The conjugate base of `NH_(2)^(-)` is

Options

A. `NH_(3)`
B. `NH_(2)OH`
C. `NH_(4)^(+)`
D. `N_(2)H_(4)`

Explanation

To find the conjugate base of \( NH_2^- \), we can follow these steps:

### Step 1: Understand the concept of conjugate acids and bases
According to the Brønsted-Lowry theory, an acid is a substance that can donate a proton (\( H^+ \)), and a base is a substance that can accept a proton. When an acid donates a proton, it forms its conjugate base, and when a base accepts a proton, it forms its conjugate acid.

### Step 2: Identify the species in question
In this case, we are given \( NH_2^- \), which is the amide ion.

### Step 3: Determine the conjugate base of \( NH_2^- \)
To find the conjugate base of \( NH_2^- \), we need to consider what happens when \( NH_2^- \) loses a proton (\( H^+ \)).

The reaction can be represented as:
\[ NH_2^- \rightarrow NH + H^- \]

Here, when \( NH_2^- \) loses a proton, it forms \( NH \) (the imide ion) and an electron (\( H^- \)).

### Step 4: Conclusion
Thus, the conjugate base of \( NH_2^- \) is \( NH \).

### Final Answer
The conjugate base of \( NH_2^- \) is \( NH \).

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