Question

Two substance $X$ and $Y$ are dissolved in water under suitable conditions. $X$ is a gas while Y is a solid under normal conditions. The 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 steps given below in a sequence.
(a) $Y$ is a solid at room temperature and its aqueous solution conducts electricity. This show 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 non-polar 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 most of the non-polar 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

Our first attempt should be to differentiate substance as ionic are polar/non-polar covalent bond. So, step $C$ will be the first step.

Now, we have to differentiate $X$ and $Y$ based on there physical state at room temperature. So, step $d$ is used as the second step.

Now, for covalent we have to check whether it is polar and non-polar based on their conductivity. So, use step $b$ as the third step.

After all the three steps finally is $a$.

So, the correct order is: $c,d,b,a.$