is the given pair is isoelectronic and isostructural ?
`NO_3^(-) and CO_3^(2-)`

Explanation

To determine whether the given pair \( NO_3^- \) (nitrate ion) and \( CO_3^{2-} \) (carbonate ion) are isoelectronic and isostructural, we will follow a systematic approach.

### Step 1: Determine the total number of electrons for each ion.

**For \( NO_3^- \):**
- Nitrogen (N) has 7 electrons.
- Each Oxygen (O) has 6 electrons, and there are 3 Oxygens.
- Therefore, the total number of electrons from Oxygen is \( 3 \times 6 = 18 \).
- The negative charge (-1) indicates one additional electron.

Calculating total electrons:
\[ \text{Total electrons in } NO_3^- = 7 + 18 + 1 = 26 \]

**For \( CO_3^{2-} \):**
- Carbon (C) has 6 electrons.
- Each Oxygen (O) has 6 electrons, and there are 3 Oxygens.
- Therefore, the total number of electrons from Oxygen is \( 3 \times 6 = 18 \).
- The negative charge (-2) indicates two additional electrons.

Calculating total electrons:
\[ \text{Total electrons in } CO_3^{2-} = 6 + 18 + 2 = 26 \]

### Step 2: Compare the total number of electrons.

Both ions have a total of 26 electrons:
\[ NO_3^-: 26 \text{ electrons} \quad \text{and} \quad CO_3^{2-}: 26 \text{ electrons} \]
Thus, \( NO_3^- \) and \( CO_3^{2-} \) are isoelectronic.

### Step 3: Determine the hybridization of each ion.

**For \( NO_3^- \):**
- The central atom is Nitrogen (N).
- The structure of \( NO_3^- \) can be represented with one double bond and two single bonds (resonance structures).
- The hybridization of Nitrogen in \( NO_3^- \) is \( sp^2 \).

**For \( CO_3^{2-} \):**
- The central atom is Carbon (C).
- The structure of \( CO_3^{2-} \) can also be represented with one double bond and two single bonds (resonance structures).
- The hybridization of Carbon in \( CO_3^{2-} \) is also \( sp^2 \).

### Step 4: Compare the hybridization.

Both ions have a hybridization of \( sp^2 \):
\[ NO_3^-: sp^2 \quad \text{and} \quad CO_3^{2-}: sp^2 \]
Thus, \( NO_3^- \) and \( CO_3^{2-} \) are isostructural.

### Conclusion

Since both ions are isoelectronic (same number of electrons) and isostructural (same hybridization), we conclude that:
\[ \text{The pair } NO_3^- \text{ and } CO_3^{2-} \text{ are both isoelectronic and isostructural.} \]

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