To determine the type of bond present in hydrogen sulfide (H₂S), we'll first need to consider the electronegativities of the involved atoms: hydrogen and sulfur. The electronegativity of hydrogen is 2.20, and the electronegativity of sulfur is 2.58.
Next, we calculate the difference in electronegativity between sulfur and hydrogen:
[tex]\[ \Delta \text{electronegativity} = |2.58 - 2.20| = 0.38 \][/tex]
Using the rules of thumb for bond types based on electronegativity difference:
- If the difference is less than 0.5, the bond is nonpolar covalent.
- If the difference is between 0.5 and 1.7, the bond is polar covalent.
- If the difference is greater than 1.7, the bond is ionic.
With the electronegativity difference calculated as 0.38, this falls into the category of less than 0.5. Therefore, the bond is classified as nonpolar covalent.
So, the correct answer is:
C. nonpolar covalent
