Question:
Group – 2 element (A) when reacts with group – 15 element (X), the general formula of the compound formed is:
Group – 2 element (A) when reacts with group – 15 element (X), the general formula of the compound formed is:
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For ionic compounds, always balance total positive and negative charges using the criss-cross method to obtain the correct formula.
Updated On: Jun 19, 2026
- \(A_3X_2\)
- \(A_3X\)
- \(A_2X_3\)
- \(AX_2\)
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The Correct Option is A
Solution and Explanation
Step 1: Understanding the nature of elements involved.
Group – 2 elements are alkaline earth metals and they generally form cations with a charge of \(+2\). Group – 15 elements are generally non-metals and they tend to gain electrons to form anions with a charge of \(-3\). Therefore, element \(A\) will form \(A^{2+}\) and element \(X\) will form \(X^{3-}\).
Step 2: Identifying the valencies of both elements.
The valency of \(A\) is 2 because it loses two electrons to achieve stable configuration. The valency of \(X\) is 3 because it gains three electrons to complete its octet. Thus, we need to balance charges \(+2\) and \(-3\).
Step 3: Applying the criss-cross method.
To form a stable neutral compound, we interchange the valencies of the two ions. The valency of \(A\) becomes the subscript of \(X\), and the valency of \(X\) becomes the subscript of \(A\). This gives the formula \(A_3X_2\).
Step 4: Verification of charge neutrality.
Checking the total charge balance: \(3 \times (+2) = +6\) from \(A\) and \(2 \times (-3) = -6\) from \(X\). Since total positive and negative charges cancel each other, the compound is electrically neutral.
Step 5: Final formula determination.
Since the ratio \(A:X = 3:2\) satisfies charge neutrality, the empirical formula of the compound formed is \(A_3X_2\). This is the most stable combination based on ionic bonding principles.
Final Answer: \[ \boxed{A_3X_2} \]
Group – 2 elements are alkaline earth metals and they generally form cations with a charge of \(+2\). Group – 15 elements are generally non-metals and they tend to gain electrons to form anions with a charge of \(-3\). Therefore, element \(A\) will form \(A^{2+}\) and element \(X\) will form \(X^{3-}\).
Step 2: Identifying the valencies of both elements.
The valency of \(A\) is 2 because it loses two electrons to achieve stable configuration. The valency of \(X\) is 3 because it gains three electrons to complete its octet. Thus, we need to balance charges \(+2\) and \(-3\).
Step 3: Applying the criss-cross method.
To form a stable neutral compound, we interchange the valencies of the two ions. The valency of \(A\) becomes the subscript of \(X\), and the valency of \(X\) becomes the subscript of \(A\). This gives the formula \(A_3X_2\).
Step 4: Verification of charge neutrality.
Checking the total charge balance: \(3 \times (+2) = +6\) from \(A\) and \(2 \times (-3) = -6\) from \(X\). Since total positive and negative charges cancel each other, the compound is electrically neutral.
Step 5: Final formula determination.
Since the ratio \(A:X = 3:2\) satisfies charge neutrality, the empirical formula of the compound formed is \(A_3X_2\). This is the most stable combination based on ionic bonding principles.
Final Answer: \[ \boxed{A_3X_2} \]
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