A polar covalent bond is formed between nitrogen (N) and fluorine (F) due to the difference in their electronegativities.
In the covalent bonding between nitrogen (N) and fluorine (F), a polar covalent bond is established. Covalent bonds involve the sharing of electrons between atoms, and the nature of this sharing is determined by the electronegativity of the atoms involved. Electronegativity is a measure of an atom's tendency to attract shared electrons.
Nitrogen and fluorine have different electronegativities, with fluorine being more electronegative than nitrogen. As a result, fluorine attracts the shared electrons more strongly, creating a partial negative charge (δ-) on the fluorine atom and a partial positive charge (δ+) on the nitrogen atom. This uneven distribution of charge along the bond gives rise to a polar covalent bond.
In the N-F bond, the higher electronegativity of fluorine means it pulls the shared electrons closer to itself, creating a dipole moment. This results in a polarized molecule, where one end (near fluorine) is more negatively charged, and the other end (near nitrogen) is more positively charged. Thus, the nitrogen-fluorine bond is an example of a polar covalent bond due to the electronegativity difference between the two atoms.
Complete ques:
What type of bond is formed between nitrogen (N) and fluorine (F) in their covalent bonding?