CH 115 Fall 2014 Worksheet 16
1.
For each of the following: name the compound (if possible), classify as ionic or molecular, draw the Lewis structure (if applicable), assign electronic/molecular geometry to the central atom, determine bond angles, decide hybridization, determine whether the molecule is polar or not, and give the intermolecular forces present in the molecule. LEWIS STRUCTURES BELOW a). SOCl
2
– molecular, no name possible (we only name BINARY molecular compounds), tetrahedral, trigonal pyramidal, less than 109.5, sp 3 , polar, dipole-dipole forces, London-dispersion forces b). PBr
3
- molecular, phosphorus tribromide, tetrahedral, trigonal pyramidal, less than 109.5, sp 3 , polar, dipole-dipole forces, London forces c). H
2
O
2
– molecular, hydrogen peroxide, tetrahedral, bent, less than 109.5, sp 3 , polar, dipole-dipole forces, hydrogen bonding, London forces d). Fe
2
(SO
4
)
3
– ionic, iron (III) sulfate, ion-ion forces, London forces e). CH
2
O – molecular, no name, trigonal planar, trigonal planar, 120, sp 2 , polar, dipole-dipole forces, London forces f). C
2
H
4
– molecular, ethylene, trigonal planar, trigonal planar, 120, sp 2 , nonpolar, London forces g). N
2
– molecular, nitrogen, linear, linear, 180, sp, nonpolar, London forces h). CaS – ionic, calcium sulfide, ion-ion forces, London forces i). AlCl
3
– molecular, aluminum trichloride, trigonal planar, trigonal planar,
120, sp 2 , nonpolar, London forces j). CH
2
F
2
– molecular, no name, tetrahedral, tetrahedral, 109.5, sp 3 , polar, dipole-dipole forces, London forces k). O
2
– molecular, oxygen, trigonal planar, no molecular geometry, less than
120 (theoretically), sp 2 , nonpolar, London forces l). H
2
CS – molecular, no name, trigonal planar, trigonal planar, 120, sp 2 , polar, dipole-dipole forces, London forces