The electronic configurations of three elements,
A,B are C are given below. Answer the
questions 14 to 17 on the basis of these
configurations .
`{:(A " "1s^(2) " "2s^(2) " "2p^(6)),(B" "1s^(2) " "2s^(2) " "2p^(6) " " 3s^(2) " "3p^(3)),(C" "1s^(2) " "2s^(2) " "2p^(6) " " 3s^(2) " "3p^(5)):}`
The bond between B and C will be

Options

A. Ionic
B. Covalent
C. Hydrogen
D. Coordinate

Explanation

To determine the type of bond between elements B and C based on their electronic configurations, we can follow these steps:

### Step 1: Identify the Elements
- **Element A**: 1s² 2s² 2p⁶ (Total electrons = 10) → This is Neon (Ne).
- **Element B**: 1s² 2s² 2p⁶ 3s² 3p³ (Total electrons = 15) → This is Phosphorus (P).
- **Element C**: 1s² 2s² 2p⁶ 3s² 3p⁵ (Total electrons = 17) → This is Chlorine (Cl).

### Step 2: Determine the Nature of the Elements
- **Element B (Phosphorus)**: A non-metal with 5 valence electrons (3s² 3p³).
- **Element C (Chlorine)**: A non-metal with 7 valence electrons (3s² 3p⁵).

### Step 3: Analyze the Bonding
- Both B and C are non-metals. Non-metals tend to form covalent bonds with each other by sharing electrons.
- Phosphorus (B) can share its 5 valence electrons, while Chlorine (C) can share its 7 valence electrons to achieve a stable electronic configuration.

### Step 4: Conclusion
- The bond between B (Phosphorus) and C (Chlorine) will be a **covalent bond** because both elements are non-metals and they will share electrons to achieve stability.

### Final Answer
The bond between B and C will be a **covalent bond**.

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