Chapter 3 – States of Matter

I. Solids, Liquids, and Gases

A. Describing the states of matter. I. Solids, Liquids, and Gases 3.1 Solids, Liquids, and Gases A. Describing the states of matter. What are the three most common states of matter? Solid Liquid Gas How would you describe what these states are to someone who didn’t know?

A. Describing the states of matter. 1. Solids 3.1 Solids, Liquids, and Gases I. Solids, Liquids, and Gases A. Describing the states of matter. 1. Solids - definite shape - definite volume Atoms in a solid are packed close together in an orderly arrangement

A. Describing the states of matter. 2. Liquids I. Solids, Liquids, and Gases A. Describing the states of matter. 2. Liquids - variable shape (takes shape of container) - definite volume Atoms in a liquid are free to move around one another

A. Describing the states of matter. 3. Gases I. Solids, Liquids, and Gases A. Describing the states of matter. 3. Gases - variable shape (takes shape of container) - variable volume (fill container) Atoms in a gas are far apart from one another and free to move around

A. Describing the states of matter. 4. Other states of matter I. Solids, Liquids, and Gases A. Describing the states of matter. 4. Other states of matter Plasmas Bose-Einstein Condensate (BEC)

kinetic energy (KE) – energy an object has due to its motion I. Solids, Liquids, and Gases B. Kinetic Theory kinetic energy (KE) – energy an object has due to its motion the faster an object moves the more kinetic energy it has all particles of matter in constant motion the particles in all matter are attracted to one another

I. Solids, Liquids, and Gases Kinetic Theory

C. Explaining the Behavior of Gases I. Solids, Liquids, and Gases C. Explaining the Behavior of Gases gas particles have a great deal of kinetic energy constant motion allows a gas to fill its container the particles are moving too fast for attractions to have any effect variable volume variable shape

D. Explaining the Behavior of Liquids I. Solids, Liquids, and Gases D. Explaining the Behavior of Liquids liquid particles have less KE than gas particles liquid particles are more closely packed compared to a gas there is a tug-of-war between particle motion and particle attraction definite volume variable shape

E. Explaining the Behavior of Solids I. Solids, Liquids, and Gases E. Explaining the Behavior of Solids solid particles have the least KE solid particles very closely packed solid particles only vibrate around fixed positions definite volume definite shape

I. Solids, Liquids, and Gases

- force distributed over an area II. The Gas Laws 3.2 The Gas Laws A. Pressure - force distributed over an area - measured in Pascals (N/m2)

The atmosphere’s pressure is measured using a barometer. 3.2 The Gas Laws II. The Gas Laws The atmosphere’s pressure is measured using a barometer.

II. The Gas Laws 3.2 The Gas Laws

Collisions of gas particles with container walls cause pressure 3.2 The Gas Laws II. The Gas Laws Collisions of gas particles with container walls cause pressure

B. Factors affecting gas pressure (there are 3) II. The Gas Laws 3.2 The Gas Laws B. Factors affecting gas pressure (there are 3) Basketball goes flat after using it for awhile in the cold weather, until you warm it up 1. Temperature - higher T, greater pressure - increased temperature increases KE of particles - particles move faster, collide with walls more

3 factors affecting gas pressure 3.2 The Gas Laws II. The Gas Laws 3 factors affecting gas pressure 2. Volume As the volume is decreased the air pressure inside is increased - lower V, greater pressure - decrease volume, particles collide with walls more often

3 factors affecting gas pressure 3.2 The Gas Laws II. The Gas Laws 3 factors affecting gas pressure As more particles are added the pressure increases 3. Number of particles - more particles, greater pressure - more particles to collide with walls more often

- as temperature increases, volume increases 3.2 The Gas Laws II. The Gas Laws C. Charles’s Law – The volume of a gas is directly proportional to its temperature in Kelvins - as temperature increases, volume increases

Absolute zero – 0 Kelvin (can’t get any colder) 3.2 The Gas Laws II. The Gas Laws Absolute zero – 0 Kelvin (can’t get any colder) Charles’s Law

- as volume decreases, pressure increases 3.2 The Gas Laws II. The Gas Laws D. Boyle’s Law – The volume of a gas is inversely proportional to its pressure - as volume decreases, pressure increases

3.2 The Gas Laws II. The Gas Laws Boyle’s Law

Algebra Practice AB = XY Solve for X 4B = X-Y Solve for X 2AB = XY Solve for A A = X Solve for A B Y A = X Solve for X

Algebra Practice AB = XY Solve for X 4B = X-Y Solve for X 2AB = XY Solve for A A = X Solve for A B Y A = X Solve for X = AB / Y = 4B + Y = XY / 2B = BX / Y = AY / B

P1V1 = P2V2 T1 T2 E. Combined Gas Law 3.2 The Gas Laws II. The Gas Laws E. Combined Gas Law - a combination of Charles’ and Boyle’ Laws P1V1 = P2V2 T1 T2

