1. UNIT 1: MATTER AND ENERGY (Review Book Topic 4)
How does the proximity of atoms or molecules to each other affect properties they exhibit?
How can we explain phase changes in terms of energy?
How can we explain the behavior of gases?
How can we explain the behavior of gases in terms of pressure?
How can we explain the relationships between P,T, & V?
What kinds of matter are there, and how can you turn one form of matter into another form?
HONORS CHEMISTRY – MS. ARGENZIO

2. Thursday 9/11/14 – A DAY
AIM: How does the proximity of atoms or molecules to each other affect properties they exhibit?
DO NOW: Answer the following questions:
1. What is matter?
2. What are the different states of matter and list one example of each?

3. Phases of Matter

4. Lets Review……
What is matter???
Anything that:
Has mass
Takes up space

5. STATES OF MATTER
There are 3 states of matter

6. SOLIDS Particles tightly packed together
Particle Movement type: vibrate
Has definite shape
Has definite volume
If you put a sneaker in a box its volume doesn’t change

7. Examples

8. LIQUIDS Particles are moderately packed together
Particle movement: Vibrate and Rotate
No definite shape, Takes the shape of its container
Has Definite Volume

9. Examples

10. GAS (vapor) Particles are loosely packed
Particle movement: Vibrate, Rotate & bounce off container
Has No Definite Shape
Has No Definite Volume

11. Examples

12. Thursday 10/10/13 – C DAY
AIM: How can we explain phase changes in terms of energy?

13. Melting change from SOLID to LIQUID Heat is absorbed (ENDOTHERMIC)
Molecules spread out
Fusion
-no temp change even though energy is added
Average KE of particles remains the same
Particles absorb heat as Potential Energy

14. FREEZING change from LIQUID to SOLID Heat is removed (EXOTHERMIC)
Molecules get closer
Solidification
no temp change
P.E. decreases

15. HEAT OF FUSION
Amount of heat needed to melt a solid under normal conditions
Freezing requires same amount of heat as melting (it is released instead of absorbed)
Table T for equation: q = mHf

16. EVAPORATION LIQUID to GAS Heat is absorbed Molecules spread out
Vaporization
No change in temp
gain P.E.

17. CONDENSATION
GAS to LIQUID
Heat is removed
Molecules get closer

18. HEAT OF VAPORIZATION
Amount of heat needed to convert a liquid to gas under normal conditions
Condensation requires same amount of heat as vaporization (it is released instead of absorbed)
Table T for equation:q = mHv

19. SUBLIMATION/ DEPOSITION
Sublimation: SOLID to GAS
Molecules spread out
Deposition: GAS to SOLID
Molecules get closer

21. AIM: How can we represent/calculate the energy associated with phase changes? DO NOW: 1. Take out reference table, and pen/pencil and HW 2. Answer the following questions : - What phase changes are endothermic? - What phase changes are exothermic? - What happens to average kinetic energy during a phase change? Temperature? - What happens to potential energy during a phase change?

22. HEATING/COOLING CURVES
Graph of temp vs. Time
Showing the phase changes of a substance
Time increases but temp stays constant represent phase changes with no slope
Places with a slope indicate temp changes

23. HEATING/COOLING CURVES
Time

24. HEATING AND COOLING CURVE - QUESTIONS
What caused the water to change phases during this experiment?
What is happening at the two plateaus on the graph?
Why doesn’t the kinetic energy change at these spots?
The melting point of water occurs at the same temperature as the _________________________ point of water.
What other phase changes happen at the same temperature?
Heating the water
Phase change
Temperature doesn’t change
freezing
Condensation and Evaporation

25. Energy Changes Associated with Phase Changes
Energy: the ability to do work or produce heat
Types: Light energy ( radio waves, microwaves, etc.), heat, mechanical, chemical, nuclear etc.
Potential energy: Stored energy
Ex) ball at the top of a hill, chemical bonds (attachments) between atoms of a substance
Kinetic Energy: (KE) the energy of motion

26. Energy Changes Associated with Phase Changes
Temperature: Measure of average kinetic energy of the particles of a substance
Heat : The flow of energy due to a temperature difference.
Heat always flows from high temp to low temp
Kelvin Temperature: scale that is directly proportional to
average KE (See Table T )

