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Chemistry ch 10 notes
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Johannes Diderik van der Waals
• His work on the kinetic theory of gases led to further work on connecting liquid and gaseous states
• He received the noble prize for physics in 1910
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Van der Waals
• He create a theory describe attractions between molecules
– The theory that describes the electrostatic attraction between molecules is called van der waals forces
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We can see his work take place around us in God’s creation today :
• The van der Waals forces can be demonstrated by observing a gecko's climbing ability
• A gecko can hang on a glass surface using only one toe.
• Efforts continue to create a synthetic "gecko tape" that exploits this knowledge.
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More on the gecko
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Intermolecular forces
• Forces that play an important role in determining the physical properties of various substances
• Classified into three groups– Dipole – dipole– Hydrogen bonds– Dispersion (London) forces
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Dipole to dipole interactions
• Remember the polar molecules have unevenly distributed electrical charges
• Positive charges of one molecule attract the negative charge of another molecule the stronger the polarity the stronger the force
• Usually this is a characteristic of ionic molecules – Example: SO2
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Hydrogen bonds
• A hydrogen bond is a special type of attractive interaction that exists between an electronegative atom and a hydrogen atom bonded to another electronegative atom.
• This type of bond always involves a hydrogen atom, hence how it gets its name.
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Dispersion (London) Forces
• The electrostatic attraction between atoms or molecules that have immediate and generated dipoles– Covalent molecules are said to have
dispersion forces– This force is not just limited to covalent
molecules, however
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The three forces
• Dispersion forces work between all kinds of molecules: polar and non-polar.
• Dipole to dipole interactions are only between polar molecules
• Hydrogen bonds only exist between polar molecules that have the correct atoms (hydrogen with nitrogen, hydrogen with oxygen, or hydrogen with fluorine)
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Flashback
• describe the behavior of a polar molecule. Is there equal or unequal sharing of electrons?
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Sample problem:
• List the types of intermolecular forces that act between the molecules of the following compounds:
• a. O=C=O b. H:F c. Br:Cl• Solution:
__________________________________________________________________________________________________________________
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Answers
• A. dispersion, this is a non-polar molecule
• B. all forces are present, hydrogen, dipole-dipole, and dispersion; this molecule is polar
• C. dipole-dipole and dispersion forces, this molecule is polar
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Questions?
• Write down 1 question you have so far.
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Chart of three forces
• Create your own chart of these three forces on a blank sheet of paper
• Include the force type, description, and example
• cut and paste in your notebook to refer back to later
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Example Type Description Example
Dipole to dipole forces
Hydrogen forces
Dispersion forces
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Bell work
• Describe one van der waals force:
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Determining boiling points
• Things to consider:– Type of bond– Draw the electron dot structure– Count the electron concentrations around the
central atom and determine its shape – Identify the intermolecular forces involved;
dipole to dipole, dispersion, or hydrogen
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Turn to page 261
• Table A-1 reveals boiling and melting points of different molecular types
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Sample problem
• Using the table 10a-1 on page 261 solve the following
• Which pair has the higher boiling point?
• a. KF or BrF
• B. Cl2 or ICl
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Bell work
• Work on the chapter review pg 285 # 2– look on pg 261 table 10A-1
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Solids pg 263
• What are some basic properties of solids?
• What is the difference between table salt and carbon tetrachloride? Pg 263
• How does the kinetic theory explain why solids have the properties they do? Pg 263– Give an example:
• Why do solids resist compression?
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Two types of solids
• Crystalline solids– Form regular 3 dimensional patterns with
distinct edges and sharp angles– When shattered: smaller shapes form with
similar edges
• Amorphous solids– Have no particular shape– When split or shattered: all kinds of fragments
result
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Look on pg 263
• Draw the two patterns on figures 10B-1 and 10 B-2
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Creating crystal structures
• Cut and tape shapes together
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Bell work
• Draw a solid object
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Freezing
• When does a molecule freeze?
