Nature of the C–X bond (NCERT Table 6.2)C–X बंध की प्रकृति (NCERT सारणी 6.2)Nature of the C–X bond (NCERT Table 6.2)

NCERT Table 6.2 · Class 12 Chemistry · Chapter 6 · interactive diagram

Parts and what they mean

• Polarised C–X bond: Cδ+ — Xδ− (ध्रुवित C–X बंध: Cδ+ — Xδ−) — Halogens are more electronegative than carbon, so the bond pair is pulled towards X. The δ+ carbon is what nucleophiles attack.
• Dipole moment arrow (towards X) (द्विध्रुव आघूर्ण तीर (X की ओर)) — The crossed arrow points from the δ+ end to the δ− end.
• C–X bond length increases F < Cl < Br < I (C–X बंध लंबाई F < Cl < Br < I) — NCERT: CH₃–F 139, CH₃–Cl 178, CH₃–Br 193, CH₃–I 214 pm — the halogen atom gets larger down the group.
• C–X bond enthalpy decreases F > Cl > Br > I (C–X बंध एन्थैल्पी F > Cl > Br > I) — NCERT: 452, 351, 293, 234 kJ mol⁻¹. Weakest C–I bond breaks most easily → R–I is the most reactive.
• Dipole moments (NCERT) (द्विध्रुव आघूर्ण (NCERT)) — CH₃F 1.847, CH₃Cl 1.860, CH₃Br 1.830, CH₃I 1.636 D. CH₃Cl is highest: Cl is less electronegative than F, but the longer C–Cl bond more than makes up.
• Trend down the group (समूह में नीचे प्रवृत्ति) — Size of X increases → longer and weaker C–X bond.

Original diagram drawn by Simple Learning Hub, based on NCERT Table 6.2. Report a mistake