27. Energy Changes Associated with Phase Changes – Heat Formulas
Heat of Fusion (q=mHf) : Clues to use this formula would be the following words- melting, freezing, solidification, crystallization, solid to liquid, liquid to solid (this value for water is located on Reference Table B)
Heat of Vaporization (q=mHv) : : Clues to use this formula would be the following words – evaporation, vaporization, condensation, liquid to gas, gas to liquid, steam (this value for water is located on Reference Table B)
Anytime there is a temperature change (a substance cooling or being heated) you would use the q=mcΔT
Where ΔT = Tfinal – Tinitial

28. HEAT CALCULATION PRACTICE

29. AIM: How can we explain the behavior of gases. DO NOW: 1
AIM: How can we explain the behavior of gases? DO NOW: 1. Take out reference table, and pen/pencil 2. Answer the following
2. Questions using heat calculations review book????

30. HEAT CALCULATION PRACTICE

31. KINETIC MOLECULAR THEORY
Scientists construct models to explain the behavior of substances
The Kinetic Molecular Theory (KMT) is a model that is used to explain the behavior of gases
It explains and/or describes the relationships among several variables used to analyze gases
The main variables that we discuss during this topic are pressure (P), volume (V), and temperature (T)

32. Kinetic Molecular Theory
Kinetic Molecular Theory: is a model or theory that is used to explain the behavior of gases

33. Kinetic Molecular Theory
Major Ideas and Assumptions of KMT
Gases contain particles that are in constant, random, straight-line motion.
Gas molecules collide with each other and the walls of their container (exerting pressure). The collisions are considered perfectly elastic ( the particles do not lose energy when they collide)

34. Kinetic Molecular Theory
Major Ideas and Assumptions of KMT
3. The particles of a gas sample are so small compared to the overall volume the sample occupies. Therefore, the particles’ individual volumes can be ignored (they have negligible volume)
4. Gas particles do not attract each other at all (do not exhibit intermolecular forces)

35. AIM: HOW CAN WE EXPLAIN THE BEHAVIOR OF GASES - IDEAL GAS BEHAVIOR
What does the kinetic molecular theory describe the behavior of: solids, liquids or gases?
What variables will be used during this topic?
What is temperature measured in?
List two ideas/assumptions from the KMT
Explain in terms of intermolecular forces why gas particles will completely fill up any container which it is placed in.

36. IDEAL GAS BEHAVIOR – how to get real gases to behave like ideal gases…
Use Hydrogen and Helium in experiments (they behave most ideally, they have smallest volume and weakest attraction)
Do experiments under condition of high Temperature and low Pressure (think Ideal vacation!) – PLIGHT!!!
PRESSURE
LOW
IDEAL
GAS
HIGH
TEMPERATURE

37. IDEAL GAS BEHAVIOR – Ideal vs. Real
IDEAL REAL
1. No volume Has volume
2. Continuous random straight line motion 2. Not always
3. No energy loss Some energy loss
4. No attractive forces Has attractive forces (weak)

38. GAS BEHAVIOR – Avogadros Hypothesis
Equal volumes of gases at the same temperature and pressure have the same number of molecules

39. AIM: How can we explain the relationships between P,T, & V?
The Gas Laws are relationships between temperature, pressure, and volume of a gas. Gas Law equations are used to determine what affect changing one of those variable will have on any of the others.

40. Gas laws- relationships AMONG VARIABLEs : Pv & t
Gases are unique in that they do not have a definite volume (solids and liquids do!)
That means we change the conditions at which a sample of gas exists (such as pressure around it or the temperature of the gas itself), we can change the volume of the gas sample

41. Gas laws- relationships AMONG VARIABLEs : Pv & t
In order to understand how the variables affect each other we need to keep one of the variables constant
Important assumption  the number of molecules is being kept constant as well (we have a closed container during the experiments)

42. AIM: How can we explain the relationships between P,T, & V? - PTV trick

43. AIM: How can we explain the relationships between P,T, & V?
Charles Law
Boyles Law
Gay – Lussacs Law

44. CHARLES LAW - http://www. youtube. com/watch. v=iSK5YlsMv4c http://www
Experiment # 1: Relationship between temperature and volume
Variable kept constant:
Describe what happened:
Draw a graph that shows the relationship:

45. Boyles LAW - http://www.youtube.com/watch?v=N5xft2fIqQU
Experiment # 2: Relationship between pressure and volume
Variable kept constant:
Describe what happened:
Draw a graph that shows the relationship:

