Chemistry Exam Review

Front 1

Scientific Notation

Back 1

numbers that are written in the form m=10n

Front 2

SI Measurement

Back 2

measurements are quantitative information, they represent quantities.

Front 3

Quantity

Back 3

any amount with a size or magnitude.

Front 4

Unit of Measurement

Back 4

compares what is being measured with a previously defined size

Front 5

Standards of Measurement

Back 5

objects or natural occurences of constant value, easy to preserve and/or reproduce, and practical in size.

Front 6

Fundamental Units

Back 6

defined by a physical standard of measurement

Front 7

Mass

Back 7

a quantity of matter; determined by comparing the mass of an object with a set of standard masses

Front 8

Weight

Back 8

the measure of the gravitational pull on matter

Front 9

Unit of length

Back 9

meter

Front 10

Unit of mass

Back 10

kilogram

Front 11

Unit of time

Back 11

second

Front 12

Unit of electric current

Back 12

ampere

Front 13

Unit of thermodynamic temperature

Back 13

kelvin

Front 14

Unit for the amount of substance

Back 14

mole

Front 15

Unit of luminous intensity

Back 15

candela

Front 16

Derived units

Back 16

units obtained from the combinations of fundamental units

Front 17

Volume

Back 17

the amount of space occupied by an object or substance

Front 18

temperature

Back 18

a measure of the average kinetic energy of the particles in a sample of matter.

Front 19

heat

Back 19

total of kinetic energies of the particles in a sample of matter

Front 20

thermometers

Back 20

an instrument to measure hte temperature based on heat transfer and the ability for its material to expand or contract

Front 21

Accuracy

Back 21

the closenes of a measurement to the true or accepted value of the quantity measured.

Front 22

Precision

Back 22

the agreement among numerical values of a set of measurements of the same quantities made in the same way.

Front 23

Significant Figures

Back 23

figures in a measurement that consist of all digits with certainty plus one final digit, which is somewhat uncertain or estimated

Front 24

Groups on a Periodic Table

Back 24

*run vertically
*numbered 1-18

Front 25

Periods on a Periodic Table

Back 25

*run horizontally
*numbered 1-7

Front 26

Periods on a Periodic Table

Back 26

*run horizontally
*numbered 1-7

Front 27

States of Matter

Back 27

form of a property

Front 28

Solids

Back 28

definite shape and volume

Front 29

Liquids

Back 29

definite volume and has the ability to flow and take the shape of the container.

Front 30

Gases

Back 30

no definite shape or volume

Front 31

Plasma

Back 31

a high temperature physical state where atoms lose their electrons so its a gaseous system of positively charged particles and negatively charged electrons

Front 32

Property

Back 32

characteristics that enable us to distinguish one kind of matter from another

Front 33

Extensive property

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depends on the amount of matter present
Ex. length, mass

Front 34

Intensive property

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does not depend on the amount of matter present
Ex. melting point, density, odor

Front 35

Physical Property

Back 35

can be observed or measured without altering the identity of the material; can be qualitative or quantitative

Front 36

Physical Change

Back 36

any change in a property of matter that doesn't result in a change in identity

Front 37

Chemical Property

Back 37

refers to the ability of a substance to undergo a change that alters its identity

Front 38

Chemical Change (reaction)

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any changes in which one or more substance are converted into different substances with different characteristic properties.

Front 39

Reactant

Back 39

substances that undergo the chemical change

Front 40

Product

Back 40

new substance(s) that are produced by a chemical reaction

Front 41

Exothermic Reaction

Back 41

a process releasing heat--becomes hotter

Front 42

Endothermic Reaction

Back 42

a process absorbing heat---becomes cooler

Front 43

Mixture

Back 43

a combination of two or more kinds of matter, each of which retains its own composition and properties

Front 44

Heterogeneous Mixture

Back 44

the composition and properties are not uniform throughout.

Front 45

Homogeneous Mixture

Back 45

the composition and properties are uniform throughout

Front 46

Pure Substance

Back 46

a homogeneous sample of matter that has a fixed composition and properties, whatever the source.

