1.Acetic acid, CH3COOH (Recall that the acid functional group contains an -OH and a double bonded oxygen.)

2.Hydrogen sulfide, H2S

3.Sulfur trioxide, SO3

4.Methylamine, CH3NH2


*ionic bonds

Dipole-dipole interactions

Hydrogen bonds

Ion-dipole forces

Ion-induced dipole forces

London forces*

I think each question has more than one answer..
But I am still confusing that which one is correct for each questions
Can you explain each molecular attractive forces?
Thanks

You really don't know any of the different types of bonding?

Ionic: Occurs between two ions of opposite charge.

Dipole-dipole: Occurs non-polar in molecules and is directly proportional to the number of electrons in the molecules.

Hydrogen bonds: Occurs in highly electronegative elements bonded to hydrogen atoms (Electronegative elements concerned N, O, F)

Ion-dipole: Occurs polar in molecules

Ion-induced dipole forces: this is the same as dipole dipole as far as I know

London forces: This is a common term for all of dipole dipole and ion dipole and hydrogen bonds.

1.Acetic acid, CH3COOH (Recall that the acid functional group contains an -OH and a double bonded oxygen.)


2.Hydrogen sulfide, H2S
Ionic bond
London forces

3.Sulfur trioxide, SO3
Ion dipole force
London forces

4.Methylamine, CH3NH2


I don't know... I am confusing to figure out.. please more help
Thanks.. Please check that answers..

CH3COOH: (molecule)
Dipole-dipole
London forces
Hydrogen bonds (H atom directly attached to electronegative O atom)
Ion dipole (because of H bonds)

H2S: (bent molecule)
Dipole-dipole
London forces
Ion dipole (because of polar nature of molecule; bent)

SO3: (triangular planar molecule)
Dipole-dipole
London forces

CH3NH2: (molecule)
Dipole-dipole
London forces
Hydrogen bonds (H atom directly attached to electronegative N atom)
Ion dipole (because of H bonds)

Note: I didn't say ion-induced dipole since I consider it the same as dipole dipole.

I put like this in my WileyPlus it say all incorrect..
So confusing please help me..

I don't know about it, but If I were to choose only one (as opposed to your question: "all intermolecular attractive forces"),the main force of attraction, because the rest are often referred to as 'too inaccurate', this is how I'd do it.

None of them contain ionic bonding, because none of them are ions, but molecules, covalent molecules.

CH3COOH: Hydrogen bonds

H2S: ion dipole (I call it permanent dipole dipole here)

SO3: dipole-dipole (I call it induced dipole dipole)

CH3NH2: Hydrogen bonds

The only intermolecular forces of attraction I learned are:
Hydrogen bonds
Permanent dipole-dipole
Induced dipole-dipole

All three of them being Van der Waals forces (or London forces)

Hydrogen bonding is a special type of permanent dipole dipole.

Unless I misunderstood one of the terms you used, I don't see how the answers I gave are wrong...

CH3COOH:
Hydrogen bonds
London forces
Dipole-dipole interactions

H2S:
Dipole-dipole interactions
London forces

SO3:
London forces

CH3NH2:
Hydrogen bonds
Dipole-dipole interactions
London forces

These were the correct answers for me in WileyPLUS.