Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Electrons are located …

A

Between nuclei

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Nuclei attract _______ in a bond.

A

both electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Bonds form because of …

A

The forces that attract the atoms together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

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

A

PE, stabilizes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Carbon forms ______ bonds.

A

4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q
A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Rules for Drawing Lewis Structures
1. …

A

Count the total valence electrons for formula.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Rules for Drawing Lewis Structures
2. …

A

Write the skeleton structure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Rules for Drawing Lewis Structures
3. …

A

Use 2 electrons for each bond.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Rules for Drawing Lewis Structures
5. …

A

If there are not enough electrons form multiple bonds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Rules for Drawing Lewis Structures
Hydrogen always forms …

A

Just one bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q
A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

__________
- Number of each type of atom
- Chemical formula

A

How isomers are similar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

__________
- Connectivity between atoms
- Properties

A

How isomers are different

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Sigma bonds allow …

A

Free rotation of the bonded atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

________ contain C-C double bond

A

Alkenes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Alkenes
Each C is ____ hybridized

A

sp^2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Alkenes
One sigma bond (______________________)

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Alkenes
One pi bond (_________________)

A

Sideways p-p overlap

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Alkenes Restricted _______ around the double bond.
Rotation
26
Pi Bonds __________ freely
Don’t rotate
27
Side-to-side overlap of atomic orbitals gives _____ bond
π
28
End-to-end overlap of atomic orbitals gives _____ bond
σ
29
Triple Bonds C is ___ hybridized
sp
30
Triple Bonds One sigma bond (_________________)
End-to-end sp-sp overlap
31
Triple Bonds Two pi bonds (_________________)
Sideways p-p overlap
32
Valence Electrons on Free Atom - # Bonds to Atom in Structure - # Non-Bonded Electrons on Atom in Structure = ...
Formal Charge
33
What is the formal charge on N? NH(sub4)^+ A. +1 B. –1 C. +2 D. –2 E. 0
A.
34
What is the formal charge on H? NH(sub4)^+ A. +1 B. –1 C. +2 D. –2 E. 0
E.
35
What is the formal charge on O? OH^– A. +1 B. –1 C. +2 D. –2 E. 0
B.
36
What is the formal charge on H? OH^– A. +1 B. –1 C. +2 D. –2 E. 0
E.
37
What is the formal charge on C? CN^– A. +1 B. –1 C. +2 D. –2 E. 0
A
38
What is the formal charge on N? CN^– A. +1 B. –1 C. +2 D. –2 E. 0
E
39
VSEPR: ...
Valence Shell Electron Pair Repulsion
40
VSEPR Assume all ________ repel each other.
Electron centers
41
VSEPR There is a minimum energy arrangement that the __________ on an atom will naturally take up.
Electron centers
42
VSEPR Lone pairs and single, double, and triple bonds each count as ...
1 center
43
VSEPR Centers of electron density (around atom): 2 Hybridization: sp Electron Center Geometry: ...
Linear
44
VSEPR Centers of electron density (around atom): 3 Hybridization: sp^2 Electron Center Geometry: ...
Trigonal planar
45
VSEPR Centers of electron density (around atom): 4 Hybridization: sp^3 Electron Center Geometry: ...
Tetrahedral
46
VSEPR Centers of electron density (around atom): 5 Hybridization: sp^3d Electron Center Geometry: ...
Trigonal bipyramidal
47
VSEPR Centers of electron density (around atom): 6 Hybridization: sp^3d^2 Electron Center Geometry: ...
Octahedral
48
Multiple bonds only count as _________ in VSEPR.
One electron center
49
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.
50
Types of Covalent Bonds ________ is always a sigma bond
A single bond
51
Sigma bonds _______ for rotation around the bond
Allow
52
Types of Covalent Bonds _________ contain one sigma and one pi bond
Double bonds
53
Pi bonds _______ rotate
Do not
54
Types of Covalent Bonds _________ contain one sigma and two pi bonds
Triple bonds
55
The centers of electrons will repel and move as far apart as possible. This tells you the _________.
Geometry
56
Each center of electrons requires a hybrid orbital. This tells you the __________.
Hybridization
57
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
58
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
