Question

Assertion
Ionic bonds are directional in nature whereas covalent bonds are non-directional.
Reason
According to orbital overlap concept, the formation of a covalent bond between two atoms results by pairing of electrons present in the valence shell having same spins.
A. Both assertion and reason are correct and reason is the correct explanation of the assertion
B. Both assertion and reason are correct but reason is not the correct explanation of the assertion
C. Assertion is correct but reason is incorrect
D. Both assertion and reason are incorrect

Answer 1

Hint: In this question we will first check whether the assertion and reason are correct or not. Then we will find out whether the reason is the correct explanation of the assertion or not.

Complete step by step answer:
The assertion says that ionic bonds are directional in nature whereas covalent bonds are non-directional.
Ionic bonds are strong electrostatic attraction forces formed between positive and negative ions. This bond is non-directional, which means that the pull of the electrons does not favor one atom over another.
In essence, the primary chemical bond (a sigma bond) is made when two atoms share electrons in between them from their electron. They will only share these electrons by approaching one another, and that they can only approach one another in a line because there are only two atoms.
So the assertion is wrong,
Now we will check the reason.
The reason is that according to the orbital overlap concept, the formation of a covalent bond between two atoms results by pairing of electrons present in the valence shell having same spins.
According to the orbital overlap concept, the greater the overlap, stronger is that the bond formed between the two atoms. Thus, consistent with the orbital overlap concept, atoms combine by overlapping their orbital and thus forming a lower energy level where their valence electrons with opposite spin, pair up to make covalent bonds.
So the reason is wrong.

So, the correct answer is Option D.

Note: The strength of chemical bonds varies considerably; there are "strong bonds" or "primary bonds" such as covalent, ionic and metallic bonds, and "weak bonds" or "secondary bonds" such as dipole–dipole interactions, the London dispersion force and hydrogen bonding.