Chem 161 Chapter 9 Molecular Geometry Worksheet - Shape Determines Function Page 30
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406. Show the atomic orbital diagrams for the formation of the three hybrid orbitals for each C
atom below:
hybridization
"
" " " " "
→
€
atomic orbital diagram before hybridizing
atomic orbital diagram after hybridizing
Each C–H bond and the first C–C bond are all sigma bonds, as shown below:
Note: The atomic orbital diagram for each C atom drawn in step 6 C shows two unhybridized p
nd
rd
orbitals. The 2
and 3
C–C bonds form from the electrons in the unhybridized p orbitals.
– Each carbon has two unpaired electrons in unhybridized p orbitals (in the 2p
and 2p
),
y
z
which are perpendicular to the sp orbitals forming the C–H and first C–C bond.
– These two electrons in the 2p
and 2p
bond to each other via a sideways overlap to make
y
z
nd
rd
the 2
and 3
bond in the triple bond, as shown above.
Note: The carbon-carbon triple bond in C
H
consists of a σ bond (shown in blue) and two
2
2
carbon-carbon π bonds (shown in green) made from the four lobes on the unhybridized p’s.
Example: HCN
1. Draw the Lewis structure for HCN:
2. The shape around C is ______________, and the bond angle is __________.
3. Electron configuration for C: ___________________
4. Given the shape around each C atom, C has _________ atomic hybrid orbitals.
5. Draw the atomic orbital diagram for
the valence electrons in C, promoting
electrons, so C can form 4 bonds.
CHEM
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