Name _______________________________________
Chemistry
Mr. Harper
CH 6: Bonding Packet
Study Guide
1. What is a chemical bond?
a. Why do atoms form chemical bonds?
b. What is the octet rule and what role does it play in chemical bonding?
c. What are the four types of chemical bonds?
2. Ionic bonding
a. How do ionic bonds form? What types of elements form ionic bonds?
b. What is a formula unit?
c. How do you show the formation of an ionic bond using electron dot notation?
d. What are the properties of ionic compounds?
e. What is lattice energy?
f. What is the structure of ionic compounds and how does it explain their properties?
3. Metallic bonding
a. How does a metallic bond form? What types of elements form metallic bonds?
b. What is a sea of electrons?
c. What are the properties of metallic compounds?
d. What is enthalpy of vaporization?
e. What is the structure of metallic compounds and how does it explain their properties?
f. Why are the properties of a metallic compound different than an ionic compound if both form a
crystal lattice?
4. Covalent bonding
a. How does a covalent bond form? What types of elements form covalent bonds?
b. What is bond energy?
c. Network
i. What are the properties of covalent network compounds?
ii. What is structure of covalent network compounds and how does it explain their
properties?
d. Molecular
i. What is a molecule?
ii. What are the properties of covalent molecular compounds?
iii. What is structure of covalent molecular compounds and how does it explain their
properties?
5. Molecular compounds
a. How do you draw the Lewis structure of a molecule?
b. How do you determine the geometry of a molecule? What is VSEPR theory?
c. How do you determine the polarity of a molecule?
d. What is the difference between polar and nonpolar covalent bonds?
e. What are the 3 intermolecular forces?
i. How do you determine the intermolecular forces of a molecular compound?
ii. How can you compare boiling points of substances based on the intermolecular forces?
1
Bookwork
1.
2.
3.
4.
5.
6.
p.177 #1-6
p.196 #1-4
p.194 #1-5
p.199 #1 and p.201 #1
p.207 #2a&b,3,5,6
p.210 #25-28,30-32
2
Bonding Lab
Purpose: To determine the type of bonding of a substance based on its properties.
Hypothesis: Make a prediction of the type of bonding for each substance to be tested.
Materials:
5 substance samples
10 test tubes
Bunsen burner
Distilled water
5, 100 mL beakers
Battery
3 alligator clips
Light bulb & socket
Test tube rack
Test tube holder & clamp
Support stand
Cork stoppers
5 Weigh boats
Triple beam balance
Graduated cylinder
Prelab:
1. Watch the teacher demonstration and record the results for the 4 types of bonding in the table below.
Substance
Type of
Bonding
Elements
Involved
Copper
Metallic
Metals
Table Salt
Ionic
Sugar
Covalent
molecular
Covalent
network
Metal &
Nonmetal
Nonmetals
Amethyst
Solid
Conductivity
Test
Melting point
test
Water
Solubility
Test
Aqueous
Conductivity
Test
Nonmetals
Procedure:
1. Make a data table to record: (1) the substance being tested, (2) your prediction of the type of bonding,
(3) result of the solid conductivity test, (4) result of the melting point test, (5) result of the water
solubility test, (6) result of the aqueous conductivity test, (7) the type of bonding for each of the
substances, and (8) the elements involved in the bond.
2. Predict the type of bonding for each unknown substance in the data table.
3. Place approximately 1 g samples of each substance into 5 weigh boats.
4. Touch both leads of your electrical circuit to each substance in the weigh boat. After each test, rinse
the leads with distilled water and carefully dry them. Note your observation in the data table.
5. Place 5 test tubes in the test tube rack. Pour each sample from the weigh boats into the test tubes.
6. Secure the test tube clamp on the support stand and then light your Bunsen burner.
7. Place one of the test tubes in the clamp and heat it over the Bunsen burner flame. As soon as the
substance melts, remove it from the flame. Do not heat any substance for more than 3 minutes. There
may be substances that will not melt.
8. Note your observation in the data table and repeat for the other substances.
3
9. Place 5 more test tubes in the test tube rack. Put 0.5 g of each substance into its own test tube. Add 5
mL of distilled water to each test tube. Put a cork stopper on each test tube and shake it in an attempt
to dissolve the substance. Note your observations.
10. Take the stopper off each test tube and pour the contents into separate 100 mL beakers. Immerse the
leads of your electrical circuit into the contents of each beaker. After each test, rinse the leads with
distilled water and carefully dry them. Note your observation in the data table.
11. Dispose of all substance samples in the waste beaker in the back of the room.
12. Clean all equipment with soap and water. Dry the equipment and return it to its proper place. Clean
your lab station and wash your hands.
Analysis:
1. Using the control substances in the prelab, determine the type of bonding for each substance. Place
your answer in the data table.
2. Using your book or the internet, look up the type of elements each substance is composed of: metals,
nonmetals, or metalloids, and record this information in the data table.
3. Why was it necessary to rinse the leads after each test?
4. Why was it necessary to use distilled water in the experiment?
5. Do all compounds of a specific type of bonding have the same properties or can the properties vary? If
so, give an example?
6. What are some other ways, properties, or characteristics that you could use to determine the type of
bonding in a substance?
Conclusion:
Think about the properties of each type of bonding that you observed and explain why they have the
properties that they have. Speculate on the chemical structure of their bonds that would give them the
properties that you observed.
Lab Report:

