Question

Electronic configurations of three elements, A, B and C are given below.

A: $1s^{2}2s^{2}2p^6$

B: $1s^{2}2s^{2}2p^{6}3s^{2}3p^3$

C: $1s^{2}2s^{2}2p^{6}3s^{2}3p^5$

The bond between B and C will be

• A. Covalent
• B. Coordinate
• C. lonic
• D. Hydrogen

Answer 1

The correct option is A Covalent

Solution:

Element Electronic configuration



$B\left(P\right)$ $1s^{2}2s^{2}2p^{6}3s^{2}3p^3$


$C\left(CI\right)$ $1s^{2}2s^{2}2p^{6}3s^{2}3p^5$

Valence shell electrons: Number of electrons in the outer shell of an atom are called valence shell electrons. These electrons take part in bond formation.

Octet rule: The elements form bond to complete 8 electrons in their valence shell.

'B' has 5 electrons in its velence shell, so it needs 3 electronce to complete its octet.
'C' has 7 electrons in its valence shell, so it needs 1 electron to complete its octet.
So , an atom of B shares 1 electron each with 3 atoms of C, this way the octets of both are completed and $B{C}_3$ is formed.



Since , the compound is formed by sharing of electrons, the bond between B and C will be covalent.

Hence, $\left(B\right)$ option is correct.