46. Gay-Lussac's law - http://www.youtube.com/watch?v=ZDFF4HeuAAg
Experiment # 3 Relationship between pressure and temperature
Variable kept constant:
Describe what happened:
Draw a graph that shows the relationship:

47. AIM: How can we explain the relationships between P,T, & V
AIM: How can we explain the relationships between P,T, & V? - Combined Gas Law Equation
To solve gas law problems follow the steps:
Make a data table (Temp ALWAYS in Kelvin) P1 P2 V1 V2 T1 T2

48. AIM: How can we explain the relationships between P,T, & V
AIM: How can we explain the relationships between P,T, & V? - Combined Gas Law Equation
Write down the gas law equation
Circle the variable you are trying to solve for, and use basic algebra to rearrange the equation
Eliminate anything that is held constant
Substitute the numbers in the rearranged equation
Round off your answer using sig figs!

49. AIM: How can we explain the relationships between P,T, & V
AIM: How can we explain the relationships between P,T, & V? - Combined Gas Law Equation
A 2.00 L sample of gas at STP is heated to 500. K and compress to 200.kPa. What is the new volume of the gas?
A 2.00 L sample of gas at 1.00 atm and 300. K is heated to K and compressed to a volume of 1.00 L. What is the new pressure of the gas?

50. AIM: How can we explain the relationships between P,T, & V
AIM: How can we explain the relationships between P,T, & V? - Combined Gas Law Equation
A 2.00 L sample of gas at 300. K and a pressure of 80.0 kPa is placed into a 1.00 L container at a pressure of 240. kPa. What is the new temperature of the gas?
A sample of gas occupies a volume of 2.00 L at STP. If the pressure is increased to 2.00 atm att constant temperature, what is the new volume of the gas?

51. AIM: How can we explain the relationships between P,T, & V
AIM: How can we explain the relationships between P,T, & V? - Combined Gas Law Equation
A sample of gas occupies a volume of 5.00 L at 300. K. If the temperature is doubled under constant pressure, what will the new volume of the gas be?
A 10.0 L sample of gas in a rigid container at 1.00 atm and K is heated to 800. K. Assuming that the volume remains constant, what s the new pressure of the gas?

52. AIM: How can we explain the relationships between P,T, & V
AIM: How can we explain the relationships between P,T, & V? - Ideal Gas Law Equation
The pressure and volume of a gas are proportional to the number of moles of gas and the Kelvin temperature (n = number of moles, R = constant atm-L/mol-K)
Mole – unit of measurement like a dozen represents 12 eggs
Since one mole of gas exerts a pressure of 1 atm and occupies a volume of 22.4 L at 273 K- we can derive the value of R from this.

53. AIM: How can we explain the relationships between P,T, & V
AIM: How can we explain the relationships between P,T, & V? - Ideal Gas Law Equation
Examples:
What is the pressure exerted by 3.00 moles of gas at a temperature of 300. K in a 4.00 L container?
What is the volume of a sample of gas if 5.00 moles if it exerts a pressure of atm at 200. K?

54. AIM: How can we explain the relationships between P,T, & V
AIM: How can we explain the relationships between P,T, & V? - Ideal Gas Law Equation
Examples:
A sample of gas is contained in a cylinder with a volume of L. At what temperature will 2.50 moles of contained gas exert 20.0 atm of pressure on the container?
A sample of gas contained in a cylinder of 5.00 L exerts a pressure of 3.00 atm at 300. K. How many moles of gas are trapped in the cylinder?

55. PRESSURE  PRESSURE: force exerted over an area
Units: atmospheres (atm), kilopascals (kPa), millimeters of mercury (mmHg)
1 atm = kPa = 760 mmHg
Conversion Examples:
2.5 atm to kPa
123.4 kpa to atm

56. Vapor Pressure
VAPOR PRESSURE: the pressure exerted by a liquid’s vapor in a sealed container at a vapor-liquid equilibrium at a given temperature; it is not dependent on the mass or volume of the liquid. The vapor pressure of a liquid can be found on Reference Table H. The stronger the attractive force between liquid molecules, the lower the vapor pressure is.
Substances with high vapor pressure evaporate quickly, these substances are called volatile

