The shape of `NH_2^(-)` is like that of

Options

A. `CS_(2)`
B. `SnCl_(2)`
C. `NO_(2)^(+)`
D. `BeCl_(2)`

Explanation

To determine the shape of the \( NH_2^{-} \) ion, we can follow these steps:

### Step 1: Identify the central atom and its valence electrons
The central atom in \( NH_2^{-} \) is nitrogen (N). Nitrogen is in group 15 of the periodic table and has 5 valence electrons.

### Step 2: Count the number of hydrogen atoms and the charge
The ion \( NH_2^{-} \) has 2 hydrogen atoms and carries a -1 charge. This means we have one additional electron to consider.

### Step 3: Calculate the total number of valence electrons
The total number of valence electrons can be calculated as follows:
- Valence electrons from nitrogen: 5
- Valence electrons from 2 hydrogen atoms: 2 (1 from each)
- Additional electron due to the -1 charge: 1

Total = \( 5 + 2 + 1 = 8 \) valence electrons.

### Step 4: Draw the Lewis structure
In the Lewis structure of \( NH_2^{-} \):
- Nitrogen is the central atom.
- It forms two single bonds with the two hydrogen atoms.
- The remaining 4 electrons (2 lone pairs) are placed on the nitrogen atom.

### Step 5: Determine the electron geometry
With 2 bonding pairs (from the N-H bonds) and 2 lone pairs on nitrogen, we can determine the electron geometry. The arrangement of 4 electron pairs (2 bonding and 2 lone pairs) around the nitrogen atom is tetrahedral.

### Step 6: Determine the molecular shape
For molecular shape, we only consider the atoms and ignore the lone pairs. The shape formed by the two hydrogen atoms and the nitrogen atom, considering the lone pairs, is bent or V-shaped.

### Conclusion
Thus, the shape of \( NH_2^{-} \) is V-shaped.