Organic Chem help please!!!?

Question

Which of the following statements is/are true concerning orbital overlap bonding, and carbon hybridization.

A. The sp^3 hybrid has one electron "left over" (i.e. not used in the hybrid)

B. The overlap between an electron is a sp^2 hybridized orbital, and an electron in a (s atomic orbital) is called a pi bond.

C. The shape of sp hybridized orbitals dictates 120 degree angkes between bonds

D. In carbon-carbon bonds, the maximum amount of orbital overlap requires that the (p orbitals) are perpendicular to each other.

E. The shape of the sp^3 hydridized orbitals is tetrehedral

F. More than one of the above

G. None of the above

Answer 1

A) False, sp3 hybridization has no left over electrons. The Lewis model treats electrons as pairs, so "left over' electrons would be characterized as an anion, radical, or cation. (or radical cation/anion, in some cases)

B)A pi bond is not a bond between 2 sp2 hybridized atoms. Let's clarify that.

If 2 sp2 hybridized orbitals overlap in a covalent bond, that is a sigma bond. sp, sp2, and sp3 orbitals all have the same orbital shape. The difference is the number of orbitals and their orientation on the xyz plane.

A pi bond is created by an overlap of p orbitals. Pi bonds allow very little rotation because the p orbitals have to align for the bonding interaction to take place.

The overlap between an sp2 orbital and an s orbital (like the C-H bond in C=C-H) is a sigma bond.

c) sp hybridization requires 180 degree bond angles, because now 2 p orbitals have to overlap and they have to be orthogonal to each other.

D) For a pi bond, the p orbitals should be parallel (or more properly, coplanar). In a sigma bond, the overlap creates a bond with free rotation, so the dihedral angle isn't important. That said, steric affects and hyperconjugation do affect the conformation of a molecule, so certain conformations are favored.

E) True, the 4 sp3 hybridized orbitals give a tetrahedral shape.

Answer 2

I'll try and answer as much as I can:
A) I am not sure what is meant with "left over". For example an oxygen atom in an alcohol group is sp3 hybridized. 2 of the 4 sp3 lobes contain a lone pair of electrons. If these lone pairs are considered "left over" then the statement is false. On the other hand a carbon atom in an alkane is also sp3 hybridized. All bonding electrons are used up in forming bonds through all 4 sp3 lobes. For that situation the statement is through.

B. Wrong: A pi bond is the bond between 2 sp2 hybridized atoms, NOT between an sp2 hybridized atom and an s-orbital.

C. Wrong: sp hybridization results in 2 orbital lobes. To get 2 lobes as far apart as possible they will be 180 degrees apart and not 120 degrees (which is sp2 hybridization)

D. Wrong: Overlap occurs when orbitals are pointing in the same direction, i.e. they are parallel to each other.

E. Correct: You have 4 lobes of negative charged electrons. To keep the negative charges as far as possible from each other in 3 dimensions, you will end up in a tetrahedral distribution.

F and G: depends on what you think about A:

Answer 3

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Answer 4

E is true (write tetrahedral)

A,C, D are false

for b, i do not understand the question