chemical bonding

• BeCl2 hybridisation : sp bond pair : 2

  lone pair : 0

  geometry : linear

  shape : linear
• BF3 hybridisation : sp2 bond pair : 3 lone pair : 0 geometry : trigonal planar shape : trigonal planar
• SO2 hybridisation : sp2 bond pair : 2 lone pair : 1 geometry : trigonal planar shape : V shaped or bent
• CH4 hybridisation : sp3 bond pair : 4 lone pair : 0 geometry : tetrahedral shape : tetrahedral
• H2O hybridisation : sp3 bond pair : 2 lone pair : 2 geometry : tetrahedral shape : V shape or angular or bent
• NH3 hybridisation : sp3 bond pair : 3 lone pair : 1 geometry : tetrahedral shape : pyramidal
• PCl5 hybridisation : sp3d bond pair : 5 lone pair : 0 geometry : trigonal bipyramidal shape : trigonal bipyramidal
• SF4 hybridisation : sp3d bond pair : 5 lone pair : 1 geometry : trigonal bipyramidal shape : see saw
• ClF3 hybridisation : sp3d bond pair : 3 lone pair : 2 geometry : trigonal bipyramidal shape : T shape
• XeF2 hybridisation : sp3d bond pair : 2 lone pair : 3 geometry : trigonal bipyramidal shape : linear
• SF6 hybridisation : sp3d2 bond pair : 6 lone pair : 0 geometry : square bipyramidal or octahedral shape : square bipyramidal or octahedral
• dipole moment :

  • C-Cl > C-F > C-Br > C-I
• dipole moment of NH3 > NF3
• • Dipole moment is directly proportional to Chlorine atoms
  • more the EN , more is dipole
• dipole of H-F > H-CL > H-Br > H-I
• O2 (16 e) is paramagnetic with 2 unpaired electrons
• bond energy :

  Cl-Cl > Br-Br > F-F > I-I
• bond order of O3 and C6H6 are 1.5 due to resonance
• • s orbital is non directional
  • p and d orbitals are directional
  • 1s-1s > 2s-2s > 3s-3s
  • 2s-2s < 2s-2p < 2p-2p
• favourable conditions of ionic bond

  1. low ionization energy of metals
  2. high electron gain enthalpy
  3. high lattice energy