What is the strongest intermolecular force present in each molecule:

H2S
CF4
NH3
CS2
PCL3
N
CH2O
C2H6
CH3OH
BH3

My work:
Hydrogen bonding
London dispersion
Dipole dipole
London dispersion
Dipole dipole
London dispersion
Hydrogen bonding
Hydrogen bonding
Hydrogen bonding

Am I right??

Yes, you are correct in identifying the strongest intermolecular forces present in each molecule. Here's a step-by-step explanation of how to determine the intermolecular forces for each molecule:

1. H2S: The central atom (Sulfur) is bonded to two Hydrogen atoms. It has a lone pair on the central atom, which allows for hydrogen bonding.

2. CF4: Carbon and Fluorine have a electronegativity difference, meaning the molecule is polar. It experiences dipole-dipole interactions due to the polarity of the molecule.

3. NH3: Nitrogen and Hydrogen have a electronegativity difference, so the molecule is polar. It experiences dipole-dipole interactions due to the polarity of the molecule.

4. CS2: Carbon and Sulfur have similar electronegativities, so the molecule is nonpolar. It experiences only London dispersion forces.

5. PCl3: Phosphorus and Chlorine have an electronegativity difference, meaning the molecule has polarity. It experiences dipole-dipole interactions due to the polarity of the molecule.

6. N: Nitrogen is a diatomic molecule, so it only experiences London dispersion forces.

7. CH2O: In this molecule, Carbon and Oxygen have an electronegativity difference, which makes the molecule polar. It experiences dipole-dipole interactions due to the polarity of the molecule.

8. C2H6: The molecule is nonpolar because the electronegativities of carbon and hydrogen are similar. It experiences only London dispersion forces.

9. CH3OH: The molecule is polar because of the electronegativity difference between Carbon, Oxygen, and Hydrogen. It experiences dipole-dipole interactions.

10. BH3: The molecule is nonpolar since the electronegativities of Boron and Hydrogen are similar. It experiences London dispersion forces.

Remember, these intermolecular forces can be ranked in terms of strength from highest to lowest as follows:
1. Hydrogen bonding (strongest)
2. Dipole-dipole interactions
3. London dispersion forces (weakest)