Unit 2 Flashcards by Spencer Ward

How many valence electrons does aluminum have?

a.
1
d.
11
b.
2
e.
13
c.
3

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Which of the following ranks the compounds from lowest to highest lattice energy?

a.
NaF < MgF2 < CaF2 < KF
d.
CaF2 < KF < NaF < MgF2
b.
KF < NaF < CaF2 < MgF2
e.
MgF2 < CaF2 < KF < NaF
c.
MgF2 < CaF2 < NaF < KF

KF < NaF < CaF2 < MgF2

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How many nonbonding electrons are there in the Lewis structure of SCO?

a.
0
d.
10
b.
4
e.
12
c.
8

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What is the approximate carbon–oxygen bond order in the acetate ion, CH3COO−?

a.
0.5
d.
2
b.
1
e.
2.5
c.
1.5

1.5

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Resonance structures indicate that __________

a.
there is more than one allotropic form of a compound.
b.
more than one ionic form of a compound exists.
c.
a molecule’s electronic structure is an average or superposition of all possible Lewis structures.
d.
more than one isotopic form of an element exists in the molecule.
e.
the molecule jumps back and forth between two or more different electronic structures.

a molecule’s electronic structure is an average or superposition of all possible Lewis structures.

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Which of the following molecules is NOT polar?

a.
PCl3
d.
CO2
b.
H2O
e.
N2O
c.
SO2

CO2

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Which of the following is a planar molecule?

a.
NH3
d.
CH3COOH
b.
PCl5
e.
SiH4
c.
KrF4

KrF4

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What is the hybridization of carbon in COCl2?

a.
sp2
d.
sp
b.
sp3
e.
sp3d 2
c.
sp3d

sp2

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Which of the following has the largest bond angle?

a.
CF4
d.
NF2–
b.
NF3
e.
NH3
c.
OF2

CF4

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Which statement regarding a σ bond between two carbon atoms linked by a single bond is NOT correct?

a.
The region of electron density lies along the bond axis connecting the nuclei of the two atoms.
b.
The bond can be described by the overlap of sp hybrid orbitals from each atom.
c.
The bond can be described by the overlap of sp2 hybrid orbitals from each atom.
d.
The bond can be described by the overlap of sp3d hybrid orbitals from each atom.
e.
The bond can be described by the overlap of an sp2 hybrid orbital from one atom with an sp3 hybrid orbital from the other atom.

The bond can be described by the overlap of sp3d hybrid orbitals from each atom.

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Which type of molecular orbital is used to describe a buildup of electron density along the axis connecting two atomic nuclei to form a bonding orbital?

a.
sigma
d.
pi*
b.
pi
e.
py
c.
sigma*

sigma

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Oxygen has two common molecular anions: peroxide (O22–) and superoxide (O2–). Use the MO energy level diagram below to identify which one of the following statements is NOT correct.

a.
The bond order of the peroxide is 1.
b.
The superoxide has a shorter bond than the peroxide.
c.
Like O2, the peroxide is paramagnetic.
d.
The superoxide has a stronger bond than the peroxide.
e.
Oxygen, O2, has a stronger bond than either of these oxides.

Like O2, the peroxide is paramagnetic.

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Use energy levels of diatomic molecules derived from molecular orbital theory to predict the bond order of the oxygen molecule O2 and the peroxide anion O22–.

a.
oxygen, bond order = 2; peroxide, bond order = 3
b.
oxygen, bond order = 2; peroxide, bond order = 2
c.
oxygen, bond order = 4; peroxide, bond order = 4
d.
oxygen, bond order = 4; peroxide, bond order = 5
e.
oxygen, bond order = 2; peroxide, bond order = 1

oxygen, bond order = 2; peroxide, bond order = 1

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Dispersion forces are due to __________

a.
permanent dipoles.
d.
ionic interactions.
b.
temporary dipoles.
e.
protons.
c.
hydrogen bonding.

temporary dipoles.

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Which of the following solvents could involve ion–dipole interactions with Na+?

a.
benzene (C6H6)
d.
cyclohexane (C6H12)
b.
carbon tetrachloride (CCl4)
e.
pentane (C5H12)
c.
chloroform (CHCl3)

chloroform (CHCl3)

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Which is NOT true about n-alkanes?

a.
Their formulas are all CnH2n+2.
b.
All the carbon atoms are centers of tetrahedral geometry.
c.
Their melting points increase with the number of carbon atoms.
d.
Their vapor pressures increase with the number of carbon atoms.
e.
All of the carbons are sp3 hybridized.

Their vapor pressures increase with the number of carbon atoms

The temperature at point a in the phase diagram below is the __________

a.
critical point.
d.
normal freezing point.
b.
triple point.
e.
normal boiling point.
c.
transition point.

normal freezing point.

Write the corresponding name or chemical formula for each chemical formula or name given below.
a. CuCl2

Copper(II) chloride

Ammonium carbonate

(NH4)2CO3

Mg3(PO4)2

Magnesium phosphate

Sodium sulfate

Na2SO4

KHCO3

Potassium bicarbonate or potassium hydrogen carbonate

Disulfur tetroxide

S2O4

PH3

Phosphorus trihydride

Tetraphosphorus decoxide

P4O10

H2S (aq)

Hydrosulfuric acid

Nitrous acid

HNO2

Which of the following bonds is considered to be ionic? C O, Ca Cl, S N, or Si O. Explain your answer.

Ca Cl is considered to be ionic because the electronegativity difference between calcium and chlorine is so large, ionic bonds normally form between metal cations and non-metal anions. The other bonds listed all have smaller differences in electronegativity and are covalent, meaning that they share valence electrons.