Do Now
Clicker #
Name …………………………………………….
Team ……………………….
Title: Types of bonding
Date ………………………
Describe each of the following types of bonding as fully as you can
Metallic bonds
Ionic bonds
Pure covalent bonds
Polar covalent bonds
Lecture note taking
More explaining
What are the quantum numbers associated with the most outer electron of carbon
Lecture continued
CFU Lecture 1
Arrange the following in order of strength strongest first
Dipole Dipole
Covalent
Hydrogen bonding
Dipole Dipole interactions can only occur in:
Polar molecules
Nonpolar molecules
Gases
Explain what properties of oxygen allow Hydrogen bonding to occur between water
molecules
Independent practice
Name …………………………………………….
Team ………………………
Title:intermolecular forces
Date ……………………
1)
Using your knowledge of molecular structure, identify the main intermolecular
force in the following compounds. You may find it useful to draw Lewis
structures to find your answer.
a)
PF3 _____________________________
b)
H2CO _____________________________
c)
HF _____________________________
2)
Explain how dipole-dipole forces cause molecules to be attracted to one another.
3)
Rank the following compounds from lowest to highest boiling point: calcium
carbonate, methane, water
4)
Explain why nonpolar molecules usually have much lower surface tension than
polar ones.
For each of the following compounds, determine the main intermolecular force.
You may find it useful to draw Lewis structures for some of these molecules:
1)
nitrogen ________________________________
2)
carbon tetrachloride ________________________________
3)
H2S ________________________________
4)
sulfur monoxide ________________________________
5)
N2H2 ________________________________
6)
boron trihydride ________________________________
7)
CH4O ________________________________
8)
SiH2O ________________________________
Exit Ticket
**
Clicker #
Name …………………………………………….
Team ………………………
Title: Intermolecular bonding
Date ………………………
1 Place the following in order of increasing strength:
1. hydrogen bonding
2. covalent bonding
3. London dispersion forces
A.
B.
C.
D.
E.
**
2, 1, 3
1, 2, 3
1, 3, 2
3, 1, 2
3, 2, 1
2a)The correct order for increasing boiling point among the noble gases is:
A.
B.
C.
D.
E.
*
He
Ne
Ar
Kr
Xe
2 b) This phenomenon is best explained in terms of:
A.
B.
C.
D.
E.
hydrogen bonding
dipole-dipole interaction
Hund's rule
London dispersion forces
covalent bonding
*
3) Which of the following 4 statements are false?
1. Liquids with large intermolecular forces tend to have very low boiling points
2. Liquids with large intermolecular forces tend to have considerable surface tension
3. When a substance changes from a solid to a liquid, the molecules remain intact
4. The hardness of diamond is due to strong dipole-dipole attraction
A.
B.
C.
D.
E.
*
1 and 3
2 and 3
2 and 4
1 and 4
3 and 4
b) Explain your answer choice
4) State which type of interaction (dipole-dipole forces or London forces) exists
between molecules in the following:
*
N2
CO2
*
CH3Cl
HBr
HWK
Name …………………………………………
Clicker #
Team ……………………….
Title: intermolecular force
Date ………………………
For each of the following molecules draw the Lewis dot diagram and decide the most
significant type of intermolecular bonding
**
1)
water H2O
**
2)
carbon tetrachloride CCl4
**
3)
ammonia NH3
4)
carbon dioxide CO2
*
5)
phosphorus trichloride PCl3
*
6) F2 and Br2 both have London Dispersion Forces. Explain which would have the most
significant amount of LDF and how effects the molecules physical state at room
temperature.