{"id":866290,"date":"2025-08-06T11:54:19","date_gmt":"2025-08-06T06:24:19","guid":{"rendered":"https:\/\/leverageedu.com\/discover\/?p=866290"},"modified":"2025-08-06T11:54:19","modified_gmt":"2025-08-06T06:24:19","slug":"ncert-solutions-class-11-chemistry-part-1-chapter-iv-chemical-bonding-molecular-structure","status":"publish","type":"post","link":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-chemistry-part-1-chapter-iv-chemical-bonding-molecular-structure\/","title":{"rendered":"NCERT Solutions Class 11 Chemistry (Part-1) Chapter 4: Chemical Bonding and Molecular Structure (Free PDF)"},"content":{"rendered":"\n

Class 11 Chemistry (Part-1) Chapter 4: Chemical Bonding and Molecular Structure has introduced you to learn how atoms combine or bond, the different bonding theories, their types, and the underlying principles that govern the formation of chemical compounds.<\/p>\n\n\n\n

This blog will provide you with exercises along with their solutions, which will help you understand the concepts more simply.<\/p>\n\n\n\n\n\n\n

Explore Notes of Class 11 Chemistry<\/strong><\/p>\n\n\n\n

Chapter 1<\/a><\/strong><\/td>Chapter 2<\/a><\/strong><\/td>Chapter 3<\/a><\/strong><\/td>Chapter 5<\/strong><\/td>Chapter 6<\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

NCERT Solutions Class 11 Chemistry (Part-1) Chapter 4: Chemical Bonding and Molecular Structure<\/h2>\n\n\n\n

Below, we have provided you with exercises mentioned in the NCERT Class 11 Chemistry (Part-1) Chapter 4: Chemical Bonding and Molecular Structure.<\/p>\n\n\n\n

Exercises<\/h2>\n\n\n\n
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  1. Explain the formation of a chemical bond.<\/li>\n\n\n\n
  2. Write Lewis dot symbols for atoms of the following elements: Mg, Na, B, O, N, Br.<\/li>\n\n\n\n
  3. Write Lewis symbols for the following atoms and ions: S and S\u00b2\u207b; Al and Al\u00b3\u207a; H and H\u207b<\/li>\n\n\n\n
  4. Draw the Lewis structures for the following molecules and ions: H\u2082S, SiCl\u2084, BeF\u2082, CO\u2083\u00b2\u207b, HCOOH<\/li>\n\n\n\n
  5. Define the octet rule. Write its significance and limitations.<\/li>\n\n\n\n
  6. Write the favourable factors for the formation of an ionic bond.<\/li>\n\n\n\n
  7. Discuss the shape of the following molecules using the VSEPR model: BeCl\u2082, BCl\u2083, SiCl\u2084, AsF\u2085, H\u2082S, PH\u2083<\/li>\n\n\n\n
  8. Although the geometries of NH\u2083 and H\u2082O molecules are distorted tetrahedral, the bond angle in water is less than that of ammonia. Discuss.<\/li>\n\n\n\n
  9. How do you express the bond strength in terms of bond order?<\/li>\n\n\n\n
  10. Define the bond length.<\/li>\n\n\n\n
  11. Explain the important aspects of resonance with reference to the CO\u2083\u00b2\u207b ion.<\/li>\n\n\n\n
  12. H\u2083PO\u2083 can be represented by structures 1 and 2 shown below. Can these two structures be taken as the canonical forms of the resonance hybrid representing H\u2083PO\u2083? If not, give reasons for the same.<\/li>\n\n\n\n
  13. Write the resonance structures for SO\u2083, NO\u2082 and NO\u2083\u207b.<\/li>\n\n\n\n
  14. Use Lewis symbols to show electron transfer between the following atoms to form cations and anions: (a) K and S, (b) Ca and O, (c) Al and N.<\/li>\n\n\n\n
  15. Although both CO\u2082 and H\u2082O are triatomic molecules, the shape of the H\u2082O molecule is bent, while that of CO\u2082 is linear. Explain this on the basis of the dipole moment.<\/li>\n\n\n\n
  16. Write the significance\/applications of the dipole moment.<\/li>\n\n\n\n
  17. Define electronegativity. How does it differ from electron gain enthalpy?<\/li>\n\n\n\n
  18. Explain with the help of a suitable example polar covalent bond.<\/li>\n\n\n\n
  19. Arrange the bonds in order of increasing ionic character in the molecules: LiF, K\u2082O, N\u2082, SO\u2082, and ClF\u2083.<\/li>\n\n\n\n
  20. The skeletal structure of CH\u2083COOH, as shown below, is correct, but some of the bonds are shown incorrectly. Write the correct Lewis structure for acetic acid.<\/li>\n\n\n\n
  21. Apart from tetrahedral geometry, another possible geometry for CH\u2084 is square planar with the four H atoms at the corners of the square and the C atom at its centre. Explain why CH\u2084 is not square planar?<\/li>\n\n\n\n
  22. Explain why the BeH\u2082 molecule has a zero dipole moment, although the Be\u2013H bonds are polar.<\/li>\n\n\n\n
  23. Which out of NH\u2083 and NF\u2083 has a higher dipole moment and why?<\/li>\n\n\n\n
  24. What is meant by hybridisation of atomic orbitals? Describe the shapes of sp, sp\u00b2, sp\u00b3 hybrid orbitals.<\/li>\n\n\n\n
  25. Describe the change in hybridisation (if any) of the Al atom in the following reaction: AlCl\u2083 + Cl\u207b \u2192 AlCl\u2084\u207b<\/li>\n\n\n\n
  26. Draw diagrams showing the formation of a double bond and a triple bond between carbon atoms in C\u2082H\u2084 and C\u2082H\u2082 molecules.<\/li>\n\n\n\n
  27. What is the total number of sigma and pi bonds in the following molecules?<\/li>\n\n\n\n
  28. Considering x-axis as the internuclear axis, which of the following will not form a sigma bond and why?\u00a0<\/li>\n<\/ol>\n\n\n\n

