Question

Identify the correct statements from the following
\[ \text{(I) } SnCl_2 \text{ is ionic, but } SnCl_4 \text{ is covalent in nature} \] \[ \text{(II) All linear diatomic molecules have zero dipole moment} \] \[ \text{(III) Both } NO \text{ and } O_2 \text{ are paramagnetic} \]

• A. (I) and (II) only
• B. (I) and (III) only
• C. (II) and (III) only
• D. (I), (II) and (III)

Hint:

Paramagnetic species contain unpaired electrons. Also, linear shape alone does not guarantee zero dipole moment; the molecule must be symmetrical or homonuclear.

Answer 1

The Correct Option is B

Step 1: Test each statement against chemical principles.
(I) Sn²⁺ has lower charge density, SnCl₂ is ionic; Sn⁴⁺ polarises Cl⁻ strongly, SnCl₄ is covalent → true. (II) Heteronuclear diatomics (HCl, CO) have bond polarity → false. (III) O₂ has 2 unpaired e⁻ (paramagnetic), NO has odd e⁻ count → paramagnetic → true.

Step 2: Final Answer:
(I) and (III) only (option 2).