Ch 1 Chemistry The Central Science

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Chemistry

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• is the study of properties of materials and changes that they undergo.
• can be applied to all aspects of life

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Matter

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• is the physical material of the universe.
• has mass.
• occupies space.
• ~100 elements constitute all matter.

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property

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A property is any characteristic that allows us to recognize a particular type of matter and to
distinguish it from other types of matter.

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Elements

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are made up of unique atoms

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atoms

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the building blocks of matter

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Molecules

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are combinations of atoms held together in specific shapes.

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States of Matter

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Solids, liquids and gases are the three forms of matter called the states of matter

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Properties of GAS described on the macroscopic level

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no fixed volume or shape, conforms to shape of container, compressible.

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Properties of LIQUID described on the macroscopic level

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volume independent of container, no fixed shape, incompressible.

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Properties of SOLID described on the macroscopic level

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volume and shape independent of container, rigid, incompressible.

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Properties of GAS described on the molecular level

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molecules far apart, move at high speeds, collide often.

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Properties of LIQUID described on the molecular level

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molecules closer than gas, move rapidly but can slide over each other

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Properties of SOLID described on the molecular level

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molecules packed closely in definite arrangements.

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Pure substances

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• are matter with fixed compositions and distinct proportions.
• are elements (cannot be decomposed into simpler substances, i.e. only one kind of atom) or
compounds (consist of two or more elements).

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Mixtures

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• are a comhttp://www.flashcardexchange.com/mycards/add/878218bination of two or more pure substances.
• Each substance retains its own identity.

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Compounds

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are combinations of elements

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What is the opposite of compound formation?

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decomposition.

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Law of Constant (Definite) Proportions (Proust)

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A compound always consists of the same
combination of elements (e.g., water is always 11% H and 89% O).

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Heterogeneous mixtures

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do not have uniform composition, properties, and appearance, e.g., sand.

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Homogeneous mixtures

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are uniform throughout, e.g., air; they are solutions .

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Physical properties

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are measured without changing the substance (e.g., color, density, odor,
melting point, etc.).

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Chemical properties

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describe how substances react or change to form different substances (e.g.,
hydrogen burns in oxygen).

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Intensive properties

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do not depend on the amount of substance present (e.g., temperature,
melting point etc.).

give an idea of the composition of a substance

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Extensive properties

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depend on the quantity of substance present (e.g., mass, volume etc.).

give an indication of the quantity of substance present.

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Physical change

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substance changes physical appearance without altering its identity (e.g., changes
of state ).

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Chemical change (or chemical reaction):

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substance transforms into a chemically different substance
(i.e. identity changes, e.g., decomposition of water, explosion of nitrogen triiodide).

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Filtration

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remove solid from liquid

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Distillation

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boil off one or more components of the mixture.

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Chromatography

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exploit solubility of components.

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The scientific method

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• Collect data (observe, experiment, etc.).
• Look for patterns, try to explain them, and develop a hypothesis or tentative explanation.
• Test hypothesis, then refine it.
• Bring all information together into a scientific law
• Bring hypotheses and laws together into a theory.

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hypothesis

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is a proposed explanation for an observable phenomenon

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scientific law

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concise statement or equation that
summarizes tested hypotheses

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theory

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A theory should explain general principles.

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metric system

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The metric system is an international decimalised system of measurement, that is the common system of measuring units used by most of the world.

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SI Units

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• 1960: All scientific units use Système International d’Unités (SI Units).
• There are seven base units.
• Smaller and larger units are obtained by decimal fractions or multiples of the base units.

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SI base unit of length

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meter

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meters to yards

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1 m = 1.0936 yards

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SI base unit of mass (not weight)

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kilogram

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kilogram to pounds

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1 kg = 2.2 pounds

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Mass

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is a measure of the amount of material in an object.

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Temperature

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is the measure of the hotness or coldness of an object.
Scientific studies use Celsius and Kelvin scales

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Celsius scale

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water freezes at 0 degrees C and boils at 100 degrees C (sea level).

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Kelvin scale

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• Water freezes at 273.15 K and boils at 373.15 K (sea level).
• is based on properties of gases.
• Zero is the lowest possible temperature (absolute zero).

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Kelvin to Celsius

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0 K = –273.15C.

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Fahrenheit conversions

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C = 5/9 (F-32)
F = 9/5 (C+32)

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Units of volume

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(units of length)3 = m3.
• cm3 [also known as mL (milliliter) or cc (cubic centimeters)]
• dm3 (also known as liters, L).
• Important: the liter is not an SI unit.

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Density

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is defined as mass divided by volume.
Units: g/cm3 or g/mL (for solids and liquids); g/L (often used for gases).

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exact numbers

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(known as counting or defined).

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inexact numbers

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derived from measurement

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Precision

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how well measured quantities agree with each other.

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Accuracy

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how well measured quantities agree with the “true value.”

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Significant Figures Rules

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Rules:
1. Nonzero numbers and zeros between nonzero numbers are always significant.
2. Zeros before the first nonzero digit are not significant. (Example: 0.0003 has one significant
figure.)
3. Zeros at the end of the number after a decimal point are significant.
4. Zeros at the end of a number before a decimal point are ambiguous (e.g., 10,300 g). Exponential
notation eliminates this ambiguity.

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Significant Figures in Multiplication and division

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Report to the least number of significant figures
(e.g., 6.221 cm x 5.2 cm = 32 cm2).

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Significant Figures in Addition and subtraction

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Report to the least number of decimal places
(e.g., 20.4 g – 1.322 g = 19.1 g).

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Significant Figures multiple step calculations

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In multiple step calculations always retain an extra significant figure until the end to prevent rounding
errors.

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Dimensional analysis

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is a method of calculation utilizing a knowledge of units.

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conversion factors

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conversion factor = (desired unit) / (given unit)
• These are fractions whose numerator and denominator are the same quantity expressed in
different units.
• Multiplication by a conversion factor is equivalent to multiplying by a factor of one.

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SI unit for mass

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kg

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SI unit for length

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m

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SI unit for Time

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sec

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SI unit for Electric Current

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A (ampere)

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SI unit for Temperature

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K (Kelvin)

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SI unit for Luminous intensity

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cd

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SI unit for Amount of substance

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mol

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List the prefixes used in the metric system from LARGEST to SMALLEST and give the scientific notation

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giga G 10^9
mega M 10^6
kilo k 10^3
centi c 10^-2
milli m 10^-3
micro μ 10^-6
nano n 10^-9
pico p 10^-12
femto f 10^-15

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What is volume measured in?

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ml or cm^3

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How do you find density?

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m/v

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How do you find volume?

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m/d

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Hod do you find mass?

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dv