Question

Two substances $X$ and $Y$ are dissolved in water under suitable conditions. $X$ is a gas while $Y$ is a solid under normal conditions. Solution of $Y$ is found to conduct electricity but not $X$. Based on the conclusion, identify the nature of bond present in $X$ and $Y$ with appropriate reasons as given below.

Arrange the step given below in a sequence:
(a) $Y$ is a solid at room temperature and its aqueous solution conducts electricity. This shows that it is an ionic compound.
(b) $X$ on dissolution in water doesn't conduct electricity and is a gas at room temperature. Hence it should be a nonpolar covalent molecule.
(c) Aqueous solutions of both ionic compounds and polar covalent compounds conduct electricity because of the presence of free ions.
(d) All ionic compounds are solids and more of the nonpolar covalent molecules are gases or solids at room temperature. Polar covalent compounds are liquids or gases.

• A. c d b a
• B. a d c b
• C. a c b d
• D. c a b d

Answer 1

The correct option is A c d b a

We know an ionic and polar covalent molecule on dissolution in water conducts electricity.

Ionic compounds are solid and in an aqueous form, they conduct electricity due to the presence of free ions. Since $X$ on dissolution does not conduct electricity means it is a non-polar covalent molecule.

And $Y$ is solid at room temperature but its aqueous solution conducts electricity which shows it is an ionic compound.