in one or more physical properties, but no change in the fundamental components that make up the substance; the most common are changes of state: solid<->liquid<->gas.

Back 139

8. Physical Change

Front 140

A change in the fundamental components of the substance; a given substance changes into a different substance or substances. These are called reactions: silver tarnishes by reacting with substances in the air; a plant forms a leaf by combining various substances from the air and soil; and so on.

Back 140

9. Chemical Change

Front 141

Chemical changes.

Back 141

10. Reaction

Front 142

A series of fundamental substances which cannot be broken down into other substances by chemical means (iron, aluminum, oxygen, and hydrogen); all of the matter in the world around us contains these, most substances contain several of these combined together.

Back 142

11. Element

Front 143

A substance composed of a given combination of elements that can be broken down into those elements by chemical methods.

Back 143

12. Compound

Front 144

Something that has variable composition.

Back 144

13. Mixture

Front 145

Something that will always have the same composition; these are either elements or compounds.

Back 145

14. Pure Substance

Front 146

A solution which is the same throughout, which does not vary in composition from one region to another (dissolving salt in water [and stirring well], will produce all regions with the same properties).

Back 146

15. Homogeneous Mixture

Front 147

A homogeneous mixture of two or more substances, which may be solids, liquids, gases, or a combination of these (or the process of forming such a mixture).

Back 147

16. Solution

Front 148

Contains regions that have different properties from those of other regions (pouring sand into water – one region contains water, and the other contains sand).

Back 148

17. Heterogeneous Mixture

Front 149

The separation of a liquid mixture into its components on the basis of differences in boiling points.

Back 149

18. Distillation

Front 150

A mechanical or physical process to separate solid particulates from fluids.

Back 150

19. Filtration

Front 151

1. ______ can exist in three states – solid, liquid, and gas – and can be described in terms of its physical and chemical properties. ________ properties describe a substance’s ability to undergo a change to a different substance. ________ properties are the characteristics a substance exhibits as long as no chemical change occurs.

Back 151

(MATTER) can exist in three states – solid, liquid, and gas – and can be described in terms of its physical and chemical properties. (CHEMICAL) properties describe a substance’s ability to undergo a change to a different substance. (PHYSICAL) properties are the characteristics a substance exhibits as long as no chemical change occurs.

Front 152

2. A ________ change involves a change in one or more physical properties, but no change in composition. A ________ change transforms a substance into a new substance or substances.

Back 152

A (PHYSICAL) change involves a change in one or more physical properties, but no change in composition. A (CHEMICAL) change transforms a substance into a new substance or substances.

Front 153

3. A mixture has variable composition. A ___________ mixture has the same properties throughout; a _____________ mixture does not. A pure substance always has the same ___________. We can physically separate mixtures of pure substances by distillation and filtration.

Back 153

A mixture has variable composition. A (HOMOGENEOUS) mixture has the same properties throughout; a (HETEROGENEOUS) mixture does not. A pure substance always has the same (COMPOSITION). We can physically separate mixtures of pure substances by distillation and filtration.

Front 154

4. Pure substances are of two types: ________, which cannot be broken down chemically into simpler substances, and _________, which can be broken down chemically into elements.

Back 154

Pure substances are of two types: (ELEMENTS), which cannot be broken down chemically into simpler substances, and (COMPOUNDS), which can be broken down chemically into elements.

Front 155

1. Matter – Anything occupying _____ and having ____; exists in three states: solid, liquid, and gas.

Back 155

Matter – Anything occupying (SPACE) and having (MASS); exists in three states: solid, liquid, and gas.

Front 156

2. Matter – Solid, is rigid, and has a fixed ______ and _____ (ice cube, diamond, and iron bar).

Back 156

Matter – Solid, is rigid, and has a fixed (VOLUME) and (SHAPE) (ice cube, diamond, and iron bar).

Front 157

3. Matter – Liquid, has a definite ______ but no specific shape, and assumes the shape of _________ (gasoline, water, alcohol, and blood).

Back 157

Matter – Liquid, has a definite (VOLUME) but no specific shape, and assumes the shape of (CONTAINER) (gasoline, water, alcohol, and blood).

