Chemistry Chapter 8A (Prentice)
 
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Chemistry Chapter 8A (Prentice)

Matching
 
 
Match each item with the correct statement below.
a.
coordinate covalent bond
d.
single covalent bond
b.
double covalent bond
e.
polar bond
c.
structural formula
f.
hydrogen bond
 

 1. 

 a depiction of the arrangement of atoms in molecules and polyatomic ions
 

 2. 

 a covalent bond in which only one pair of electrons is shared
 

 3. 

 a covalent bond in which two pairs of electrons are shared
 

 4. 

 a covalent bond in which the shared electron pair comes from only one of the atoms
 

 5. 

 a covalent bond between two atoms of significantly different electronegativities
 

 6. 

 a type of bond that is very important in determining the properties of water and of important biological molecules such as proteins and DNA
 

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

 7. 
Which is a typical characteristic of an ionic compound?
a.
Electron pairs are shared among atoms.
b.
The ionic compound has a low solubility in water.
c.
The ionic compound is described as a molecule.
d.
The ionic compound has a high melting point.
 

 8. 
What is shown by the structural formula of a molecule or polyatomic ion?
a.
the arrangement of bonded atoms
c.
the number of metallic bonds
b.
the number of ionic bonds
d.
the shapes of molecular orbitals
 

 9. 
Which of these elements does not exist as a diatomic molecule?
a.
Ne
c.
H
b.
F
d.
I
 

 10. 
How do atoms achieve noble-gas electron configurations in single covalent bonds?
a.
One atom completely loses two electrons to the other atom in the bond.
b.
Two atoms share two pairs of electrons.
c.
Two atoms share two electrons.
d.
Two atoms share one electron.
 

 11. 
Why do atoms share electrons in covalent bonds?
a.
to become ions and attract each other
b.
to attain a noble-gas electron configuration
c.
to become more polar
d.
to increase their atomic numbers
 

 12. 
Which of the following elements can form diatomic molecules held together by triple covalent bonds?
a.
carbon
c.
fluorine
b.
oxygen
d.
nitrogen
 

 13. 
Which noble gas has the same electron configuration as the oxygen in a water molecule?
a.
helium
c.
argon
b.
neon
d.
xenon
 

 14. 
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
 

 15. 
Which of the following is the name given to the pairs of valence electrons that do not participate in bonding in diatomic oxygen molecules?
a.
unvalenced pair
c.
inner pair
b.
outer pair
d.
unshared pair
 

 16. 
Which of the following electron configurations gives the correct arrangement of the four valence electrons of the carbon atom in the molecule methane (CHmc016-1.jpg)?
a.
2smc016-2.jpg2pmc016-3.jpg
c.
2smc016-7.jpg2pmc016-8.jpg3smc016-9.jpg
b.
2smc016-4.jpg2pmc016-5.jpg3smc016-6.jpg
d.
2smc016-10.jpg2pmc016-11.jpg
 

 17. 
Which of the following diatomic molecules is joined by a double covalent bond?
a.
mc017-1.jpg
c.
mc017-3.jpg
b.
mc017-2.jpg
d.
mc017-4.jpg
 

 18. 
A molecule with a single covalent bond is ____.
a.
COmc018-1.jpg
c.
CO
b.
Clmc018-2.jpg
d.
Nmc018-3.jpg
 

 19. 
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
 

 20. 
Once formed, how are coordinate covalent bonds different from other covalent bonds?
a.
They are stronger.
c.
They are weaker.
b.
They are more ionic in character.
d.
There is no difference.
 

 21. 
When Hmc021-1.jpg forms a bond with Hmc021-2.jpgO to form the hydronium ion Hmc021-3.jpgOmc021-4.jpg, this bond is called a coordinate covalent bond because ____.
a.
both bonding electrons come from the oxygen atom
b.
it forms an especially strong bond
c.
the electrons are equally shared
d.
the oxygen no longer has eight valence electrons
 

 22. 
Which of the following bonds is the least reactive?
a.
C—C
c.
O—H
b.
H—H
d.
H—Cl
 

 23. 
How many valid electron dot formulas—having the same number of electron pairs for a molecule or ion—can be written when a resonance structure occurs?
a.
0
c.
2 only
b.
1 only
d.
2 or more
 

 24. 
In which of the following compounds is the octet expanded to include 12 electrons?
a.
Hmc024-1.jpgS
c.
PClmc024-3.jpg
b.
PClmc024-2.jpg
d.
SFmc024-4.jpg
 

 25. 
How many electrons can occupy a single molecular orbital?
a.
0
c.
2
b.
1
d.
4
 

 26. 
Molecular orbital theory is based upon which of the following models of the atom?
a.
classical mechanical model
c.
quantum mechanical model
b.
Bohr model
d.
Democritus’s model
 

 27. 
A bond that is not symmetrical along the axis between two atomic nuclei is a(n) ____.
a.
alpha bond
c.
pi bond
b.
sigma bond
d.
beta bond
 

 28. 
How is a pair of molecular orbitals formed?
a.
by the splitting of a single atomic orbital
b.
by the reproduction of a single atomic orbital
c.
by the overlap of two atomic orbitals from the same atom
d.
by the overlap of two atomic orbitals from different atoms
 

 29. 
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
 

 30. 
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
 



 
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