Name KEY
Period
Date
Chemical Bonding
Chapter 6: Review
Bonding Comparison Chart
IONIC
COVALENT
METALLIC
Metals and nonmetals
Nonmetals
Metals and metals
Positive ions bonding
with negative
ions…Transfer of
Electrons
Sharing valence
electrons
Valence electrons are
shared among
atoms…A Sea of
Electrons
Type of Structure
Crystalline
Molecular
Crystalline with
electrons moving
throughout all atoms
Physical State
Solid
Gases, liquids, or low
melting point solids
Solid
High melting point
Low melting point
High melting point
Solubility in Water?
Soluble
Insoluble / soluble
Low solubility
Electrical
Conductivity ?
High (as liquid)
Does not conduct
Relatively high
conductivity
Other Properties
Most are hard
Flammable
Malleable
Types of Atoms
Involved
(Metal, Nonmetal)
Method of
Bond Formation
(Valence Electrons)
(Solid, Liquid or Gas)
Melting/Boiling Point
(High or Low)
Low (as solid)
CHAPTER 6 REVIEW
1. Why do most atom form chemical bonds?
Atoms form chemical bonds to minimize their potential energy
Atoms have high potential energy. Atoms bonded have lower potential energy.
2. What are the exceptions to the octet rule?
Exceptions are 1 ) HYDROGEN = 2 valence electrons
2) BORON = 6 valence electrons
3. Explain why some elements can have an expanded octet?
3rd period elements have access to the “d - block” which allows an expanded octet.
4. Explain why ionic compounds do not conduct electricity in their crystalline lattice form.
Electrons are “FIXED” in their solid forms positions.
5. Identify bond types as either ionic, metallic or covalent
HCN:__Covalent___ Fe: _Metallic___
PbO:_Ionic___
Si: _Covalent____
6. A molecule of which of the following compounds contains a double bond?
a) C3H8
c) C2H4
b) C2H6
d) C2H5OH
e) CH4
7. A compound that exhibits resonance is:
a) SO2
b) N2
c) CO2
d) HCl
e) NH3
8. The best example of a non-polar molecule containing polar bonds is
a) F2
c) CO2
b) SO2
d) PCl3
9. Which of the following is non-polar molecule?
a) F2O
b) PCl3
d) NO21+
e) NO21-
c) PCl3
d) PCl5
e) SO3
c) O2 2-
d) HO2 1-
c) SO2
10. Which of the following compound has an expanded octet?
a) H2O
b) PH3
11. Which contains the shortest oxygen-oxygen bond?
a) O2
b) O3
12. Which of the following molecules has the shortest bond length?
a) N2
b) O2
c) Cl2
d) Br2
e) l2
13. Which of the following has zero dipole moment (i.e. is non-polar molecule)?
b) NO21-
a) H2O
d) SO3 2-
c) CCl4
e) HF
14. Ionic bonds are the electrostatic attraction between oppositely charged atom. What determines their
ionic strength? Explain
1) SIZE (distance) of the atom
2)
↑ size (distance) α
↓electrostatic force
Magnitude (amount) - PRODUCT of the charges involved
15. Arrange the following types of attractions in order of increasing strength: Covalent, Electrostatic, Ionic,
Dipole-dipole, Hydrogen and London Dispersion forces.
IONIC

Electrostatic 
(Ion-Ion)
COVALENT
Hydrogen Bonding  Dipole-Dipole  London Dispersion
w/ FON
POLAR
NONPOLAR
16. What is the difference between intramolecular and intermolecular bonding?
INTRAmolecular force: holds atoms together in an ionic, covalent or metallic bond.
INTERmolecular force: force is BETWEEN molecules or formula units.
17. Identify the types of INTERMOLECULAR forces for the following chemical compounds
(HINT: Dipole-Dipole, Electrostatic, Hydrogen or London Dispersion)
NaCl : ____ELECTROSTATIC
CO2: ___L.D. _____________________
H2CO : __L.D. \ DIPOLE-DIPOLE
NH3: _L.D. \ DIPOLE-DIPOLE \ _HYDROGEN
18. True or False
___T___ a) Water is a polar molecule
___F____ b) Pyramidal molecules have two unshared electron pairs on the central atom.
ONE LONE PAIR
___F___ c) A molecule cannot be non-polar if it contains only polar bonds.
___T___ d) A molecule consisting of 2 atoms is always linear.
___T__ e) Polar molecules have stronger attractions for each other than non-polar molecules have.
19. Describe the TWO factors that determine whether a molecule is polar or non-polar.
1) SYMMETRY
2) ELECTRONEGATIVITY DIFFERENCE
20. Define electronegativity. How does it relate to the intermolecular force between molecules?
Electronegativity – is a relative scale used to determine an element ability to grab electrons.
↑ ΔEN α ↑ intermolecular force (dipole - dipole force)
21. Explain why Chlorine (Cl2) is a gas, bromine (Br2) is a liquid, and iodine (I2) is a solid. Be very specific!
Intermolecular force (IMF) is responsible for the different states of the halogens.
Chlorine, Bromine & lodine are all NONPOLAR MOLECULES which implies
their only intermolecular force is LONDON DISPERSION FORCE.
↑ Atomic size α ↑ London Dispersion Force
22. Rank the following substance from strongest to weakest intermolecular force:
He
NH3
NF3
NaCl
__NaCl_ > __ NH3___ > __ NF3___ > __ He ___
Electrostatic
Hydrogen
Dipole
London Dispersion
23. Rank the following substances from strongest to weakest intermolecular force:
HF
F2
FCl
____HF____ > ___FCl___ > ____F2_____
Hydrogen
Dipole
London Dispersion
24. CENTRAL ATOMS – Most of the time SINGLE atoms become the central atom. However if you are
required to determine the central atom, it must meet the best two out of three requirements:
1) Atom with the largest number of valence electrons
2) Atom with the largest atomic radius
3) Least electronegative atom
**Note: _Hydrogen___ and __Halogens____ can not be central atoms.
25. Explain why nonpolar molecules usually have much lower surface tension than polar ones.
Nonpolar molecules have NO attraction for each other, therefore
they have a significantly lower surface tension (invisible skin) than polar molecules.
26. Rank the molecules from lowest to highest polarity.
PH3
PF3
NH3
NF3
___PH3____ < __ NH3 ____ < __ NF3____ < ___ PF3 _____
ΔEN = 0
ΔEN = 0.9
ΔEN = 1.0
ΔEN = 1.9
27. Which of the following has dispersion forces as its only intermolecular force?
CH4
HCl
C6H13NH2
NaCl
CH3Cl
28. Rank the following substances from strongest to weakest intermolecular force
Calcium Chloride
Potassium Chloride
Sodium Chloride
__CaCl2_____ > ___KCl____ > ___NaCl____
29. CH3CH2CH3 (propane) or CH3CH2CH2CH3 (butane) has the highest melting point
because they both have the same IMF (London Dispersion)
however butane has the higher molecular weight.
30. Draw the lewis structure, identify the shape, state whether it is polar or nonpolar and identify the one
with lowest boiling point?
PH3
H2S
HCl
SiH4
ΔEN = 2.1 – 3.0 = 0.9
Lowest Boiling Point
SHAPE:
SHAPE:
Trigonal Pyramidial
SHAPE:
Bent
SHAPE:
Linear
Tetrahedral
NONPOLAR or POLAR
NONPOLAR or POLAR
NONPOLAR or POLAR
NONPOLAR or POLAR