Front 158

4. Matter – Gas, has no fixed ______ or _____, and takes the shape and volume of its container (air, helium, and oxygen).

Back 158

Matter – Gas, has no fixed (VOLUME) or (SHAPE), and takes the shape and volume of its container (air, helium, and oxygen).

Front 159

5. Physical Properties – The characteristics of matter that can be changed without changing its ___________; characteristics that are directly __________ (odor, color, volume, state [solid, liquid, or gas], density, melting point, and boiling point).

Back 159

Physical Properties – The characteristics of matter that can be changed without changing its (COMPOSITION); characteristics that are directly (OBSERVABLE) (odor, color, volume, state [solid, liquid, or gas], density, melting point, and boiling point).

Front 160

6. Chemical Properties – A substances ability to form new __________, the characteristics that determine how the composition of matter changes as a result of contact with other matter or the influence of ______; characteristics that describe the behavior of matter (flammability, rusting of steel, and the digestion of food).

Back 160

Chemical Properties – A substances ability to form new (SUBSTANCES), the characteristics that determine how the composition of matter changes as a result of contact with other matter or the influence of (ENERGY); characteristics that describe the behavior of matter (flammability, rusting of steel, and the digestion of food).

Front 161

7. Physical and Chemical Properties – Concept Check – Classify each of the following as a physical or chemical property: Ethyl alcohol boiling at 78˚ C (________); Hardness of a diamond (________); Sugar fermenting to form ethyl alcohol (________).

Back 161

Physical and Chemical Properties – Concept Check – Classify each of the following as a physical or chemical property: Ethyl alcohol boiling at 78˚ C ([PHYSICAL]); Hardness of a diamond ([PHYSICAL]); Sugar fermenting to form ethyl alcohol ([CHEMICAL]).

Front 162

8. Physical Change – Change in the form of a _________, not in its ________ composition (boiling or freezing water).

Back 162

Physical Change – Change in the form of a (SUBSTANCE), not in its (CHEMICAL) composition (boiling or freezing water).

Front 163

9. Three States of Water – In all three phases, water molecules are still intact; _______ of molecules and the _________ between them change.

Back 163

Three States of Water – In all three phases, water molecules are still intact; (MOTIONS) of molecules and the (DISTANCES) between them change.

Front 164

10. Chemical Change – A given substance becomes a new substance or substances with different __________ and different ___________. (Bunsen burner [methane reacts with oxygen to form carbon dioxide and water]).

Back 164

Chemical Change – A given substance becomes a new substance or substances with different (PROPERTIES) and different (COMPOSITION). (Bunsen burner [methane reacts with oxygen to form carbon dioxide and water]).

Front 165

11. Electrolysis of Water – Water decomposes to ________ and ______ gases.

Back 165

Electrolysis of Water – Water decomposes to (HYDROGEN) and (OXYGEN) gases.

Front 166

12. Physical and Chemical Properties – Concept Check – How many of the following are examples of a chemical change? Pulverizing (crushing) rock salt, Burning of wood, Dissolving of sugar in water, Melting a popsicle on a warm summer day; =_______________=

Back 166

Physical and Chemical Properties – Concept Check – How many of the following are examples of a chemical change? Pulverizing (crushing) rock salt, Burning of wood, Dissolving of sugar in water, Melting a popsicle on a warm summer day. =(BURNING OF WOOD)=

Front 167

13. Physical and Chemical Properties – Concept Check – Classify each of the following as a physical or chemical change: Sugar fermenting to form ethyl alcohol (________); Iron metal melting (________); Iron combining with oxygen to form rust (________).

Back 167

Physical and Chemical Properties – Concept Check – Classify each of the following as a physical or chemical change: Sugar fermenting to form ethyl alcohol ([CHEMICAL]); Iron metal melting ([PHYSICAL]); Iron combining with oxygen to form rust ([CHEMICAL]).

Front 168

14. Element – A substance that cannot be broken down into other substances by ________ methods (contains only one type of ____). Examples: Iron (Fe), aluminum (Al), oxygen (O²), and hydrogen (H²). All of the ______ in the world around us contains elements.

