Sigma and pi bond hybridisation

Edit Answers
123456789101112131415
Across
  1. 1. Type of orbital overlap where orbitals approach head-on along the internuclear axis.
  2. 5. Weaker bond formed by sideways overlapping of orbitals.
  3. 9. Geometry where atoms form a triangle in a plane, seen in sp² hybridized atoms.
  4. 10. Mixing of one s and one p orbital forming two linear orbitals.
  5. 11. Strong bond formed by axial overlapping of orbitals.
  6. 12. Spatial arrangement with bond angles of ~109.5°, typical in sp³ hybridized atoms.
  7. 14. Mixing of one s and three p orbitals forming four equivalent orbitals with tetrahedral geometry.
  8. 15. Mixing of one s and two p orbitals forming three orbitals arranged in a trigonal planar geometry.
Down
  1. 2. Arrangement where bonded atoms are in a straight line, typical of sp hybridization.
  2. 3. Two electrons occupying the same orbital with opposite spins.
  3. 4. Orbital overlap where orbitals approach side by side, leading to pi bond formation.
  4. 6. Equal energy achieved by orbitals of different types during hybridization.
  5. 7. Bond where one atom provides both electrons for the bond, often seen in NOâ‚‚ groups.
  6. 8. System of alternating single and double bonds, common in benzene-like compounds.
  7. 13. Visual method to show orbital filling using boxes and arrows.