Answer: See below
Step-by-step explanation:
For the first molecule, Al3H, there are:
- 3 bond pairs and 0 lone pairs on the main atom
- The total number of electron pairs is 3.
- So, the hybridization of the molecule will be sp2, and the shape according to VSEPR theory will be a trigonal planar
For the second molecule, CH2F2, there are:
- 4 bond pairs and 0 lone pair on the central atom. T
- There are 4 electron pairs
- Therefore, the hybridization of the molecule will be sp2, and the shape will be tetrahedral
For the third molecule, PH3, there are
- 3 bond pairs and 1 lone pair.
- So, the hybridization of the molecule will be sp3. However, the 4th spot on the molecule will be occupied by a lone pair, so the overall shape will be trigonal pyramidal and not tetrahedral
For the final molecule, O3, there are:
- 2 bond pairs and 1 lone pairs.
- The number of electron pairs is 3.
- Hence, the hybridization of the molecule will be sp2. But due to the 3rd position being taken by a lone pair, and the VSEPR theory assuming that electron pairs will sort themselves to decrease the effects of repulsion, the overall shape will be bent and not linear.