Back 168

Element – A substance that cannot be broken down into other substances by (CHEMICAL) methods (contains only one type of [ATOM]). Examples: Iron (Fe), aluminum (Al), oxygen (O²), and hydrogen (H²). All of the (MATTER) in the world around us contains elements.

Front 169

15. Compound – A substance composed of a given ___________ of different elements that can be broken down into those elements by chemical methods. Examples: Water (H²O), carbon dioxide (CO²), table sugar (C¹²H²²O¹¹). A compound always contains atoms of different ________, always has the same ___________, and the same combination of atoms in the same ___________.

Back 169

Compound – A substance composed of a given (COMBINATION) of different elements that can be broken down into those elements by chemical methods. Examples: Water (H²O), carbon dioxide (CO²), table sugar (C¹²H²²O¹¹). A compound always contains atoms of different (ELEMENTS), always has the same (COMPOSITION), and the same combination of atoms in the same (PROPORTIONS).

Front 170

16. Elements and Compounds – Concept Check – How many of the following are compounds? H²O, N²O, NaOH, MnO², HF. =____________________=

Back 170

Elements and Compounds – Concept Check – How many of the following are compounds? H²O, N²O, NaOH, MnO², HF. =5 – ALL OF THE SUBSTANCES ARE COMPOUNDS=

Front 171

17. Pure Substances – Always have the same composition, and are either ________ or _________ (pure water [H²O], carbon dioxide [CO²], hydrogen [H²], gold [Au]).

Back 171

Pure Substances – Always have the same composition, and are either (ELEMENTS) or (COMPOUNDS) (pure water [H²O], carbon dioxide [CO²], hydrogen [H²], gold [Au]).

Front 172

18. Mixtures – Have ________ composition, and can be separated into ____ substances: elements and/or compounds, these are two or more ____ substances (wood, wine, coffee).

Back 172

Mixtures – Have (VARIABLE) composition, and can be separated into (PURE) substances: elements and/or compounds, these are two or more (PURE) substances (wood, wine, coffee).

Front 173

19. Homogeneous Mixture – Is the ____ throughout, has visibly _________________ parts, is a ________, and does not vary in composition from one region to another (the air around us, brass, table salt dissolved into water).

Back 173

Homogeneous Mixture – Is the (SAME) throughout, has visibly (INDISTINGUISHABLE) parts, is a (SOLUTION), and does not vary in composition from one region to another (the air around us, brass, table salt dissolved into water).

Front 174

20. Heterogeneous Mixture – Having visibly _______________ parts, contains regions that have different __________ from those of other regions (oil and vinegar dressing, sand stirred into water).

Back 174

Heterogeneous Mixture – Having visibly (DISTINGUISHABLE) parts, contains regions that have different (PROPERTIES) from those of other regions (oil and vinegar dressing, sand stirred into water).

Front 175

21. Mixtures and Pure Substances – Concept Check – Which of the following is a homogeneous mixture? Pure water, gasoline, jar of jelly beans, soil, copper metal. =____________=

Back 175

Mixtures and Pure Substances – Concept Check – Which of the following is a homogeneous mixture? Pure water, gasoline, jar of jelly beans, soil, copper metal. =GASOLINE=

Front 176

22. Separation of Mixtures – Mixtures can be separated based on different physical properties of the __________. Different Physical Property (Technique): _______ Point (Distillation), State of Matter – Solid/Liquid/Gas (Filtration), Adherence to a Surface (Chromatography), __________ (Evaporation).

Back 176

Separation of Mixtures – Mixtures can be separated based on different physical properties of the (COMPONENTS). Different Physical Property (Technique): (BOILING) Point (Distillation), State of Matter – Solid/Liquid/Gas (Filtration), Adherence to a Surface (Chromatography), (VOLATILITY) (Evaporation).

Front 177

23. Separation of Mixtures – No ________ change occurs when salt water is distilled.

Back 177

Separation of Mixtures – No (CHEMICAL) change occurs when salt water is distilled.

Front 178

24. Filtration – separates a ______ from a _____.

Back 178

Filtration – separates a (LIQUID) from a (SOLID).

