Question

Which option correctly describes the influence of electronegativity difference (ΔEN) on bond character? Select all that apply.

A. A bond with ΔEN greater than 1.7 is considered to be mostly ionic.
B. A bond with ΔEN greater than 1.7 is considered to be mostly covalent.
C. Any bond with ΔEN greater than 0.0 is considered to be polar.
D. A bond with ΔEN of 0.4 or less is considered mostly covalent

Answer 1

The influence of electronegativity difference (ΔEN) on bond character can be classified into ionic, polar covalent, and covalent bonds based on the electronegativity difference between atoms.

Step-by-step explanation:

The influence of electronegativity difference (ΔEN) on bond character can be described as follows:

1. A bond with ΔEN greater than 1.7 is considered to be mostly ionic. This means that the electronegativity difference between the two atoms is significantly high and the electrons are transferred from one atom to another, forming charged ions. Example: Na-Cl bond.
2. A bond with ΔEN greater than 0.4 is considered to be mostly polar covalent, where there is an unequal sharing of electrons between the atoms. Example: H-Cl bond.
3. A bond with ΔEN of 0.4 or less is considered mostly covalent. This means that the electrons are shared equally between the atoms, resulting in a nonpolar bond. Example: H-H bond.