ORGANIC CHEMISTRY 8Th Edition International Edition by John E. McMurry - Test Bank

,Chapter 1—Structure and Bonding


SHORT ANSWER

1. Give the ground-state electron configuration for carbon (atomic number 6).

ANS:
1s22s22px12py1 or 1s22s22p2


2. Give the ground-state electron configuration for fluorine (atomic number 9).

ANS:
1s22s22px2 2py2 2pz1 or 1s22s22p5


3.Give the ground-state electron configuration for magnesium (atomic number 12).

ANS:
1s22s22p63s2


4. How many electrons does silicon have in its valence shell?

ANS:
four


Exhibit 1-1
Write valid Lewis (electron-dot) structures for each formula below. Show all electrons as dots and show
all non-bonding electrons.

5. C2Cl4 tetrachloroethylene

ANS:




6. CO2 carbon dioxide

ANS:



7. CH4O methanol




1

,Structure and Bonding


ANS:




Exhibit 1-2
Consider the structure of urea, shown below, to answer the following question(s).




8. Refer to Exhibit 1-2. Fill in any non-bonding valence electrons that are missing from the line-bond
structure.

ANS:




9. Refer to Exhibit 1-2. The carbon atom in urea is:

sp3 hybridized
sp2 hybridized
sp hybridized
not hybridized

ANS:
b


10. Refer to Exhibit 1-2. The predicted NH2C=O bond angle in urea is:

109.5
120
180
not predictable

ANS:
b




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, Chapter 1


Exhibit 1-3
Determine the hybridization for the indicated atoms in each structure below.




11. Refer to Exhibit 1-3. The hybridization of this oxygen atom (A) is ______.

ANS:
sp2


12. Refer to Exhibit 1-3. The hybridization of this oxygen atom (B) is ______.

ANS:
sp3


13. Refer to Exhibit 1-3. The hybridization of this carbon atom (C) is ______.

ANS:
sp3


14. Refer to Exhibit 1-3. The hybridization of this carbon atom (D) is ______.

ANS:
sp


15. The molecular formula C2H4O can be converted into three-line bond (Kekulé) structures that are
consistent with valence rules.




Which one of the Kekulé structures is not consistent with valence rules?
Explain why the structure you chose in part a is not consistent with valence rules.

ANS:
d
The carbon bonded to the oxygen atom in structure d is pentavalent; it has 10 valence
electrons. Carbon can only have eight valence electrons. In addition, the other carbon
has only six valence electrons when it would prefer to have eight.




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