59
What is the hybridization of the O? H(sub 2)O
sp^3
60
What is the electron center geometry around the N? NH(sub 4) A. Tetrahedral B. Trigonal planar C. Linear D. Bent E. Pyramidal
A
61
What is the hybridization of the N? NH(sub 4)
sp^3
62
# Lone Pairs: e– centers: 2 Hybridization: sp Electron geometry: ... Num Lone Pairs: 0 Molecular Shape: ... Bond angle: 180°
Linear, Linear
63
e– centers: 3 Hybridization: sp^2 Electron geometry: ... Num Lone Pairs: 0 Molecular Shape: ... Bond angle: 120°
Trigonal planar, Trigonal planar
64
e– centers: 3 Hybridization: sp^2 Electron geometry: ... Num Lone Pairs: 1 Molecular Shape: ... Bond angle: 120°
Trigonal planar, Bent
65
e– centers: 4 Hybridization: sp^3 Electron geometry: ... Num Lone Pairs: 0 Molecular Shape: ... Bond angle: 190°
Tetrahedral, Tetrahedral
66
e– centers: 4 Hybridization: sp^3 Electron geometry: ... Num Lone Pairs: 1 Molecular Shape: ... Bond angle: ~190°
Tetrahedral, Trigonal pyramidal
67
e– centers: 4 Hybridization: sp^3 Electron geometry: ... Num Lone Pairs: 2 Molecular Shape: ... Bond angle: ~190°
Tetrahedral, Bent
68
What is the shape of the molecule? NH(sub 3) A. Tetrahedral B. Trigonal planar C. Linear D. Bent E. Trigonal pyramidal
E
69
What is the shape of the molecule? NH(sub 4)+ A. Tetrahedral B. Trigonal planar C. Linear D. Bent E. Trigonal pyramidal
A.
70
What is the shape of the molecule? CO(sub 2) A. Tetrahedral B. Trigonal planar C. Linear D. Bent E. Trigonal pyramidal
C.
71
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 ...
Electronegativity
72
Electronegativity: Ability of an element to attract electrons to itself ...
In a bond
73
Which is most electronegative? A. N B. O C. F D. Ne
C
74
Which is most electronegative? A. Cl B. Br C. I
A
75
Electronegativity Ability of an element to ...
Attract electrons to itself in a bond
76
Electronegativity Depends on _________ and __________.
Effective nuclear charge, size of orbitals
77
Electronegativity _________ across the periodic table.
Increases
78
Electronegativity _________ down the periodic table.
Decreases
79
_________ When two atoms of different electronegativities bond, the electrons are not shared equally. Results in a bond _________. We say the bond is _________.
Polar Bonds, dipole, polar
80
Is this bond polar? H–Cl A. Yes B. No
A
81
Is this bond polar? H–O A. Yes B. No
A
82
Is this bond polar? C–C A. Yes B. No
B
83
Is this bond polar? H–C A. Yes B. No
B (polar isn't significant enough)
84
Bond dipoles are __________. They have magnitude and direction and we must take both into account.
Vector quantities
85
The ______________ helps you see how to determine if a molecule is polar.
Molecule Polarity application
86
Symmetrical Molecule Requirements: 1. All bands must be the same 2. Shape: ...
Linear, trigonal planar, tetrahedral
87
Is BF(sub 3) polar? A. Yes B. No
B
88
Is NH(sub 3) polar? A. Yes B. No
A
89
Is CF(sub 4) polar? A. Yes B. No
B
90
Is CH(sub 3)F polar? A. Yes B. No
A
91
Do molecules interact with other molecules? A. Yes B. No
A
92
Which has the highest bp? A. He B. Ne C. Ar D. Kr E. Xe
E
93
What interactions are overcome when noble gases boil? A. LDFs B. Covalent bonds C. Others (not yet specified)
A
94
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
C
95
IMF LDFs < dipole-dipole < H-bonds __________ ___________
Weakest, strongest
96
_______________ - 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
London dispersion forces (LDFs)
97
_______________ - 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
Dipole-dipole interactions
98
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
99
What effect would increasing molecular polarity have on the strength of the intermolecular force? A. Increase B. Decrease C. Same
A
100
What effect would increasing molecular polarity have on the mp and bp of the substances? A. Increase B. Decrease C. Same
A
101
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
102
Which do you predict will have the highest BP? A. NH(sub 3) B. H(sub 2)O C. HF D. All the same
B SLIDE 106
103
Do samples of H2O, NH3, and HF contain the same number of H-bonding interactions? A. Yes B. No C. Maybe
B
104
___________: as energy is added the IMFs in ice are overcome causing the rigid cage-like structure to collapse and liquid water to form.
Ice melting
105
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
106
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
107
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
108
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
C
109
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
C
110
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
111
IMF Forces ________ < ________ < ________ weakest strongest
LDFs, dipole-dipole, H-bonds

CEM 141 (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions