10. Shown below are the structures of six molecules. For each molecule:i.) Indicate whether the molecule features delocalized n bonding.ii.) Indicate which atoms in each molecule possessp orbitals that are not hybridized.iii.) If the molecule does feature delocalized r bonding, draw at least one resonance structurethat exists for the molecule.А.В.С.F.NH2D.Е.`NH2

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Answered: 10. Shown below are the structures of…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.118QE

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Use Figs. 4-54 and 4-55 to answer the following questions. a. Would the bonding molecular orbital in HF place greater electron density near the H or the F atom? Why? b. Would the bonding molecular orbital have greater fluorine 2p character, greater hydrogen 1s character, or an equal contribution from both? Why? c. Answer the previous two questions for the antibonding molecular orbital in HF.
The antibiotic thiarubin-A was discovered by studying the feeding habits of wild chimpanzees in Tanzania. The structure for thiarubin-A is a. Complete the Lewis structure, showing all lone pairs of electrons. b. Indicate the hybrid orbitals used by the carbon and sulfur atoms in thiarubin-A. c. How many and bonds are present in this molecule?
Compare Figs. 4-47 and 4-49. Why are they different? Because B2 is known to be paramagnetic, the 2p and 2p molecular orbitals must be switched from the first prediction. What is the rationale for this? Why might one expect the 2p to be lower in energy than the 2p? Why cant we use diatomic oxygen to help us decide whether the 2p, or 2p, is lower in energy?
Which atomic orbitals overlap to form the bonds in ClF?
7.57 What observation about molecules compels us to consider the hybridization of atomic orbitals?
10. Shown below are the structures of six molecules. For each molecule: i.) Indicate whether the molecule features delocalized n bonding. ii.) Indicate which atoms in each molecule possessp orbitals that are not hybridized. iii.) If the molecule does feature delocalized n bonding, draw at least one resonance structure that exists for the molecule. F. NH2 D. Е. `NH2
VSEPR: Molecular Geometry 1. For the following molecules: 1) draw a Lewis Dot structure, including contributing resonance structures, if present; 2) use VSEPR to draw an appropriate structure; 3) give an appropriate designation for the ideal molecular geometry; 4) describe any deviations to the ideal molecular geometry; *don't worry about corrections for e and h. g. HOCI h.* SO;2 i. NO2*
Consider the molecule OA || H;CA- CB – OBH 1. Indicate the hybridization employed by each central atom. CA : b. Св: а. OA : d. Ов: с. 2. Indicate the electron pair geometry about each central atom. CA : b. Св: а. OA : d. Ов: с. 3. Indicate the predicted bond angles around each central atom having more than one bond. CA : b. Св: Ов: а. с. 4. Describe all the o and t bonds in this molecule in the form of a hybridization and bonding scheme. For example, a hypothetical O-H bond = 0 (2 sp) – H (1 s). sigma bond(s) pi bond(s) 5. Which bond is the: а. shortest? b. strongest?
17. HCOOH а. Lewis structure b. Drawing of shape (label angles) С. Name of shape d. Polar or nonpolar? e. Hybridization 18. BrO, а. Lewis structure b. Drawing of shape (label angles) Name of shape С. d. Polar or nonpolar? e. Hybridization 19. NO (exception to the octet) а. Lewis structure b. Drawing of shape (label angles) с. Name of shape d. Polar or nonpolar? e. Hybridization
6. СО, а. Lewis structure b. Drawing of shape (label angles) Name of shape С. d. Polar or nonpolar? e. Hybridization 7. HCN а. Lewis structure b. Drawing of shape (label angles) С. Name of shape d. Polar or nonpolar? e. Hybridization
List the correct electron and molecular geometries that correspond to each set of electron groups around the central atom of a molecule.a. four electron groups overall; three bonding groups and onelone pairb. four electron groups overall; two bonding groups and two lone pairsc. five electron groups overall; four bonding groups and one lone paird. five electron groups overall; three bonding groups and two lone pairse. five electron groups overall; two bonding groups and three lone pairsf. six electron groups overall; five bonding groups and one lone pairg. six electron groups overall; four bonding groups and two lone pairs
6. Identify the geometry and predict the actual shape of the following chemical species, support your answer with a drawing. Include an estimation of the bond angles. (Example; <120 because...) A. NH2 В. 13 C. PCI6 D. ASF5

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