Mechel Golenberke: My First Website
Chapter 3 States of Matter
3.1 Solids, Liquids, and Gases
3.1.1 Describe the five states of matter
3.1.2 Classify materials as solids, liquids, or gases
3.1.3 Explain the behavior of gases, liquids, and solids using kinetic theory
- Materials can be classified as solids, liquids, or gases based on whether their shapes and volumes are definite or variable.
- The kinetic theory of matter states that all particles of matter are in constant motion.
- There are forces of attraction among the particles in all matter.
- The constant motion of particles in a gas allows a gas to fill a container of any shape or size.
- A liquid takes the shape of its container because particles in a liquid can flow to new locations. The volume of a liquid is constant because forces of attraction keep the particles close together.
- Solids have a definite volume and shape because particles in a solid vibrate around fixed locations.
solid – the state of matter in which materials have a definite shape and a definite volume
liquid – the state of matter in which a material has a definite volume but not a definite shape
gas – the state of matter in which a material has neither a definite shape nor a definite volume
kinetic energy – the energy an object has due to its motion
Day 1 & Day 2:
Chapter 3 Pretest http://websites.pdesas.org/mgolenberke/2011/10/29/372263/file.aspx
Talking to the Text: Chapter Summary http://websites.pdesas.org/mgolenberke/2011/10/29/372262/file.aspx
Brightstorm: Matter: States of Matter (2:37)
States of matter are the different phases which matters can take - gas, liquid and solid. Gas has no fixed shape and conforms to the volume of its container. A liquid has a distinct volume but assumes the shape of its container. A solid has definite shape and volume, regardless of its container. In the case of H20 steam is a gas, water is a liquid and ice is a solid. Most substances are more dense in their solid form, but water is an exception.
3.1 Interest Grabber http://websites.pdesas.org/mgolenberke/2011/10/29/372264/file.aspx
3.1 PowerPoint & NoteGuide (48 slides) http://websites.pdesas.org/mgolenberke/2011/10/29/372258/file.aspx
3.1 Reading & Study Workbook http://websites.pdesas.org/mgolenberke/2011/10/25/371391/file.aspx
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3.2 The Gas Laws
3.2.1 Define pressure and gas pressure
3.2.2 Identify factors that affect gas pressure
3.2.3 Predict changes in gas pressure due to changes in temperature, volume, and number of particles
3.2.4 Explain Charles’s law, Boyle’s law, and the combined gas low
3.2.5 Apply gas laws to solve problems involving gases
- Collisions between particles of a gas and the walls of the container cause the pressure in s closed container of gas.
- Factors that affect the pressure of an enclosed gas are its temperature, its volume, and the number of its particles.
- Raising the temperature of a gas will increase its pressure if the volume of the gas and the number of particles is constant.
- Reducing the volume of a gas increases its pressure if the temperature of the gas and the number of particles are constant.
- Increasing the number of particles will increase the pressure of a gas if the temperature and the volume are constant.
- The combined gas law can be expressed as: P1V1 = P2V2
T1 T2
pressure – the result of a force distributed over an area
absolute zero – the temperature of 0 kelvins
Charles’s law – the direct proportion of the volume of a gas to its temperature (in kelvins) if the pressure anf the number of particles of the gas are constant
Boyle’s law – the inverse variation of the volume of a gas with its pressure if the temperature and the number of particles are constant
Day 3
Investigating Space Between Particles in Matter http://websites.pdesas.org/mgolenberke/2011/10/29/372302/file.aspx
Day 4
3.2 Interest Grabber http://websites.pdesas.org/mgolenberke/2011/10/29/372274/file.aspx
Brightstorm Kinetic-Molecular Theory: Gases (3:34)
The gaseous state is one of the three phases of matte. Gases are obtained through vaporization from liquid and sublimation from solid. When a liquid vaporizes, it is often called boiling. Gases are the least dense state of matter because they contain high kinetic energy.
