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Chemistry > Chapter 5 > Flashcards

Chapter 5 Flashcards

Ionic and Covalent Compounds

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1
Q

OH^-

A

Hydroxide

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2
Q

H2PO4^-

A

dihydrogen phosphate

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3
Q

How many oxygen atoms are there in phosphate?

A

4

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4
Q

Different samples of a given compound always contain the same elements in the same mass ratio.

A

Law of definite Proportions

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5
Q

C2O4^2-

A

Oxalate

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6
Q

SO4^2-

A

sulfate

1 less O = -ite (sulfite)

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7
Q

A polyatomic anion that contains one or more oxygen atoms bonded to a central atom. (5.7)

A

Oxoanions

Relative Oxygen to …ate
1 more O = per …ate
1 Less O = …ite
2 Less O = hypo …ite

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8
Q

Molecule that has lost or gained one or more electrons giving it a positive or negative charge.

A

Polyatomic Ion

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9
Q

An electrostatic attraction that holds oppositely charged ions together in an ionic compound.

A

Ionic Bonding

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10
Q

The simplest hydrocarbons, having the general formula CnH2n+2, where n = 1, 2,… (5.6)

A

Alkane

I.e. Methane (CH4), ethane (C2H6), etc.

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11
Q

How many oxygen atoms are there in sulfate?

A

4

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12
Q

A molecule that contains two atoms.

A

Diatomic Molecule

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13
Q

A chemical formula that gives the number of atoms of each element in a molecule. (5.5)

A

Molecular Formula

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14
Q

Average molecular mass. (5.8)

A

Molecular Weight (amu)

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15
Q

The mass in grams of 1 mole of a substance.

A

Molar mass (ℳ)

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16
Q

A higher melting point corresponds to ___.

A

Higher Lattice Energy

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17
Q

CN^-

A

cyanide

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18
Q

Oxalate

A

C2O4^2-

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19
Q

Names of molecular compounds containing ___ don’t usually conform to systematic nomenclature guidelines.

A

Hydrogen

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20
Q

SCN^-

A

Thiocyanate

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21
Q

ammonium

A

NH4^+

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22
Q

Consisting of cations and anions in an electrically neutral combination; held together by electrostatic attraction.

A

Ionic Compound

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23
Q

Subsequent electron affinities are always ___.

A

Negative

Anions repel additional electrons.

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24
Q

H2S

A

Hydrogen sulfide

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25
Q

Heptane

A

C7H16

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26
Q

Butane

A

C4H10

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27
Q

A group of atoms that determines the chemical properties of an organic compound.

A

Functional Group

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28
Q

hydrogen phosphate

A

HPO4^2-

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29
Q

A substance composed of atoms of two or more elements chemically united in fixed proportions. (5.1)

A

Compound

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30
Q

chromate

A

CrO4^2-

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31
Q

How many oxygen atoms are there in chlorate?

A

3

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32
Q

When are roman numerals used in naming ionic compounds?

A

> 1 possible charges on metal cation.

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33
Q

dihydrogen phosphate

A

H2PO4^-

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34
Q

Peroxide

A

O2^2-

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35
Q

HSO4^-

A

bisulfate

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36
Q

Diborane

A

B2H6

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37
Q

The atom that can be removed in water on an acidic substance.

A

Ionizable Hydrogen Atom

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38
Q

A substance that consists of just two different elements; typically a metal and nonmetal.

A

Binary Compound

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39
Q

C3H8

A

Propane

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40
Q

Decane

A

C10H22

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41
Q

Permanganate

A

MnO4^-

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42
Q

Which cation would have a higher charge? Ending with -ic, or -ous.

A

-ic

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43
Q

cyanide

A

CN^-

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44
Q

acetate

A

C2H3O2^-

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45
Q

A three-dimensional array of cations and anions in an electrically neutral combination; held together by electrostatic attraction.

A

Lattice

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46
Q

C9H20

A

Nonane

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47
Q

PO4^3-

A

phosphate

1 less O = -ite (phosphite)

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48
Q

C5H12

A

Pentane

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49
Q

Phosphine

A

PH3

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50
Q

HPO4^2-

A

hydrogen phosphate

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51
Q

Compounds that do not contain carbon or that are derived from nonliving sources.

A

Inorganic Compound

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52
Q

O2^2-

A

Peroxide

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53
Q

Which has a larger effect on Lattice Energy: Magnitude of charge or Distance Between Ions?

A

Magnitude of Charge

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54
Q

NO3^-

A

Nitrate

1 less O = -ite (Nitrite)

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55
Q

An acid with one ionizable hydrogen atom.

A

Monoprotic Acid

56
Q

Monatomic anions are named by changing the ending to ___.

A

-ide

57
Q

The amount of energy required to

convert a mole of ionic solid to its constituent ions in the gas phase.

A

Lattice Energy

58
Q

Compounds containing carbon and hydrogen, sometimes in combination with other elements such as oxygen, nitrogen, sulfur, and the halogens. (5.6)

A

Organic Compound

59
Q

Cr2O7^2-

A

dichromate

60
Q

C6H14

A

Hexane

61
Q

Ammonia

A

NH3

62
Q

Greek prefixes are used to specify the number of each kind of atom in ___.

A

Molecular Compounds

63
Q

sulfate

A

SO4^2-

64
Q

Refers to an acid with more than one ionizable hydrogen atoms..

