Name: 
 

IB Topic 4


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

 1. 
What is the name given to the electrons in the highest occupied energy level of an atom?
a.
orbital electrons
c.
anions
b.
valence electrons
d.
cations
 

 2. 
What is the electron configuration of the calcium ion?
a.
1smc002-1.jpg2smc002-2.jpg2pmc002-3.jpg3smc002-4.jpg3pmc002-5.jpg
c.
1smc002-12.jpg2smc002-13.jpg2pmc002-14.jpg3smc002-15.jpg3pmc002-16.jpg4smc002-17.jpg
b.
1smc002-6.jpg2smc002-7.jpg2pmc002-8.jpg3smc002-9.jpg3pmc002-10.jpg4smc002-11.jpg
d.
1smc002-18.jpg2smc002-19.jpg2pmc002-20.jpg3smc002-21.jpg
 

 3. 
The octet rule states that, in chemical compounds, atoms tend to have ____.
a.
the electron configuration of a noble gas
b.
more protons than electrons
c.
eight electrons in their principal energy level
d.
more electrons than protons
 

 4. 
What is the formula of the ion formed when potassium achieves noble-gas electron configuration?
a.
Kmc004-1.jpg
c.
Kmc004-3.jpg
b.
Kmc004-2.jpg
d.
Kmc004-4.jpg
 

 5. 
What is the formula of the ion formed when tin achieves a stable electron configuration?
a.
Snmc005-1.jpg
c.
Snmc005-3.jpg
b.
Snmc005-2.jpg
d.
Snmc005-4.jpg
 

 6. 
How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration?
a.
1
c.
3
b.
2
d.
4
 

 7. 
The electron configuration of a fluoride ion, Fmc007-1.jpg, is ____.
a.
1smc007-2.jpg2smc007-3.jpg2pmc007-4.jpg
c.
1smc007-5.jpg2smc007-6.jpg2pmc007-7.jpg3smc007-8.jpg
b.
the same as that of a neon atom
d.
the same as that of a potassium ion
 

 8. 
A compound held together by ionic bonds is called a ____.
a.
diatomic molecule
c.
covalent molecule
b.
polar compound
d.
salt
 

 9. 
Which of the following is true about the melting temperature of potassium chloride?
a.
The melting temperature is relatively high.
b.
The melting temperature is variable and unpredictable.
c.
The melting temperature is relatively low.
d.
Potassium chloride does not melt.
 

 10. 
Which of the following elements can form diatomic molecules held together by triple covalent bonds?
a.
carbon
c.
fluorine
b.
oxygen
d.
nitrogen
 

 11. 
Which elements can form diatomic molecules joined by a single covalent bond?
a.
hydrogen only
b.
halogens only
c.
halogens and members of the oxygen group only
d.
hydrogen and the halogens only
 

 12. 
When one atom contributes both bonding electrons in a single covalent bond, the bond is called a(n) ____.
a.
one-sided covalent bond
c.
coordinate covalent bond
b.
unequal covalent bond
d.
ionic covalent bond
 

 13. 
The side-by-side overlap of p orbitals produces what kind of bond?
a.
alpha bond
c.
pi bond
b.
beta bond
d.
sigma bond
 

 14. 
Where are the electrons most probably located in a molecular bonding orbital?
a.
anywhere in the orbital
b.
between the two atomic nuclei
c.
in stationary positions between the two atomic nuclei
d.
in circular orbits around each nucleus
 

 15. 
Sigma bonds are formed as a result of the overlapping of which type(s) of atomic orbital(s)?
a.
s only
c.
d only
b.
p only
d.
s and p
 

 16. 
The shape of the methane molecule is called ____.
a.
tetrahedral
c.
four-cornered
b.
square
d.
planar
 

 17. 
What causes water molecules to have a bent shape, according to VSEPR theory?
a.
repulsive forces between unshared pairs of electrons
b.
interaction between the fixed orbitals of the unshared pairs of oxygen
c.
ionic attraction and repulsion
d.
the unusual location of the free electrons
 

 18. 
What is the shape of a molecule with a triple bond?
a.
tetrahedral
c.
bent
b.
pyramidal
d.
linear
 

 19. 
What type of hybridization occurs in the orbitals of a carbon atom participating in a triple bond with another carbon atom?
a.
mc019-1.jpg
c.
mc019-3.jpg
b.
mc019-2.jpg
d.
mc019-4.jpg
 

 20. 
How many pi bonds are formed when spmc020-1.jpg hybridization occurs in ethene, Cmc020-2.jpgHmc020-3.jpg?
a.
0
c.
2
b.
1
d.
3
 

 21. 
A bond formed between a silicon atom and an oxygen atom is likely to be ____.
a.
ionic
c.
polar covalent
b.
coordinate covalent
d.
nonpolar covalent
 

 22. 
Which of the following covalent bonds is the most polar?
a.
H—F
c.
H—H
b.
H—C
d.
H—N
 

 23. 
What are the weakest attractions between molecules?
a.
ionic forces
c.
covalent forces
b.
Van der Waals forces
d.
hydrogen forces
 

 24. 
What causes hydrogen bonding?
a.
attraction between ions
b.
motion of electrons
c.
sharing of electron pairs
d.
bonding of a covalently bonded hydrogen atom with an unshared electron pair
 

 25. 
What is required in order to melt a network solid?
a.
breaking Van der Waals bonds
c.
breaking hydrogen bonds
b.
breaking ionic bonds
d.
breaking covalent bonds
 

Essay
 

 26. 
Explain how a pure metal is held together. Include a definition of a metallic bond in your explanation.
 

 27. 
Can some atoms exceed the limits of the octet rule in bonding? If so, give an example.
 

 28. 
Explain what is meant by VSEPR theory. Give an example of how VSEPR theory can be applied to predict the shape of a molecule.
 



 
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