Question

The oxide of the element whose electronic configuration is $1{s^2}2{s^2}2{p^6}3{s^1}$ is:
A. amphoteric
B. basic
C. Acidic
D. Neutral

Answer 1

From the given electronic configuration $1{s^2}2{s^2}2{p^6}3{s^1}$ we can know that the total number of electrons present is 11 and so the atomic number of the element is 11 which is of sodium.

Complete step by step answer:
Oxides are defined as the binary compounds which are formed by the reaction of chemical elements with the oxygen. On the basis of their nature, oxides are classified as acidic oxide, basic oxides, neutral oxides and amphoteric oxides.
Acidic oxides are defined as the oxides which on dissolution in water give an acidic solution. They are acidic in nature.
Basic oxides are defined as the oxides which on dissolution in water give a basic solution. They are basic in nature.
Amphoteric oxides are defined as those oxides which can react as both acid and base. They are amphoteric in nature.
Neutral oxides are defined as the oxides which on dissolution in water do not form acidic solution or basic solution. They are neutral in nature.
The given electronic configuration is $1{s^2}2{s^2}2{p^6}3{s^1}$. The outermost orbital of the element contains 1 electron that means it is a monovalent compound which forms an oxide with chemical formula ${M_2}O$. From the given electronic configuration it can be known that total 11 electrons are present so the atomic number of the element is 11. Thus the element with atomic number 11 is sodium.
The oxide formed by sodium reacting with oxygen is $N{a_2}O$.
The reaction of sodium oxide and water is shown below.
$N{a_2}O + {H_2}O \to 2NaOH$
Sodium oxide reacting with water gives sodium hydroxide which is a strong base.
Thus, the oxide of the element whose electronic configuration is $1{s^2}2{s^2}2{p^6}3{s^1}$ is basic.
So, the correct answer is “Option B”.

Note:
Non-metals generally form acidic oxide on reacting with oxygen and metals generally form basic oxides on reacting with oxygen.