    (a) 1s and 1s (b) 1s and 2p\u2093 (c) 2p\u1d67 and 2p\u1d67 (d) 1s and 2s.<\/p>\n\n\n\n

      \n
    1. Which hybrid orbitals are used by carbon atoms in the following molecules?<\/li>\n<\/ol>\n\n\n\n

      (a) C\u2082H\u2082 (b) C\u2082H\u2084 (c) CH\u2083\u2013CH\u2083 (d) CH\u2083\u2013CH=CH\u2082 (e) CH\u2083\u2013CH\u2082\u2013OH (f) CH\u2083\u2013CHO (g) CH\u2083COOH<\/p>\n\n\n\n

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      1. What do you understand by bond pairs and lone pairs of electrons? Illustrate by giving one example of each type.<\/li>\n\n\n\n
      2. Distinguish between a sigma and a pi bond.<\/li>\n\n\n\n
      3. Explain the formation of the H\u2082 molecule on the basis of valence bond theory.<\/li>\n\n\n\n
      4. Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.<\/li>\n\n\n\n
      5. Use molecular orbital theory to explain why the Be\u2082 molecule does not exist.<\/li>\n\n\n\n
      6. Compare the relative stability of the following species and indicate their magnetic properties: O\u2082\u00b2\u207b (peroxide), O\u2082\u207b (superoxide), O\u2082<\/li>\n\n\n\n
      7. Write the significance of a plus and a minus sign shown in representing the orbitals.<\/li>\n\n\n\n
      8. Describe the hybridisation in the case of PCl\u2085. Why are the axial bonds longer as compared to equatorial bonds?<\/li>\n\n\n\n
      9. Define hydrogen bond. Is it weaker or stronger than the van der Waals forces?<\/li>\n\n\n\n
      10. What is meant by the term bond order? Calculate the bond order of: N\u2082, O\u2082, O\u2082\u207a , and O\u2082\u207b.<\/li>\n<\/ol>\n\n\n\n

        Also Read: NCERT Notes Class 11 Geography Fundamentals of Physical Geography Chapter 14: Biodiversity and Conservation (Free PDF)<\/strong><\/a><\/strong><\/p>\n\n\n\n

        Solutions<\/h2>\n\n\n\n
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        1. Atoms combine to complete their octet and achieve a stable electronic configuration. This leads to formation of a chemical bond, either by transfer (ionic bond) or sharing (covalent bond) of electrons. [p. 99]<\/li>\n\n\n\n
        2. Lewis dot symbols for: Mg, Na, B, O, N, Br<\/li>\n<\/ol>\n\n\n\n