kinetic theory and states of matter chapter 13 section 13.1 gases use the kinetic-molecular theory...

Section 13.1 Gases

• Use the kinetic-molecular theory to explain the behavior of gases and introduce Gas Laws

Review Vocabulary

kinetic energy: energy due to motion

• Explain how gas pressure is measured

The Kinetic-Molecular Theory

• The kinetic-molecular theory describes the behavior of matter in terms of particles in motion.

Section 13-1Section 13-1

Explaining the Behavior of Gases• Great amounts of space exist between

gas particles.• Compression reduces the empty spaces

between particles.

Explaining the Behavior of Gases (cont.)

• Gases easily flow past each other because there are no significant forces of attraction.

• Diffusion is the movement of a material across a concentration gradient

Temperature is a measure of the average kinetic energy of the particles in a sample of matter.

The Kinetic-Molecular Theory (cont.)

• Kinetic energy of a particle depends on mass and velocity.

Gas Pressure

• Pressure is defined as force per unit area.

• Gas particles exert pressure when they collide with the walls of their container.

https://www.youtube.com/watch?v=t-Iz414g-ro

https://www.youtube.com/watch?v=kkUvU-elGtw



https://www.youtube.com/watch?v=kkUvU-elGtw


Gas Pressure (cont.)

• The particles in the earth’s atmosphere exert pressure in all directions called air pressure.

• There is less air pressure at high altitudes because there are fewer particles present, since the force of gravity is less.


• The SI unit of force is the newton (N).

• One Pascal (Pa) is equal to a force of one Newton per square meter or N/m2.

• One atmosphere is equal to 760 mm Hg or 101.3 kilopascals.

• https://www.youtube.com/watch?v=GRxglLS1YWI

https://www.youtube.com/watch?v=GRxglLS1YWI


• Torricelli invented the barometer.

• Barometers are instruments used to measure atmospheric air pressure.


Ptotal = P1 + P2 + P3 +...Pn

• Partial pressure can be used to calculate the amount of gas produced in a chemical reaction.

Section 13.2 Forces of Attraction

• Describe intramolecular forces.

polar covalent: a type of bond that forms when electrons are not shared equally• Compare and contrast

intermolecular forces.

Intermolecular forces—including dispersion forces, dipole-dipole forces, and hydrogen bonds—determine a substance’s state at a given temperature.


Intermolecular Forces

• Attractive forces between molecules cause some materials to be solids, some to be liquids, and some to be gases at the same temperature.

http://education-portal.com/academy/lesson/metallic-bonding-the-electron-sea-model-why-metals-are-good-electrical-conductors.html

https://www.youtube.com/watch?v=XHV9LzCH2KAhttps://www.youtube.com/watch?v=eVv3TpaQ2-A

https://www.youtube.com/watch?v=XHV9LzCH2KA



https://www.youtube.com/watch?v=eVv3TpaQ2-A

https://www.youtube.com/watch?v=eVv3TpaQ2-A


Intermolecular Forces (cont.)

• London Dispersion forces are weak forces that result from temporary shifts in density of electrons in electron clouds.


• Dipole-dipole forces are attractions between oppositely charged regions of polar molecules.


• Hydrogen bonds are special dipole-dipole attractions that occur between molecules that contain a hydrogen atom bonded to a small, highly electronegative atom with at least one lone pair of electrons, typically fluorine, oxygen, or nitrogen.


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Section 13.2 Assessment

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Which of the following molecules can form hydrogen bonds?

A. CO2

B. C2H6

C. NH3

D. H2


Section 13.3 Liquids and Solids

• Contrast the arrangement of particles in liquids and solids.

meniscus: the curved surface of a column of liquid

• Describe the factors that affect viscosity.

• Explain how the unit cell and crystal lattice are related.

Section 13.3 Liquids and Solids (cont.)

viscosity

surface tension

crystalline solid

The particles in solids and liquids have a limited range of motion and are not easily compressed.

unit cell

amorphous solid

Liquids

• Forces of attraction keep molecules closely packed in a fixed volume, but not in a fixed position.

