States of Matter Chapter 3 Pg. 68-91

Solids, Liquids, and Gases Chapter 3 Section 1 Pg. 68-74

Describing the States of Matter Materials can be classified as _____, liquids, or gases based on whether their shapes and _______ are definite or ________

States of Matter SOLIDS Definite _____ Definite ______ Changing the container doesn’t change the shape or volume Atoms are packed close together and are arranged in a _______ pattern

States of Matter LIQUIDS Definite ________ ___ definite shape Takes the _____ of its container Atoms are close together, but arrangement is more _______

States of Matter GASES ___ definite shape NO definite _______ Takes shape of _________ More space between atoms, ___ arranged in a regular pattern (scattered)

OTHER States of Matter PLASMA At extremely ____ temperatures, such as those found on the sun or other stars, matter exists as ______. BOSE-EINSTEIN CONDENSATE (BEC)- est. 1995 Predicted by _______ At extreme ___ temperatures (-273°C) atoms behave as though they were a single particle

KINETIC THEORY Kinetic ______- the energy an object has due to its motion Kinetic Theory of matter says that __ particles of matter are in constant ______.

Behavior of Gases Motion in Gases Particles in a ___ are never at ____ Atoms move in a straight line until it _______ with another atom or with a wall of the container One atom may ____ kinetic energy while the other atom _____ kinetic energy There are forces of attraction among the particles in ALL matter

Kinetic Theory of Gases Behavior of Gases Kinetic Theory of Gases The constant motion of particles in a gas allows a gas to ____ a container of any shape or size. Particles in a gas are in constant, random ______. The motion of ___ particle is unaffected by the motion of other particles unless the particles ______. Forces of attraction among particles in a gas can be ______ under ordinary conditions.

Behavior of Liquids Particles in a liquid are more closely ______. A liquid takes the shape of its container because particles in a liquid can ____ to new locations. The ______ of a liquid is constant because forces of attraction keep the particles _____ together.

Behavior of Solids ______ have a definite volume and shape because particles in a solid ______ around ____ locations.

The Gas Laws Chapter 3 Section 2 Pg. 75-81

Pressure Pressure is the result of a _____ distributed over an ____. Pressure = Force/area Force is measured in _______ (N) Area is measured in square meters (m2) Pressure is N/m2, the SI unit is ______ (Pa) 1 kPa = 1000 Pa

Pressure _________ between particles of a gas and the walls of the ________ cause the pressure in a closed container of gas. More frequent collisions = ______ pressure Speed and mass of particles also affect pressure

Factors that Affect Gas Pressure Factors that affect the pressure of an enclosed gas are its __________, its volume, and the _____ of its particles

Factors that Affect Gas Pressure Temperature _______ the temperature of a gas will ______ its pressure if the volume of the gas and the number of particles are _______. Ex: Tires on highway- temp. rises -> kinetic energy increases-> particles move faster and collide more-> hit with greater force-> increase in pressure

Factors that Affect Gas Pressure Volume _______ the volume of a gas increases its pressure if the _______ of the gas and the number of particles are _______. Ex: your lungs and diaphragm when you breathe

Factors that Affect Gas Pressure Number of Particles ______ the number of particles will _____ the pressure of a gas if the temperature and the volume are ______. Ex: inflating tires

Boyle’s Law Relationship between _______ and ______ of a gas Boyle’s Law states that the volume of a gas is ______ proportional to its _______ if the temperature and the number of particles are _______. P1V1 = P2V2

Boyle’s Law Example: To make an air horn, 1.50 L of air at 101 kPa are compressed into a can with a volume of 0.462 L. Assuming a constant temperature, what is the pressure on the compressed air? Given: P1= 101 kPa, V1= 1.50 L, V2= 0.462 L Unknown: P2= ? P1V1 = P2V2 P1V1 P2= V2

Boyle’s Law P1V1 P2= V2 P2= (101 kPa)(1.50 L) 0.462 L P2= ____ kPa

Temperatures must be expressed in ______ Charles’s Law Charles’s Law states that the _____ of a gas is ______ proportional to its temperature in kelvins if the pressure and the number of particles of the gas are ______. Temperatures must be expressed in ______

Charles’s Law Example: The volume of a gas is 7.5 L at a temperature of 435 K. What will the volume of the gas be if the temperature is lowered to 300 K? Given: V1= 7.5 L T1= 435 K T2= 300 K Unknown: V2=?