Name of Lab

Names of Group Members

Period #

Date

Lab Purpose

Data Table

2-3 Sources of Error
(What affected your ability to make accurate observations?)

Analysis
(Answer questions 2-6 in the analysis section.)

Conclusion
(Yours at the top of the list)
4
Electron Dot Diagrams for Ionic Compounds
Directions: Show the formation of the ionic bond between each of the following elements. Then, write the
chemical formula.
1. Lithium and nitrogen
2. Sodium and oxygen
3. Potassium and fluorine
4. Beryllium and phosphorus
5. Magnesium and sulfur
6. Calcium and fluorine
7. Aluminum and nitrogen
8. Gallium and oxygen
9. Indium and fluorine
10. Strontium and sulfur
5
Lewis Structures 1
Draw the Lewis structures for the following molecular compounds using the procedure below.
1.
2.
3.
4.
5.
6.
7.
8.
Add up the total number of valence electrons.
Put the element that needs the most electrons in the center.
Give that element an octet of electrons.
Place the other elements around the central atom at pairs of electrons.
Fill in the rest of the electrons trying to get an octet around each atom.
If this is not possible, try double or triple bonds between atoms.
Count the number of electrons in the Lewis structure to be sure you have the right amount.
Turn all shared pairs of electrons into dashes to represent covalent bonds.
Compounds:
1. CH4
2. Br2
3. NF3
4. HCl
5. H2Se
6. ICl
7. CF4
8. PCl3
9. CF3I
10. Br2O
11. CS2
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Lewis Structures 2: Multiple Bonds
Draw the Lewis structures for the following molecular compounds.
1. H2
2. O2
3. CO2
4. CH3I
5. NH2Cl
6. N2
7. C2H4
8. CH2O
9. ONCl
10. C2HBr
7
Molecular Geometry Worksheet (VSEPR Theory)
Molecule
Lewis Structure
# of e- pairs /
groups
around the
central atom
# of atoms
bonded to
the
central
atom
Molecular Shape
(Use the VSEPR
theory to build
the model of the
molecule. Then,
draw it.)
Geometry
(Name of
molecular
shape. Use p.
200 in the
textbook.)
New example
(Give the
formula of
another
molecule with
same shape.)
SiH4
PF3
H2S
CH2O
SPI
CO2
PCl5
SF6
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Intermolecular Forces
Dipole-dipole
1. Attraction between dipoles of
_____________________ molecules
2. A ________________ is a distribution of
Hydrogen Bonding
1. ____________________ type of
_____________-_____________ force
2. Happens when _________________ is
charge where opposite charges are on
bonded to a highly ________________
opposite sides of a molecule or atom
element, such as ______, _____, & _____
3. Happen between _________________
molecules
3. Exposes hydrogen’s ______________ on
London Dispersion
1. _______________ intermolecular force
2. Exists in any atom or molecule regardless
of ____________________
3. Happens because electrons are in
constant __________________
4. At times, there is an _______________
one side of the molecule, making the
distribution of ___________________
4. Effective only over a ___________ range
molecule highly _________________
around the atom or molecule.
5. Always present for _________________
4. Reason for surface _______________ of
5. This distribution causes a
molecules; may be induced in
water and unusually high
____________________ dipole to form
________________ molecules or atoms
___________________ points of three
which results in the attraction between
compounds: ______, ______, & ______
two ____________________.
6. ___________________ of a molecule is
determined from molecular geometry
6. When two neighboring molecules form
and type of covalent bond: polar or non-
these dipoles they _____________ each