A

Polyprotic

65
Q

A ___ electron affinity means its more difficult to add an electron

A

lower

66
Q

MnO4^-

A

Permanganate

67
Q

Nomenclature system for oxoacid based on -ite oxoanion is ___.

A

-ous acid

I.e. HClO2 is chlorous acid

68
Q

C2H6

A

Ethane

69
Q

___ in oxoanion names are retained in naming the oxoacids.

A

Prefixes (per- and hypo-)

I.e. HClO4 is perchloric acid
and HClO is hypochlorus acid

70
Q

CH4

A

Methane

71
Q

An electrically neutral group of two or more atoms.

A

Molecule

72
Q

Thiocyanate

A

SCN^-

73
Q

SiH4

A

Silane

74
Q

Nitrate

A

NO3^-

75
Q

The chemical formula that conveys with the smallest possible whole numbers the ratio of combination of elements in a compound.

A

Empirical Formula

76
Q

Monatomic Cations are named by adding ___ to the name of the element.

A

ion

77
Q

phosphate

A

PO4^3-

78
Q

Silane

A

SiH4

79
Q

If two elements can form more than one compound, the mass ratio of one will be related to the mass ratio of the other by a small whole factor.

A

Law of multiple Proportions

80
Q

PH3

A

Phosphine

81
Q

C2H3O2^-

A

acetate

82
Q

A compound containing only carbon and hydrogen.

A

Hydrocarbon

83
Q

azide

A

NH3^-

84
Q

Pentane

A

C5H12

85
Q

Hydrogen sulfide

A

H2S

86
Q

bisulfate

A

HSO4^-

87
Q

Hydroxide

A

OH^-

88
Q

Hg2^2+

A

mercury(I)

89
Q

carbonate

A

CO3^2-

90
Q

C10H22

A

Decane

91
Q

H3O+

A

hydronium

92
Q

Methane

A

CH4

93
Q

A substance that generates hydrogen ions when dissolved in water.

A

Acid

94
Q

Containing atoms of only one element. (5.5)

A

Homonuclear

95
Q

If a compound contains a metal and a nonmetal, the compound is most likely ___.

A

Ionic

96
Q

A main group elemental symbol surrounded by dots, where each dot represents a valence electron.

A

Lewis dot symbol

97
Q

A chemical bond involves atoms sharing electrons.

A

Lewis theory of bonding

98
Q

The sum of the masses of all atoms in an ionic compound.

A

Formula mass (amu)

99
Q

NH3

A

Ammonia

100
Q

C7H16

A

Heptane

101
Q

Acids based on oxoanions.

A

Oxoacids

102
Q

bicarbonate

A

HCO3^-

103
Q

Shows the arrangement of atoms in a substance.

A

Structural Formula

104
Q

Which 4 transition metal cations have only one possible charge?

A

Silver, Aluminium, Cadmium, and Zinc

Connected on periodic table

105
Q

Ethane

A

C2H6

106
Q

Hexane

A

C6H14

107
Q

CrO4^2-

A

chromate

108
Q

CO3^2-

A

carbonate

109
Q

How many oxygen atoms are there in nitrate?

A

3

110
Q

HCO3^-

A

bicarbonate

111
Q

Propane

A

C3H8

112
Q

One of two or more distinct forms of an element.

A

Allotrope

I.e., oxygen (O2) and ozone (O3).

113
Q

Octane

A

C8H18

114
Q

Shows the general arrangement of atoms within a molecule. (5.5)

A

Structural Formula

115
Q

The average formula mass for an ionic compound.

A

Formula weight (amu)

116
Q

Nomenclature system for oxoacid based on -ate oxoanion is ___.

A

-ic acid

I.e. HClO3 is chloric acid

117
Q

Molecules containing more than two atoms. (5.5)

A

Polyatomic Molecule

118
Q

dichromate

A

Cr2O7^2-

119
Q

chlorate

A

ClO3^-

120
Q

The sum of the atomic masses (in amu) of the atoms that make up a molecule. (5.8)

A

Molecular Mass (amu)

121
Q

C8H18

A

Octane

122
Q

hydronium

A

H3O+

123
Q

Which suffix implies more oxygen atoms in the oxoanion? -ite or -ate?

A

-ate

1 more O = per- -ate
1 Less O = -ite
2 less O = hypo- -ite

124
Q

A ___ Ionization energy means it is more difficult to remove an electron.

A

higher

125
Q

A compound with a specific number of water molecules within its solid structure.

A

Hydrate

126
Q

When atoms share electrons.

A

Covalent Bonding

127
Q

Nonane

A

C9H20

128
Q

B2H6

A

Diborane

129
Q

Containing two or more different elements. (5.5)

A

Heteronuclear

130
Q

Under what circumstance would one remove -gen from hydrogen and change -ide to -ic?

A

Naming acidic binary compounds.

I.e. hydrochloric acid (HCl) and Hydrocyanic acid (HCN*)

131
Q

mercury(I)

A

Hg2^2+

132
Q

NH4^+

A

ammonium

133
Q

NH3^-

A

azide

134
Q

C4H10

A

Butane

135
Q

ClO3^-

A

chlorate

1 more O = per- -ate (perchlorate)
1 Less O = -ite (chlorite)
2 less O = hypo- -ite (hypochlorite)

Chemistry (13 decks)

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