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CEM 141 > Chapter 4 (Exam 3) > Flashcards

Chapter 4 (Exam 3) Flashcards

1
Q

Valence electrons of one atom are attracted to …

A

Nucleus of other atom

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2
Q

Electrons are located …

A

Between nuclei

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3
Q

Nuclei attract _______ in a bond.

A

both electrons

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4
Q

Bonds form because of …

A

The forces that attract the atoms together

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5
Q

Bond formation lowers the _______ of the system and _______ the system.

A

PE, stabilizes

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6
Q

Carbon forms ______ bonds.

A

4

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7
Q
A
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8
Q

Based on your knowledge of carbon, what type of orbitals do you predict C is using to form these bonds?
A. sp hybrid orbitals
B. sp2 hybrid orbitals
C. sp3 hybrid orbitals
D. s and p atomic orbitals

A

C

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9
Q

Rules for Drawing Lewis Structures
1. …

A

Count the total valence electrons for formula.

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10
Q

Rules for Drawing Lewis Structures
2. …

A

Write the skeleton structure.

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11
Q

Rules for Drawing Lewis Structures
3. …

A

Use 2 electrons for each bond.

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12
Q

Rules for Drawing Lewis Structures
4. …

A

Starting on the outside and working your way in, make sure each atom (except H or B) has 8 valence electrons. If not, add lone pairs.

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13
Q

Rules for Drawing Lewis Structures
5. …

A

If there are not enough electrons form multiple bonds.

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14
Q

Rules for Drawing Lewis Structures
Hydrogen always forms …

A

Just one bond

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15
Q
A
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16
Q

__________
- Number of each type of atom
- Chemical formula

A

How isomers are similar

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17
Q

__________
- Connectivity between atoms
- Properties

A

How isomers are different

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18
Q

How many different isomers can you draw for the formula C(sub)5H(sub)12?
A. 2
B. 3
C. 4
D. 5
E. 6

A

B

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19
Q

Sigma bonds allow …

A

Free rotation of the bonded atoms

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20
Q

What is the formula for a linear hydrocarbon with 7 carbon atoms?
A. C(sub)7H(sub)12
B. C(sub)H(sub)14
C. C(sub)7H(sub)16
D. C(sub)7H(sub)15
E. C(sub)7H(sub)18

A

C

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21
Q

________ contain C-C double bond

A

Alkenes

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22
Q

Alkenes
Each C is ____ hybridized

A

sp^2

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23
Q

Alkenes
One sigma bond (______________________)

A

End-to-end sp^2-sp^2 overlap

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24
Q

Alkenes
One pi bond (_________________)

A

Sideways p-p overlap

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25
Q

Alkenes
Restricted _______ around the double bond.

A

Rotation

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26
Q

Pi Bonds __________ freely

A

Don’t rotate

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27
Q

Side-to-side overlap of atomic orbitals gives _____ bond

A

π

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28
Q

End-to-end overlap of atomic orbitals gives _____ bond

A

σ

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29
Q

Triple Bonds
C is ___ hybridized

A

sp

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30
Q

Triple Bonds
One sigma bond (_________________)

A

End-to-end sp-sp overlap

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31
Q

Triple Bonds
Two pi bonds (_________________)

A

Sideways p-p overlap

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32
Q

Valence Electrons on Free Atom - # Bonds to Atom in Structure - # Non-Bonded Electrons on Atom in Structure = …

A

Formal Charge

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33
Q

What is the formal charge on N?
NH(sub4)^+
A. +1
B. –1
C. +2
D. –2
E. 0

A

A.

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34
Q

What is the formal charge on H?
NH(sub4)^+
A. +1
B. –1
C. +2
D. –2
E. 0

A

E.

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35
Q

What is the formal charge on O?
OH^–
A. +1
B. –1
C. +2
D. –2
E. 0

A

B.

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36
Q

What is the formal charge on H?
OH^–
A. +1
B. –1
C. +2
D. –2
E. 0

A

E.

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37
Q

What is the formal charge on C?
CN^–
A. +1
B. –1
C. +2
D. –2
E. 0

A

A

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38
Q

What is the formal charge on N?
CN^–
A. +1
B. –1
C. +2
D. –2
E. 0

A

E

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39
Q

VSEPR: …

A

Valence Shell Electron Pair Repulsion

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40
Q

VSEPR
Assume all ________ repel each other.

A

Electron centers

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41
Q

VSEPR
There is a minimum energy arrangement that the __________ on an atom will naturally take up.

