9bii and 11b the hybridization orbital overlap for the following molecules. Label the bondIBr(vi)(v) CN-(ii) НОBr(iii) NO(iv) NO*PH3What is the change in hybridization of the central atoms in the reactants to theproducts (as underlined) in the following reactions?Draw the the structures othe reactants and the products according to thehybridization theory:(i)BF3 +F→BF4->(ii). PCIS + CF → PC16the hybridization orbital overlap for the following molecules. Label the bonds between the bonds.(ii)(11)HH-C-N-HHPINCentfor Founddies For the following species,(i)(ii)(iii)State the orbital hybrid for the atoms labelled 1,2,3,4.State the bond angles labelled a,b,c.Draw the orbital overlap diagram using the hybridization theory and state thetypes of bonds formed.(a)(byH.kHH-0-HH -C--N-H.13

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Answered: Draw the the structures of the…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter7: Molecular Structures

Section: Chapter Questions

Problem 74QRT

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Why do we hybtidize atomic orbitals to explain the bonding in covalent compounds? What type of bonds form from hybrid orbitals: sigma or pi? Explain.
Bromine forms a number of oxides of varying stability. (a) One oxide has 90.90% Br and 9.10% O. Assuming its empirical and molecular formulas are the same, draw a Lewis structure of the molecule and specify the hybridization of the central atom (O). (b) Another oxide is unstable BrO. Assuming the molecular orbital diagram in Figure 9. 16 applies to BrO, write its electron configuration (where Br uses 45 and 4p orbitals). What is the highest occupied molecular orbital (HOMO) for the molecule?
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) LiBe+ (b) CO+ (c) CN (d) OF Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
In the hybrid orbital model, compare and contrast bonds with bonds. What orbitals form the bonds and what orbitals form the bonds? Assume the z-axis is the internuclear axis.
For the molecule allene, H2C=C=CH2, give the hybridization of each carbon atom. Will the hydrogen atoms be in the same plane or perpendicular planes?
The uracil molecule is one of the bases in DNA. Estimate the approximate values of the indicated bond angles. Its skeleton (not its Lewis structure) is given below.
Give the hybridization of each atom (except H) in the solvent dimethylsulfoxide. (Unshared electron pairs are not shown.)
Discuss the nature of the bonding in the nitrite ion (NO2) . Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central nitrogen atom, and the geometry of the ion. Show how the use of resonance structures can be avoided by introducing a de-localized MO. What bond order does the MO model predict for the NO bonds in the nitrite ion?
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) CN (b) CO (c) BeB (d) BC+ Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
What is the hybridization of the central atom in each of the following? (a) BeH2 (b) SF6 (c) PO43 (d) PCl5

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Draw the the structures of the reactants and the products according to the hybridization theory: (i) BF3 +F→ BF (ii). PCIs + CF → PC16 for Found