Name: 
 

Chemistry 12 - Chapter 4 Quiz



True/False
Indicate whether the sentence or statement is true or false.
 

1. 

The shape of molecules of the rocket fuel hydrazine, N2H4(l), is predicted by VSEPR theory to be trigonal planar around each nitrogen.
 

2. 

Diborane gas, B2H6(g), is used to dope semiconductors. However, a Lewis structure cannot be drawn without modifying the theory; nor is a VSEPR diagram possible even though the compound exists, and is well known.
 

3. 

A central atom with two bonded atoms and two unshared electron pairs has a linear arrangement of its electron pairs.
 

4. 

Ionic substances are network solids, with a special type of metallic bonding.
 

5. 

Hydrogen bonding is possible whenever the molecule contains hydrogen atoms as well as N, O, and F atoms.
 

6. 

A molecule with a pyramidal shape and polar bonds will be nonpolar.
 

7. 

Larger atoms, like sulfur, can bond as central atoms in more ways than smaller atoms, like oxygen, because they have more complex electron structures.
 

8. 

Of the molecules HCl, HBr, and HI, the HI should have the highest boiling point.
 

9. 

The end of a soap molecule that attracts and dissolves oily dirt must be polar.
 

10. 

Covalent network solids generally have high melting points compared with molecular crystals.
 

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

11. 

The Lewis model of the atom emphasizes the concept of
a.
atoms gaining or losing electrons to become ions.
b.
orbital hybridization.
c.
electron energy level changes.
d.
electron orbital overlap.
e.
the stable octet of electrons.
 

12. 

The Lewis symbol for an oxide ion would show dots to represent
a.
2 electrons.
b.
8 electrons.
c.
10 electrons.
d.
18 electrons.
e.
32 electrons.
 

13. 

A Lewis symbol for an atom with a configuration of 1s2 2s2 2p3 would show
a.
1 unpaired electron and 3 electron pairs.
b.
2 unpaired electrons and 2 electron pairs.
c.
1 unpaired electron and 2 electron pairs.
d.
3 unpaired electrons and 1 electron pair.
e.
3 unpaired electrons and 2 electron pairs.
 

14. 

A Lewis structure for the molecule NCl3 would show
a.
13 electron pairs.
b.
10 electron pairs.
c.
8 electron pairs.
d.
4 electron pairs.
e.
3 electron pairs.
 

15. 

X-ray diffraction evidence about the structure of compounds in crystals led to development of
a.
structural models.
b.
Lewis models.
c.
VSEPR theory.
d.
the octet rule.
e.
energy level theory.
 

16. 

Which of the following molecules has a trigonal planar shape?
a.
NH3
b.
CO2
c.
PCl3
d.
H2O
e.
BBr3
 

17. 

Which of the following covalent bonds is the most polar?
a.
N–O
b.
C–H
c.
O–H
d.
H–Cl
e.
C–Cl
 

18. 

The property that is best explained by intermolecular forces is
a.
surface tension of a liquid.
b.
electrical conductivity of a metal.
c.
hardness of a covalent network solid.
d.
melting point of an ionic solid.
e.
the colour of copper.
 

19. 

Metallic bonding depends on
a.
high electronegativity.
b.
delocalized electrons.
c.
polar covalent bonds.
d.
electrical conductivity.
e.
full valence orbitals.
 

20. 

A molecule of a substance with physical properties primarily determined by London forces would be
a.
SiC
b.
KCl
c.
Na3P
d.
PCl3
e.
H2O2
 



 
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