Front 179

1. Matter is:
a) Anything occupying space and having mass.
b) Has physical and chemical properties
c) The physical and chemical properties of a substance of matter are determined by its ___________ and _________

Back 179

Matter is:
a) Anything occupying space and having mass.
b) Has physical and chemical properties
c) The physical and chemical properties of a substance of matter are determined by its (COMPOSITION) and (STRUCTURE)

Front 180

2. Physical Properties
The characteristics of matter that can be _______ without changing its composition.

Back 180

Physical Properties
The characteristics of matter that can be (CHANGED) without changing its composition.

Front 181

3. Physical Change
Change in the ____ of a substance, not in its chemical composition.

Back 181

Physical Change
Change in the (FORM) of a substance, not in its chemical composition.

Front 182

4. Chemical Properties
A substance’s ability to form ___ __________.

Back 182

Chemical Properties
A substance’s ability to form (NEW SUBSTANCES).

Front 183

5. Chemical Change
A substance becomes a new substance or substances with different properties and different ___________.

Back 183

Chemical Change
A substance becomes a new substance or substances with different properties and different (COMPOSITION).

Front 184

6. Concept Check
Classify each of the following as a physical or chemical property.
 Ethyl alcohol boiling at 78°C
 Hardness of a diamond
 Sugar fermenting to form ethyl alcohol

Back 184

Ethyl alcohol boiling at 78°C -Physical
Hardness of a diamond -Physical
Sugar fermenting to form ethyl alcohol -Chemical

Front 185

7. Concept Check
How many of the following are examples of a chemical change?
 Pulverizing (crushing) rock salt
 Burning of wood
 Dissolving of sugar in water
 Melting a popsicle on a warm summer day

Back 185

1. Concept Check
How many of the following are examples of a chemical change?
 Burning of wood

Front 186

8. Concept Check
Classify each of the following as a physical or chemical change.
 Sugar fermenting to form ethyl alcohol
 Iron metal melting
 Iron combining with oxygen to form rust

Back 186

Sugar fermenting to form ethyl alcohol-Chemical
Iron metal melting-Physical
Iron combining with oxygen to form rust-Chemical

Front 187

9. Element
A substance of matter that cannot be ______ ____ into other substances by chemical methods
a) Contains only one type of atom
Examples:
b) Iron (Fe), aluminum (Al), oxygen (O²), and hydrogen (H²)
All of the ______ in the world around us contains elements.

Back 187

Element
A substance of matter that cannot be (BROKEN DOWN) into other substances by chemical methods
c) Contains only one type of atom
Examples:
d) Iron (Fe), aluminum (Al), oxygen (O²), and hydrogen (H²)
All of the (MATTER) in the world around us contains elements.

Front 188

10. Compound
A substance composed of a given combination of different ________ that can be broken down into those ________ by chemical methods.
Examples:
a) Water (H²O), carbon dioxide (CO²), table sugar (C¹²H²²O¹¹)
A compound always contains atoms of _________ elements.
A compound always has the same composition
Same combination of _____ in the same proportions.

Back 188

Compound
A substance composed of a given combination of different (ELEMENTS) that can be broken down into those (ELEMENTS) by chemical methods.
Examples:
b) Water (H2O), carbon dioxide (CO²), table sugar (C¹²H²²O¹¹)
A compound always contains atoms of (DIFFERENT) elements.
A compound always has the same composition
Same combination of (ATOMS) in the same proportions.

Front 189

11. Pure Substances
______ have the same ___________.
Either elements or compounds.
Examples:
Pure water (H²O), carbon dioxide (CO²), hydrogen (H²), gold (Au)

Back 189

Pure Substances
(ALWAYS) have the same (COMPOSITION).
Either elements or compounds.
Examples:
Pure water (H²O), carbon dioxide (CO²), hydrogen (H²), gold (Au)

Front 190

12. Mixtures
Have variable composition.
Examples
a) Wood, wine, coffee
Can be separated into pure substances: ________ and/or _________.

Back 190

Mixtures
Have variable composition.
Examples
b) Wood, wine, coffee
Can be separated into pure substances: (ELEMENTS) and/or (COMPOUNDS).

