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The bond angle in H2S ( H-S-H) is:
- a)same as that of CI-Be-CI in BeCI2
- b)greater than H-N-H bond angle in NH3
- c)greater than H-Se-H and less than H-O-H
- d)same as CI-Sn-CI in SnCI2
Correct answer is option 'C'. Can you explain this answer?
Verified Answer
The bond angle in H2S ( H-S-H) is: a)same as that of CI-Be-CI in BeCI2...
Bond angle decreases on moving down the group.
Most Upvoted Answer
The bond angle in H2S ( H-S-H) is: a)same as that of CI-Be-CI in BeCI2...
The bond angle in a molecule is determined by the arrangement of atoms and the repulsion between electron pairs. In the case of H2S, which has a bent molecular geometry, the bond angle is influenced by the lone pairs of electrons on the sulfur atom.
1. Molecular geometries:
- H2S: The sulfur atom has two bonding electron pairs and two lone pairs, resulting in a bent or V-shaped molecular geometry.
- BeCl2: The beryllium atom has two bonding electron pairs and no lone pairs, resulting in a linear molecular geometry.
- NH3: The nitrogen atom has three bonding electron pairs and one lone pair, resulting in a trigonal pyramidal molecular geometry.
- H2O: The oxygen atom has two bonding electron pairs and two lone pairs, resulting in a bent or V-shaped molecular geometry.
- SnCl2: The tin atom has two bonding electron pairs and no lone pairs, resulting in a linear molecular geometry.
2. Electron pair repulsion:
- Lone pairs of electrons exert greater repulsion compared to bonding electron pairs.
- The repulsion between lone pairs and bonding pairs pushes the bonding pairs closer together, resulting in a decrease in the bond angle.
Explanation:
- The bond angle in H2S is greater than the H-Se-H bond angle in H2Se and less than the H-O-H bond angle in H2O.
- This is because the electronegativity of oxygen is greater than that of sulfur, resulting in a stronger pull on the bonding electron pairs in H2O.
- The stronger electron-electron repulsion between the lone pairs and bonding pairs in H2O leads to a smaller bond angle compared to H2S.
- Similarly, the bond angle in H2S is greater than the bond angle in NH3 because the repulsion between the lone pairs and bonding pairs in NH3 is greater than that in H2S due to the higher electronegativity of nitrogen compared to sulfur.
- The bond angle in H2S is also greater than the bond angle in BeCl2 because BeCl2 has no lone pairs of electrons, and the repulsion between the bonding pairs is minimal.
In summary, the bond angle in H2S is greater than the H-Se-H bond angle in H2Se and less than the H-O-H bond angle in H2O.
1. Molecular geometries:
- H2S: The sulfur atom has two bonding electron pairs and two lone pairs, resulting in a bent or V-shaped molecular geometry.
- BeCl2: The beryllium atom has two bonding electron pairs and no lone pairs, resulting in a linear molecular geometry.
- NH3: The nitrogen atom has three bonding electron pairs and one lone pair, resulting in a trigonal pyramidal molecular geometry.
- H2O: The oxygen atom has two bonding electron pairs and two lone pairs, resulting in a bent or V-shaped molecular geometry.
- SnCl2: The tin atom has two bonding electron pairs and no lone pairs, resulting in a linear molecular geometry.
2. Electron pair repulsion:
- Lone pairs of electrons exert greater repulsion compared to bonding electron pairs.
- The repulsion between lone pairs and bonding pairs pushes the bonding pairs closer together, resulting in a decrease in the bond angle.
Explanation:
- The bond angle in H2S is greater than the H-Se-H bond angle in H2Se and less than the H-O-H bond angle in H2O.
- This is because the electronegativity of oxygen is greater than that of sulfur, resulting in a stronger pull on the bonding electron pairs in H2O.
- The stronger electron-electron repulsion between the lone pairs and bonding pairs in H2O leads to a smaller bond angle compared to H2S.
- Similarly, the bond angle in H2S is greater than the bond angle in NH3 because the repulsion between the lone pairs and bonding pairs in NH3 is greater than that in H2S due to the higher electronegativity of nitrogen compared to sulfur.
- The bond angle in H2S is also greater than the bond angle in BeCl2 because BeCl2 has no lone pairs of electrons, and the repulsion between the bonding pairs is minimal.
In summary, the bond angle in H2S is greater than the H-Se-H bond angle in H2Se and less than the H-O-H bond angle in H2O.
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The bond angle in H2S ( H-S-H) is: a)same as that of CI-Be-CI in BeCI2 b)greater than H-N-H bond angle in NH3 c)greater than H-Se-H and less than H-O-H d)same as CI-Sn-CI in SnCI2Correct answer is option 'C'. Can you explain this answer? for Class 12 2025 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about The bond angle in H2S ( H-S-H) is: a)same as that of CI-Be-CI in BeCI2 b)greater than H-N-H bond angle in NH3 c)greater than H-Se-H and less than H-O-H d)same as CI-Sn-CI in SnCI2Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Class 12 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The bond angle in H2S ( H-S-H) is: a)same as that of CI-Be-CI in BeCI2 b)greater than H-N-H bond angle in NH3 c)greater than H-Se-H and less than H-O-H d)same as CI-Sn-CI in SnCI2Correct answer is option 'C'. Can you explain this answer?.
The bond angle in H2S ( H-S-H) is: a)same as that of CI-Be-CI in BeCI2 b)greater than H-N-H bond angle in NH3 c)greater than H-Se-H and less than H-O-H d)same as CI-Sn-CI in SnCI2Correct answer is option 'C'. Can you explain this answer? for Class 12 2025 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about The bond angle in H2S ( H-S-H) is: a)same as that of CI-Be-CI in BeCI2 b)greater than H-N-H bond angle in NH3 c)greater than H-Se-H and less than H-O-H d)same as CI-Sn-CI in SnCI2Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Class 12 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The bond angle in H2S ( H-S-H) is: a)same as that of CI-Be-CI in BeCI2 b)greater than H-N-H bond angle in NH3 c)greater than H-Se-H and less than H-O-H d)same as CI-Sn-CI in SnCI2Correct answer is option 'C'. Can you explain this answer?.
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