Question

Which of the following statements is false about covalent bonds?

• A. The electrons are shared between atoms to get stable electronic arrangement.
• B. The bonds are non-directional.
• C. The strength of the bond depends upon the extent of overlapping.
• D. The bond may or may not be polar.

Answer 1

Answer: (B)

Covalent bond is formed by the sharing of electrons or combining the atomic orbitals to form the hybrid orbitals. Hybrid orbitals have the more probability of electron density at one end of the orbital while others end the probability of finding the electron is negligible. Due to this, all covalent bonds are directional in nature.

The strength of the bond depends on the extent of overlapping. More overlapping then stronger will be the bond.

If the electrons are sharing between the two same kinds of atoms then it will form a non-polar molecule. Eg:- $H_{2,}{N}_{2,}and{F}_{2}etc.$

If the sharing of electrons between the two different kinds of elements then the more electronegative element attracts shared pair of electrons towards itself and gets the partial negative charge corresponding the less electronegative atom carries the partial positive charge. Due to this, there is one dipole generated and these molecules known as polar molecules by consisting polar covalent bonds. Eg:- $HCl$