Sigma Bonding Ac bond arises from the straight-on overlap of two atomic orbitals. The electron density lies along the axis of the two bonded nuclei. sp3 hybrid orbital Example: Sigma Bonding in methane, CH, 1s orbital What atomic or hybrid orbitals make up the sigma bond between Cl and F in chlorine trifluoride, CIF3 ? orbital on Cl + orbital on F What are the approximate F-CI-F bond angles ? (list all possible) Submit Answer Retry Entire Group 8 more group attempts remaining

Sigma Bonding Ac bond arises from the straight-on overlap of two atomic orbitals. The electron density lies along the axis of the two bonded nuclei. sp3 hybrid orbital Example: Sigma Bonding in methane, CH, 1s orbital What atomic or hybrid orbitals make up the sigma bond between Cl and F in chlorine trifluoride, CIF3 ? orbital on Cl + orbital on F What are the approximate F-CI-F bond angles ? (list all possible) Submit Answer Retry Entire Group 8 more group attempts remaining

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter1: Covalent Bonding And Shapes Of Molecules

Section: Chapter Questions

Problem 1.61P: Using cartoon representations, draw a molecular orbital mixing diagram for a CO bond. In your...

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Consider acetyl salicylic acid, better known as aspirin. Its structure is (a) How many sigma and pi bonds are there in aspirin? (b) What are the approximate values of the angles marked (in blue) A, B, and C? (c) What is the hybridization of each atom marked (in red) 1, 2, and 3?
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.
Consider the following computer-generated model of caffeine: Complete a Lewis structure for caffeine in which all atoms have a formal charge of zero (as is typical with most organic compounds). How many C and N atoms are sp2 hybridized? How many C and N atoms are sp3 hybridized? sp hybridized? How many and bonds are there?
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.
Using cartoon representations, draw a molecular orbital mixing diagram for a CO bond. In your picture, consider the relative energies of C and O and how this changes the resulting bonding and antibonding molecular orbitals relative to a CC bond.
1. Calculate the percentage s and p characters in sp, sp^2 and sp^3 hybrid orbitals. 2. Draw the molecular orbital diagram of propene, CH3-CH=CH2. 3. Draw an orbital diagram of an allene, H2C=C=CH2. What hybridization must the central carbon atom have in order to form two double bonds? 4. Describe the shape of sp^3 hybrid orbitals. 5. Dicuss, with illustrations, the two main steps in the hybridization of a carbon atom. 6.a. Arrange the following organic molecules in order of increasing acidity, starting with the least acidic. CH3CH3, HC(=_)CH and CH2=CH2 b. How many hybrid orbitals are formed when one 2s atomic orbital mixes with two 2p atomic orbitals? What shape do they form? c. Describe in detail, the shape of p atomic orbitals. d. Giving an example, explain what is meant by the excited-state electronic configuration of an atom of an element. e. Using clear illustrations, discuss the main differences between E1 and E2 mechanisms in organic reactions.
In the formate ion, HCO2-, the carbon atom is the centralatom with the other three atoms attached to it. (a) Draw aLewis structure for the formate ion. (b) What hybridizationis exhibited by the C atom? (c) Are there multiple equivalentresonance structures for the ion? (d) How many electrons arein the p system of the ion?
In the formate ion, HCO2-, the carbon atom is the centralatom with the other three atoms attached to it. (a) Draw aLewis structure for the formate ion. (b) What hybridizationis exhibited by the C atom? (c) Are there multiple equivalentresonance structures for the ion? (d) How many electrons arein the π system of the ion?
a) Consider a molecule of acetone cyanohydrin, shown below. What is the hybridization and molecular geometry at CA, CB, and O? (b) For Carbon B (CB) and nitrogen (N), draw orbital energy diagrams showing the orbitals involved in bonding after hybridization. Be sure to fill the orbitals appropriately with valence electrons. c) In your diagrams in part (b), which orbitals are involved in sigma and pi bonding? Orbitals Involved in Sigma Bonding Orbitals Involved in Pi Bonding 2p sp sp2 sp3 2p sp sp2 sp3 (d) In a sample containing many molecules of acetone cyanohydrin (and no other substances), what type(s) of intermolecular forces could be present? Choose all that apply. Covalent Bonds Hydrogen Bonds Dipole-Dipole Forces London Dispersion Forces
I have a question regarding hybrid vs atomic orbitals: 1) What would be the hybridizations of C and O in the molecule H2CO? It asks to draw an electron orbital diagram (with arrows) of all the electrons in C before and after hybridization. 2) Draw a diagram of the H2CO molecule showing the overlap of orbitals between the C and O atoms that make up the sigma (σ) and pi (π) bonds. Which orbitals make up the σ bond? Which ones form the π bond?
1. Construct the molecular orbital diagram for H2+2, H2+, and H2- and find there bond orders in decimal form. part b of question 6 what is the bond order of Be2+? also numerical.
(a) If the valence atomic orbitals of an atom are sp hybridized,how many unhybridized p orbitals remain in thevalence shell? How many p bonds can the atom form?(b) Imagine that you could hold two atoms that are bondedtogether, twist them, and not change the bond length.Would it be easier to twist (rotate) around a single s bondor around a double 1s plus p2 bond, or would they be thesame?