26 Jun this information to calculate the percent ionic
Question
QUESTION 1
The gas-phase dipole moment of the hydroxyl radical, •OH, is 1.66 D, and the bond length for this species is 97.1 pm. Use this information to calculate the percent ionic character of the O—H bond.
1- 1- Charge in esu:
2- 2- Charge in e-
3- Percent ionic character of the O—H bond:
A. 1.61 X 10-10 esu
B. 1.71 X 10-10 esu
C. 5.85 X 109 esu
D. 0.21 e-
E. 0.36 e-
F. 0.60 e-
G. 21%
H. 36%
I. 60%
QUESTION 2
Azide ion, N3− has the bond linkage N—N—N. It belongs to point group D∞h. Integrate your knowledge of symmetry, covalent bond theory and resonance to: Predict resonance structures, bond angle and distances.
Abbreviations: FC: Formal Charge ; HO: Hybrid orbital
1- Most important resonance structure(s)
2- Secondary resonance structure(s)
3- Hybrid orbitals (HO) on the central N atom:
4- Bond angle:
5- Bond lengths
A. Two structures: each has two double bonds linking the three N atoms; central N atom has FC = 1+; each of the lateral N atoms has FC = 1–
B. One structure: has two double bonds linking the three N atoms; central N atom has FC = 1+; each of the lateral N atoms has FC = 1–
C. Two structures: each has one single bond and one triple bond linking the three N atoms; central N atom has FC = 1+; the lateral N atom that has a single bond has FC = 0; the lateral N atom that has a triple bond has FC = 2–
D. Two structures: each has one single bond and one triple bond linking the three N atoms; central N atom has FC = 1+; the lateral N atom that has a single bond has FC = 2–; the lateral N atom that has a triple bond has FC = 0
E. Two sp HO
F. Three sp2 HOs
G. Four sp3 HOs
H. < 109.5
I. < 120
J. < 180
K. 180
L. single bond > double bond > triple bond
M. Both bonds are equal in length
N. Both bonds are equal in length, since N3− has σh plane of symmetry.
O. The two bonds differ in length
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