1. States of matter and thermodynamics

2. Solid
Does not flow.
Definite shape.
Definite volume.

3. Liquid It flows. Takes on the shape of its container.
Has a definite volume.

4. Gas It flows. Takes on the shape of its container
Has NO definite volume. Always fills the container it’s in.

5. pHet States of Matter Lab

6. 4/7/11 – “C” Day
Objective: To understand the relationships between pressure, temperature, and kinetic energy.
Do Now: Sketch a graph showing the relationship between Temperature and Kinetic Energy of Particles. Where would you place a solid, liquid and a gas on this graph?
Today:
Complete Test Corrections
Complete Phet States of Matter Activity
Intermolecular Forces - HW

7. 4/8/11 – “D” Day
Objective: To understand the relationships between pressure, temperature, and kinetic energy.
Do Now: In our Weblab – Why did some particles stick together and others not? What do you think this did to the temperature needed to turn from a solid  liquid or liquid  gas?
Today:
Collect Intermolecular Forces – HW
Discuss Phet States of Matter Activity
States of Matter Notes
Gases Lab

8. Kinetic theory and phases of matter
Kinetic theory – all matter is made up of tiny particles that are constantly in motion. Remember kinetic = motion
Energy is Directly Related to Temperature
Remember q (heat or energy) = mcΔT

9. What determines if something is a solid, liquid or gas?
Temperature
Pressure
Intermolecular Forces

10. Temperature Average KE per molecule in a substance.
Measure w/ thermometer. Alcohol in thermometer expands as it is heated.
Units:
Fahrenheit
Celsius
Kelvin

11. Temperature
Temperature is related to the random motion of atoms & molecules in a substance.
(Molecules will refer to : atoms & molecules)
↑ Temp = ↑ average KE of molecules
↓ Temp = ↓ average KE of molecules

12. Temperature
Q: Consider 1L vs 2L of boiling water. Which has a higher temperature?
A: Same temp. Average KE of molecules is the same.

13. Absolute Zero Temp has no upper limit. Stars (plasma): MANY MILLION °C
Absolute Zero- Nature’s lowest possible temperature.
0 Kelvin = -273 ° C
Molecules lost all available KE. No motion
No more E can be removed…. Can’t get any colder than this!

15. Heat and temperature
Heat- the thermal energy transferred from one substance to another due to a temperature difference (Av. KE) between the molecules of two substances.

16. Heat and Temperature
Temperature is the average kinetic energy in a system
Heat is the transfer of energy between objects because of the difference in temperature
Heat transfers spontaneously from hot to cold

17. Which has the higher temperature, 1 L or 2 L of boiling water?
Which has more energy?

18. Intermolecular Forces
Attraction between particles
Ionic bonds
Hydrogen bonds
Van der waal’s forces

19. Ionic bonds
Ionic compounds are not arranged in molecules, but instead form large crystals held together
by ionic bonds.
Charge on ions
provides
attraction.

20. Hydrogen bonds
Covalent molecules form solids when intermolecular forces are great enough to hold molecules together, usually as a crystal.
Strongest intermolecular force is hydrogen bonding, between the H of one molecule, and an N, O or F of another. These molecules are very polar and have strong + and - ends

21. Water – example of H bonds
The dashed lines are the hydrogen bonds in an ice crystal

22. Van der waal’s forces
Other molecules are attracted by weaker dipole and London dispersion forces. These forces are also between positive and negative ends of a molecule, but the charges are usually much smaller than in hydrogen bonds.

23. Dipole-Dipole

24. Solids
Held together by intermolecular forces in highly organized patterns.
Dense and incompressible
Do not flow

25. Liquids
Intermolecular forces hold particles together, but particles are not locked in place. Can move freely through the liquid. This allows the liquid to flow, but keeps the volume constant.

26. Gases
Particles in constant rapid motion, independent of each other. Gases are not held together by intermolecular forces, do not have a constant shape or volume

28. Liquids and Kinetic Theory
Liquids have three properties that relate to the Kinetic Theory:
Evaporation
Vapor pressure
Boiling point

29. Evaporation
Remember, temperature is a measure of the average kinetic energy.
Some particles have more kinetic energy
Particles with a high enough kinetic energy can break free from the surface and become a gas

30. Vapor Pressure
In a closed system, molecules move back and forth between liquid and gas.

31. Vapor pressure
The vapor pressure is a measure of how much gas there is at a given temperature.
The higher the
temperature, the
higher the vapor
pressure

32. Boiling point
Boiling occurs at specific temperatures and pressures. Pockets of gas form in the liquid as bubbles and move to the surface.

33. Boiling point
When the vapor pressure equals the atmospheric pressure the liquid boils

34. Changes of state Solid to liquid – melting Liquid to solid – freezing
Liquid to gas – evaporation
Gas to liquid – condensation
Solid to gas - sublimation

35. Construct a heating curve for water
Heating curve lab

36. Heating curve
What is happening between B and C?

37. Heat of Fusion Energy required to go from a solid to a liquid
at the same temperature.
Between B and C, energy is being used to melt the material

38. Heat of Fusion 100/18 = 5.6 moles 5.6 moles *6.01kJ/1 mole = 33.66 kJ
How many Joules are required to melt 100 g of ice at 0°C? Heat of fusion for water is 6.01kJ/mole
How many moles of water is 100g?
100/18 = 5.6 moles
5.6 moles *6.01kJ/1 mole = kJ

39. What is happening between D and E?

40. Heat of vaporization Energy required to go from a liquid to a solid
at the same temperature.
Between D and E, energy is being used to evaporate (boil) the material

41. Heat of vaporization 150/18 = 8.3 moles
How many Joules are required to convert 150 g of water at 100°C to steam? Heat of vaporization for water is 40.67kJ/mole
How many moles of water is 150g?
150/18 = 8.3 moles
8.3 moles *40.67kJ/1 mole = kJ

42. Sublimation
Under certain conditions, a material can go directly from a solid to a gas. This is called sublimation.
Air freshener mini lab