A

Electron centers

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42
Q

VSEPR
Lone pairs and single, double, and triple bonds each count as …

A

1 center

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43
Q

VSEPR
Centers of electron density (around atom): 2
Hybridization: sp
Electron Center Geometry: …

A

Linear

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44
Q

VSEPR
Centers of electron density (around atom): 3
Hybridization: sp^2
Electron Center Geometry: …

A

Trigonal planar

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45
Q

VSEPR
Centers of electron density (around atom): 4
Hybridization: sp^3
Electron Center Geometry: …

A

Tetrahedral

46
Q

VSEPR
Centers of electron density (around atom): 5
Hybridization: sp^3d
Electron Center Geometry: …

A

Trigonal bipyramidal

47
Q

VSEPR
Centers of electron density (around atom): 6
Hybridization: sp^3d^2
Electron Center Geometry: …

A

Octahedral

48
Q

Multiple bonds only count as _________ in VSEPR.

A

One electron center

49
Q

What is the electron center geometry around the O for H(sub 2)O?
For H(sub 2)O
A. Tetrahedral
B. Trigonal planar
C. Linear
D. Bent
E. Pyramidal

A

A.

50
Q

Types of Covalent Bonds
________ is always a sigma bond

A

A single bond

51
Q

Sigma bonds _______ for rotation around the bond

A

Allow

52
Q

Types of Covalent Bonds
_________ contain one sigma and one pi bond

A

Double bonds

53
Q

Pi bonds _______ rotate

A

Do not

54
Q

Types of Covalent Bonds
_________ contain one sigma and two pi bonds

A

Triple bonds

55
Q

The centers of electrons will repel and move as far apart as possible. This tells you the _________.

A

Geometry

56
Q

Each center of electrons requires a hybrid orbital. This tells you the __________.

A

Hybridization

57
Q

What is the electron center geometry around the O?
H(sub 2)O
A. Tetrahedral
B. Trigonal planar
C. Linear
D. Bent
E. Pyramidal

A

A

58
Q

What is the electron center geometry around the O?
H(sub 2)O
A. Tetrahedral
B. Trigonal planar
C. Linear
D. Bent
E. Pyramidal

A

A

59
Q

What is the hybridization of the O?
H(sub 2)O

A

sp^3

60
Q

What is the electron center geometry around the N?
NH(sub 4)
A. Tetrahedral
B. Trigonal planar
C. Linear
D. Bent
E. Pyramidal

A

A

61
Q

What is the hybridization of the N?
NH(sub 4)

A

sp^3

62
Q

Lone Pairs:

e– centers: 2
Hybridization: sp
Electron geometry: …
Num Lone Pairs: 0
Molecular Shape: …
Bond angle: 180°

A

Linear, Linear

63
Q

e– centers: 3
Hybridization: sp^2
Electron geometry: …
Num Lone Pairs: 0
Molecular Shape: …
Bond angle: 120°

A

Trigonal planar, Trigonal planar

64
Q

e– centers: 3
Hybridization: sp^2
Electron geometry: …
Num Lone Pairs: 1
Molecular Shape: …
Bond angle: 120°

A

Trigonal planar, Bent

65
Q

e– centers: 4
Hybridization: sp^3
Electron geometry: …
Num Lone Pairs: 0
Molecular Shape: …
Bond angle: 190°

A

Tetrahedral, Tetrahedral

66
Q

e– centers: 4
Hybridization: sp^3
Electron geometry: …
Num Lone Pairs: 1
Molecular Shape: …
Bond angle: ~190°

A

Tetrahedral, Trigonal pyramidal

67
Q

e– centers: 4
Hybridization: sp^3
Electron geometry: …
Num Lone Pairs: 2
Molecular Shape: …
Bond angle: ~190°

A

Tetrahedral, Bent

68
Q

What is the shape of the molecule?
NH(sub 3)
A. Tetrahedral
B. Trigonal planar
C. Linear
D. Bent
E. Trigonal pyramidal

A

E

69
Q

What is the shape of the molecule?
NH(sub 4)+
A. Tetrahedral
B. Trigonal planar
C. Linear
D. Bent
E. Trigonal pyramidal

A

A.

70
Q

What is the shape of the molecule?
CO(sub 2)
A. Tetrahedral
B. Trigonal planar
C. Linear
D. Bent
E. Trigonal pyramidal

A

C.

71
Q

An atom that has a high effective nuclear charge attracts its own valence electrons strongly AND it attracts electrons from other atoms in bonds. This is called …

A

Electronegativity

72
Q

Electronegativity: Ability of an element to attract electrons to itself …

A

In a bond

73
Q

Which is most electronegative?
A. N
B. O
C. F
D. Ne

A

C

74
Q

Which is most electronegative?
A. Cl
B. Br
C. I

A

A

75
Q

Electronegativity
Ability of an element to …

A

Attract electrons to itself in a bond

76
Q

Electronegativity
Depends on _________ and __________.

A

Effective nuclear charge, size of orbitals

77
Q

Electronegativity _________ across the periodic table.

A

Increases

78
Q

Electronegativity _________ down the periodic table.

A

Decreases

79
Q

_________
When two atoms of different electronegativities bond, the electrons are not shared equally. Results in a bond _________. We say the bond is _________.

