Question

Are the bonds in each of the following substances ionic, nonpolar covalent, or polar covalent? (a)KCl (b)P4 (c)BF3 (d)SO2 (e)Br2 (f)NO2 For those substances with polar covalent bonds, which has the least polar bond? For those substances with polar covalent bonds, which has the most polar bond?

Answer 1

Answer:

(a) Ionic

(b) Nonpolar covalent

(c) Polar covalent

(d) Polar covalent

(e) Nonpolar covalent

(f) Polar covalent

For those substances with polar covalent bonds, which has the least polar bond? NO₂

For those substances with polar covalent bonds, which has the most polar bond? BF₃

Explanation:

Are the bonds in each of the following substances ionic, nonpolar covalent, or polar covalent?

The nature of a bond depends on the modulus of the difference of electronegativity (|ΔEN|) between the atoms that form it.

• If |ΔEN| = 0, the bond is nonpolar covalent.
• If 0 < |ΔEN| ≤ 2, the bond is polar covalent.
• If |ΔEN| > 2, the bond is ionic.

(a) KCl    |ΔEN| = |EN(K) - EN(Cl)| = |0.8 - 3.0| = 2.2. The bond is ionic.

(b) P₄      |ΔEN| = |EN(P) - EN(P)| = |2.1 - 2.1| = 0.0. The bond is nonpolar covalent.

(c) BF₃    |ΔEN| = |EN(B) - EN(F)| = |2.0 - 4.0| = 2.0. The bond is polar covalent.

(d) SO₂   |ΔEN| = |EN(S) - EN(O)| = |2.5 - 3.5| = 1.0. The bond is polar covalent.

(e) Br₂    |ΔEN| = |EN(Br) - EN(Br)| = |2.8 - 2.8| = 0.0. The bond is nonpolar covalent.

(f) NO₂   |ΔEN| = |EN(N) - EN(O)| = |3.0 - 3.5| = 0.5. The bond is polar covalent.