tain viruses Unless you need to edit its safer to stay in Pr

tain viruses. Unless you need to edit it\'s safer to stay in Protected View. Enable Editing 2) Which one of the following substances will not have hydrogen bonding as one of its intermolecular forces? 0 (B) H-0-0-H (A) CH3 CH3 N-N 3) The predominant intermolecular force in (CH3)2NH is A) London dispersion forces D) dipole-dipole forces B) ion-dipole forces E) hydrogen bonding C) ionic bonding 4) The predominant intermolecular force in AsH3 is A) London dispersion forces D) dipole-dipole forces B) ion-dipole forces E) hydrogen bonding C) ionic bonding 5) C12H26 molecules are held together by A) ion-ion interactions D) dipole-dipole interactions B) hydrogen bonding E) dispersion forces 6) Which of the following molecules has hydrogen bonding as its only intermolecular force? A) HF E) None, all of the above exhibit dispersion forces

Solution

2)- Option B is Correct i.e H2O2 cannot form hydrogen bond rather H₂O₂ has a covalent bond between the two Oxygen atoms

3)-as dimehyl amine contains hydrogen atom and electronegative nitrogen atom so it can form strong H-bonding with water so Option E is correct.

4)-AsH3 has Van der Waals forces and further,Van der Waals forces\' is a general term used to define the attraction of intermolecular forces between molecules. There are two kinds of Van der Waals forces: weak London Dispersion Forces and stronger dipole-dipole forces.AaH3 has London dispersion forces so Option A is correct.

5)-C12H26 is an hydrocarbon(paraffin) compound so it has weak dispersion forces so Option E is correct.

6)-Option E is correct i.e all the bove compounds have dispersion forces also i.e,

HF is a polar molecule: dipole-dipole forces. Hydrogen is bounded to F.Hydrogen bonds exist. There are also dispersion forces between HF molecules.

water has all three types of intermolecular forces, with the strongest being hydrogen bonding. All things have London dispersion forces and dipole-2 forces.

Primary amine C6H13NH2 form hydrogen bonds with each other as well as van der Waals dispersion forces and dipole-dipole interactions.

Hydrogen bonding isn\'t the only intermolecular force in C5H11OH. There are also van der Waals dispersion forces and dipole-dipole interactions. The hydrogen bonding and the dipole-dipole interactions will be much the same for all the alcohols, but the dispersion forces will increase as the alcohols get bigger.