The halide which does not give a precipitate with `AgNO_(3)` is

Options

A. `F^(Theta)`
B. `CI^(Theta)`
C. `Br^(Theta)`
D. `I^(Theta)`

Explanation

To determine which halide does not give a precipitate with AgNO3, we can analyze the reactions of different halides with silver nitrate.

### Step-by-Step Solution:

1. **Understanding the Reaction**: When halides react with AgNO3 (silver nitrate), they typically form silver halides, which can precipitate out of solution. The general reaction can be represented as:
\[ \text{Halide} + \text{AgNO}_3 \rightarrow \text{AgHalide} + \text{NO}_3^- \]

2. **Analyzing Each Halide**:
- **Chlorine (Cl-)**: When chlorine reacts with AgNO3, it forms silver chloride (AgCl), which is a white precipitate.
\[ \text{Cl}^- + \text{AgNO}_3 \rightarrow \text{AgCl (s)} + \text{NO}_3^- \]
- **Bromine (Br-)**: When bromine reacts with AgNO3, it forms silver bromide (AgBr), which is a cream-colored precipitate.
\[ \text{Br}^- + \text{AgNO}_3 \rightarrow \text{AgBr (s)} + \text{NO}_3^- \]
- **Iodine (I-)**: When iodine reacts with AgNO3, it forms silver iodide (AgI), which is a yellow precipitate.
\[ \text{I}^- + \text{AgNO}_3 \rightarrow \text{AgI (s)} + \text{NO}_3^- \]
- **Fluorine (F-)**: When fluorine reacts with AgNO3, it forms silver fluoride (AgF), which is soluble in water and does not precipitate.
\[ \text{F}^- + \text{AgNO}_3 \rightarrow \text{AgF (aq)} + \text{NO}_3^- \]

3. **Conclusion**: From the analysis, we see that:
- Chlorine, bromine, and iodine all form precipitates with AgNO3.
- Fluoride does not form a precipitate with AgNO3 because it remains soluble in water.

Thus, the halide that does not give a precipitate with AgNO3 is **Fluoride (F-)**.

### Final Answer:
The halide which does not give a precipitate with AgNO3 is **Fluoride (F-)**.