Electronic configuration of an element A is `1s^2 2s^2 2p^6 3s^1` and electronic configuration of another element B is `1s^2 2s^2 2p^6 3s^2 3p^4`. The possible compound that can be formed between A and B is

Options

A. AB
B. `AB_2`
C. `A_2B`
D. `A_2B_2`

Answer

To determine the possible compound that can be formed between elements A and B based on their electronic configurations, we can follow these steps:

### Step 1: Identify the electronic configurations
- Element A has the electronic configuration: `1s² 2s² 2p⁶ 3s¹`
- Element B has the electronic configuration: `1s² 2s² 2p⁶ 3s² 3p⁴`

### Step 2: Determine the valence electrons
- For element A, the valence shell is the third shell (n=3), which contains 1 electron (3s¹).
- For element B, the valence shell is also the third shell (n=3), which contains 6 electrons (3s² 3p⁴).

### Step 3: Analyze the stability of elements
- Element A can achieve stability by losing its 1 valence electron, forming a cation A⁺:
- A → A⁺ + e⁻
- The electronic configuration of A⁺ becomes: `1s² 2s² 2p⁶` (which has 8 electrons in the second shell, achieving stability).

- Element B can achieve stability by gaining 2 electrons to complete its octet, forming an anion B²⁻:
- B + 2e⁻ → B²⁻
- The electronic configuration of B²⁻ becomes: `1s² 2s² 2p⁶ 3s² 3p⁶` (which also has 8 electrons in the third shell, achieving stability).

### Step 4: Determine the type of bond formed
- The bond formed between A⁺ and B²⁻ is an ionic bond because A loses an electron and B gains electrons.

### Step 5: Write the formula of the compound
- The charges of the ions are A⁺ (1+) and B²⁻ (2-).
- To balance the charges, we can use the formula:
- The formula for the compound formed will be A₂B, as two A⁺ ions will balance one B²⁻ ion.

### Final Answer
The possible compound that can be formed between A and B is **A₂B**.

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