Question

Increasing order of electronegativity of the following elements is?
(a)- $C$ $<$ $N$ $<$ $Si$ $<$ $P$
(b)- $N$ $<$ $Si$ $<$ $C$ $<$ $P$
(c)- $Si$ $<$ $P$ $<$ $C$ $<$ $N$
(d)- $P$ $<$ $Si$ $<$ $N$ $<$ $C$

Answer 1

Electronegativity of the element is the property that estimates the ability of the atom to form a negative ion by attracting electrons towards it. In the periodic table, we have a trend in the electronegativity, in the period the electronegativity increases, and in the period the electronegativity decreases.

Complete step by step answer:
Electronegativity of the element is the property that estimates the ability of the atom to form a negative ion by attracting electrons towards it. The metals have lesser electronegativity than the non-metals. As the non-metallic character of the elements increases the electronegativity of the element also increases.
In the periodic table, we have a trend in the electronegativity, in the period the electronegativity increases, and in the period the electronegativity decreases.
So in the questions, we are given four elements, carbon, nitrogen, phosphorus, and silicon. Carbon and nitrogen belong to the same period. Phosphorus and silicon belong to the same period. Nitrogen and carbon belong to period 2, and phosphorus and silicon belong to period 3. So the electronegativity of carbon and nitrogen will be greater than phosphorus and silicon. In carbon and nitrogen, nitrogen is more electronegative, and in phosphorus and silicon, phosphorus is more electronegative. Hence the order will be:
$Si$ $<$ $P$ $<$ $C$ $<$ $N$

Therefore, the correct answer is an option (c).

Note: The electronegativity of the element is used for finding the metallic and non-metallic character of the element. It is also used for finding the polar and non-polar bonds in the molecules.