Chemistry Final

Front 1

An element that contains just one kind of atom.

Back 1

Element

Front 2

A substance that contains more than one kind of atom

Back 2

Compound

Front 3

The smallest particle of an element that retains the identity of the element

Back 3

Atom

Front 4

A neutrally charged particle resulting from atoms sharing electrons; example water.

Back 4

Molecule

Front 5

The apparent charge on an atom or its combing capacity due to gaining, losing or sharing electrons.

Back 5

Oxidation Number

Front 6

Mass of an atom is concentrated in the ______ which contains ______ and ______.

Back 6

Nucleus, protons, neutrons

Front 7

The mass of an electron is ______.

Back 7

Negligible

Front 8

a chemical unit that is equal to one gram formula mass(molar mass) of a substance and contains 6.02 x 1023 particles(atoms, ions, molecules or formula units)

Back 8

Mole

Front 9

The standard for atomic mass

Back 9

Carbon-12

Front 10

The most important safety rule in the lab is to _____.

Back 10

Follow instructions carefully.

Front 11

Atoms increase in size ____ and to the ____ on the periodic table.

Back 11

Down, left

Front 12

Atoms become more active as metals _____ and to the ____ on the periodic table

Back 12

Down, left

Front 13

Atoms become more active as nonmetals ___ and to the ___ on the periodic table.

Back 13

Up, right

Front 14

Rare Earth Elements- ___ block elements

Back 14

F

Front 15

Rare earth metals are also known as the _____ and _____ series.

Back 15

Actinide and Lanthanide

Front 16

Transition elements- ___ block elements

Back 16

D

Front 17

Digits we can read for sure plus one that is doubtful or estimated.

Back 17

Significant Digits (sigfigs)

Front 18

The ______ formula indicates the exact composition of the substance.

Back 18

Molecular

Front 19

The _____ formula indicates the simplest whole number ratio of the combination of atoms.

Back 19

Empirical

Front 20

Measurement of pull of gravity on an object and is variable depending on location.

Back 20

Weight

Front 21

A meausre of the amount of matter or inertia a body possesses and is constant everywhere in the universe.

Back 21

Mass

Front 22

The modern concept of atomic theory indicated that the position of an electron can best be described by a _________ ________

Back 22

Probability Cloud

Front 23

As electrons fall to lower energy states they _____ _______.

Back 23

emit energy

Front 24

______ ______ indicates the number of protons in an atom and identifies the atom. (subscript)

Back 24

atomic notation

Front 25

The _____ number indicates the sum of the protons and neutrons in the nucleus and is the superscript in atomic notation.

Back 25

mass

Front 26

A + B = AB

Back 26

combination or synthesis

Front 27

AB = A + B

Back 27

decomposition

Front 28

AB + C = AC + B

Back 28

single replacement

Front 29

AB + CD = AD + BC

Back 29

double replacement

Front 30

hydrocarbon + O2 = CO2 + H2O

Back 30

combustion

Front 31

Energy in motion

Back 31

kinetic energy

Front 32

Energy stored up or due to position

Back 32

potential energy

Front 33

A reaction that absorbs energy

Back 33

endothermic reaction

Front 34

A reaction that releases energy.

Back 34

exothermic reaction

Front 35

Quantum number that indicates the location of the electron in terms of the energy level or shell (also indicates the size of the electron cloud)

Back 35

n / prinicpal

Front 36

Quantum number that locates the sublevel (shape of electron cloud) values = 0,1,2,3 …(n-1)

Back 36

L / secondary

Front 37

Quantum number that locates orbital(orientation in space) values = -l …0…+l

Back 37

m / magnetic

Front 38

Quantum number that indicates the spin of electon(+1/2 clockwise, -1/2 counter-clockwise)

Back 38

s / spin

Front 39

An expression in terms of mass per unit volume.

Back 39

Density

Front 40

All binary compound names end with the suffix ____

Back 40

-ide

Front 41

The modern periodic table is organized according to _____ ________.

