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Chemisty > Units 9 And 10 > Flashcards

Units 9 And 10 Flashcards

1
Q

2 electrons = electron pair geometry of

A

Linear

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2
Q

3 electrons = electron pair geometry of

A

Trigonal planar

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3
Q

4 electrons = electron pair geometry of

A

Tetrahedral

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4
Q

5 electrons = electron pair geometry of

A

Trigonal bipyramidal

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5
Q

6 electrons = electron pair geometry of

A

Octahedral

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6
Q

Linear

A

2 electrons = electron pair geometry of

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7
Q

Trigonal planar

A

3 electrons = electron pair geometry of

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8
Q

Tetrahedral

A

4 electrons = electron pair geometry of

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9
Q

Trigonal bipyramidal

A

5 electrons = electron pair geometry of

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10
Q

Octahedral

A

6 electrons = electron pair geometry of

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11
Q

Linear with no lone pairs molecular geometry

A

Linear

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12
Q

Trigonal planar with no lone pairs

A

Trigonal planar

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13
Q

Trigonal planar with 1 lone pairs

A

Bent

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14
Q

Tetrahedral with no lone pairs

A

Tetrahedral

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15
Q

Tetrahedral with one lone pair

A

Trigonal pyramidal

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16
Q

Tetrahedral with 2 lone pairs

A

Bent

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17
Q

Trigonal bipyramidal with 1 lone pair

A

See-saw

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18
Q

Trigonal bipyrmidal with 2 lone pairs

A

T shaped

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19
Q

Trigonal bipyramidal with 3 lone pairs

A

Linear

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20
Q

Octahedral with no lone pairs

A

Octahedral

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21
Q

Octahedral with 1 lone pair

A

Square pyramidal

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22
Q

Octahedral with 2 lone pairs

A

Square planar

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23
Q

Octahedral with 3 lone pairs

A

T shaped

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24
Q

Octahedral with 4 lone pairs

A

Iinear

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25
Q

Transfer one or more electrons from one to another to form ions

A

Ionic

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26
Q

Electrons are shared between atoms

A

Covalent

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27
Q

Energy change occurring when separated ions are packed together to form a crystalline solid

A

Lattice energy

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28
Q

Based on Coulomb’s law, which of the following is predicted to have a larger lattice energy?

A

LiF

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29
Q

Does MgO have a larger Latrice than NaCl?

A

Yes

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30
Q

Molecule formed by covalent bonds

A

Covalent compound

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31
Q

A 2D representation of bonding and non bonding electrons a molecule or polyatomic ion

A

Lewis structure

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32
Q

An electron pair found in the space between atoms

A

Bonding pair

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33
Q

An electron pair localized on a given atom

A

Lone pair

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34
Q

Valence electrons equal

A

Group Number

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35
Q

A condition occurring when a Lewis structure can be drawn for a particular ion

A

Resonance

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36
Q

Has fewer than 8 electrons

A

BF3

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37
Q

Has more than 8 electrons

A

SF6

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38
Q

Formal charge

A

Group # - (# lp + 1/2 bonding)

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39
Q

The best Lewis structure is the

A

One that minimizes formal charge

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40
Q

The octet rule usually occurs with

A

Boron and elements of higher periods (3 and up)

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41
Q

Linear geometry angle

A

180

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42
Q

Example of linear geometry

A

BeF2

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43
Q

Example of trigonal planar

A

BF3

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44
Q

Trigonal planar angle

A

120

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45
Q

Tetrahedral example

A

CF4

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46
Q

Tetrahedral angle

A

109.5

47
Q

Trigonal bipyramidal example

A

PF5

48
Q

Trigonal bipyramidal angle

A

120 and 90

49
Q

Octahedral example

A

SF6

50
Q

Octahedral angle

A

90

51
Q

H2O is

A

Bent

52
Q

Repulsive forces decrease in the following order

A

Lp vs lp greater then lp vs bonding greater than bonding vs bonding

53
Q

Electrons are not shared equally, one atom attracts them more strongly than the other

A

Polar covalent bond

54
Q

Electrons shared equally

A

No polar covalent bond

55
Q

Example for ionic bond

A

NaCl

56
Q

Example for covalent bond

A

HCl

57
Q

Example for no polar covalent bond

A

Cl2

58
Q

Ionic character of bond decreases from (blank) to (blank)

A

Ionic to nonpolar

59
Q

The tendency of an atom in a molecule to attract density to itself

A

Electronegativity

60
Q

Who came up with electronegativity

A

Linus Pauling

61
Q

The greater the electronegativity difference between 2 atoms in a bond, the (blank) the polarity

