Molecule What would be the What would be Circle the Circle the electron geometry of the the molecular molecule? hybridization of intermolecular geometry of the the central atom forces present molecule? in 1 mol of the molecules ion - dipole London\'s Dispersion dipole dipole none of the above hydrogen bonding ion - dipole SF6 London\'s Dispersion dipole dipole none of the above hydrogen bondin ion - dipole London\'s Dispersion dipole dipole none of the above hydrogen bonding Solution HF electron geometry =tetrahedral (4 lone pains in sp3 orbitals) molecular geometry = linear (sp hybridization, one orbital occupied by electron from H, other with lone pair, so linear) hybridization = sp intermolecular forces = hydrogen bonding (due to the presence of d+ charge H atom due to the electronegativity of F, strong H bonding takes place F…..H-F) SF6 electron geometry = octahedral (6 , S-F bonds) molecular geometry = octahedral (sp3d2 Hybridization) hybridization = none of the above (sp3d2) inter molecular forces = London\'s Dispersion (SF6 has non-polar structure due to symmetry and bonds, so only possibility is London Dispersion interactions) BrF3 electron geometry = trigonal pyramidal (3 Br -F bonds, 2 lone pairs) molecular geometry = T-shape (due to asymmetric charge distribution about the central atom) hybridization = none of the above (sp3d) inter molecular forces = dipole-dipole interactions because of the T-shape, BrF3 is polar. .

1. Molecule What would be the What would be Circle the Circle the electron geometry of the the
molecular molecule? hybridization of intermolecular geometry of the the central atom forces
present molecule? in 1 mol of the molecules ion - dipole London's Dispersion dipole dipole
none of the above hydrogen bonding ion - dipole SF6 London's Dispersion dipole dipole none of
the above hydrogen bondin ion - dipole London's Dispersion dipole dipole none of the above
hydrogen bonding
Solution
HF
electron geometry =tetrahedral (4 lone pains in sp3 orbitals)
molecular geometry = linear (sp hybridization, one orbital occupied by electron from H, other
with lone pair, so linear)
hybridization = sp
intermolecular forces = hydrogen bonding (due to the presence of d+ charge H atom due to the
electronegativity of F, strong H bonding takes place F…..H-F)
SF6
electron geometry = octahedral (6 , S-F bonds)
molecular geometry = octahedral (sp3d2 Hybridization)
hybridization = none of the above (sp3d2)
inter molecular forces = London's Dispersion (SF6 has non-polar structure due to symmetry and
bonds, so only possibility is London Dispersion interactions)
BrF3
electron geometry = trigonal pyramidal (3 Br -F bonds, 2 lone pairs)

2. molecular geometry = T-shape (due to asymmetric charge distribution about the central atom)
hybridization = none of the above (sp3d)
inter molecular forces = dipole-dipole interactions because of the T-shape, BrF3 is polar.