• Can a molecule freeze in warm temperatures? Explain. – Salt melts and freezes at temperatures above
800ºC– This is due to its intermolecular forces
between the molecules
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Heat • There are two types of heat: sensible and
latent heat
• What is sensible heat? – This type of heat results in a change in
temperature
• Latent heat: when a phase change occurs – the temperature remains constant
• Look on page 264 graphs
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Example
• Ice can be heated until it reaches a temperature of zero degrees sensible heat
• The addition of heat at this point will not raise the temperature; it will supply the energy needed for breaking its intermolecular bonds – This is known as latent heat
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Differences
• What is the difference between crystal lattice and unit cell – Look on pg 266-267
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Answer
• Crystal lattice is a crystals pattern/shape and a crystals unit cell is the smallest part of the crystal
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Polymorphs
• Substances that can form more than one type of crystal lattice/pattern
• Allotropic: name give to polymorphous elements
• Allotropes: name give to different forms of allotropic elements – Examples: sulfur, phosphorus, and arsenic
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Answer the following in your notes
• What makes strong crystals?
• Explain lattice energy
• Look on pg 269
• Video (diamonds)
• Work on chapter review pg 286 # 12-13
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Lab today
• cathedrals
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Start working on chapter review
• Pg 286 3-15
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Bell work
• Name one crystalline solid shape pg 267
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Kinetic description of liquids
• Molecules in liquids are bound together by intermolecular forces that balance out the kinetic energy of the molecule
• Liquid molecules have movement but it is limited unlike gases that have free movement
• They flow and match the shape of the container
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Effects of intermolecular attractions
• Surface tension can be demonstrated in liquids such as water, a drop of oil, and a water spider skating across the surface of a pond
• Surface tension is the result of molecules forming an elastic “skin” over the surface of liquids
• The skin forms due to the intermolecular forces of all molecules pointing in the same direction at the surface
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Surfactants and Meniscus
• Surfactants– These are detergents known as self-active
agents– They are able to decrease the natural surface
tension
• Meniscus– Is the result of intermolecular attractions
within the liquid as well as between the liquid and the container, the liquid climbs the walls of the container
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Capillary rise
• Occurs when the adhesive intermolecular forces between the liquid and a substance are stronger than the cohesive intermolecular forces inside the liquid. – Definition: the movement of a liquid up a narrow tube
caused by the attraction of the molecules in the walls of the tube for the molecules of the liquid
– Capillary action, capillarity, or capillary motion is the ability of a substance to draw another substance into it.
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More on capillary rise
• The effect causes a concave meniscus to form where the substance is touching a vertical surface.
• The same effect is what causes porous materials to soak up liquids.
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Viscosity
• A liquids ability to resist flowing• This is revealed in how strong the intermolecular
attraction between molecules are• The stronger the attraction the more viscous the
fluid • Temperature affects these forces
– The colder the temperature the more viscous the substance
– The warmer the temperature the less viscous the substance
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Problems
• Work on chapter review
pg 287 # 16, 20-21
• Surface tension lab today
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Work on problems
• Turn to pg 286 work on 3-15
•
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Bell work
• What are surfactants? Given an example of one.
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Distillation
• The process of vaporization and condensation
• The process are combined together and are used to separate mixtures
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• Describe the difference between critical temperature and critical pressure
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Answer
• Critical temperature and critical pressure both bring a gas to its liquid state, critical temperature involves the amount of temperature needed to bring a gas to its liquid state while critical pressure is the pressure exerted on the gas
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Specific heat
• The amount of heat required to raise the temperature of one gram of the substance 1 degree Celsius
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Sample problem
• What is the boiling point of methanol that is subjected to an atmospheric pressure of 300 torr. Use the graph on page 275 figure 10C-3
• Solution: look across at the vapor pressure of 300 torr (on the side of the graph) find methanol, go straight down and find the temperature in degrees celcius– This is the boiling point
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Answer
• 40 degrees Celsius
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Sample problem
• If 225 cal of heat energy is added to 50.0 g of water at 25.1°C, what is the final temperature of the water?
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Solution
• First determine the temperature change that occurred
• Take 225 cal over 50.0 grams multiply it times the specific heat of water:
• 225 cal x 1.0 g x ºC = 4.50 ºC
50.0g 1.00 cal
Next add 4.5 to the starting temperature, 25.1 ºC = 29.6 ºC ( your answer)
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Sample problem
• A 28 g mass of silver is heated from 15ºC to 85ºC. How many joules were added to the sample?
• First determine the rise in temp: 85-15=70ºC• Next use the specific heat determined from table
10C-4 as the conversion factor• Then multiply the specific heat of sliver times
the grams of silver, times the temp change of silver
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Solution
• 28 g x 70ºC x 0.23 J = 450J
1.00 g x ºC
↑
from table 10C-4
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Questions
• Work on section review 10C
page 285 # 1-3
• When finished: work on crystalline shape cut outs
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Bell work
• Answer prelab questions on page 65