To determine which of the given molecules contains a nonpolar covalent bond, we need to consider the nature of the covalent bonds in each molecule by looking at the electronegativity differences between the atoms involved. A nonpolar covalent bond forms when the electrons are equally shared between the two atoms due to the electronegativity difference being very small or nonexistent.
Let's analyze each molecule:
A. Lil (Lithium Iodide)
- Lithium iodide is an ionic compound, not a covalent one. The bond between lithium (a metal) and iodine (a nonmetal) involves the transfer of electrons from lithium to iodine, forming an ionic bond.
B. [tex]\( HCl \)[/tex] (Hydrochloric Acid)
- Hydrogen and chlorine form a covalent bond. However, chlorine is significantly more electronegative than hydrogen, leading to an unequal sharing of electrons, making the bond polar covalent.
C. [tex]\( H_2 \)[/tex] (Hydrogen Gas)
- In hydrogen gas, the bond is between two hydrogen atoms. Since both atoms have the same electronegativity, the electrons are shared equally, resulting in a nonpolar covalent bond.
D. [tex]\( H_2O \)[/tex] (Water)
- In water, the bonds are between hydrogen and oxygen. Oxygen is much more electronegative than hydrogen, leading to a significant unequal sharing of electrons, making these bonds polar covalent.
Given this analysis, the molecule that contains a nonpolar covalent bond is:
C. [tex]\( H_2 \)[/tex] (Hydrogen Gas)