• Liquids are much denser than gases because of the stronger intermolecular forces holding the particles together.

Liquids (cont.)

• Fluidity is the ability to flow and diffuse; liquids and gases are fluids.

• Viscosity is a measure of the resistance of a liquid to flow and is determined by the type of intermolecular forces, size and shape of particles, and temperature.

Liquids (cont.)

• The stronger the intermolecular attractive forces, the higher the viscosity.

• Larger molecules create greater viscosity.

• Long chains of molecules result in a higher viscosity.

• Increasing the temperature decreases viscosity because the added energy allows the molecules to overcome intermolecular forces and flow more freely.

Liquids (cont.)

• Surface tension tendency of liquids which makes it acquire the least surface area possible.

http://en.wikipedia.org/wiki/Liquids

Liquids (cont.)

• Cohesion is the force of attraction between identical molecules.

• Adhesion is the force of attraction between molecules that are different.

• Capillary action is the upward movement of liquid into a narrow cylinder, or capillary tube.

Vaporization is the process by which a liquid changes to a gas or vapor.

• Evaporation is vaporization only at the surface of a liquid.

Solids

• Solids contain particles with strong attractive intermolecular forces.

• Particles in a solid vibrate in a fixed position.

• Most solids are more dense than liquids.

• Ice is not more dense than water.

Solids (cont.)

• Crystalline solids are solids with atoms, ions, or molecules (or unit cells) arranged in an orderly, geometric shape.


Solids (cont.)

Solids (cont.)

• Amorphous solids are solids in which the particles are not arranged in a regular, repeating pattern.


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The smallest arrangement of atoms in a crystal that has the same pattern as the crystal is called ____.

A. crystal lattice

B. unit cell

C. crystalline

D. geometric cell


A. AB. BC. CD. D


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The viscosity of a liquid will increase as:

A. particle size decreases

B. temperature decreases

C. intermolecular forces decrease

D. particle size increases


Section 13.4 Phase Changes

• Explain how the addition and removal of energy can cause a phase change.

phase change: a change from one state of matter to another

• Interpret a phase diagram.


Section 13.4 Phase Changes (cont.)

melting point

vaporization

evaporation

vapor pressure

boiling point

Matter changes phase when energy is added or removed.

freezing point

condensation

deposition

phase diagram

triple point

Phase Changes That Require Energy• Melting occurs when heat flows into a solid

object.• Heat is the transfer of energy from an object

at a higher temperature to an object at a lower temperature.

Phase Changes That Require Energy (cont.)

• When ice is heated, the ice eventually absorbs enough energy to break the hydrogen bonds that hold the water molecules together.

• When the bonds break, the particles move apart and ice melts into water.

• The melting point of a crystalline solid is the temperature at which the forces holding the crystal lattice together are broken and it becomes a liquid.



• Vaporization is the process by which a liquid changes to a gas or vapor.

• Evaporation is vaporization only at the surface of a liquid.


• In a closed container, the pressure exerted by a vapor over a liquid is called vapor pressure.


• The boiling point is the temperature at which the vapor pressure of a liquid equals the atmospheric pressure. At that temperature, the vapor pressure of the liquid becomes sufficient to overcome atmospheric pressure and allow bubbles of vapor to form inside the bulk of the liquid.


• Sublimation is the process by which a solid changes into a gas without becoming a liquid.

Phase Changes That Release Energy

• As heat flows from water to the surroundings, the particles lose energy.

• The freezing point is the temperature at which a liquid is converted into a crystalline solid.

Phase Changes That Release Energy (cont.)

• As energy flows from water vapor, the velocity decreases.

• The process by which a gas or vapor becomes a liquid is called condensation.

• Deposition is the process by which a gas or vapor changes directly to a solid, and is the reverse of sublimation.


Phase Diagrams

• A phase diagram is a graph of pressure versus temperature that shows in which phase a substance will exist under different conditions of temperature and pressure.

Phase Diagrams (cont.)

