Using cartoon representations, draw a molecular orbital mixing ...

[erika]

Using cartoon representations, draw a molecular orbital mixing diagram for a C-O -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 C-C -bond.
 
Question 2

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Question 3

What is the hybridization of the highlighted atoms in the following structures, and what are your estimates for the bond angles around these highlighted atoms? In each case, in what kind of orbital does the lone pair of electrons on the nitrogen reside.
 
Question 4

Draw structural formulas for
  (a) The four primary (1) amines with the molecular formula C₄H_{1 1}N.
  (b) The three secondary (2) amines with the molecular formula C₄H_{1 1}N.
  (c) The one tertiary (3) amine with the molecular formula C₄H_{1 1}N.

Question 5

What is the meaning of the term tertiary (3) when it is used to classify amines? Draw a structural formula for the one tertiary (3) amine known as Hunigs base (N,N-diisopropylethylamine).

Question 6

What is the meaning of the term tertiary (3) when it is used to classify alcohols? Draw a structural formula for the one tertiary (3) alcohol with the molecular formula C₄ H_{1 0}O.

Question 7

Draw Lewis structures for these functional groups. Be certain to show all valence electrons on each.
  (a) Carbonyl group
  (b) Carboxyl group
  (c) Hydroxyl group
  (d) Ester group
  (e) Amide group

Question 8

Use VSEPR to predict bond angles about each highlighted atom.

[Eazy416]

Answer to Question 1



Answer to Question 2

The O atom, being more electronegative, is of lower energy than the C atom. This means the O orbital makes a larger contribution to the -bonding orbital, while the C atom makes a larger contribution to the -antibonding orbital. For a -bonding orbital formed from two C atoms of the same hybridization, both C orbitals make equal contributions.

Answer to Question 3

In each case there are significant contributing structures that have a  bond involving nitrogen.


These are examples of nitrogen lone pairs delocalizing into adjacent  bonds, a common feature of many organic

molecules you will come across. For this to happen, the nitrogen atoms must be sp² hydridized, so the lone pairs on nitrogen are best thought of as being in 2p orbitals. Such delocalization of electron density in  orbitals is stabilizing and therefore favorable, a phenomenon that is best explained using quantum mechanical arguments (beyond the scope of this text).

Answer to Question 4

(a) The four primary (1) amines with the molecular formula C₄H_{1 1}N.

(b) The three secondary (2) amines with the molecular formula C₄H_{1 1}N.

(c) The one tertiary (3) amine with the molecular formula C₄H_{1 1}N.


Answer to Question 5

[erika]

Thank you!

[Eazy416]

Always glad to help...