Name _________________________ Chem 6 Section # ________
Hybrid Orbitals, Bonding
1. Using the following structure:
H2C=C=CH2
a) How many sigma bonds are there? How many pi bonds?
b) What is the hybridization of the central C atom?
(a) sp
(d) dsp3
2
2
3
(b) sp
(e) d sp
(c) sp3
c) What is the hybridization of the terminal carbon atoms?
d) What is the C=C=C bond angle? What is the HCH bond angle?
a)
90°
c) 120°
b)
109.5°
d) 180°
2. Using the following structure:
a) How many sigma bonds are there? How many pi bonds?
H
C
1
3
H
O
C
C
C
H
C
H
H
b) What is the hybridization of the two O atoms?
(a) sp
(d) dsp3
2
3
(b) sp2
(e) d sp
(c) sp3
O
H
2
c) What is the hybridization of the carbon atoms labeled 1, 2 and 3?
d) What are the angles of the bonds labeled 1, 2, 3?
H
C
1
a)
b)
Class 7
90°
109.5°
c)
d)
H
O
C
C
C
H
C
H
3
O
H
H 2
120°
180°
Page 1
Group Work
Name _________________________ Chem 6 Section # ________
1.
How many σ and π bonds are in the following molecules? (Hint: Draw out the
complete Lewis structure before counting.)
(i)
CH3CH
CHCH2CH3
CH2CH2OH
(ii)
2.
Give the Lewis structures for ClF2+ and ClF2−. What are the hybridizations of the Cl
atoms in each structure?
(a)
(b)
(c)
(d)
(e)
sp
sp2
sp3
dsp3
d2sp3
3. Give the hybridization of sulfur and the bond angles in each of the following
molecules of ions:
a) SO2
b) SO3
c) SO42−
4. a)
b)
Class 7
Which species in question 3 has the longest SO bond length?
Which one has the shortest SO bond length?
Page 2
Group Work
Name _________________________ Chem 6 Section # ________
1. What is the electron domain geometry about the C in CH3OH? What hybrid orbitals are
used by the C for bonding?
2.
A) What is the molecular geometry of NCl3?
B)
What is the molecular geometry of CCl4?
C)
Which bond angle is greater the ClNCl bond angle in NCl3 or the ClCCl
bond angle in CCl4?
D) What hydrid orbitals are used for bonding in NCl3 and CCl4?
2.
What is the hybridization of the Cl atom in ClF3?
(a)
(b)
(c)
(d)
(e)
3.
sp
sp2
sp3
dsp3
d2sp3
What is the hybridization of the Be atom in BeBr2?
(a)
(b)
(c)
(d)
(e)
Class 7
sp
sp2
sp3
dsp3
d2sp3
Page 3
Group Work
Name _________________________ Chem 6 Section # ________
Intermolecular Forces
1. Which one of the following molecules has the highest normal boiling point?
(a)
(b)
(c)
(d)
(e)
CH3Cl
CH3Br
CH3I
CH4
CH3OH
HINT: Use the flow chart on 34 of the Study guide to help you determine the important intermolecular
forces of each molecule.
Rank the molecules listed above from lowest normal boiling point to highest normal
boiling point.
2.
Which intermolecular forces are important for the pure liquid CH3F?
A. London forces only
B. dipole-dipole interactions only
C. H-bonding only
D. London forces and dipole-dipole interactions
E. London forces, H-bonding and dipole-dipole interactions
3. What type (or types) of intermolecular forces would be important in the following
molecules or atoms? (It is possible for a molecule to interact via more than one of
these. List ALL that are important.)
Choose from these answers:
a) London Dispersion Forces b) dipole-dipole c) H-bonding, d) ion-ion (lattice energy)
i)
ii)
Cl
Cl
Cl
iii)
iv)
Cl
Class 7
OH
Cl
Page 4
Group Work