South Pasadena • Honors Chemistry
Name
10 • Bonding
Period
10.3
Date
PROBLEMS
–
SOLIDS
1. State the type of solid each substance forms (ionic, metallic, molecular, or network covalent), and the interparticle forces that are involved (covalent bond, dipole-dipole interactions, hydrogen bonding, ionic bond,
London dispersion forces, metallic bond).
Compound
Type of Solid
Inter-Particle Forces
(a)
Chlorine
molecular solid
LDF
(b)
Water
molecular solid
LDF, DDI, HB
(c)
MgCl2
ionic solid
ionic bond
(d)
Iron
metallic solid
metallic bond
(e)
HCl
molecular solid
LDF, DDI
(f)
Graphite
network covalent solid
covalent bond
(g)
NH3 (ammonia)
molecular solid
LDF, DDI, HB
(h)
CaO
ionic solid
ionic bond
(i)
Silica
network covalent solid
covalent bond
(j)
CH4 (methane)
molecular solid
LDF
(k)
Cobalt
metallic solid
metallic bond
(l)
CO
molecular solid
LDF, DDI
2. The following picture represents a sample of solid
benzene, C6H6.
(a) These molecules form a(n) molecular solid.
(b) What forces are between the molecules?
LDF
(b)
(c)
(c) What forces are within a molecule?
covalent bonds
(d) What forces are broken when benzene
vaporizes? C6H6 (ℓ)  C6H6 (g)
LDF
(e) This compound is [ polar | non-polar ] and
[ will | will not ] dissolve in water.
3. The following picture represents a sample of
diamond. Each sphere represents a carbon atom.
5. The following picture represents a sample of solid
gold, Au.
(b)
(a) This is a(n) metallic solid.
(a) This is a(n) network covalent solid.
(b) What forces are between carbon atoms in
diamond?
covalent bonds
(c) Diamond is expected to have [ lower | higher ]
melting point than benzene (C6H6).
4. The following picture represents a sample of solid
zinc sulfide, ZnS. The smaller sphere represent
Zn2+ ions, while the larger sphere represent S2–
ions.
(b) What forces are between the atoms in this
solid?
metallic bonds
(c) List three properties of this solid.
lustrous, electrical conductor, ductile,
malleable
6. Predict which substance in each of the following
pairs would have the stronger IMFs. Explain
briefly.
(a) CO2 or OCS
OCS
(b)
(CO2 is non-polar and has LDF
< OCS is polar and has DDI)
(b) NH3 or PH3
NH3
(NH3 has HB > PH3 has LDF)
(c) HF or HCl
HF
(HF has HB > HCl has DDI)
(d) SO2 or SO3
SO2
(a) This is a(n) ionic solid.
(b) What forces are between the atoms in this
solid?
ionic bonds
(c) ZnS is expected to have a [ lower | higher ]
boiling point than benzene (C6H6).
(d) Draw the Lewis Structure for this compound.
2+
Zn
2S
(SO2 is bent geometry, is polar,
has DDI > SO3 is trigonal planar
geometry, is non-polar has LDF)
7. In each of the following groups of substances,
select the one that has the given property. Explain
briefly.
(a) Highest boiling point: HCl, Ar, F2
HCl
HCl is polar and has DDI, while Ar
and F2 are non-polar and have only
LDF.
(b) Highest freezing point: H2O, NaCl, HF
NaCl has ionic bonds, while H2O and HF
have only HB.
(c) Lowest freezing point: N2, CO, CO2
N2
CO is polar and has DDI (strongest IMF),
while N2 and CO2 are non-polar and have
only LDF.
Since N2 has fewer electrons, it has weaker
LDF than CO2.
(d) Lowest boiling point: CH4, C2H6, C3H8
CH4
All are non-polar and have LDF, but
CH4 has fewest electrons so it has
weakest LDF.
(e) Highest boiling point: HF, HCl, HBr
HF
HBr is non-polar and has LDF
< HCl is polar and has DDI
< HF has HB.
(f) Lowest boiling point: C3H6, CH3COCH3,
C3H7OH
C3H6
8.
C3H7OH has HB
> CH3COCH3 has DDI
> C3H6 is non-polar, has LDF.