If carbon which has an electrongavity of 2.5 bonds with hydrogen, which has an electrongavity of 2.1, the bond between the two atoms will be classified as a(n) covalent bond

If carbon which has an electrongavity of 2.5 bonds with hydrogen, which has an electrongavity of 2.1, the bond between the two atoms will be classified as a(n) covalent bond → Totally TRUE

Explanation:

We must follow the Pauling's rules to solve these question.

The electonegativity of an element is defined as the ability it has to attract electrons that link it to another element. It is a periodic property, which allows predicting the polarity of the bond formed between two atoms, as well as its covalent or ionic character.

The Pauling scale values range from 0.7 for Francium (the least electronegative element) to 4 for Fluorine, the most electronegative. Using the electronegativities table we can predict the polarity of some compounds

ΔEn (C-H) = 2.5 - 2.1 = 0.4 → This is a covalent bond.

ΔEn ≤ 0.4 → Covalent non polar bond

0.5 < ΔEn < 1.7 → Covalent polar bond

ΔEn ≥ 1.7 → Ionic bond