Question

In which of the following, oxides of three elements \(X\), \(Y\) and \(Z\) are correctly arranged in the increasing order of acidic nature. The electronic configurations of \(X\), \(Y\) and \(Z\) are \([\text{Ne}]3s^23p^1\), \([\text{Ne}]3s^23p^5\), \([\text{Ne}]3s^2\) respectively.

• A. \(X\lt Y\lt Z\)
• B. \(Y\lt Z\lt X\)
• C. \(Z\lt X\lt Y\)
• D. \(X\lt Z\lt Y\)

Hint:

Across a period, metallic character decreases and non-metallic character increases. Therefore, acidic nature of oxides generally increases from left to right.

Answer 1

The Correct Option is C

Step 1: Identify the elements.
For \(X\), \[ [\text{Ne}]3s^23p^1 \] This element is aluminium \((Al)\).
For \(Y\), \[ [\text{Ne}]3s^23p^5 \] This element is chlorine \((Cl)\).
For \(Z\), \[ [\text{Ne}]3s^2 \] This element is magnesium \((Mg)\).

Step 2: Compare acidic nature of their oxides.
Magnesium forms \[ MgO \] which is basic in nature.
Aluminium forms \[ Al_2O_3 \] which is amphoteric in nature.
Chlorine forms acidic oxides such as \[ Cl_2O_7 \] which are strongly acidic.

Step 3: Arrange in increasing acidic nature.
Basic oxide has least acidic nature, amphoteric oxide has intermediate acidic nature, and non-metal oxide has highest acidic nature.
Therefore, \[ MgO\lt Al_2O_3\lt \text{chlorine oxides} \] So, \[ Z\lt X\lt Y \]

Step 4: Final conclusion.
Hence, the correct order is \[ \boxed{Z\lt X\lt Y} \]