Front 191

13. Homogeneous Mixture
Same throughout.
Having visibly _________________ parts.
A solution.
Does not vary in ___________ from one region to another.

Back 191

Homogeneous Mixture
Same throughout.
Having visibly (INDISTINGUISHABLE) parts.
A solution.
Does not vary in (COMPOSITION) from one region to another.

Front 192

14. Concept Check
Which of the following is a homogeneous mixture?
 Pure water
 Gasoline
 Jar of jelly beans
 Soil
 Copper metal

Back 192

1. Concept Check
Which of the following is a homogeneous mixture?
 Gasoline

Front 193

15. Heterogeneous Mixture
Having visibly _______________ parts.
Contains regions that have different __________ from those of other regions.

Back 193

Heterogeneous Mixture
Having visibly (DISTINGUISHABLE) parts.
Contains regions that have different (PROPERTIES) from those of other regions.

Front 194

16. Mixtures can be separated based on different physical properties of the components.
Name the technique for:
Boiling Point
(solid/liquid)

Back 194

Front 195

17. Distillation of a Solution Consisting of Salt Dissolved in Water

Back 195

Front 196

18. Filtration
Separates a liquid from a solid.

Back 196

Front 197

19. Multistep Example: Sand and Saltwater

Back 197

Front 198

20. The Organization of Matter

Back 198

Front 199

21. Concept Check:
Describe these pure substances and mixtures: A mixture is something that has variable composition (wood, wine, coffee, water, etc) and is two or more pure substances; a pure substance will always have the same composition, a pure substance is either an element or a compound.

Back 199

Describe these pure substances and mixtures: A mixture is something that has variable composition (wood, wine, coffee, water, etc) and is two or more pure substances; a pure substance will always have the same composition, a pure substance is either an element or a compound.

Front 200

22. Concept Check:
The physical and chemical properties of a substance are determined by its composition:
Typical physical properties of a substance include odor, color, volume, state (gas, liquid, or solid), density, melting point, and boiling point, and can also be described in terms of its chemical properties. Chemical properties refer to its ability to form new substances (wood burning [gives off heat and gases and leaves residue of ashes] rusting of a metal, the digestion of food, and the growth of grass), in a chemical change a given substance changes to a fundamentally different substance or substances.

Back 200

The physical and chemical properties of a substance are determined by its composition:
Typical physical properties of a substance include odor, color, volume, state (gas, liquid, or solid), density, melting point, and boiling point, and can also be described in terms of its chemical properties. Chemical properties refer to its ability to form new substances (wood burning [gives off heat and gases and leaves residue of ashes] rusting of a metal, the digestion of food, and the growth of grass), in a chemical change a given substance changes to a fundamentally different substance or substances.

Front 201

1. What are the three states of matter?
1. solid, liquid, and gas
2. solid, liquid, and plasma
3. solid, glass, and compounds
4. compounds, elements, and gases

Back 201

Choice #1 provides the correct answer. The three physical states of matter are solids, liquids, and gases.

Front 202

2. Which state of matter has a definite volume but no specific shape?
1. solid
2. liquid
3. gas
4. plasma

Back 202

Choice #2 is the correct answer. Liquids have a definite volume but takes the shape of its container.

Front 203

3. When a sample of mercury at room temperature and pressure is heated and boiled to dryness it changes state from a
1. solid to a liquid
2. liquid to a gas
3. solid to a gas
4. gas to a liquid

Back 203

Choice #2 provides the correct description of the change in state. At room temperature mercury is a liquid metal and when it boils, it goes into the gaseous state.

Front 204

4. How many of the following are examples of physical properties?
Ethyl alcohol boiling at 78°C
Hardness of a diamond
Sugar fermenting to form ethyl alcohol
1. 1
2. 2
3. 3
4. 0

Back 204

Choice # 2 is the correct response.
Ethyl alcohol boiling at 78°C is a physical property. Boiling point is associated with a phase change. It describes an inherent characteristic of alcohol.
Hardness of a diamond is a physical property. It describes an inherent characteristic of diamond – hardness.
Sugar fermenting to form ethyl alcohol is a chemical property. It describes the behavior of sugar – forming a new substance (ethyl alcohol) through a chemical reaction.

