Chapter 13:
States of Matter
This is a picture of a really creepy guy with a sword that looks like Hamlet. So perhaps it has to do with relating his state of mind "To be or not to Be" with states of matter
13.1 Gases
Kinetic-molecular theory, particle size, elastic collision, temperature, diffusion, Graham’s Law of Effusion (smaller molecules of gas diffuse faster)
Rate of Effusion: alpha * (molar mass)
-1/2
Rate
A/Rate
B=[(MolarMass
B)/(MolarMass
A]
1/2
pressure, barometer, pascal ( Pa, kPa ), atmosphere ( atm ), torr = mmHg,
Dalton’s Law of Partial Pressures
P
total = P1 + P2 + P3 + . . .
particle energy (kinetic energy or KE)
KE = ½ mv
2
Density of gas is low, can be compressed,
Gas pressure, barometer
Section 13.1 Gases
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Section 13.2 Forces of Attraction
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Section 13.3 Liquids and solids
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Section 13.4 Phase Changes
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Section 13.1 Gases
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Section 13.2 Forces of Attraction
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Section 13.3 Liquids and solids
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Section 13.4 Phase Changes
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Section 13.1 Gases
Standard 4 a - Gases and their Properties
View Standard 4 State Standard: The random motion of molecules and their collisions with a surface create the observable pressure on that surface.
Students Will be able to:Explain how molecular motion and collisions create pressure. Book Reference Pages: 386-389, 392
Standard 4 b - Gases and their Properties
View Standard 4 State Standard: The random motion of molecules explains the diffusion of gases.
Students Will be able to:Explain how molecular motion and collisions result in diffusion. Book Reference Pages: 387, 388
Standard 4 c - Gases and their Properties
View Standard 4 State Standard: How to apply the gas laws to relations between the pressure, temperature, and volume of any amount of an ideal gas or any mixture of ideal gases.
Students Will be able to:Solve mathematical problems using the gas laws. Perform an experiment and graph the data relating volume, temperature, and/or pressure. I&E (12E): Solve scientific problems using quadratic equations, and simple trigonometric, exponential, and logarithmic functions. Book Reference Pages: 391, 392
Standard 4 g - Gases and their Properties
View Standard 4 State Standard: The kinetic theory of gases relates the absolute temperature of a gas to the average kinetic energy of its molecules or atoms.
Students Will be able to:Book Reference Pages: 385, 386
Standard 4 i - Gases and their Properties
View Standard 4 State Standard: How to apply Dalton's Law of Partial Pressures to describe the composition gases, and Graham's Law to describe diffusion of gases.
Students Will be able to:Book Reference Pages: 387, 388, 391, 392
Standard 7 a - Chemical Thermodynamics
View Standard 7 State Standard: How to describe temperature and heat flow in terms of the motion of molecules (or atoms).
Students Will be able to:Explain temperature and heat flow in terms of the kinetic theory. Book Reference Pages: 386
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Section 13.2 Forces of Attraction
Standard 2 h - Chemical Bonds
View Standard 2 State Standard: How to identify solids and liquids held together by Van der Waals forces to volatility and boiling/melting point temperatures.
Students Will be able to:Describe how hydrogen bonding and Van der Waals forces effect physical properties such as boiling point, melting point, and volatility Book Reference Pages: 393-395
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Section 13.3 Liquids and solids
Standard 2 d - Chemical Bonds
View Standard 2 State Standard: In a liquid the inter-molecular forces are weaker that in a solid, so that the molecules can move in a random pattern relative to one another
Students Will be able to:Compare and contrast the intermolecular forces that determine the states of matter Book Reference Pages: 396, 397, 399, 403
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Section 13.4 Phase Changes
Standard 7 a - Chemical Thermodynamics
View Standard 7 State Standard: How to describe temperature and heat flow in terms of the motion of molecules (or atoms).
Students Will be able to:Explain temperature and heat flow in terms of the kinetic theory. Book Reference Pages: 404, 408, 409
Standard 7 c - Chemical Thermodynamics
View Standard 7 State Standard: Energy is released when a material condenses or freezes and absorbed when a material evaporates or melts.
Students Will be able to:Measure the energy changes that occur with changes of state. Book Reference Pages: 404, 408, 409
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- Tutorial on Effusion (also fits Diffusion): Two problems from the textbook on EFFISION (formula for DIFFUSION IS IDENTICAL) are worked out in detail with suggestions on general method to solve.
Ch 13.1 - KMT
● Kinetic Molecular Theory is demonstrated by this wonderful animation of diatomic gas molecules in a chamber separated by a thermally conductive wall (McDougal-Little - Classzone) Visit Site
● Ideal Island is a short video that helps us understand why and Ideal Gas is ideal. Visit Site
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Diffusion
● Diffusion applet for diffusion of perfume Visit Site
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Effusion
● Interactive applet effuses H2 or O2 for 30 sec Visit Site
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Hydrogen Bonding
● Hydrogen bonding animation w narration showing 3 H-bonded molecules. Also compares to boiling point in different groups (YouTube) Visit Site
● Hydrogen Bonding animation w narration. Explaination of NOF and H requirement to have H-bonding and shows how water molecules group, first in liq. form then in solid crystals. (YouTube) Visit Site
● Hydrogen Bonding - shows break and forming of hydrogen bonds between molecules (YouTube) Visit Site
● Java Applet showing forming & breaking of H-bonds between 2 water molecules Visit Site
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Wigger Vids
● This is a description of important points demonstrated in a video on Kinetic Molecular Theory Visit Site
● Graham's Law of Effusion Part 1, differentces between diffusion and effusion shown along with the basic formula for Graham's Law. 2 different gas simulators are used during the discussion Visit Site
● Graham's Law of Effusion - p. 878 #1, Part 2 of my 3 part series. Visit Site
● This is Part # 3 of my 4 part series on the Graham's Law of Effusion. p. 878 #2 from HW and shows how to square both sides of Graham's law to get solution. Visit Site
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