To determine the nature of the Se-Cl bond in selenium chloride (SeClâ‚‚), we can look at the difference in electronegativity between selenium and chlorine.
The electronegativity of selenium (Se) is 2.55, and the electronegativity of chlorine (Cl) is 3.16.
First, we calculate the difference in electronegativity:
\[ \text{Difference} = |\text{Electronegativity of Cl} - \text{Electronegativity of Se}| = |3.16 - 2.55| = 0.61 \]
Now we can classify the bond type based on the electronegativity difference:
- Nonpolar covalent: Difference of 0.0 to 0.4
- Polar covalent: Difference of 0.4 to 1.7 (further divided into moderately and highly polar categories)
- Ionic: Difference greater than 1.7
Since the difference in electronegativity (0.61) falls within the range of 0.4 to 1.7, we categorize the bond as polar covalent.
Considering the options provided:
- A. nonpolar covalent
- B. moderately polar covalent
- C. highly polar covalent
- D. ionic
- E. polar ionic
The closest classification for a difference of 0.61 is B. moderately polar covalent.
So, the answer is B. moderately polar covalent.