Review of Inter- and IntraMolecular Forces and Types of Solids
Get out a separate sheet of paper.
You will first write down substance then answers the
following questions for each substance. (# them on your
paper)
1. Identify the type of intramolecular force present
2. Indentify the type(s) (if any) of intermolecular forces
present
3. What type of solid would form.
Intramolecular forces
• Metallic- between metals (sea of electrons)
• Ionic- cation and an anion (transfer of
electrons)
• Covalent- non-metal and a non-metal (sharing
of electrons)
Intermolecular Forces
• Only covalent molecules have intermolecular
• Dipole-dipole- opposite partial charges attract
each other on separate molecules.
• Hydrogen bond- the partial positive hydrogen
(attached to a NOF) attracts a partial negative
NOF on a separate molecule
• LDF- instantaneous dipole which causes a
momentary partial positive which is attracted to
the partial negative on a separate molecule.
1. Identify the type of intramolecular force present
2. Indentify the type(s) (if any) of intermolecular forces
present
3. What type of solid would this form?
gold
1. Identify the type of intramolecular force present: Metallic
2. Indentify the type(s) (if any) of intermolecular forces
present N/A
3. What type of solid would this form? Metallic
gold
1. Identify the type of intramolecular force present
2. Indentify the type(s) (if any) of intermolecular
forces present
3. What type of solid would this form?
sodium chloride
1. Identify the type of intramolecular force present: Ionic
2. Indentify the type(s) (if any) of intermolecular forces
present: N/A
3. What type of solid would this form? Ionic
sodium chloride
1. Identify the type of intramolecular force present
2. Indentify the type(s) (if any) of intermolecular forces
present
3. What type of solid would this form?
Bromine, Br2
(Think Br, I, N, Cl, H, O, F)
1. Identify the type of intramolecular force present:
Covalent
2. Indentify the type(s) (if any) of intermolecular
forces present: LDF
3. What type of solid would this form? Molecular
Bromine, Br2
1. Identify the type of intramolecular force present
2. Indentify the type(s) (if any) of intermolecular
forces present
3. What type of solid would it form?
water
1. Identify the type of intramolecular force present:
Covalent
2. Indentify the type(s) (if any) of intermolecular
forces present: LDF, Dipole-dipole, hydrogen bond
3. What type of solid would it form? Molecular
water
1. Identify the type of intramolecular force present
2. Indentify the type(s) (if any) of intermolecular
forces present
3. What type of solid would it form?
dimethyl ether
1. Identify the type of intramolecular force present:
Covalent
2. Indentify the type(s) (if any) of intermolecular forces
present: LDF, Dipole-dipole
3. What type of solid would it form? molecular
dimethyl ether
More practice
• List the three types of solid.
• What types of elements form each solid
(metal, nonmetal)?
• List the three types of solid.
– Metallic, ionic, molecular
• What types of elements form each solid
(metal, nonmetal)?
– Metallic – metals
– Ionic – metal and nonmetal
– molecular- nonmetals
• For each of the three solids, identify if that
solid is malleable or brittle.
• Then, explain WHY it is malleable or brittle.
• For each of the three solids, identify if that
solid is malleable or brittle.
– Metallic – malleable (metal cores can change
positions within the sea of electrons)
– Ionic – brittle (when a plane of ions shift, repulsive
forces cause the solid to break)
– Molecular – brittle (weak intermolecular forces
hold it together)
• Then, explain WHY it is malleable or brittle. (in
parenthesis)
1. Identify the type of intramolecular force present:
2. Indentify the type(s) (if any) of intermolecular
forces present
3. What type of solid would it form?
hydrogen sulfide
1. Identify the type of intramolecular force present:
Covalent
2. Indentify the type(s) (if any) of intermolecular forces
present: LDF, Dipole-dipole
3. What type of solid would it form? Molecular
hydrogen sulfide (H2S)
(Not an acid, it’s usually a gas we
will talk later)
