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CHEM 130 > Final EXAM > Flashcards

Final EXAM Flashcards

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1
Q

Matter

A

Anything that occupies space and has mass

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2
Q

Pure substances

A

Same composition throughout and from sample to sample

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3
Q

Element

A

A substance that cannot be broken down into simpler substances even by chemical reaction

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4
Q

Compound

A

A substance composed of 2 or more elements combined in definite proportions

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5
Q

Metal

A

Lustrous, malleable, conductor of heat and electricity

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6
Q

Non metal

A

Dull, brittle, insulator of heat and electricity

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7
Q

Metalloid

A

An element having properties of both metals and non metals

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8
Q

Mixture

A

Two or more elements or compounds

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9
Q

Homogenous

A

Same composition throughout

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10
Q

Heterogeneous

A

Do not have uniform composition throughout

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11
Q

Property

A

Characteristic that we can observe

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12
Q

Change

A

A process that changes the properties of a substance

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13
Q

Physical property

A

Characteristic that we can observe without changing composition of substance

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14
Q

Qualitative properties

A

Color, odor

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15
Q

Quantitative properties

A

Mass, density

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16
Q

1 mL

A

1 cm^3

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17
Q

Density formula

A

D = mass/volume

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18
Q

Exothermic

A

Release energy

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19
Q

Endothermic

A

Requires energy input

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20
Q

Law of conservation of mass

A

Mass is not gained or lost in a chemical reaction

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21
Q

Law of definite proportions

A

A compound always has the same mass ratio of the elements that compose it

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22
Q

Protons

A

Positively charged,

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23
Q

Isotopic symbol

A

A/Z (X)
A=mass number (protons and neutrons)
N=number of neutrons to in the nucleus

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24
Q

Cations

A

Positively charged ions, add ion to elemental name

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25
Q

Anions

A

Negatively charged ions, add ide ion

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26
Q

Relative atomic mass

A

(isotope mass of 1 x relative abundance of 1) + (isotope mass of 2 x relative abundance of 2)
/ relative atomic mass

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27
Q

Group/family

A

Elements in the same column having similar properties

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28
Q

Period

A

Horizontal row of elements having properties that tend to vary in regular fashion

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29
Q

Alkali metals

A

Group 1 metals (not hydrogen)

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30
Q

Alkaline earth metals

A

Group 2 metals

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31
Q

Halogens

A

Group 17, exist as diatomic molecules

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32
Q

Noble gases

A

Group 18 nonmetals

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33
Q

Diatomic molecules

A

N, O, F, Cl, Br, I, H

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34
Q

Molecular compounds

A

Composed of 2 or more nonmetals

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35
Q

Ionic compound

A

Composed of cation (metal) and anion (nonmetal)

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36
Q

Dissociation/ionization

A

Substance releases ions when dissolved in water

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37
Q

Strong electrolyte

A

Dissociate completely, conduct electricity well

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38
Q

Weak electrolyte

A

Dissociate partially, conduct electricity fairly

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39
Q

Non electrolyte

A

Do not dissociate, don’t conduct electricity

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40
Q

Monoatomic charges

A

Group 1A (charge of +1), Group 2A (charge of +2), Group 4A (charge of 3-), Group 6A (charge of 2-), Group 7A (charge of 1-), Al+3, Ni+2, Ag+, Zn+2, Cd+2,

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41
Q

S2-

A

Sulfide

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42
Q

SO3 2-

A

Sulfite

43
Q

SO4 2-

A

Sulfate

44
Q

Oxyanions

A

Contain oxygen, will end in ite or ate, depending on number of oxygens present

45
Q

Anion

A

Will end in ide

46
Q

Water

A

H2O

47
Q

Ammonia

A

NH3

48
Q

Methane

A

CH4

49
Q

CO

A

carbon monoxide

50
Q

CO2

A

carbon dioxide

51
Q

CCl4

A

carbon tetrachloride

52
Q

SO3

A

sulfur trioxide

53
Q

N2O4

A

dinitrogen tetroxide

54
Q

PF5

A

phosphorus pentafluoride

55
Q

Acids

A

Can be recognized by formulas that start with H, water ionizes to form ions

56
Q

Bases

A

Substances that loses an OH- when reacting with water, dissociate in water to form hydroxide ions

57
Q

Neutralization reactions

A

acids and bases reacting with each other

58
Q

Binary acids

A

made from Hydrogen and one nonmetal, hydro prefix, root of non-hydrogen element, add -ic acid

59
Q

HF

A

hydrofluoric acid

60
Q

HCl

A

hydrochloric acid

61
Q

HI

A

hydroiodic acid

62
Q

H2S

A

hydrosulfuric acid

63
Q

Oxyacids

A

made from Hydrogen and polyatomic anion, change ending, ate becomes ic acid, ite ion becoems ous acid, ide ion is named as a binary acid

64
Q

H2SO4

A

sulfuric acid

65
Q

H2SO3

A

sulflurous acid

66
Q

HClO4

A

perchloric acid

67
Q

HClO3

A

chloric acid

68
Q

HCIO2

A

chlorous acid

69
Q

HClO

A

hypochlorous acid

70
Q

CO3 -2

A

carbonate

71
Q

NO2 -

A

nitrite

72
Q

NO3 -

A

nitrate

73
Q

PO3 -3

A

phosphite

74
Q

PO4 3-

A

phosphate

75
Q

SO3 2-

A

sulfite

76
Q

SO4 -2

A

sulfate

77
Q

HCO3 -1

A

hydrogen carbonate

78
Q

HPO4 -2

A

hydrogen phosphate

79
Q

H2PO4 -

A

dihydrogen phosphate

80
Q

FO-

A

hypofluorite

81
Q

FO2 -

A

fluorite

82
Q

FO3 -

A

fluorate

83
Q

FO4 -

A

perfluorate

84
Q

BrO-

A

hypobromite

85
Q

BrO2 -

A

bromite

86
Q

BrO3 -

A

bromate

87
Q

BrO4 -

A

perbromate

88
Q

MnO4 -

A

permanganate ion

89
Q

CrO4 2-

A

chromate ion

90
Q

OH-

A

hydroxide ion

91
Q

C2H3O2 -

A

acetate ion

92
Q

CN-

A

cyanide ion

93
Q

NH4 +

A

ammonium ion

94
Q
A
95
Q

STP conditions

A

0 °C and 1 atm. Molar volume is STP at 22.4 L/mol for all gases

96
Q

Combined gas law

A

P1V1 / T1 = P2V2 / T2

97
Q

Temperature and gas velocity are

A

Directly proportional

98
Q

Molecular mass and gas velocity are

A

Inversely proportional

99
Q

Diffusion and effusion rates are

A

Inversely proportional with molar mass

100
Q

Solutions

A

Solute + solvent

101
Q

H-bonding

A

Involved a bond between hydrogen and a more electronegative atom

102
Q

Dipole-dipole

A

Established between two molecules with a difference in electronegativity

103
Q

LDF

A

Weakest force. Forces caused by instantaneous mutual polarization of two molecules

104
Q

Ideal gas law

A

PV = nRT, p pressure, v volume, n moles, r gas constant (22.4 L/mole), t temperature

CHEM 130 (16 decks)

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