• The triple point is the point on a phase diagram that represents the temperature and pressure at which all three phases of a substance can coexist.


Phase Diagrams (cont.)

The phase diagram for different substances are different from water.


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The addition of energy to water molecules will cause them to ____.

A. freeze

B. change to water vapor

C. form a crystal lattice

D. move closer together


A. AB. BC. CD. D


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The transfer of energy from one object to another at a lower temperature is ____.

A. heat

B. degrees

C. conductivity

D. electricity

End of Section 13-4End of Section 13-4

Resources MenuResources Menu

Chemistry Online

Study Guide

Chapter Assessment

Standardized Test Practice

Image Bank

Concepts in Motion

http://www.glencoe.com/

Study Guide 1Study Guide 1

Section 13.1 Gases

Key Concepts

• The kinetic-molecular theory explains the properties of gases in terms of the size, motion, and energy of their particles.

• Dalton’s law of partial pressures is used to determine the pressures of individual gases in gas mixtures.

• Graham’s law is used to compare the diffusion rates of two gases.


Section 13.2 Forces of Attraction

Key Concepts

• Intramolecular forces are stronger than intermolecular forces.

• Dispersion forces are intermolecular forces between temporary dipoles.

• Dipole-dipole forces occur between polar molecules.


Section 13.3 Liquids and Solids

Key Concepts

• The kinetic-molecular theory explains the behavior of solids and liquids.

• Intermolecular forces in liquids affect viscosity, surface tension, cohesion, and adhesion.

• Crystalline solids can be classified by their shape and composition.


Section 13.4 Phase Changes

Key Concepts

• States of a substance are referred to as phases when they coexist as physically distinct parts of a mixture.

• Energy changes occur during phase changes.

• Phase diagrams show how different temperatures and pressures affect the phase of a substance.

Chapter Assessment 1Chapter Assessment 1

A. AB. BC. CD. D

A B C D

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760 mm Hg is equal to ____.

A. 1 Torr

B. 1 pascal

C. 1 kilopascal

D. 1 atmosphere


A. AB. BC. CD. D

A B C D

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A collision in which no kinetic energy is lost is a(n) ____ collision.

A. net-zero

B. elastic

C. inelastic

D. conserved


A. AB. BC. CD. D

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Solids with no repeating pattern are ____.

A. ionic

B. crystalline

C. liquids

D. amorphous


A. AB. BC. CD. D

A B C D

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What is the point at which all six phase changes can occur?

A. the melting point

B. the boiling point

C. the critical point

D. the triple point


A. AB. BC. CD. D

A B C D

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What are the forces that determine a substance’s physical properties?

A. intermolecular forces

B. intramolecular forces

C. internal forces

D. dispersal forces

STP 2STP 2

A. AB. BC. CD. D

A B C D

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A sealed flask contains helium, argon, and nitrogen gas. If the total pressure is 7.5 atm, the partial pressure of helium is 2.4 atm and the partial pressure of nitrogen is 3.7 atm, what is the partial pressure of argon?

A. 1.3 atm

B. 6.1 atm

C. 1.4 atm

D. 7.5 atm

STP 3STP 3

A. AB. BC. CD. D

A B C D

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Adding energy to a liquid will:

A. cause it to form crystal lattice

B. decrease the viscosity

C. compress the particles closer together

D. increase the velocity of the particles

STP 4STP 4

A. AB. BC. CD. D

A B C D

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Hydrogen bonds are a special type of ____.

A. ionic bond

B. covalent bond

C. dipole-dipole force

D. dispersion force

STP 5STP 5

A. AB. BC. CD. D

A B C D

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How many atoms of oxygen are present in 3.5 mol of water?

A. 2.1 x 1024

B. 3.5 x 1023

C. 6.02 x 1023

D. 4.2 x 1024

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Table 13.4 Unit Cells

Table 13.5 Types of Crystalline Solids

Figure 13.30 Phase Diagrams

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kinetic theory and states of matter chapter 13 section 13.1 gases use the kinetic-molecular theory...

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