chemsitry last question

Question

A student attempts to dissolve solid sodium chloride in water and in hexane (C6H14). NaCl dissolves in one of the solvents but not in the other. which of the following statements most accurately describes what will happen AND why it happens?

select one:

A) NaCl will only dissolve in water. water has a much larger dipole movement than hexane.The strength of the ion-dipole interactions between water and Na+ and between water and Cl- is sufficient to allow the NaCl to be soluble in water

b) NaCl will only dissolve in water. water is capable of participating in hydrogen bonding, whereas hexane cannot. The strength of the hydrogen bonding interactions between water and NaCl is sufficient to allow the NaCl to be soluble in water

Answer 1

Both of these answer are correct in saying that NaCl will dissolve in water, but now it's our job to decide which reasoning is correct. There are a couple requirements for hydrogen bonding to occur. One such requirement is there has to be an oxygen, fluorine, or nitrogen in both participating parties, one of which has a lone pair of electrons, and one which has a hydrogen atom attached to it. In this case, NaCl doesn't meet those requirements, so it is not capable of hydrogen bonding. It does, however, dissociate into individual ions, allowing for ion-dipole interactions, as mentioned in answer A.

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