The hydride with more basic nature is

Options

A. `PH_(3)`
B. `NH_(3)`
C. `BiH_(3)`
D. `AsH_(3)`

Answer

To determine which hydride has the most basic nature among PH3, NH3, BiH3, and AsH3, we can analyze the basicity of these compounds based on the properties of their central atoms and the trends in the periodic table.

### Step 1: Identify the central atoms and their group
The hydrides in question are:
- NH3 (Ammonia) - central atom is Nitrogen (N)
- PH3 (Phosphine) - central atom is Phosphorus (P)
- AsH3 (Arsine) - central atom is Arsenic (As)
- BiH3 (Bismuthine) - central atom is Bismuth (Bi)

All these elements belong to Group 15 (VA group) of the periodic table.

### Step 2: Understand the basicity trend in hydrides
Basicity in hydrides is largely influenced by the availability of the lone pair of electrons on the central atom. As we move down the group from Nitrogen to Bismuth, the size of the central atom increases, leading to the following trends:
- The lone pair of electrons becomes more diffused.
- The nucleophilicity (ability to donate the lone pair) decreases as the size of the atom increases.

### Step 3: Compare the basicity of the hydrides
Based on the above understanding, we can rank the basicity of these hydrides:
- NH3 (most basic) > PH3 > AsH3 > BiH3 (least basic)

### Step 4: Conclusion
Thus, among the given hydrides, NH3 (Ammonia) is the most basic hydride.

### Final Answer
The hydride with more basic nature is **NH3** (Ammonia).

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