The average charge on each O atom and average bond order of S-O bond in `SO_4^(2-)` is :

Options

A. -11.67
B. `-1//2` & 1.5
C. `-1//2` & 1.67
D. `-1//2` & 1.33

Explanation

To find the average charge on each oxygen atom and the average bond order of the S-O bond in the sulfate ion \(\text{SO}_4^{2-}\), we can follow these steps:

### Step 1: Determine the total charge on the sulfate ion
The sulfate ion \(\text{SO}_4^{2-}\) has a total charge of \(-2\).

### Step 2: Calculate the average charge on each oxygen atom
The sulfate ion contains 4 oxygen atoms. To find the average charge on each oxygen atom, we divide the total charge by the number of oxygen atoms:

\[ \text{Average charge on each O atom} = \frac{\text{Total charge}}{\text{Number of O atoms}} = \frac{-2}{4} = -0.5 \]

### Step 3: Draw the Lewis structure of \(\text{SO}_4^{2-}\)
In the Lewis structure of \(\text{SO}_4^{2-}\), sulfur is the central atom bonded to four oxygen atoms. The structure can be represented with resonance forms where some of the S-O bonds are double bonds and some are single bonds.

### Step 4: Identify the bond types
In the resonance structures, we can have:
- Two S-O double bonds
- Two S-O single bonds

### Step 5: Calculate the average bond order of the S-O bond
The average bond order can be calculated using the formula:

\[ \text{Average bond order} = \frac{\text{Total number of bonds}}{\text{Number of resonance structures}} \]

In the case of \(\text{SO}_4^{2-}\), the total number of bonds (considering all resonance structures) is 6 (2 double bonds and 2 single bonds). The number of resonance structures is 4.

Thus, the average bond order is:

\[ \text{Average bond order} = \frac{6}{4} = 1.5 \]

### Final Answer
- Average charge on each oxygen atom: \(-0.5\)
- Average bond order of S-O bond: \(1.5\)