Chem: Ch.1

Front 1

Chemistry

Back 1

The study of matter and its properties, the changes that matter undergoes, and the energy associated with those changes.

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Matter

Back 2

Anything that has mass and occupies space (has volume).

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Composition

Back 3

The types and amounts of simpler substance that make up a sample of matter.

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Property

Back 4

A characteristic that can be observed.

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Physical property

Back 5

Can be observed without changing the composition or identity of a substance. Includes melting point, malleability, electrical conductivity, and density.

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Physical change

Back 6

Occurs when a substance alters it physical properties, not its composition (i.e., when ice melts).

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Chemical property

Back 7

Can be observed only during a chemical change, and will result in a different substance. Includes flammability, corrosiveness, and reactivity with acids.

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Chemical change

Back 8

A change in the composition or identity of a substance.

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States

Back 9

The three physical forms matter commonly occurs in -- solid, liquid, and gas.

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Solid

Back 10

Has a fixed shape and a definite volume.

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Liquid

Back 11

Has an indefinite shape but definite volume.

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Gas

Back 12

Has indefinite shape and indefinite volume.

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Potential energy

Back 14

The energy due to the position of the object relative to other objects (i.e., when an object is raised high above the ground, its potential energy increases).

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Kinetic energy

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The energy due to the motion of the object (i.e., when an object is dropped from the air, the potential energy turns into kinetic energy, which is due to the motion of the object).

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Steps of the scientific approach

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1) Hypothesis
2) Experiment
3) Model (Theory)
4) Further Experiment
*Model is altered if predicted events do not match it.

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Natural Law

Back 18

A summary of an observation made by many investigators with no clear exceptions. Often in mathematical terms.

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Variables

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Quantities that can have more than one value.

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Controlled

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Describes an experiment that measures the effect of one variable on another while keeping all other variables constant.

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Dimensional Analysis

Back 21

The factor label method.

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Base units

Back 22

There are seven in the SI system. For instance, the base unit for length is meter, for temperature is K, and for amount of substance is mol.

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Derived units

Back 23

Combinations of the seven base units.

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Kilo

Back 24

k, 10^3, 1km = 1X10^3m

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Deci

Back 25

d, 10^-1, 10dm = 1m

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Centi

Back 26

c, 10^-2, 100cm = 1m

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Milli

Back 27

m, 10^-3, 1000mm = 1m

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Micro

Back 28

u,10^-6, 10^6um = 1m

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Nano

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n, 10^-9, 10^9nm = 1m

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Base quantity for mass

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Kilogram, kg

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B.q. for length

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Meter, m

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B.q. for time

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Second, s

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B.q. for temperature

Back 33

Kelvin, K

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B.q. for amount of substance

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Mole, mol

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Angstrum

Back 35

Used for sizes of atoms, symbolized by a circle over the letter A. 10^10 Angstrums equal 1 m.

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Substance

Back 36

Matter that has a definite, fixed composition and distinct properties (i.e., either an element or a compound).

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Mixture

Back 37

Matter composed of a physical intermingling of two or more substances with a variable composition. No chemical reaction involved.

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Macroscopic properties

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Properties that can be measured directly (instruments can be used).

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Submicroscopic properties

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Properties that cannot be measured directly (i.e., an electron).

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Mass

Back 40

A measure of the quantity of matter in an object. Does not change due to location.

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Weight

Back 41

The force that gravity exerts on an object. Does change with location.

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Heat

Back 42

The transfer of thermal energy from a warm object to a cooler object.

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Thermal energy

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The kinetic energy (energy due to motion) possessed by the submicroscopic particles that make up each object.

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Temperature

Back 44

A measure of the amount of thermal energy an object contains. Not heat or thermal energy itself, but a measure.

Front 45

Convert from degrees C to K

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T (in C) = T (in K) -273.15

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SI unit for volume

Back 46

m^3, but in chemistry, cm^3 is commonly used.

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Volume unit for fluids

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Liters (L).

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1 mL =

Back 48

1 cm^3

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Density

Back 49

Mass/volume

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SI unit for Density

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kg/m^3, but the more commonly used units of density are g/cm^3 for liquids and solids and g/L for gases.

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Extensive properties

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Properties that depend on the amount of substance (i.e., mass, volume, energy).

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Intensive properties

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Properties that do not depend on "sample size" (i.e., density and temperature).

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Systematic error

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Consistency errors, in which all the data is either too high or too low.

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Random error

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Random error, and all results will have some, since measurements are comparisons to a standard.

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Accuracy

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A measured value that is "correct."

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Precision

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A set of measured values that agree with each other.

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Defined quantities

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Numerical values which represent a counted number of objects and do not have significant digit restrictions. Also called "exact numbers."

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Error analysis

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Analysis of the effects of what would happen if the uncertain last digit varies.

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Conversion factors

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The ratios used in the factor label method.