57. Boiling Point
 BOILING POINT: the temperature at which a liquid’s vapor pressure equals the pressure exerted on the liquid by outside forces. Use Reference Table H to determine a liquid’s boiling point. Boiling point increases as exerted pressure is increased.
NORMAL BOILING POINT: the boiling point of a liquid under a pressure of 1.00 atmospheres
** substances with higher boiling points have stronger intermolecular forces, holding the molecules closer together, requiring more energy to overcome the attractive forces **

58. How to Use Table H

59. How to Use Table H

60. AIM: How can we explain the behavior of gases in terms of pressure
AIM: How can we explain the behavior of gases in terms of pressure? – Daltons Law of Partial Pressure
Daltons Law of Partial Pressures: The total pressure exerted by a mixture of gases is equal to the sum of the pressures exerted by each of the gases in the mixture
 PTOTAL = PA + PB + PC + …..

61. AIM: How can we explain the behavior of gases in terms of pressure
AIM: How can we explain the behavior of gases in terms of pressure? – Daltons Law of Partial Pressure
Examples:
What is the total pressure of a mixtues of O2 (g), N2 (g) and NH3 (g) if the pressure of the O2 (g) is 20. kPa, N2 (g) is 60. kPa and the NH3 (g) is 15 kPa?
A mixture of 1 mole of O2 and 2 moles of N2 exerts a pressure of 150 kPa. What is the partial pressure of each gas?

62. AIM: How can we explain the behavior of gases in terms of pressure
AIM: How can we explain the behavior of gases in terms of pressure? – Grahams Law of Effusion and Diffusion
Diffusion: used to describe the mixing of gases; the rate of diffusion is the rate of mixing (picture below)

63. AIM: How can we explain the behavior of gases in terms of pressure
AIM: How can we explain the behavior of gases in terms of pressure? – Grahams Law of Effusion and Diffusion
Effusion: describes the passage of gas through a tiny orifice into an evacuated chamber; the rate of effusion measures the speed at which the gas is transferred (picture to the right)

64. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Classification of matter

65. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Classification of matter
SUBSTANCES (elements and compounds): are all HOMOGENEOUS (containing the same composition of material throughout the sample)
Elements: substances that cannot be broken down by chemical change (symbols are on Periodic Table) Ex. N (nitrogen) Ni (nickel)
Compounds: substances that are made up of elements chemically bonded together, can be decomposed by chemical means. (Two or more element symbols combined) Ex. NaCl (sodium and chlorine) constant composition
MIXTURES: combination of substances that are not chemically combined together, and can be broken down by physical means ratio will vary

66. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Classification of matter
MIXTURES: combination of substances that are not chemically combined together, and can be broken down by physical means ratio will vary
Homogeneous Mixture: (SOLUTION) uniform composition Ex: salt water
Heterogeneous Mixture: non uniform composition Ex: sand water

67. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Particle Diagrams

68. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Particle Diagrams

69. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Separation of Mixtures
Filtration: separate solid from liquid or liquid
from gas, or two immiscible (not capable of mixing) liquids
Distillation: separate two miscible (capable of mixing) liquids, solids and liquids in homogeneous mixtures, separate out gases

70. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Separation of Mixtures
Chromatography: used to separate the components of a mixture based on attraction for substances not in the mixture (gas chromatography, paper chromatography)

71. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Physical Properties and Changes
Physical Changes: changes that change only the appearance of the substance, not its chemical identity
Physical Properties: properties that can be observed though physical change

72. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Physical Properties and Changes

73. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Chemical Properties and Changes
Chemical Changes: changes that result in changing the chemical composition of a substance, can be reversed by another chemical change – results in a new substances being formed
Chemical Properties: properties that can only be observed through a chemical change

74. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Law of Conservation
MATTER CANNOT BE CREATED NOR DESTROYED, BUT CAN CHANGE FROM ONE FORM TO ANOTHER

75. AIM: What kinds of matter are there, and how can you turn one form of matter into another form? – Law of Conservation
Examples:
If 40 grams of substance A are reacted with 20 grams of substance B to form substance C, what will the mass of substance C be?
35 grams of liquid water are evaporated off in a closed container. How many grams of water vapor will there be when the process is done?
Magnesium metal is reacted with oxygen to form magnesium oxide. How will the mass of the magnesium oxide be compared to the combined masses of the magnesium metal and the oxygen that formed it?