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Chem 1211 > Computer Midterm 2 Review > Flashcards

Computer Midterm 2 Review Flashcards

1
Q

Hg22+

A

Mercury(I)

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2
Q

NH4+

A

Ammonium

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3
Q

NO2-

A

Nitrite

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4
Q

NO3-

A

Nitrate

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5
Q

SO32-

A

Sulfite

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6
Q

SO42-

A

Sulfate

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7
Q

HSO4-

A

Hydrogen sulfate (bisulfate)

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8
Q

OH-

A

Hydroxide

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9
Q

CN-

A

Cyanide

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10
Q

PO43-

A

Phosphate

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11
Q

HPO42-

A

Hydrogen phosphate

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12
Q

H2PO4-

A

Dihydrogen Phosphate

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13
Q

NCS- or SCN-

A

Thiocyante

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14
Q

CO32-

A

Carbonate

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15
Q

HCO3-

A

Hydrogen Carbonate (bicarbonate)

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16
Q

ClO- OCl-

A

Hypochlorite

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17
Q

ClO2-

A

Chlorite

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18
Q

ClO3-

A

Chlorate

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19
Q

ClO4-

A

Perchlorate

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20
Q

C2H3O2-

A

Acetate

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21
Q

MnO4-

A

Permanganate

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22
Q

Cr2O72-

A

Dichromate

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23
Q

CrO42-

A

Chromate

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24
Q

O22-

A

Peroxide

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25
Q

C2O42-

A

Oxalate

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26
Q

S2O32-

A

Thiosulfate

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27
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 2
​# of lone pair electrons on ‘central’ atom: 0

A

Linear

Linear

180

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28
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 3
​# of lone pair electrons on ‘central’ atom: 0

A

Trigonal Planar

Trigonal Planar

120

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29
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 2
​# of lone pair electrons on ‘central’ atom: 1

A

Trigonal Planar

Bent

Less than 120

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30
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 4
​# of lone pair electrons on ‘central’ atom: 0

A

tetrahedral

tetrahedral

109.5

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31
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 3
​# of lone pair electrons on ‘central’ atom: 1

A

Tetrahedral

Trigonal Pyramidal

Less than 109.5

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32
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 2
​# of lone pair electrons on ‘central’ atom: 2

A

Tetrahedral

Bent

less than 109.5

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33
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 5
​# of lone pair electrons on ‘central’ atom: 0

A

Trigonal Bipyramidal

Trigonal Bipyramidal

90, 120, and 180

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34
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 4
​# of lone pair electrons on ‘central’ atom: 1

A

Trigonal Bipyramidal

Seesaw

90, 120, and 180

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35
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 3
​# of lone pair electrons on ‘central’ atom: 2

A

Trigonal Bipyramidal

T-shaped

90 and 180

36
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 2
​# of lone pair electrons on ‘central’ atom: 3

A

Trigonal Bipyramidal

Linear

180

37
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 6
​# of lone pair electrons on ‘central’ atom: 0

A

Octahedral

Octahedral

90 and 180

38
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 5
​# of lone pair electrons on ‘central’ atom: 1

A

Octahedral

Square Pyramidal

90 and 180

39
Q

Electron-pair Geometry
Molecular Geometry
Bond Angle

of bonding groups/domains on ‘central’ atom: 4
​# of lone pair electrons on ‘central’ atom: 2

A

Octahedral

Square Planar

90 and 180

40
Q

Define Isoelectric

A

Same number of electrons

41
Q

Define nuclear charge

A

Attractive force between the protons in the nucleus and the electrons in the energy levels.

42
Q

More protons = (greater/smaller) nuclear charge

43
Q

Define shielding

A

When inner (core) electrons shield outer electrons (valence) from the attractive forces of the nucleus.

44
Q

Less shielding, electrons pulled (towards/away) nucleus, (more/less) stable, (more/less) energy.

A

towards, more, less

45
Q

An orbital that penetrates into the region occupied by core electrons is ____ shielded from nuclear charge and therefore has ______ energy.

A

less, lower

46
Q

When drawing arrows for dipoles, arrow points towards molecule that is more . . .

A

electronegative.

47
Q

Formal Charge =

A

Valence e- - lone e- - (shared e-/2)

48
Q

When doing hybridization, use the ____ geometry.

A

electron-pair geometry

49
Q

Lattice Energy =

A

q1 * q2 / r2

where q is charge of ion
r is distance between them

50
Q

Lattice energy __________ upon ___________ size of ions.

A

decreases, increasing

52
Q

Mercury(I)

53
Q

Ammonium

54
Q

Nitrite

55
Q

Nitrate

56
Q

Sulfite

57
Q

Sulfate

58
Q

Hydrogen sulfate (bisulfate)

59
Q

Hydroxide

60
Q

Cyanide

61
Q

Phosphate

62
Q

Hydrogen phosphate

63
Q

Dihydrogen Phosphate

64
Q

Thiocyante

A

NCS- or SCN-

65
Q

Carbonate

66
Q

Hydrogen Carbonate (bicarbonate)

67
Q

Hypochlorite

68
Q

Chlorite

69
Q

Chlorate

70
Q

Perchlorate

71
Q

Acetate

72
Q

Permanganate

73
Q

Dichromate

74
Q

Chromate

75
Q

Peroxide

76
Q

Oxalate

77
Q

Thiosulfate

78
Q

Copper Electron Configuration

A

[Ar]4s13d10

79
Q

Chromium Electron Configuration

A

[Ar]4s13d5

80
Q

Silver Electron Configuration

A

[Kr]5s14d10

81
Q

Naming Acids
Simple binary acids
consists of:
prefix:
suffix:

A

Naming Acids
Simple binary acids
consists of: plain ion attached to hydrogen
prefix: hydro
​suffix: ic

82
Q

Naming Acids
Polyatomic ion
consists of:
prefix:
​suffix:

A

prefix: na
suffix: ic

83
Q

Naming Acids
Polyatomic Ion with extra oxygen

prefix:
​suffix:

A

prefix: per
suffix: ic

84
Q

Naming Acids
Polyatomic Ion one less oxygen

prefix:
​suffix:

A

prefix: na
suffix: ous

85
Q

Naming Acids
Polyatomic Ion with two less oxygen

prefix:
​suffix:

A

prefix: hypo
suffix: ous

Chem 1211 (8 decks)

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