A

Polar Bonds, dipole, polar

80
Q

Is this bond polar?
H–Cl
A. Yes
B. No

A

A

81
Q

Is this bond polar?
H–O
A. Yes
B. No

A

A

82
Q

Is this bond polar?
C–C
A. Yes
B. No

A

B

83
Q

Is this bond polar?
H–C
A. Yes
B. No

A

B (polar isn’t significant enough)

84
Q

Bond dipoles are __________. They have magnitude and direction and we must take both into account.

A

Vector quantities

85
Q

The ______________ helps you see how to determine if a molecule is polar.

A

Molecule Polarity application

86
Q

Symmetrical Molecule Requirements:
1. All bands must be the same
2. Shape: …

A

Linear, trigonal planar, tetrahedral

87
Q

Is BF(sub 3) polar?
A. Yes
B. No

A

B

88
Q

Is NH(sub 3) polar?
A. Yes
B. No

A

A

89
Q

Is CF(sub 4) polar?
A. Yes
B. No

A

B

90
Q

Is CH(sub 3)F polar?
A. Yes
B. No

A

A

91
Q

Do molecules interact with other molecules?
A. Yes
B. No

A

A

92
Q

Which has the highest bp?
A. He
B. Ne
C. Ar
D. Kr
E. Xe

A

E

93
Q

What interactions are overcome when noble gases boil?
A. LDFs
B. Covalent bonds
C. Others (not yet specified)

A

A

94
Q

Which has the highest boiling point?
Electrons
A. CH(sub 4) 10
B. NH(sub 3) 10
C. H(sub 2)O 10
D. HF 10
E. Ne 10

A

C

95
Q

IMF
LDFs < dipole-dipole < H-bonds
__________ ___________

A

Weakest, strongest

96
Q

_______________
- Temporary fluctuating dipoles
- Depends on size, surface area, and shape of the molecule
- Present in ALL substances in solid and liquid states (between discrete molecules or atoms)
- For non-polar molecules this is the only intermolecular force present

A

London dispersion forces (LDFs)

97
Q

_______________
- Present in polar substances (along with LDF)
(How do you determine if a substance is polar?)
- Typically stronger than LDF (for molecules of the same size

A

Dipole-dipole interactions

98
Q

Do dipole-dipole interactions exist in a sample of CH(sub 2)F(sub 2)?
A. Yes, because CH(sub 2)F(sub 2) is polar
B. No, because CH(sub 2)F(sub 2) is non-polar
C. Sometimes, because CH(sub 2)F(sub 2) can be polar or non-polar depending on how you draw the Lewis structure

A

A

99
Q

What effect would increasing molecular polarity have on the strength of the intermolecular force?
A. Increase
B. Decrease
C. Same

A

A

100
Q

What effect would increasing molecular polarity have on the mp and bp of the substances?
A. Increase
B. Decrease
C. Same

A

A

101
Q

Which would you predict would have the highest BP?
A. CH3NH2
B. CH2O
C. BP is the same
D. Cannot tell from info given

A

A

102
Q

Which do you predict will have the highest BP?
A. NH(sub 3)
B. H(sub 2)O
C. HF
D. All the same

A

B
SLIDE 106

103
Q

Do samples of H2O, NH3, and HF contain the same number of H-bonding interactions?
A. Yes
B. No
C. Maybe

A

B

104
Q

___________: as energy is added the IMFs in ice are overcome causing the rigid cage-like structure to collapse and liquid water to form.

A

Ice melting

105
Q

What is the strongest type of IMF present in liquid:
- He BP: 4K
A. LDFs
B. Dipole-dipole interactions
C. Hydrogen bonding
D. Covalent bonding

A

A

106
Q

What is the strongest type of IMF present in liquid:
- H(sub 2) BP: 20K

A. LDFs
B. Dipole-dipole interactions
C. Hydrogen bonding
D. Covalent bonding

A

A

107
Q

What is the strongest type of IMF present in liquid:
- CH4 BP: 112K

A. LDFs
B. Dipole-dipole interactions
C. Hydrogen bonding
D. Covalent bonding

A

A

108
Q

What is the strongest type of IMF present in liquid:
- NH3 BP: 240K

A. LDFs
B. Dipole-dipole interactions
C. Hydrogen bonding
D. Covalent bonding

A

C

109
Q

What is the strongest type of IMF present in liquid:
- H2O BP: 373K

A. LDFs
B. Dipole-dipole interactions
C. Hydrogen bonding
D. Covalent bonding

A

C

110
Q

What is the strongest type of IMF present in liquid:
- CO2 BP: 217K

A. LDFs
B. Dipole-dipole interactions
C. Hydrogen bonding
D. Covalent bonding

A

A

111
Q

IMF Forces
________ < ________ < ________
weakest strongest

A

LDFs, dipole-dipole, H-bonds

CEM 141 (7 decks)

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