Across
- 3. HYBRIDISATION The mixing of one s and three p orbitals to form four equivalent hybrid orbitals arranged tetrahedrally with bond angle approximately 109.5°.
- 5. The special stability shown by planar cyclic conjugated molecules containing (4n + 2) π electrons as per Hückel’s rule.
- 6. HYBRIDISATION The mixing of one s and two p orbitals forming three equivalent hybrid orbitals arranged in a trigonal planar geometry with 120° bond angles.
- 8. The phenomenon in which a molecule cannot be represented by a single Lewis structure and is best described by multiple canonical forms.
- 9. A covalent bond formed by the head-on overlap of atomic orbitals along the internuclear axis, allowing free rotation.
- 10. HYBRIDISATION The mixing of one s and one p orbital forming two linearly arranged hybrid orbitals with 180° bond angle.
- 11. The permanent displacement of sigma electrons along a carbon chain due to electronegativity differences.
Down
- 1. The delocalization of electrons from a σ-bond (usually C–H) into an adjacent π-bond or empty p-orbital, contributing to molecular stability.
- 2. The dynamic equilibrium between two structural isomers differing in the position of a proton and a double bond, such as the keto–enol equilibrium.
- 4. The ability of carbon to bond with itself to form long chains, branched chains, and cyclic structures due to strong C–C covalent bonding.
- 7. A covalent bond formed by the sideways overlap of parallel p-orbitals above and below the internuclear axis, restricting rotation.