Front 47

Element

Back 47

a pure substance that cannot be decomposed by ordinary chemical changes and is only made up of one kind of atom

Front 48

atom

Back 48

the smallest unit of an element that maintains the properties of that element

Front 49

Compound

Back 49

a pure substance that can be decomposed into two or more simpler substances

Front 50

Law of Definite Composition

Back 50

a chemical compund contains the same element in exactly the same proportions by mass regardless of size or source of the compound

Front 51

Science

Back 51

all of the human efforts put forth to achieve a systematic understanding of the physical universe through disciplined inquiry

Front 52

Chemistry

Back 52

the study of the compostion, structure, and properties of matter and the changes they undergo

Front 53

Dictionary Definition of Chemical

Back 53

a substance produced or used in a chemical process

Front 54

Scientific Definition of Chemical

Back 54

any substance that has a definite composition

Front 55

Organic Chemistry

Back 55

study of most carbon-containing compounds.
Ex. any life form, petroleum, polymers, gasoline, synthetic fibers, pop, etc.

Front 56

Inorganic Chemistry

Back 56

study of all substances containign elements other than carbon

Front 57

Physical Chemistry

Back 57

study of properties, transformations, and relationships between energy and matter.

Front 58

Biochemistry

Back 58

study of all substances and processes that occur in living things.

Front 59

Analytical Chemistry

Back 59

the identification of substances and the qualitative and quantitative determination of the composition of materials
Ex. forensic sciences

Front 60

Theoretical Chemistry

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the use of math and computers to understand the principles behind observed chemical behavior and to design and predict the properties of new compounds

Front 61

Basic Research

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carried out for the sake of increasing knowledge.

Front 62

Applied Research

Back 62

carried out to solve a problem

Front 63

Technological Research

Back 63

carried out to create products that will improve the quality of our lives.

Front 64

Part of Dalton's Atomic Theory That Still Holds True

Back 64

all matter is composed of small particles called atoms.

Front 65

Part of Dalton's Atomic Theory That Still Holds True

Back 65

atoms of different elements can combine in simple whole number ratios to form chemical compounds

Front 66

Part of Dalton's Atomic Theory That Still Holds True

Back 66

in chemical reactions, atoms are combined, separated, or rearranged.

Front 67

Law of Multiple Proportions

Back 67

if two or more different compounds are composed of the same 2 elements, the mass of the second element combined with a certain mass of the first element can be expressed as ratios of small whole numbers

Front 68

Alchemy

Back 68

the practical pursuit of the transmutation of elements into one another

Front 69

Aristotle

Back 69

-father of alchemy
-didnt believe in atoms
-thought there were 4 elements: earth, wind, water, and fire.

Front 70

Democritus

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-coined the term atom

Front 71

Nucleus

Back 71

the positively charged, dense, central portion of the atom that contains nearly all of its mass but takes up only an insignificant fraction of its volume.

Front 72

Ernest Rutherford

Back 72

-found the nucleus
-Gold Foil Experiment

Front 73

Ernest Marsden

Back 73

Rutherford's assistant

Front 74

Hans Geiger

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Rutherford's assistant

Front 75

Robert Millikan

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he found the mass of the electron using Oil Drop Experiment

Front 76

JJ Thomson

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-made the discovery of the electron
-found that all cathode rays contained the same negatively charged particles.

Front 77

Average atomic mass

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the weighted average of the atomic masses of the naturally occuring isotopes of an element.

Front 78

Atomic Mass Unit

Back 78

1/12 of the mass of a carbon-12 atom

Front 79

Relative Atomic mass

Back 79

the mass of an atom expressed in atomic mass units (amu)

Front 80

Mass number

Back 80

total number of protons and neutrons in the nucleus of an isotope

Front 81

Isotopes of Hydrogen:
Protium

Back 81

1 proton
1 electron
0 neutron
**MOST COMMON FORM

Front 82

Isotopes of Hydrogen
Deuterium

Back 82

1 proton
1 electron
1 neutron

Front 83

Isotopes of Hydrogen

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1 proton
1 electron
2 neutrons
**radioactive, very rare form

Front 84

Isotope

Back 84

atom of the same element with different masses
*different masses b/c different # of neutrons

Front 85

Atomic Number

Back 85

*the number of protons in the nucleus of an element
* identifies the element

Front 86

Nuclear Fusion

Back 86

less massive nuclei coming together to form a more stable and massive nuclei, with the release of energy.

Front 87

3 Problems Using Nuclear Fusion

Back 87

1 .Temperature
2. Density
3. Time

Front 88

Critical Mass

Back 88

the mass and concentration of nuclei that is sufficient enough to sustain a chain reaction

Front 89

Chain reaction

Back 89

a reaction where the products are able to produce more reactions in a self-sustaining series

Front 90

Nuclear Fission

Back 90

splitting a massive nulceus into more stable, less massive nuclei with the release of energy.