Question

Describe the type of bonding that exists in the \(\mathrm{F}_{2}(g)\) molecule. How does this type of bonding differ from that found in the \(\mathrm{HF}(g)\) molecule? How is it similar?

Short answer

In the F₂(g) molecule, a nonpolar covalent bond exists as two fluorine atoms share a pair of electrons equally due to their same electronegativity value. In contrast, the HF(g) molecule forms a polar covalent bond as electrons are not shared equally between the hydrogen and fluorine atoms due to the significant electronegativity difference. Both molecules possess covalent bonds but differ in the electron distribution, resulting in nonpolar and polar covalent bonds respectively.

Step-by-step solution

Identify bonding in F₂(g) molecule

In a F₂(g) molecule, there are two fluorine atoms sharing one pair of electrons that creates a bond between them. This type of bond is called a covalent bond. Since both fluorine atoms have the same electronegativity value (3.98), the electrons are shared equally between them. This results in a nonpolar covalent bond.

Identify bonding in HF(g) molecule

In an HF(g) molecule, there is one hydrogen atom and one fluorine atom. These two atoms share a pair of electrons, creating a bond between them. This bond is also a covalent bond. However, due to the high electronegativity difference between fluorine (3.98) and hydrogen (2.20), the electrons are not shared equally. Fluorine attracts the electrons more towards itself, resulting in a polar covalent bond.

Compare the bonding types

Now that we have identified the bonding types in F₂(g) and HF(g) molecules, let's compare them. 1. Similarity: Both F₂(g) and HF(g) molecules have covalent bonds, which involve the sharing of electron pairs between atoms. 2. Difference: The covalent bond in F₂(g) is a nonpolar covalent bond as the bonding electrons are shared equally between the two fluorine atoms. On the other hand, the covalent bond in HF(g) is a polar covalent bond due to the unequal sharing of electrons with fluorine attracting the bonding electrons more towards itself because of its higher electronegativity value compared to hydrogen.