Match the geometry of following from List - I with List - II: List - I – List - II (A) $NH_{3}$ – (i) See-saw (B) $CIF_{3}$ – (ii) Trigonal pyramidal (C) $SO_{2}$ – (iii) T- shape (D) $SF_{4}$ – (iv) Bent (V-Shaped)

Q: Match the geometry of following from List - I with List - II : List - I – List - II (A) $NH_{3}$ – (i) See-saw (B) $CIF_{3}$ – (ii) Trigonal pyramidal (C) $SO_{2}$ – (iii) T- shape (D) $SF_{4}$ – (iv) Bent (V-Shaped)

Match the geometry of following from List - I with List - II : List - I – List - II (A) $NH_{3}$ – (i) See-saw (B) $CIF_{3}$ – (ii) Trigonal pyramidal (C) $SO_{2}$ – (iii) T- shape (D) $SF_{4}$ – (iv) Bent (V-Shaped)

Question

Accepted Answer

To justify why Option 4 is the correct answer, let's analyze the molecular geometry of each compound listed in List - I and match it with the appropriate geometry from List - II.

**(A) $NH_{3}$ – Trigonal pyramidal (ii):**

- Ammonia ($NH_{3}$) has a central nitrogen atom bonded to three hydrogen atoms with one lone pair of electrons. The presence of the lone pair results in a trigonal pyramidal shape due to the repulsion between the lone pair and the bonding pairs, which pushes the hydrogen atoms downwards. This matches with (ii) Trigonal pyramidal.

**(B) $CIF_{3}$ – T-shape (iii):**

- Chlorine trifluoride ($CIF_{3}$) has a central chlorine atom bonded to three fluorine atoms and has two lone pairs of electrons. The lone pairs occupy equatorial positions in a trigonal bipyramidal arrangement, leading to a T-shaped molecular geometry. This matches with (iii) T-shape.

**(C) $SO_{2}$ – Bent (V-Shaped) (iv):**

- Sulfur dioxide ($SO_{2}$) has a central sulfur atom double-bonded to two oxygen atoms and has one lone pair of electrons. The lone pair causes a repulsion that results in a bent or V-shaped geometry. This matches with (iv) Bent (V-Shaped).

**(D) $SF_{4}$ – See-saw (i):**

- Sulfur tetrafluoride ($SF_{4}$) has a central sulfur atom bonded to four fluorine atoms with one lone pair of electrons. The lone pair occupies an equatorial position in a trigonal bipyramidal arrangement, resulting in a see-saw shape. This matches with (i) See-saw.

Now, let's explain why the other options are incorrect:

**Option 1: (A)-(i), (B)-(ii), (C)-(iii), (D)-(iv)**

- This option incorrectly matches $NH_{3}$ with See-saw (i), $CIF_{3}$ with Trigonal pyramidal (ii), $SO_{2}$ with T-shape (iii), and $SF_{4}$ with Bent (V-Shaped) (iv). None of these match the actual geometries of the molecules.

**Option 2: (A)-(iv), (B)-(iii), (C)-(ii), (D)-(i)**

- This option incorrectly matches $NH_{3}$ with Bent (V-Shaped) (iv), $CIF_{3}$ with T-shape (iii) (which is correct), $SO_{2}$ with Trigonal pyramidal (ii), and $SF_{4}$ with See-saw (i) (which is correct). Only two matches are correct, making this option incorrect.

**Option 3: (A)-(iii), (B)-(i), (C)-(iv), (D)-(ii)**

- This option incorrectly matches $NH_{3}$ with T-shape (iii), $CIF_{3}$ with See-saw (i), $SO_{2}$ with Bent (V-Shaped) (iv) (which is correct), and $SF_{4}$ with Trigonal pyramidal (ii). Only one match is correct, making this option incorrect.

Therefore, Option 4 is the only option that correctly matches each compound with its respective geometry, making it the correct answer.