polar.
other, but the attraction only lasts for an
____________________.
9
Paper Chromatography Lab
Purpose: To see the difference between polar and nonpolar substances.
Hypothesis: Predict which color dyes are in a black marker (ex. red, blue, yellow, etc.).
Materials:
Large filter papers
Pencil
6 Beakers
Water
Assorted markers
Scissors
Ruler
Rubbing alcohol
Procedure:
1. Cut large filter paper circles into 6 strips approximately 1’’ x 4’’.
2. Measure 1’’ from the bottom of each strip and make a horizontal PENCIL line with an X in the
middle.
3. Put a dot of marker on the X for each strip. Use a black permanent marker, a black washable
marker, and 4 others of your choosing.
4. Place each paper strip in a beaker with a small amount of warm water in the bottom so that the
paper is wet but the ink dot is not touching the water. You may want to crease the paper over
the edge of the beaker so that it stays upright.
5. Let the water travel up the paper until it nearly reaches the top.
6. Record your observations:
7. Repeat steps 1-6 using cold water instead.
8. Record your observations with the cold water:
9. Repeat steps 1-6 using rubbing alcohol instead.
10. Record your observations with the rubbing alcohol:
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Analysis:
1. Describe the colors found in each marker. List the color of the marker as well as the colors that
made it up. Did any of these surprise you?
2. Compare the separations for the warm water, cold water, and rubbing alcohol. Was there any
difference? Explain.
3. Which type of marker is most polar: permanent or water soluble? How do you know?
4. Which color dye is most polar? Which color dye is most nonpolar? How do you know this?
5. We have learned that water is a polar molecule. From the results of this lab, what polarity
would you predict for rubbing alcohol? Explain your reasoning.
6. Why does the water travel up the filter paper and defy gravity? (Hint: Google “capillary
action.”)
7. Think about why separating compounds based on polarity and intermolecular forces might be
useful. List at least 2 ways that it can be useful.
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Polarity Worksheet
Molecule
Lewis Structure
Molecular
Geometry
(Build the model
so you can
visualize it.)
Is the molecule
symmetrical?
(Yes or No)
What kind of
bonds does it
contain, polar,
non-polar, or
both?
Is the molecule
as a whole polar
or non-polar?
What intermolecular
forces apply?
(Dipole-dipole,
Hydrogen bonding,
London dispersion)
State of matter at
room temp. (solid,
liquid, or gas)? List
the boiling point.
See p.204.
CH4
NH3
H2O
CO2
N2
HF
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Chemical Bonding Comparison
Characteristic or property
Ionic
Metallic
Covalent
Molecular
Network
Types of elements in the bond
(metals, nonmetals, metalloids)
Basic unit of compound
(molecule, formula unit, atom)
Components of compound
(atoms, shared electrons,
cations, anions, sea of e-)
Structure of compound (crystal
lattice or individual molecules)
Behavior of electrons (shared,
free, transferred)
Measurement of bond strength
(lattice energy, enthalpy of
vaporization, bond energy)
Relative melting point (high,
low, medium)
Typical water solubility (Yes,
No, Depends on polarity)
Solid conductivity
(Yes, No)
Aqueous conductivity
(Yes, No, N/A)
Other properties: (e.g. Hard,
brittle, malleable, ductile, weak
intermolecular forces)
Example: Name and chemical
formula
Model: Draw a representation
of each compound. (Use back of
sheet if necessary.)
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