Units Pressure: Pascals (Pa) OR atmosphere (atm) Volume: Liters (L) OR meters cubed (m3) Temperature: Celsius (C) OR Kelvin (K)

The Gas Laws V1 = V2 T1 T2 P1 V1 = P2 V2 P1 V1 = P2 V2 T1 T2 Charles’s Law Boyle’s Law Combined Gas Law

Solving Gas Law Problems Write the name of the law that applies. Write a description what is happening in the problem. Write the equation of the law that applies. Plug in all known values into the equation Solve the equation

Solving Gas Law Problems Write the name of the law that applies. Write a description what is happening in the problem. Write the equation of the law that applies. Plug in all known values into the equation Solve the equation Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!)

Solving Gas Law Problems Write the name of the law that applies. Write a description what is happening in the problem. Write the equation of the law that applies. Plug in all known values into the equation Solve the equation Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!) Charles’s Law (relates T and V) Boyle’s Law (relates P and V)

Solving Gas Law Problems Write the name of the law that applies. Write a description what is happening in the problem. Write the equation of the law that applies. Plug in all known values into the equation Solve the equation Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!) Charles’s Law (relates T and V)

Solving Gas Law Problems Write the name of the law that applies. Write a description what is happening in the problem. Write the equation of the law that applies. Plug in all known values into the equation Solve the equation Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!) Volume getting bigger, temperature changing

Solving Gas Law Problems Write the name of the law that applies. Write a description what is happening in the problem. Write the equation of the law that applies. Plug in all known values into the equation Solve the equation Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!) V1 = V2 T1 T2 P1 V1 = P2 V2

Solving Gas Law Problems Write the name of the law that applies. Write a description what is happening in the problem. Write the equation of the law that applies. Plug in all known values into the equation Solve the equation Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!) V1 = V2 T1 T2

Solving Gas Law Problems Write the name of the law that applies. Write a description what is happening in the problem. Write the equation of the law that applies. Plug in all known values into the equation Solve the equation Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!) 3.00 = 5.00 300 T2

Solving Gas Law Problems Write the name of the law that applies. Write a description what is happening in the problem. Write the equation of the law that applies. Plug in all known values into the equation Solve the equation Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!) 3.00 = 5.00 300 T2 T2 = 300(5.00) 3.00 3.00(T2) = 300(5.00)

Solving Gas Law Problems Write the name of the law that applies. Write a description what is happening in the problem. Write the equation of the law that applies. Plug in all known values into the equation Solve the equation Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!) T2 = 500

Solving Gas Law Problems Write the name of the law that applies. Write a description what is happening in the problem. Write the equation of the law that applies. Plug in all known values into the equation Solve the equation Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!) T2 = 500 K

P1V1 = P2V2 T1 T2 E. Combined Gas Law 3.2 The Gas Laws II. The Gas Laws E. Combined Gas Law P1V1 = P2V2 T1 T2

Section 3.2

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Section 3.2

Section 3.2

Section 3.2

Section 3.2

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Section 3.2

Riding on Air II. The Gas Laws 3.2 The Gas Laws What gases have been used in balloons that carry passengers? Why do the particles of a gas inside a balloon fill the entire balloon? What causes a hot-air balloon to lift off and rise from a surface? Why did Piccard design the balloon so that it could become airborne when it was only partially filled? Why must the air pressure inside the cabin be controlled?

A. Characteristics of Phase Changes III. Phase Changes A. Characteristics of Phase Changes Phase Change – substance changes from one state to another (it is a reversible physical change)

III. Phase Changes

1. Temperature and Phase Changes: III. Phase Changes 1. Temperature and Phase Changes: We can use temperature as a way to determine when a phase change is taking place The temperature of a substance does not change during a phase change

III. Phase Changes Figure 16

The temperature of a substance does not change during a phase change. III. Phase Changes The temperature of a substance does not change during a phase change. Instead the energy added is used to overcome the attractions between molecules

The temperature of a substance does not change during a phase change III. Phase Changes The temperature of a substance does not change during a phase change Time (minutes) Temperature (ºC) boiling (100 ºC) melting (0 ºC)

III. Phase Changes Time (minutes) Temperature (ºC)

III. Phase Changes 2. Energy and Phase Changes + = SOLID LIQUID

III. Phase Changes 2. Energy and Phase Changes + = LIQUID GAS

2. Energy and Phase Changes III. Phase Changes 2. Energy and Phase Changes Energy is absorbed or released during a phase change Endothermic change - energy absorbed by a substance Melting is an example of an endothermic change

Energy is absorbed or released during a phase change III. Phase Changes Energy is absorbed or released during a phase change Exothermic change - energy is released by a substance Freezing is an example of an exothermic change

III. Phase Changes B. Melting and Freezing The arrangement of molecules in water becomes less orderly as water melts and more orderly as water freezes.