Back 41

atomic structure

Front 42

Around ____ B.C. , _______ came up with the first atomic theory.

Back 42

400, Democritus

Front 43

_____ reintroduced the atomic theory around 1803.

Back 43

Dalton

Front 44

______ realized the electrical nature of the atom in 1898

Back 44

Thomson

Front 45

_____ saved Rutherfords atom by using the quantum theory

Back 45

Bohr

Front 46

Metals tend to ____ electrons to form _____ ______ that are ____ that the atom

Back 46

lose, positive, cations, smaller

Hint 46

Gain/Lose, Positive/Negative, Anions/Cations, Larger/Smaller

Front 47

Nonmetals tend to ____ electrons to form ______ _____ that are _____ than the atom.

Back 47

gain, negative, anions, larger

Hint 47

Gain/Lose, Positive/Negative, Anions/Cations, Larger/Smaller

Front 48

______ may act either as a metal or nonmetal and border stairstep or zigzag line on periodic table.

Back 48

metalloids

Front 49

A highly probable region in space where an electron may be found as designated by the n, l, and m quantum numbers.

Back 49

orbital

Front 50

Vertical columns on the period table that have the same number of outermost or valence electrons, causing similar properties

Back 50

groups or families

Front 51

A horizontal row of elements on the periodic table.

Back 51

period

Front 52

The maximum number of electrons possible in an energy level can be determined by the formula ______

Back 52

2n2

Front 53

Atoms of the same element that have different masses due to the different numbers of neutrons in the nucleus.

Back 53

Isotopes

Front 54

An s sublevel may contain __ electrons

Back 54

2

Front 55

A p sublevel may contain __ electrons

Back 55

6

Front 56

A d sublevel may contain __ electrons.

Back 56

10

Front 57

An f sublevel may contain __ electrons.

Back 57

14

Front 58

The average atomic mass of the naturally occurring isotopes of an element

Back 58

atomic weight

Front 59

The mass of an atom relative to C-12.

Back 59

atomic mass

Front 60

The ____ rule states most atoms strive to attain the very stable electron configuration of a noble gas

Back 60

octet

Front 61

The father of the modern periodic table.

Back 61

Mendeleev

Front 62

Products - _____ materials Reactants - _____ materials

Back 62

final, initial

Front 63

Group IA elements are called ____ ______.

Back 63

alkali metals

Front 64

Group IIA elements are called _____ ______ ______

Back 64

alkali earth metals

Front 65

Group VII elements are called ______.

Back 65

halogens

Front 66

Group VIIIA elements are called ____ _____.

Back 66

noble gases

Front 67

Homogeneous mixture of solvent and solute.

Back 67

solution

Front 68

The material that is the dissolving medium or substance in greatest amounts

Back 68

solvent

Front 69

The material that gets dissolved or the material in lesser amounts.

Back 69

solute

Front 70

Electrons in the outermost energy level of an atom.

Back 70

valence

Front 71

A generalization that describes a behavior in nature.

Back 71

scientific law

Front 72

An electrically charged atom or group of atoms

Back 72

Ion

Front 73

The study of the quantative relationships expressed in balanced chemical equations.

Back 73

Stoichiometry

Front 74

The ________number of an element indicates the apparent charge on an atom

Back 74

oxidation

Front 75

The measurement of 0.00010020 contains ________ significant digits.

Back 75

5

Front 76

How many sig figs in 0.0006783308430

Back 76

10

Front 77

How many sig figs in 14.0045003980

Back 77

12

Front 78

How many sig figs in 79000.3

Back 78

6

Front 79

How many sig figs in 12004.001200

Back 79

11

Front 80

How many sig figs in 567.000

Back 80

6

Front 81

_____ energy is due to position.

Back 81

Potential

Front 82

Air is a solution of ____ gas and _____ gas

Back 82

Nitrogen, oxygen

Front 83

Percentage composition is determined by dividing the ___ of an element in a compound by its _____ _____

Back 83

Formula mass