Ammonia molecule is formed by the following hybrid orbitals:

Options

A. `dsp^2`
B. `sp^3`
C. `sp^3 d`
D. `d^2 sp`

Explanation

To determine the hybrid orbitals involved in the formation of an ammonia (NH₃) molecule, we can follow these steps:

### Step 1: Identify the central atom and its electronic configuration
- The central atom in ammonia is nitrogen (N).
- The electronic configuration of nitrogen is 1s² 2s² 2p³.

### Step 2: Determine the number of valence electrons
- Nitrogen has 5 valence electrons (2 from 2s and 3 from 2p).

### Step 3: Understand the bonding in ammonia
- Ammonia has three hydrogen atoms bonded to nitrogen.
- Each hydrogen atom contributes one electron, resulting in a total of 3 electrons from hydrogen.

### Step 4: Calculate the total number of electrons around nitrogen
- The total number of electrons around nitrogen in ammonia is 5 (from nitrogen) + 3 (from three hydrogen atoms) = 8 electrons.

### Step 5: Determine the hybridization
- To accommodate these 8 electrons, nitrogen undergoes hybridization.
- The 2s and three 2p orbitals of nitrogen combine to form four equivalent hybrid orbitals.
- This process is known as sp³ hybridization.

### Step 6: Identify the arrangement of the hybrid orbitals
- Out of the four sp³ hybrid orbitals formed, one contains a lone pair of electrons, and the other three contain unpaired electrons that form bonds with hydrogen atoms.

### Step 7: Describe the molecular geometry
- The presence of the lone pair affects the geometry of the molecule.
- The molecular shape of ammonia is trigonal pyramidal due to the lone pair, and the bond angle is approximately 107 degrees.

### Conclusion
- The ammonia molecule is formed by sp³ hybrid orbitals.

### Final Answer
- The hybrid orbitals involved in the formation of the ammonia molecule are **sp³**.

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