The structure and hybridization of `NO_(2) ^(+)` is

Options

A. Linear, sp
B. Trigonal, `sp^(2)`
C. Octahedral, `sp^(3)d`
D. Tetrahedral,`sp^(3)`

Answer

To determine the structure and hybridization of the nitronium ion, \( NO_2^+ \), we can follow these steps:

### Step 1: Identify the central atom and its valence electrons
The central atom in \( NO_2^+ \) is nitrogen (N). Nitrogen is in group 15 of the periodic table and has 5 valence electrons.

### Step 2: Determine the total number of electrons in the ion
Since \( NO_2^+ \) has a positive charge, we need to subtract one electron from the total count. The total number of valence electrons is calculated as follows:
- Nitrogen: 5 electrons
- Oxygen: 6 electrons (2 oxygen atoms contribute 12 electrons)
- Total: \( 5 + 12 - 1 = 16 \) electrons

### Step 3: Draw the Lewis structure
In the Lewis structure of \( NO_2^+ \):
- Nitrogen is the central atom.
- Each oxygen atom is bonded to nitrogen.
- To satisfy the octet rule, nitrogen will form one double bond with one oxygen and a single bond with the other oxygen. This results in one oxygen having a formal charge of 0 and the other oxygen having a formal charge of -1.

### Step 4: Calculate the steric number
The steric number is calculated as the number of sigma bonds plus the number of lone pairs on the central atom (nitrogen):
- Nitrogen forms 2 sigma bonds (one with each oxygen).
- There are no lone pairs on nitrogen.
- Therefore, the steric number = \( 2 + 0 = 2 \).

### Step 5: Determine hybridization
Based on the steric number:
- A steric number of 2 corresponds to an \( sp \) hybridization.

### Step 6: Determine the geometry and shape
With \( sp \) hybridization, the geometry of the molecule is linear. The bond angles are approximately 180 degrees.

### Final Answer
The structure of \( NO_2^+ \) is linear, and the hybridization of the nitrogen atom is \( sp \).

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