Bonding Set I
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1
2
3Bonding Set I
1. NF
and PF
are stable molecules. Write the Lewis electron-dot formulas for these molecules. On the
3
5
basis of structural and bonding considerations, account for the fact that NF
and PF
are stable molecules
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5
but NF
does not exist.
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2-
2. (a)
Draw the Lewis electron-dot structures for CO
, CO
, and CO, including resonance structures
3
2
where appropriate.
(b) Which of the three species has the shortest C-O bond length? Explain the reason for your answer.
(c) Predict the molecular shapes for the three species. Explain how you arrived at your predictions.
3.
CF
XeF
ClF
4
4
3
(a) Draw a Lewis electron-dot structure for each of the molecules above and identify the shape of each.
(b) Use the valence shell electron-pair repulsion (VSEPR) model to explain the geometry of each of
these molecules.
4. Answer the following questions about the structures of ions that contain only sulfur and fluorine.
(a) The compounds SF
and BF
react to form an ionic compound according to the following
4
3
equation.
→ SF
SF
+ BF
BF
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3
3
4
+
(i)
Draw a complete Lewis structure for the SF
cation in SF
BF
.
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3
4
+
(ii) Identify the type of hybridization exhibited by sulfur in the SF
cation.
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+
(iii) Identify the geometry of the SF
cation that is consistent with the Lewis structure drawn in
3
part (a)(i).
+
(iv) Predict whether the F—S—F bond angle in the SF
cation is larger than, equal to, or
3
smaller than 109.50˚. Justify your answer.
(b) The compounds SF
and CsF react to form an ionic compound according to the following
4
equation.
+ CsF → CsSF
SF
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5
–
(i)
Draw a complete Lewis structure for the SF
anion in CsSF
.
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5
–
(ii) Identify the type of hybridization exhibited by sulfur in the SF
anion.
5
–
(iii) Identify the geometry of the SF
anion that is consistent with the Lewis structure drawn in
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part (b)(i).
(iv) Identify the oxidation number of sulfur in the compound CsSF
.
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