Question

question 4
1 pts
which one of these is not a hybrid orbit?
sp
sp³
d²sp³
dp
question 5
1 pts
of the 3 p orbits, how many will form a σ bond?
2
1
3
0

Explanation:

Question 4

Hybrid orbitals are formed by mixing atomic orbitals. Common hybrid orbitals include \( sp \) (mix of \( s \) and \( p \)), \( sp^3 \) (mix of \( s \) and three \( p \) orbitals), \( d^2sp^3 \) (mix of \( s \), \( p \), and \( d \) orbitals). \( dp \) is not a recognized hybrid orbital as hybridizations typically involve \( s \) with \( p \) or \( d \), and standard hybridizations don't include \( dp \) (valid ones involve \( s \) in the mix for common cases).

Step1: Recall \( p \)-orbital orientation and \( \sigma \)-bond formation

\( p \)-orbitals are oriented along the x, y, and z axes. A \( \sigma \)-bond is formed by head - on (axial) overlap of orbitals. Among the three \( p \)-orbitals, only one (the one along the internuclear axis) can form a \( \sigma \)-bond through head - on overlap. The other two \( p \)-orbitals form \( \pi \)-bonds through side - on overlap.

Answer:

\( dp \) (the option with "dp")

Question 5