Answer to Question #86525 in Organic Chemistry for Joshua

Question

3.Explain why the bonds formed in
SP^3
hybrid orbitals are stronger and stable compare to the bonds formed by using pure atomic orbitals?
a.The lobes in
SP^3
hybrid orbitals are separated by anode.
b.In
SP^3
hybrid orbital, the electron density is concentrated in one direction leading to greater overlap.
c.
SP^3
hybrid orbitals are similar to p orbitals.
d.
SP^3
hybrid orbitals have two lobes of unequal sizes

4.Which of these shows how a sigma
(δ)
bond is formed.
a.sideway overlap of S and P orbitals
b.Edge on overlap of p orbitals
c.sideway overlap of p orbitals
d.edge on overlaps of pure S and P orbitals

Answer 1

Sp3

hybrid orbital is formed by the combination of one S & three P orbitals. This

result lowering of energy of hybrid orbital compared pure atomic orbitals and also (b.)In

SP^3 hybrid orbital, the electron density is concentrated in one direction leading to greater

overlap.That is why ,Sp3

hybrid orbitals are stronger and stable compare to the bonds formed

by using pure atomic orbitals.

4.Which of these shows how a sigma(δ) bond is formed.

a.sideway overlap of S and P orbitals

b.Edge on overlap of p orbitals

c.sideway overlap of p orbitals

d.edge on overlaps of pure S and P orbitals

Solution: Generally edge on overlap of pure S &P and P & P orbitals form a sigma(δ)

bond. While sideway overlap of two atomic orbitals result formation of Pi(π) bond.

Therefore a sigma (δ) bond is formed by(b).Edge on overlap of p orbitals & (d).edge on

overlaps of pure S and P orbitals