Pasadena • Honors Chemistry
Name
10 • Bonding
Period
Date
STATION
1
– BOND
State the type of bond that will form from each pair of elements:
Type
Mg F
Ag Cu
K Na
O F
Type
S
Cl
H
Li
Ionic Bond
Metallic Bond
Metallic Bond
Nonpolar Covalent Bond
TYPES
O
Br
Cl
I
Polar Covalent Bond
Polar Covalent Bond
Polar Covalent Bond
Ionic Bond
Write the type of bond that matches each description.
Nonpolar Covalent Bond Electrons are shared equally between two atoms.
Ionic Bond
Electrons are transferred, the two oppositely charged atoms attract.
Metallic Bond
Electrons are delocalized and move from atom to atom.
Polar Covalent Bond
Electrons are shared unequally between two atoms.
10  Bonding
STATION
Draw the Lewis structures of the following species:
Al
S2-
– LEWIS SYMBOLS
KBr
Al
S
Mg2+
2
2-
P
Br
HF
H F
P
2+
-
+
K
Mg
H2O
Al3+
Cl2
O H
H
Cl Cl
3+
Al
10  Bonding
STATION
3
–
MORE LEWIS SYMBOLS
Draw the Lewis structures of the following molecules and name their shapes.
NH3
SO2
H
H N H
Trigonal pyramidal
CO2
O S O
O S O
O C O
Linear
Bent
NO2–
BF3
F
F B F
Trigonal Planar
OF2
O F
F
Bent
-
O N O
O N O
Bent
10  Bonding
STATION
4
–
Determine the shape of the molecule and decide whether each compound is polar or nonpolar.
PH3
CF4
BH3
F
H
F C F
H P H
POLARITY
H
H B H
F
Trigonal Pyramidal
Non-Polar
SO2
Tetrahedral
Non-Polar
CO2
O S O
O S O
Bent
Polar
Trigonal Planar
Non-Polar
SCl2
O C O
Linear
Non-Polar
S Cl
Cl
Bent
Polar
10  Bonding
STATION
5
– IMF’s AND ATTRACTIONS
Match the statement with the Inter-Particle Forces
A Dipole-Dipole Interactions B. Covalent bonds
D. Ionic Bonds
E. Metallic Bonds
C. Hydrogen-bonding
F. London Dispersion Forces
F
1.
Is used to explain why BP of Xe > Kr > Ar > Ne > He
B
2.
Is present in C(graphite) and C(diamond)
E
3.
Is used to explain why Cu is a good conductor
D
4.
Is used to explain why NaCl(l) is a good conductor
A
5.
Is used to explain why ICl has a higher BP then Br2
C
6.
Is used to explain why boiling point of CH3OH is higher than CH4.
E
7.
A lattice of positive ions in a sea of delocalized electrons
A
8.
Positive ends of molecules attract negative ends of other molecules
D
9.
Lattice of alternating positively and negatively charged particles
C
10. Hydrogen atoms tethered between small, highly electronegative atoms N, O, and F.
F
11. Polarized electron clouds induce dipoles in their neighboring atoms
10  Bonding
STATION
6
–
MORE IMF’s
Here are the attractive forces in order from weakest to strongest:
London
Dispersion
Forces
Dipole-Dipole
Interactions
HydrogenBonding
Metallic Bonding
Ionic Bonding
Covalent
Bonding
Indicate the strongest IMF in each of the following:
SO2 Dipole-Dipole Interaction
CO2 London Dispersion Forces
CH3OH Hydrogen Bonding
Na Metallic Bonds
NH3 Hydrogen Bonding
KOH Ionic Bonds
Xe London Dispersion Forces
SiO2 Covalent Bonds
K2S Ionic Bonds
HCl Dipole-Dipole Interactions
H2S London Dispersion Forces
CH4 London Dispersion Forces
List the three examples of covalent network solids:
Cdiamond
Cgraphite
SiO2, Silica
10  Bonding
STATION
7
–
STRENGTHS
OF ATTRACTIONS
In each case, circle the species with the STRONGER inter-particle forces.
Cl2
or
Br2
Both have LDF, Br2 has more electrons
NaCl
or
HCl
NaCl has ionic bonds, HCl has DDI
KBr
or
LiF
Both have ionic bonds, Li+ and F– are smaller
H2S
or
HCl
H2S has LDF, HCl has DDI
C3H8
or
CH4
Both have LDF, C3H8 has more electrons
H2O
or
H2S
H2O has hydrogen bonding, H2S has LDF
CH3OH
or
CH4
CH3OH has hydrogen bonding, CH4 has LDF
HCl
or
HF
HF has hydrogen bonding, HCl has DDI
10  Bonding
STATION
8
–
EXPLAINING
TRENDS
This graph shows the BP’s of analogous compounds using elements from
periods 2, 3, 4, and 5.
Explain why the BP of Xe > Kr > Ar > Ne:
All have LDF, but the species with more electrons has a more polarizable
electron cloud, resulting in stronger LDFs.
Explain why the BP of H2Te > H2Se > H2S:
All have LDF, but the species with more electrons has a more polarizable
electron cloud, resulting in stronger LDFs.
Why is the BP of H2O > the others in its group?
H2O has hydrogen bonding, while the rest have LDF.
10  Bonding
STATION
9
– VISUALIZING
SOLIDS
For each image, name the type of solid and the inter-particle forces.
Molecular Solid
Dipole Dipole Interactions
Ionic Solid
Ionic Bonds
Metallic Solid
Metallic Bonds
Molecular Solid
London Dispersion Forces
Network Covalent Solid
Covalent Bonds
Molecular Solid
Hydrogen Bonding