M2S8 – Intermolecular Forces

In which of these molecules do the intermolecular forces arise largely from attractions between temporary dipoles?

In which of these molecules do the intermolecular forces arise largely from attractions between permanent dipoles?

In which of these molecules do the intermolecular forces arise largely from hydrogen bonding?

Which of these materials owe their strength to intermolecular forces?

In which of these solids are there two types of bonding: one strong and one weak?

(i) diamond

(ii) ice

(iii) sodium chloride

(iv) graphite

Which of these bonds are polar covalent bonds?

(i) C-C

(ii) H-Br

(iii) N-N

(iv) C=O

Which of these molecules are overall non-polar?

(i) H₂O

(ii) CO₂

(iii) SO₂

(iv) CCl₄

Which of these statements are true for the hydrides of group 5: NH₃, PH₃, AsH₃ and SbH₃:

(i) the molecules decrease in size down the group

(ii) the boiling point of ammonia is higher than expected from the general trend in values down the group

(iii) none of the molecules is polar

(iv) only ammonia is affected by hydrogen bonding

Which of these true statements can help to explain why iodine is a solid while chlorine is a gas at room temperature and pressure?

(i) iodine molecules have a larger surface area than chlorine molecules

(ii) iodine atoms are heavier than chlorine atoms

(iii) the outer shell electrons in iodine atoms are further from the nucleus than they are in chlorine atoms

(iv) the charge on the nucleus of an iodine atom is larger than the charge on the nucleus of a chlorine atom

In the family of hydrocarbons called alkanes:

(i) the boiling points of the straight chain compounds rise as the number of carbon atoms increases

(ii) the intermolecular forces arise from attractions between temporary dipoles

(iii) in any pair of isomers the compound with the more highly branched molecules has the lower boiling point

(iv) the unbranched compounds are all liquids at room temperature.