Based on knowledge of intermolecular forces and bonding principles, which of the following compounds would be expected to be both the most soluble in water at room temperature and have the highest melting point?

N a F

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C B r_{4}

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C_{6} H_{12} O_{6}

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K B r

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Solution

The correct option is B $N a F$
As $N a^{+}$ being electropositive metal and $F^{-}$ being highly electronegative attracts each other strongly forming strong intermolecular forces.

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Question 34.1

Structures of molecules of two compounds are given below.

Which of the two compounds will have intermolecular hydrogen bonding and which compound is expected to show intramolecular hydrogen bonding?

(ii) The melting point of the compound depends on, among other things, the extent of hydrogen bonding. On this basis explain which of the above two compounds will show higher melting point?

(iii) The solubility of compounds in water depends on power to form hydrogen bonds with water. Which of the above compounds will form a hydrogen bond with easily and be more soluble in it?

Q. Most solid compounds melt at a specific temperature. Based on knowledge of interparticle forces, which of the following melts over a range of temperatures, not at a specific value?

Q. Which of the following compounds would you expect to be most soluble in water?

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Of the following halogens bonded to carbon, which molecular compound would be expected to be a gas at room pressure and temperature?

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Based on knowledge of intermolecular forces and bonding principles, which of the following compounds would be expected to be both the most soluble in water at room temperature and have the highest melting point?

The correct option is B NaFAs Na+ being electropositive metal and F− being highly electronegative attracts each other strongly forming strong intermolecular forces.

The correct option is B $N a F$
As $N a^{+}$ being electropositive metal and $F^{-}$ being highly electronegative attracts each other strongly forming strong intermolecular forces.