1. Identify the type of intramolecular force present
2. Indentify the type(s) (if any) of intermolecular
forces present
3. What type of solid would this form?
iodine
1. Identify the type of intramolecular force present:
Covalent
2. Indentify the type(s) (if any) of intermolecular forces
present: LDF
3. What type of solid would this form? molecular
Iodine (I2)
1. Identify the type of intramolecular force present
2. Indentify the type(s) (if any) of intermolecular
forces present
3. What type of solid would it form?
ethanol
1. Identify the type of intramolecular force present:
Covalent
2. Indentify the type(s) (if any) of intermolecular
forces present: LDF, Dipole-dipole, hydrogen bonds
3. What type of solid would it form? molecular
ethanol
1. Identify the type of intramolecular force present
2. Indentify the type(s) (if any) of intermolecular forces
present
3. What type of solid would it form?
calcium oxide
1. Identify the type of intramolecular force present: Ionic
2. Indentify the type(s) (if any) of intermolecular forces
present: N/A
3. What type of solid would it form? Ionic
calcium oxide
What type of force would keep these two
molecules together in the solid state?
What type of force would keep these two
molecules together in the solid state?
• LDF
Which of these orientations would
allow for hydrogen bonds to occur
between molecules of ethanol?
Which of these orientations would
allow for hydrogen bonds to occur
between molecules of ethanol?
Draw this molecule.
Why does oxygen have a partial negative
charge while carbon has a partial positive
charge?
Draw this molecule.
Why does oxygen have a partial negative
charge while carbon has a partial positive
charge?
A: The oxygen is more electronegative than the carbon.
Draw a second molecule, arranging it
to show the IMF.
(What type of IMF is this?)
Draw a second molecule, arranging it
to show the IMF.
(What type of IMF is this?)
Draw two ammonia (NH3)molecules,
showing IMF’s.
(What shape is ammonia?)
Draw the lewis structures for carbon dioxide and
water. Identify inter- and intra-molecular
forces for both.
Draw the lewis structures for carbon dioxide and
water. Identify inter- and intra-molecular
forces for both.
CO2: Intra-covalent,
Inter- LDF
Water: Intracovalent, Inter-LDF,
Dipole-dipole,
hydrogen bond
At room temperature, what state is carbon
dioxide? What state is water?
Explain the difference.
At room temperature, what state is carbon
dioxide? What state is water?
Explain the difference.
CO2 is a gas and water is a liquid. The sum of
the intermolecular forces in water are
stronger than just the LDF of CO2
Water is a liquid while hydrogen sulfide is a gas
at room temperature. Which has a higher
boiling point? How do you know?
Draw the molecules, identify the inter- and
intra-molecular forces, and explain why one is
a liquid at room temperature while the other
is a gas.
Water is a liquid while hydrogen sulfide is a gas
at room temperature. Which has a higher
boiling point? How do you know?
Water because it is a liquid at room temperature
while hydrogen sulfide has already boiled to
the gaseous state.
Draw the molecules, identify the inter- and
intra-molecular forces, and explain why one is
a liquid while the other is a solid.
Check with your neighbor
Predict whether dimethyl ether or ethanol will
have a higher boiling point. Explain your
choice using correct vocabulary.
Predict whether dimethyl ether or ethanol will have a higher
boiling point. Explain your choice using correct vocabulary.
Ethanol has a higher boiling point because it has LDF,
dipole-dipole and hydrogen bonds while dimethyl ether
has only LDF, and dipole-dipole.
Draw depictions of chlorine, bromine, and
iodine at room temperature. Draw at least 10
molecules of each. [Hint: if you don’t know
their state at room temperature, look at the
colors on the big periodic table.]
chlorine
bromine
iodine
• Why is chlorine a gas, bromine a liquid, and
iodine a solid? [Hint: identify inter- and intramolecular forces]