Describe a double bond according to valence bond theory

Question # 00106858 Posted By: solutionshere Updated on: 09/24/2015 07:40 PM Due on: 10/24/2015
Subject Chemistry Topic General Chemistry Tutorials:
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A. In Lewis theory, the two bonds in a double bond look identical. However, valence bond theory
shows that they are not.
1. Describe a double bond according to valence bond theory.
2. Explain why rotation is restricted about a double bond, but not about a single bond.
B. The following figures show several molecular geometries (Express your answers as integers
separated by commas.)

1. Give the number of total electron groups, the number of bonding groups, and the number of lone
pairs for (a) geometry.

2. Give the number of total electron groups, the number of bonding groups, and the number of lone
pairs for (b) geometry.

3. Give the number of total electron groups, the number of bonding groups, and the number of lone
pairs for (c) geometry.

B. Determine the electron geometry, molecular geometry, and idealized bond angles for each of
the following molecules. In which cases do you expect deviations from the idealized bond
angle?
(a) CF4
(b) NF3
(c) OF2
(d) H2S
1. Determine the electron geometry for each molecule: linear, tetrahedral, trigonal planar, trigonal
bipyramidal
2. Determine the molecular geometry for each molecule: tetrahedral, trigonal planar, bent, linear
3. Determine the idealized bond angle for each molecule: 90. 180. 109.5, 120
4. In which cases do you expect deviations from the idealized bond angle?

C. ..
1. Determine the molecular geometry of BrF5.
a. seesaw
b. trigonal bypyramidal

c. square pyramidal
d. octahedral

2. Make a sketch of BrF5, using the bond conventions shown in the Box in Section 10.4 in the
textbook. Draw the molecule, with the correct chirality, by placing atoms on the grid and
connecting them with bonds.
3. Determine the molecular geometry of SCl6.

seesaw
trigonal bipyramidal
square pyramidal
octahedral
4. Make a sketch of SCl6.Draw the molecule, with the correct chirality, by placing atoms on
the grid and connecting them with bonds.
5. Determine the molecular geometry of PF5.

seesaw
trigonal bipyramidal
square pyramidal
octahedral
6. Make a sketch of PF5.
Draw the molecule, with the correct chirality, by placing atoms on the grid and connecting
them with bonds.
7. Determine the molecular geometry of IF+4.

seesaw
trigonal bipyramidal
square pyramidal
octahedral
8. Make a sketch of IF+4.
Draw the molecule, with the correct chirality, by placing atoms on the grid and connecting
them with bonds. Show the formal charges of all atoms in the correct structure.

9.
D. Each of the following ball-and-stick models shows wrong electron and molecular geometry of a
generic molecule.

1. Provide the correct molecular geometry for (a), given the number of lone pairs and bonding
groups on the central atom.

octahedral
tetrahedral
trigonal planar
trigonal pyramidal
square pyramidal
seesaw
bent
linear
trigonal bipyramidal
2. Provide the correct molecular geometry for (b), given the number of lone pairs and bonding
groups on the central atom.

trigonal planar
trigonal bipyramidal
octahedral
square pyramidal
bent
seesaw
trigonal pyramidal
linear
Tetrahedral

3. Provide the correct molecular geometry for (c), given the number of lone pairs and bonding
groups on the central atom.

seesaw
octahedral
bent
linear
tetrahedral
trigonal planar
square pyramidal
trigonal pyramidal
trigonal bipyramidal
E. ..
1. How do you determine whether a molecule is polar?
2. Why is polarity important?
F. CH3F is a polar molecule, even though the tetrahedral geometry often leads to nonpolar molecules.
1. Draw the Lewis structure of CH3F. Draw the molecule by placing atoms on the grid and
connecting them with bonds. Include all lone pairs of electrons and all hydrogen atoms.

G. Determine whether each molecule given below is polar or nonpolar.
1. CH2Cl2

nonpolar
polar
2. PBr5

polar
nonpolar
3. XeF2

polar
nonpolar
4. H2S

polar
nonpolar
H. Determine whether each of the following molecules is polar or nonpolar.
1. SiCl4

nonpolar
polar
2. CO2

polar
nonpolar
3. SeF6

polar
nonpolar
4. XeF2

polar
nonpolar
I.

What is a chemical bond according to valence bond theory?

J.

The valence electron configurations of several atoms are shown. How many bonds can each atom
make without hybridization?

1. Mg3s2
2. N2s22p3
3. O2s22p4
K. Consider the structure of the amino acid aspartic acid. Indicate the hybridization about each interior
atom: sp sp^2, sp^3

L. Use the drawing of MO energy diagram to predict the bond order of Li2+ and Li2−.
1. Do you expect Li2+ to exist in the gas phase?

yes

no
2. Do you expect Li2− to exist in the gas phase?

yes
no
M. Use molecular orbital theory to predict whether or not each of the following molecules or ions should
exist in a relatively stable form.
1. C2+2

will exist
will not exist
2. Li2

will exist
will not exist
3. Be2+2

will exist
will not exist
4. Li2−2

will exist
will not exist
N. Use the drawing of energy diagram for HCl to predict the bond order.
Express your answer using two significant figures.

O. Draw Lewis structures for CN+, CN, and CN−.
1. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include
all lone pairs of electrons and nonbonding electrons. Show the formal charges of all
nonhydrogen atoms in the correct structure.
2. Draw Lewis structure for CN.Draw the molecule by placing atoms on the grid and connecting
them with bonds. Include all lone pairs of electrons and nonbonding electrons.
3. Draw Lewis structure for CN−. Draw the molecule by placing atoms on the grid and
connecting them with bonds. Include all lone pairs of electrons and nonbonding electrons.
Show the formal charges of all nonhydrogen atoms in the correct structure.
4. According to Lewis theory, which species is most stable?

CN
+

CN
CN


5. According to MO theory, which species is most stable?

CN
+

CN
CN


P. Classify each of the following compounds as organic or inorganic.
1. C8H18

organic
inorganic
2. H2CO3

inorganic
organic
3. CaO

inorganic
organic
4. C12H16N2O

organic
inorganic
Q. Classify each of the following hydrocarbons as an alkane, alkene, or alkyne.
1. HC≡CH

alkane
alkene

alkyne
2. H3C−CH=CH−CH3

alkane
alkene
alkyne
3. CH3−C−CH3 H−CH3

alkane

alkene

alkyne

4. H3C−C≡C−CH3

alkane
alkene
alkyne
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Tutorials for this Question
  1. Tutorial # 00101287 Posted By: solutionshere Posted on: 09/24/2015 07:40 PM
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