Element A of group VA combines with element B of group VI A. The resulting compound may have the formula?

Options

A. `A_2 B_3 `
B. `A_3 B_2 `
C. `A_5 B_6 `
D. `A_6 B_5 `

Answer

To determine the formula of the compound formed by element A from group VA (15) and element B from group VIA (16), we can follow these steps:

### Step 1: Identify the Groups and Their Charges
- **Element A (Group VA)**: This group corresponds to group 15 in the periodic table. The general electronic configuration is \(ns^2 np^3\). Elements in this group typically can lose 3 electrons to form a cation with a charge of +3 (A³⁺) or gain 5 electrons to achieve a stable octet, but gaining 5 is less common.
- **Element B (Group VIA)**: This group corresponds to group 16 in the periodic table. The general electronic configuration is \(ns^2 np^4\). Elements in this group typically gain 2 electrons to form an anion with a charge of -2 (B²⁻) or can lose 6 electrons, but losing 6 is not feasible.

### Step 2: Determine the Most Likely Ionic Charges
- For element A, the most likely ionic form is A³⁺ (losing 3 electrons).
- For element B, the most likely ionic form is B²⁻ (gaining 2 electrons).

### Step 3: Balance the Charges
To form a neutral compound, the total positive charge must equal the total negative charge.
- The charge from 2 A³⁺ ions is \(2 \times (+3) = +6\).
- The charge from 3 B²⁻ ions is \(3 \times (-2) = -6\).

This means we can combine 2 A³⁺ ions with 3 B²⁻ ions to achieve a neutral compound.

### Step 4: Write the Formula
From the above, we can deduce that the formula of the compound formed will be:
- \(A_2B_3\)

### Final Answer
The resulting compound may have the formula **A₂B₃**.

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