Front 205

5. In order to break down water into its constituent elements, water would have to undergo
1. distillation
2. fusion
3. chemical change
4. physical change

Back 205

Choice # 3 is the correct response. Water is a compound and must undergo a chemical change (reaction) in order to form its constituent elements, hydrogen and oxygen.

Front 206

6. How many of the following are examples of a chemical change?
Pulverizing (crushing) rock salt
Burning of wood
Dissolving of sugar in water
Melting a popsicle on a warm summer day
1. 1
2. 2
3. 3
4. 4

Back 206

Choice # 1 is the correct answer. Burning of wood is a chemical reaction. It reacts with oxygen to create carbon dioxide and water.

Front 207

7. The electrolysis of water, where an electric current is passed through water to form hydrogen and oxygen gases, is a
1. physical change because hydrogen and oxygen are what compose water.
2. physical change because water is merely turning into a gas.
3. chemical change because bubbles are observed.
4. chemical change because hydrogen and oxygen gases are chemically different than water.

Back 207

Choice # 4 is the correct answer. New substances are being created due to the chemical reaction.

Front 208

8. Which of the following processes is a chemical change?
1. Dry ice sublimes when left on the table in lab.
2. The light on a candle burns until a bell jar is placed over it for a period of time.
3. When a few drops of red food coloring are added to a beaker of hot water, the water immediately turns red.
4. Liquid nitrogen dumped onto the floor vaporizes at room temperature.

Back 208

Choice # 2 is the correct answer. The candle burning is a chemical reaction (the wick is reacting with oxygen to form carbon dioxide and water). After the bell jar is placed over the lit candle, the reaction stops when the oxygen inside the jar is all used up.

Front 209

9. How many of the following are compounds?
N²O⁴, NaOH, MnO², HF
1. 1
2. 2
3. 3
4. 4

Back 209

Choice # 4 is the correct answer. All of the substances are compounds. Compounds always contain atoms of different elements.

Front 210

10. A mixture has a __________ composition, whereas a compound always has a _________ composition.
1. pure; complex
2. complex; pure
3. constant; variable
4. variable; constant

Back 210

Choice #4 is correct. For example, hydrogen and oxygen can be mixed in any proportions, but water is always 88 % oxygen and 12 % hydrogen by mass.

Front 211

11. The brass in what might be a favorite candlestick is classified as a(n)
1. pure substance
2. element
3. heterogeneous mixture
4. homogeneous mixture

Back 211

Choice #4 is the correct answer. Brass is a homogeneous mixture of copper and zinc. It is not a pure substance because it can be broken down into its constituent elements by physical means.

Front 212

12. Which of the following is a homogeneous mixture?
1. Gasoline
2. Pure water
3. Jar of jelly beans
4. Copper metal

Back 212

Choice #1 is a homogeneous mixture. Gasoline is a solution. A jar of jelly beans is a heterogeneous mixture. Pure water is a pure substance (a compound). Copper metal is also a pure substance (an element). A mixture consists of two or more pure substances.

Front 213

13. Which of the following best describes the substance XeF⁴?
I. Element
II. Molecule
III. Compound
IV. Heterogeneous mixture
V. Homogeneous mixture
1. III only
2. I, II, III, IV
3. II, III, V
4. II, III

Back 213

Choice #4 is the correct answer. A molecule consists of more than one atom bonded together. A compound consists of different elements. A mixture consists of at least two or more pure substances.

Front 214

14. To separate a sand-saltwater mixture into pure substances one would have to employ
1. electrolysis
2. filtration
3. distillation
4. filtration followed by distillation

Back 214

Choice #4 correctly supplies the procedure, as shown below.

Front 215

15. Pure substances consist of either
1. elements or compounds
2. elements or mixtures
3. elements or solutions
4. elements or energy

Back 215

Choice #1 is correct, as shown in the figure here:

Front 216

16. If one were to remove all the pollutants, air would be classified as a(n)
1. pure substance
2. compound
3. element
4. solution

Back 216

Choice #4 is the correct answer because even “pure air” is a complex mixture of many gases, including nitrogen, oxygen, argon, and others. Because it is a homogeneous mixture, it is a solution.