The arrangement of molecules becomes LESS orderly III. Phase Changes 1. Melting melting (Endothermic) The arrangement of molecules becomes LESS orderly

The arrangement of molecules becomes MORE orderly III. Phase Changes 2. Freezing freezing (Exothermic) melting The arrangement of molecules becomes MORE orderly

Attractions between particles have an effect III. Phase Changes Freezing Attractions between particles have an effect

C. Vaporization and Condensation III. Phase Changes C. Vaporization and Condensation Vaporization - change from liquid to a gas - two types of vaporization Condensation – change from gas to liquid

Molecular arrangement less orderly III. Phase Changes Vaporization vaporization (Endothermic) melting freezing Molecular arrangement less orderly

Two Types of Vaporization III. Phase Changes Two Types of Vaporization 1. Evaporation – takes place at the surface of liquid

Two Types of Vaporization III. Phase Changes Two Types of Vaporization 1. Evaporation – takes place at the surface of liquid

Two Types of Vaporization III. Phase Changes Two Types of Vaporization Evaporation - takes place at the surface of liquid - can occur at temperatures below boiling. Vapor pressure – pressure exerted by the vapor above a liquid

Two Types of Vaporization III. Phase Changes Two Types of Vaporization 2. Boiling – bubbles form within the liquid when the vapor pressure equals atmospheric pressure

III. Phase Changes Vaporization

Molecular arrangement more orderly III. Phase Changes 3. Condensation condensation (Exothermic) melting freezing vaporization Molecular arrangement more orderly

C. Sublimation and Deposition III. Phase Changes C. Sublimation and Deposition Sublimation – change from solid to a gas Deposition – change from a gas to a solid

Molecular arrangement less orderly III. Phase Changes Sublimation sublimation (Endothermic) melting freezing vaporization condensation Molecular arrangement less orderly

Molecular arrangement more orderly III. Phase Changes Deposition deposition (Exothermic) melting freezing vaporization condensation sublimation Molecular arrangement more orderly

Sublimation and Deposition III. Phase Changes Sublimation and Deposition

III. Phase Changes 1. Why would Earth’s weather be much different without water? 2. When water freezes, it behaves differently than other substances. How so? 3. Why does water behave as you explained in the previous question? 4. If water didn’t behave this way when it froze, what would happen to all the aquatic life in a pond during the wintertime? 5. Is it possible that some very deep ponds and lakes would never completely thaw out? 6. What is a popcorn hull? 7. Why does popcorn pop? 8. Does the method by which popcorn pops remind you of any particular gas law? It should!! Which one? 9. What prevents some popcorn kernels from popping? Does the popping of a corn kernel require an exothermic or endothermic change of water?

III. Phase Changes liquid Charles’s law condensation exothermic solid absolute zero endothermic vapor pressure deposition pressure Boyle’s law kinetic energy evaporation phase change vaporization gas sublimation

Chapter 3 Vocabulary liquid Charles’s law exothermic solid absolute zero endothermic vapor pressure deposition pressure Boyle’s law kinetic energy evaporation phase change vaporization gas sublimation

Chapter 3 Vocabulary liquid Charles’s law exothermic absolute zero endothermic vapor pressure deposition pressure Boyle’s law kinetic energy evaporation phase change vaporization gas sublimation

Chapter 3 Vocabulary liquid Charles’s law exothermic absolute zero endothermic vapor pressure deposition pressure Boyle’s law evaporation phase change vaporization gas sublimation

Chapter 3 Vocabulary liquid Charles’s law exothermic absolute zero endothermic vapor pressure pressure Boyle’s law evaporation phase change vaporization gas sublimation

Chapter 3 Vocabulary liquid Charles’s law absolute zero endothermic vapor pressure pressure Boyle’s law evaporation phase change vaporization gas sublimation

Chapter 3 Vocabulary liquid Charles’s law absolute zero endothermic vapor pressure pressure Boyle’s law evaporation vaporization gas sublimation

Chapter 3 Vocabulary liquid Charles’s law absolute zero endothermic vapor pressure Boyle’s law evaporation vaporization gas sublimation

Chapter 3 Vocabulary liquid Charles’s law endothermic vapor pressure Boyle’s law evaporation vaporization gas sublimation

Chapter 3 Vocabulary liquid Charles’s law endothermic vapor pressure evaporation vaporization gas sublimation

Chapter 3 Vocabulary liquid Charles’s law vapor pressure evaporation vaporization gas sublimation

Chapter 3 Vocabulary Charles’s law vapor pressure evaporation vaporization gas sublimation

Chapter 3 Vocabulary Charles’s law vapor pressure evaporation gas sublimation

Chapter 3 Vocabulary Charles’s law vapor pressure gas sublimation

Chapter 3 Vocabulary Charles’s law gas sublimation

Chapter 3 Vocabulary Charles’s law sublimation

Chapter 3 Vocabulary sublimation