Question:
Match List I with List II
LIST I LIST II A XeF4
I See-saw B SF4
II Square planar C NH4+
III Bent T-shaped D BrF3 IV Tetrahedral
Choose the correct answer from the options given below :
Match List I with List II
| LIST I | LIST II | ||
| A | XeF4 | I | See-saw |
| B | SF4 | II | Square planar |
| C | NH4+ | III | Bent T-shaped |
| D | BrF3 | IV | Tetrahedral |
Choose the correct answer from the options given below :
Show Hint
Molecular shapes are determined by the VSEPR theory, which helps predict the geometry based on electron pairs and bond angles.
Updated On: Mar 31, 2026
- A-IV, B-I, C-II, D-III
- A-II, B-I, C-III, D-IV
- A-II, B-I, C-IV, D-III
- A-IV, B-III, C-II, D-I
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The Correct Option is C
Approach Solution - 1
Correct answer is (C): A-II, B-I, C-IV, D-III
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Approach Solution -2
- A. \( \text{XeF}_4 \) has a square planar structure.
- B. \( \text{SF}_4 \) has a see-saw shape.
- C. \( \text{NH}_4^+ \) has a tetrahedral geometry.
- D. \( \text{BrF}_3 \) has a bent T-shaped structure.
A-I, B-I, C-IV, D-III.
In this matching, the structures of various molecules are being analyzed based on the number of bonding pairs and lone pairs. The tetrahedral geometry of \( \text{NH}_4^+ \) is typical for molecules with four bonding pairs and no lone pairs. \( \text{BrF}_3 \), with its lone pairs, adopts a bent T-shaped structure, while \( \text{XeF}_4 \) adopts a square planar structure due to the presence of two lone pairs and four bonding pairs.
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Concepts Used:
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