The total number of covalent bonds present in the `NO_(2)^(+)` ion is :

Options

A. three
B. two
C. four
D. six

Explanation

To determine the total number of covalent bonds present in the \( NO_2^+ \) ion, we can follow these steps:

### Step 1: Draw the Lewis Structure of \( NO_2 \)
- Nitrogen (N) is the central atom, and it is bonded to two oxygen (O) atoms.
- Each oxygen atom will typically form two bonds with nitrogen.

### Step 2: Account for the Charge
- Since we are dealing with \( NO_2^+ \), we need to account for the positive charge. This means we have one less electron than we would in a neutral molecule.
- The positive charge suggests that one of the electrons in the nitrogen-oxygen bonds is removed.

### Step 3: Determine the Bonding
- In the Lewis structure of \( NO_2 \), nitrogen forms a double bond with one oxygen and a single bond with the other oxygen.
- The double bond consists of one sigma bond and one pi bond.
- The single bond consists of one sigma bond.

### Step 4: Count the Covalent Bonds
- From the double bond with one oxygen, we have:
- 1 sigma bond + 1 pi bond = 2 covalent bonds
- From the single bond with the other oxygen, we have:
- 1 sigma bond = 1 covalent bond
- Therefore, the total number of covalent bonds in \( NO_2^+ \) is:
- \( 2 (from \, double \, bond) + 1 (from \, single \, bond) = 3 \, covalent \, bonds \)

### Conclusion
- The total number of covalent bonds present in the \( NO_2^+ \) ion is **3**.

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