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61 Cards in this Set

  • Front
  • Back
  • 3rd side (hint)
Chemistry
The study of matter, its chemical and physical properties, the chemical and physical changes it undergoes, and the energy changes that accompany those processes.
3
Matter
Anything that has mass and occupies space.
3
Energy
The ability to do work to accomplish some change.
3
Biochemistry
The study of life at the molecular level and the process associated with life.
3
Organic chemistry
The study of matter that is composed principally of carbon and hydrogen.
3
Inorganic chemistry
The study of matter that consists of all of the elements other than carbon and hydrogen and their combinations.
3
Analytical chemistry
The analysis of matter to determine its composition and the quantity of each kind of matter that is present.
3
Physical chemistry
The study of the way matter behaves.
3
Scientific method
A systematic approach to the discovery of new information. Organized approach to solving scientific problems. It consist of Observation, Formulation of question, Patter recognition, Developing theories, Experimentation, and Summarizing information.
3-6
hypothesis vs theory
Hypothesis is an attempt to explain an observation, educated guess. When experiments support a hypothesis it is a theory.
4
Properties
Characteristics of matter and are classified as either physical or chemical.
7
List the three states of matter:
gaseous state, the liquid state, and the solid state.
7
Gaseous state
Made up of particles that are widely separated. Will expand to fill and container, has no definite shape or volume.
7
Liquid state
Made up of particles that are closer together than gaseous state, has a definite volume, but no definite shape, and will take the shape of its container.
7
Solid state
Made up of particles closer together than liquid state with a fixed volume and shape.
Physical change
A recognizable difference in the appearance of a substance without causing any change in its composition or identity.
7
physical properties
Observations or measurements without changing the composition or identity of a substance.
7
chemical properties
Change in composition of a substance observed only through chemical reactions.
8
Chemical reaction
A process of rearranging, removing, replacing or adding atoms to produce new substances.
8
Intensive property
A property of matter that is independent of the quantity of the substance. Density, boiling and melting point, and specific gravity are intensive properties.
9
Extensive property
A property of matter that depends on the quantity of a substance. Mass and volume are extensive properties.
9
Pure substance
Has only one component.
9
Element
A pure substance that cannot be changed into a simpler form of matter by any chemical reaction.
Ex:hydrogen, and oxygen.
9
Compound
A substance resulting from the combination of two or more elements in a definite, reproducible way. The elements of hydrogen and oxygen combine to form the compounds of water, H2O.
9
Mixture
A combination of two or more pure substances in which each substance retains its own identity.
9
A mixture may be...
homogeneous or heterogeneous.
10
Homogeneous mixture
Has uniform composition. Its particles are well mixed, or thoroughly intermingled. Such as alcohol and water, is described as a solution. Air, a mixture of gases, is an example of a gaseous solution.
10
Heterogeneous mixture
Has a nonuniform composition. A mixture of salt and pepper , concrete, etc.
10
Three basic units of metric system.
Mass is represented as the gram, length as the meter, and volume as the liter.
12
Common relationships used in the English system:weight
1 pound=16 ounces,
1 ton=2000 pounds
14
Common relationships used in the English system:length
1 foot=12 inches,
1 yard=3 feet,
1 mile=5280 feet
14
Common relationships used in the English system:volume
1 gallon=4 quarts,
1 quart=2 pints,
1 quart=32 fluid ounces.
14
Bridging Units:mass
1 pound=454 grams,
2.2 pounds=1 kilogram
15
Bridging Units:Length
1 inch=2.54 centimeters,
1 yard=0.91 meter
15
Bridging Units:Volume
1 quart=0.946 liters,
1 gallon=3.78 liters
15
Significant figures
All digits in a number representing data or results that are known with certainty plus one uncertain digit.
17
The six sig fig rules
(1) All nonzero digits are significant.
(2) The number of significant digits is independent of the position of the decimal point.
(3) Zeros located between nonzero digits are significant.
(4) Zeros at the end of a number (trailing zeros) are significant if the number contains a decimal point.
(5) Trailing zeros are insignificant if the number does not contain a decimal point and are significant if a decimal point is indicated.
(6) Zeros to the left of the first nonzero integer are not significant; they serve only to locate the position of the decimal point.
17-18
Scientific notation
The representation of a number as a power of ten.
18
error
The difference between the true value and our estimation, or measurement, of the value.
19
Accuracy
The degree of agreement between the true value and the measured vale.
19
Uncertainty
The degree of doubt in a single measurement.
19
Precision
A measure of the agreement of replicate measurements.
20
Mass
The quantity of matter in an object. The terms weight and mass, in common usage, are often synonymous. They are not, in fact. Weight is the force of gravity on an object.
23
Length
The distance between two points, is the meter. Large distances are measure in kilometers, smaller distances are measured in millimeters or centimeters. Even smaller is nanometers.
24
Volume
The space occupied by an object, is the liter.
24
The standard metric unit of times is the...
second.
25
Temperature
The degree of "hotness" of an object.
25
To convert Fahrenheit to Celsius:
C=F-32/1.8
26
To convert Celsius to Fahrenheit
F=1.8C+32
26
To convert Celsius to Kelvin
K=C+273.15
26
Energy
The ability to do work. Kinetic, the energy of motion (in process), and potential, the energy of position (stored).
27
Concentration
A measure of the number of particles of a substance, or the mass of those particles, that are contained in a specified volume.
27
Density
The ratio of mass to volume, is independent of the amount of material (intensive property).
d=m/v.
29
Specific gravity
The ratio of the density of the object in question in to the density of pure water at 4 degrees Celsius. SG=density of object(g/mL)/density of water(g/mL). Density of water at 4 degrees Celsius is 1.00 g/mL.
31
Mm
Megameter

1,000,000 times larger or 1X10 to the 6th

1,000,000m=1Mm
km
kilometer

1,000 times larger or 1X10to the 3rd

1,000m=1km
dm
Dekameter

10 times larger or 1X10 to the 1

10m=1dm
cm
centimeter

100 times smaller or 1X10 to the -2

100cm=1m
mm
milimeter

1,000 times smaller or 1X10 to the -3

1,000mm=1m
um (funny lookin u)
micrometer

1,000,000 times smaller or 1X10 to the -6

1,000,000um=1m
nm
nanometer

1,000,000,000 times smaller or 1X10 to the -9

1,000,000,000nm=1m