A

Greater

62
Q

Which element has the highest electronegativity

A

F 4.0

63
Q

Covalent usually has a electronegativity difference of

A

0-0.3

64
Q

Polar covalent usually has a electronegativity difference of

A

0.4-2.0

65
Q

Ionic usually has a electronegativity difference of

A

2.1-4

66
Q

of bonds between atoms

A

Bond order

67
Q

Distance between the nuclei of two bonded atoms

A

Bond length

68
Q

1 pair of electrons shared = bond order of

A

Single: 1

69
Q

2 pair of electrons shared = bond order of

A

Double: 2

70
Q

3 pairs of electrons shared = bond order of

A

Triple: 3

71
Q

Energy required to break a chemical bond

A

Bond energy

72
Q

Bond enthalpies are always

A

Positive

73
Q

Energy of reaction equation

A

Sum of bond energy of bonds broken - sum of bond energy of bonds formed

74
Q

Based on their Lewis structure which molecule has the longest carbon oxygen bond? Carbon dioxide and carbon monoxide

A

Carbon dioxide

75
Q

Order bond number from shorter to longest bond

A

Triple, double, single

76
Q

Bond length (blank) as the # of shared electrons increases

A

Shortens

77
Q

Single bond has the (blank) bond length

A

Longest

78
Q

Double bond has the (blank) bond length

A

Middle

79
Q

Triple bond has the (blank) bond length

A

Shortest

80
Q

Single bond has the (blank) bond energy

A

Lowest

81
Q

Double bond has the (blank) bond energy

A

Middle

82
Q

Triple bond has the (blank) bond energy

A

Highest

83
Q

Bonds formed from the overlap of atomic orbitals

A

Valence bond theory

84
Q

3 factors affect the overall energy of molecule

A
  • Electron nuclei attraction
  • nuclei nuclei repulsion
  • electron electron repulsion
85
Q

When 2 orbitals share a common region of space

A

Overlap

86
Q

Covalent bond formed by overlapping end to end

A

Sigma bond

87
Q

In a sigma bond, electron density is concentrated between the (blank) of the bonded atoms

A

Nuclei

88
Q

Triple bonds are (blank) than single bonds

A

Shorter and stronger

89
Q

Mixing or atomic orbitals to form special (hybrid) orbitals for bonding

A

Hybridization

90
Q

Form new set of orbitals and give max overlap in correct geometry

A

Orbital hybridization

91
Q

2 effective electron pairs

Hybridization =

A

Sp

92
Q

3 effective electron pairs

Hybridization =

A

Sp2

93
Q

4 effective electron pairs

Hybridization =

A

Sp3

94
Q

5 effective electron pairs

Hybridization =

A

Sp3d

95
Q

6 effective electron pairs

Hybridization =

A

Sp3d2

96
Q

Sp3 hybridization =

A

1s orbital and 3 p orbitals

97
Q

Double bond in ethylene consists of (blank) sigma bond and (blank) pi bond

A

1, 2

98
Q

Determining bond order from molecular theory- hydrogen2 =

A

1

99
Q

Determining bond order from molecular theory- helium2 =

A

0

100
Q

Greater the (blank), the stronger and more stable the molecule

A

Bond order

101
Q

Sp3 consists of

A

One S, 3 p

102
Q

Sp2 consists of

A

One s, 2 p

103
Q

Sp consists of

A

One S, one p

104
Q

How many remaining unhybrid orbitals does sp3 have?

A

None

105
Q

How many remaining unhybrid orbitals does sp2 have?

A

One p

106
Q

How many remaining unhybrid orbitals does sp have?

A

Two p

107
Q

Atomic orbitals to help explain bonding within molecules

A

Molecular orbital (MO) theory

108
Q

Constructive interference means

A

Increased amplitude between nuclei

109
Q

Destructive interference means

A

Node forms between the nuclei

110
Q

S atomic orbitals can form

A

Sigma molecular orbitals

111
Q

Three principles of molecular theory

A

1) # of MOs = # of atomic orbitals used
2) bonding MO is lower in energy than the atomic orbitals, the antibonding MO is higher
3) electrons assigned to MOs of successively higher energy

112
Q

Bond order equation determined by MO

A

bonding e - # antibonding e divided by 2

113
Q

How many electrons should be added to the MO diagram of the He2 molecule

A

4

Chemisty (10 decks)

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