Boyle’s Law Graph Charles’s Law Graph See pg. 78 for example of each graph

Combined Gas Laws The combined gas law describes the _________ among the temperature, volume, and pressure of a gas when the number of _______ is constant.

Combined Gas Laws Example: A child has a toy balloon with a volume of 1.80 L. The temperature of the balloon when it was filled was 20°C and the pressure was 1.00 atm. If the child were to let go of the balloon and it rose into the sky where the pressure is 0.667 atm and the temperature is -10°C, what would the new volume of the balloon be? Given: V1= 1.80 L T1= 273+20= 293K P1= 1.0 atm P2= 0.667 atm T2= 273+(-10)= 263K Unknown: V2= ?

Combined Gas Laws Given: V1= 1.80 L T1= 273+20= 293K P1= 1.0 atm P2= 0.667 atm T2= 273+(-10)= 263K Unknown: V2= ? P1V1 = P2V2  (1.0atm)(1.80L) = (0.667atm)V2 T1 T2 (293K) (263K) (1.0atm)(1.80L)(263K) = (0.667atm)(293K)V2 (0.667atm)(293K) (0.667atm)(293K) V2= 2.42 L

Phase Changes Chapter 3 Section 3 Pg. 84-91

Characteristics of Phase Changes A phase change is the __________ physical change that occurs when a substance changes from one _____ of matter to _______. Melting, freezing, vaporization, condensation, sublimation, and deposition are 6 common phase changes. ___ phase changes share certain characteristics related to ______ and temperature.

Temperature and Phase Changes The temperature of a substance does ___ change during a phase change. Temperature remains _______ until phase change is complete.

Temperature and Phase Changes

Energy and Phase Change During a phase change, energy is ________ between a substance and its surroundings. Energy is either _______ or ________ during a phase change.

Energy and Phase Change ___________- during an endothermic change, the system ______ energy from its __________ Heat of Fusion- the _______ of energy absorbed (Fusion is another term for _______)

Energy and Phase Change _________- during an exothermic change, the system ______ energy to its surrounding.

Energy and Phase Change

Melting and Freezing The arrangement of molecules in water becomes ___________ as water melts and more orderly as water _______.

Melting and Freezing _________ When ice cubes are removed from a freezer and placed in an empty glass, heat flows from the air to the ice. As the ice gains energy, the molecules ______ more quickly.

Melting and Freezing Freezing When liquid water is placed in a freezer, _____ flows from the water to the air in the freezer, and the water cools down. As the average ______ energy of its molecules decreases, they move more ______.

Vaporization and Condensation The phase change in which a substance changes from a liquid to a gas is __________. This amount of energy is the heat of vaporization; ___________ Evaporation takes place at the ______ of a liquid and occurs at temperatures _____ the boiling point.

Vaporization and Condensation Evaporation is the process that changes a substance from a _____ to a ___ at temperatures below the substance’s boiling point. The greater the surface area of the container, the _____ the water evaporates. Vapor pressure the pressure caused by the __________ of vapor and the walls of the container

Vaporization and Condensation Boiling As you heat a pot of water, both the temperature and the vapor pressure of the water _______. When the vapor pressure becomes ______ to atmospheric pressure, the water boils. Boiling point of a substance depends on the __________ pressure BP of water in Denver is 95°C

Vaporization and Condensation Condensation is the phase change in which a substance changes from a ___ or vapor to a _____ Condensation is an __________ process

Sublimation and Deposition Sublimation is the phase change in which a substance changes from a ____ to a ___ or vapor _______ changing to a liquid first. Sublimation is an ___________ change

Sublimation and Deposition Deposition when a ___ or vapor changes directly into a _____ without first changing to a liquid Deposition is an ___________ phase change