Final answer:
The bond in H2S is a polar covalent bond with a difference in electronegativity of 0.4, resulting in a bent molecular geometry and a net dipole moment due to electrons being more strongly attracted to the more electronegative sulfur atom.
Step-by-step explanation:
The difference in electronegativity between hydrogen and sulfur is 0.4, indicating a bond in the molecule H2S. Based on the electronegativity values and the difference, the bond is not nonpolar but is rather a polar covalent bond. In a polar covalent bond, the sharing of electrons is unequal, leading to a dipole moment in the molecule due to the electrons being drawn more towards the more electronegative atom. In the case of H2S, sulfur is the more electronegative atom compared to hydrogen, so the electrons are more strongly attracted to sulfur, resulting in a molecular geometry that is bent. This bent geometry ensures that the bond dipoles do not cancel each other, hence H2S has a net dipole moment.