Question

The electronic configuration of X and Y are given below:
X: 1s²2s²2p⁶3s²3p³
Y: 1s²2s²2p⁶3s²3p⁵
Which of the following is the correct molecular formula and type of bond formed between X and Y?

• A. X₂Y₃, coordinate bond
• B. X₃Y₃, covalent bond
• C. X₂Y₃, covalent bond
• D. X₃Y, ionic bond

Hint:

For covalent bonding, elements share electrons to complete their octet. The number of bonds formed depends on the number of valence electrons each element needs to reach a stable configuration.

Answer 1

The Correct Option is B

X has the electronic configuration 1s²2s²2p⁶3s²3p³, which indicates that it is in Group 15 of the periodic table (with 5 valence electrons).
Y has the electronic configuration 1s²2s²2p⁶3s²3p⁵, which places it in Group 17 (with 7 valence electrons).

When X (a group 15 element) and Y (a group 17 element) combine, X will tend to lose 3 electrons, and Y will gain 1 electron to complete their octets.
This results in the formation of a molecule with the formula X₂Y₃.
The bond formed between X and Y is an ionic bond because X loses electrons to form a cation (X³⁺) and Y gains electrons to form an anion (Y^–), and these oppositely charged ions are held together by electrostatic forces.

Final Answer:
Molecular Formula: X₂Y₃
Bond Type: Ionic Bond