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?

The given molecule \(\mathrm{F}_{2}(g)\) consists of two fluorine (F) atoms joined together. In this case, since both atoms are of the same element (fluorine), the type of bonding between the atoms would be covalent, as they share a pair of electrons to achieve a full octet and reach stability. Covalent bonds occur typically between non-metallic elements, which is the case with fluorine.

Now, for the other molecule, \(\mathrm{HF}(g)\), it consists of a hydrogen (H) and a fluorine (F) atom combined. To identify the nature of bonding, we have to consider the electronegativity difference between the two elements involved. Fluorine is highly electronegative, while hydrogen is of comparatively lower electronegativity. Due to this electronegativity difference, fluorine attracts the shared pair of electrons more towards itself, creating a polar covalent bond in the \(\mathrm{HF}\) molecule.

Comparing the type of bonding found in the \(\mathrm{F}_{2}(g)\) and \(\mathrm{HF}(g)\) molecules, we can conclude the following: 1. Similarity: - Both \(\mathrm{F}_{2}\) and \(\mathrm{HF}\) exhibit covalent bonding as they share a pair of electrons to achieve a stable state (an octet in the case of fluorine and the H-atom reaches a stable duet in the case of hydrogen). 2. Differences: - The bonding in \(\mathrm{F}_{2}\) is non-polar covalent bonding, as both fluorine atoms have the same electronegativity, resulting in equal sharing of the electron pair. - In \(\mathrm{HF}\), the bonding is polar covalent, as fluorine attracts the shared electron pair more towards itself, due to its higher electronegativity compared to hydrogen. This creates a dipole moment in the molecule, resulting in the polar nature of the bond. In conclusion, both \(\mathrm{F}_{2}(g)\) and [\(\mathrm{HF}(g)\) exhibit covalent bonding, with \(\mathrm{F}_{2}(g)\) being non-polar and \(\mathrm{HF}(g)\) being polar, due to the differences in electronegativity between the elements involved in each molecule.