OnlineCBT Logo OnlineCBT
⚲
English
OnlineCBT Logo OnlineCBT
⚲

Chemistry · CHEMICAL BONDING AND MOLECULAR STRUCTURE

हिन्दी

According to Nyholm and Gillespie (1957) refinement of the VSEPR theory, why do lone pairs of electrons produce greater repulsion than bonding pairs?

  1. A lone pair is localised on the central atom alone and occupies more space compared to a bonding pair which is shared between two atoms.
  2. Lone pairs have higher principal quantum numbers compared to the corresponding bonding pairs of the valence shell.
  3. Lone pairs possess an opposite spin sign compared to bonding pairs, reducing exchange stabilization.
  4. Lone pairs are shared between two nuclei and hence exert electrostatic forces in multiple directions simultaneously.

Correct answer · Option 1

A lone pair is localised on the central atom alone and occupies more space compared to a bonding pair which is shared between two atoms.

Explanation

As stated by Nyholm and Gillespie, lone pairs are localised on the central atom and occupy more space, exerting greater repulsive forces on neighbouring electron pairs.

Related questions

Consider the following statements regarding hybridization and orbital characteristics: (A) Hybrid orbitals are always equivalent in energy and shape. (B) Promotion of an electron is an essential condition prior to hybridization. (C) A \( \pi \) bond is stronger than a \( \sigma \) bond because of greater extent of orbital overlap. (D) Only half-filled orbitals of valence shell take part in hybridization; fully filled orbitals can never participate. Which of the above statements is/are correct?→Consider the following isoelectronic pairs/species: \( \text{N}_2 \), \( \text{CO} \), \( \text{NO}^+ \), \( \text{F}_2 \), and \( \text{O}_2^{2-} \). Let \( S_1 \) be the sum of bond orders of \( \text{N}_2 \), \( \text{CO} \), and \( \text{NO}^+ \), and \( S_2 \) be the sum of bond orders of \( \text{F}_2 \) and \( \text{O}_2^{2-} \). What is the value of \( S_1 - 2S_2 \)?→In terms of orbital overlap and bond directionality, which statement explains why simple atomic orbital overlap fails to describe the geometry of \( \text{CH}_4 \)?→Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R). Assertion (A): Two isolated hydrogen atoms do not form a bond when their total potential energy increases as they approach each other. Reason (R): A covalent bond between two atoms is formed only when the net attractive forces overcome the repulsive forces and the system acquires minimum potential energy. In the light of the above statements, choose the correct answer from the options given below:→
ऑनलाइन कंप्यूटर आधारित परीक्षा

हमारा मिशन है – "विद्यार्थियों को शिक्षित करना और उन्हें प्रतिस्पर्धी परीक्षाओं की तैयारी में उनकी पूर्ण क्षमता के साथ उत्कृष्टता प्राप्त करने में सहायता करना। साथ ही उनमें अच्छे संस्कारों का संचार करना और उनके व्यक्तित्व का विकास करना।"

उपयोगी लिंक
महत्वपूर्ण पेज
कोर्सेज और अभ्यास
संपर्क करें
पता

प्लॉट नं. 10, धोलीगुमटी, पंडितपुरा रोड, बंदीकुई, दौसा (राजस्थान) – 303313

संपर्क करें

+91 7877547686

 ई-मेल

onlinecbtportal@gmail.com

 हेल्पलाइन नंबर

+91 7877547686
साझा करें
डाउनलोड करने के लिए क्लिक करें
Get it on Google Play

ऐप डाउनलोड करने
के लिए Google Play पर
उपलब्ध है

उपयोग की शर्तें | गोपनीयता नीति | कुकी नीति | अस्वीकरण | संपादकीय नीति | तथ्य जांच | सुधार | DMCA | विज्ञापन विकल्प

Copyright © 2026 - OnlineCBT.in. All Rights Reserved.

WhatsApp Chat