Bonding Set I (Page 2 of 3) in pdf

Bonding Set I Page 2

Answers

: :

Your Lewis structures should show the sp

hybridization in NF

and the sp

d hybridization in PF

. The

reason NF

doesn’t exist is because N has no d orbitals available for hybridization.

(a)

-2

(b) CO has the shortest bond length because of the triple bond.

is trigonal planar because of the sp

hybridization, which puts three sigma bonds in a

plane with lobes of an unhybridized p orbital above and below that plane, forcing the planar

shape. CO

has two double bonds, forcing it to be linear (because of the perpendicular pi

bonds). CO has a triple bond, which is also linear for the same reason as CO

3. (a)

Tetrahedral

Square planar

T-shaped

(b) CF

has 4 shared, no unshared pairs. The maximum angular separation gives a tetrahedron.

XeF

has two unshared pairs on opposite sides of the Xe. This forces the remaining F atoms into a

central plane.

Bonding Set I Page 2