3.2 PowerPoint & NoteGuide (55 slides) – slides 1-13 pressure http://websites.pdesas.org/mgolenberke/2011/10/29/372259/file.aspx
Brightstorm Kinetic-Molecular Theory: Charles Law (5:04)
Charles Law states that the volume of a given mass of a gas is directly proportional to its Kevin temperature at constant pressure. In mathematical terms, the relationship between temperature and volume is expressed as V1/T1=V2/T2.
slides 14-25 Charles Law
Charles Law Worksheet (jeff) http://websites.pdesas.org/mgolenberke/2011/10/29/372266/file.aspx
Day 5
Brightstorm Kinetic-Molecular Theory: Boyle's Law (4:32)
Boyle’s Law states that volume of a given amount of gas held at a constant temperature varies inversely the with pressure. The relationship between pressure and volume of Boyle’s Law is expressed in mathematical terms as P1V1=P2V2.
3.2 PowerPoint & NoteGuide (55 slides) – slides 26-30 Boyles Law http://websites.pdesas.org/mgolenberke/2011/10/29/372259/file.aspx
Boyles Law Worksheet (jeff) http://websites.pdesas.org/mgolenberke/2011/10/29/372265/file.aspx
Day 6
3.2 PowerPoint & NoteGuide (55 slides) – finish slides 31-55 (combined Gas Law) http://websites.pdesas.org/mgolenberke/2011/10/29/372259/file.aspx
Brightstorm Kinetic-Molecular Theory: Combined Gas Law (4:02)
The Combined Gas Law combines Charles’ Law, Boyle’s Law and Gay Lussac’s Law. The Combined Gas Law states that a gas’ pressure x volume x temperature = constant.
Practice Worksheets: Section 3.2 The Gas Laws (Math Skills & Problem Solving)
Math Skills the Combined Gas Law
Day 7
Show this Flash animation with audio of "The Gas Laws."
Virtual Charles & Boyles Law Lab http://websites.pdesas.org/mgolenberke/2011/11/13/378742/file.aspx
3.2 Reading & Study Workbook http://websites.pdesas.org/mgolenberke/2011/10/29/372272/file.aspx
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3.3 Phase Change
3.3.1 Describe phase changes
3.3.2 Explain how temperature can be used to recognize a phase change
3.3.3 Explain what happens to the motion, arrangement, and average kinetic energy of water molecules during phase changes
3.3.4 Describe each of the six phase changes
3.3.5 Identify phase changes as endothermic or exothermic
- Melting, freezing, vaporization, condensation, sublimation, and deposition are six common phase changes.
- The temperature of a substance does not change during a phase change.
- Energy is either absorbed or released during a phase change.
- The arrangement of molecules in water becomes less orderly as water melts, and more orderly when water freezes.
- Evaporation takes place at the surface of a liquid and occurs at temperatures below the boiling point.
phase change – a reversible physical change that occurs when a substance changes from one state of matter to another
endothermic – a description of a change in which a system absorbs energy from its surroundings
heat of fusion – the energy of substance must absorb in order to change from a solid to a liquid
exothermic – a description of a change in which a system releases energy to its surroundings
vaporization – the phase change in which a substance changes from a liquid to a gas
heat of vaporization – the energy a substance must absorb in order to change from a liquid to a gas
evaporation – the process that changes a substance from a liquid to a gas at temperatures below the substances boiling point
vapor pressure – the pressure caused by the collisions of particles in a vapor with the walls of a container
condensation – the phase change in which a substance changes form a gas or vapor to a liquid
sublimation – the phase change in which a substance changes from a solid to a gas or vapor without changing to a liquid first
deposition – the phase change in which a gas or vapor changes directly into a solid without first changing into a liquid
Day 8 – check 3.2 homework, 3.1 & 3.2 vocabulary quiz & begin 3.3
3.3 Interest Grabber http://websites.pdesas.org/mgolenberke/2011/10/29/372277/file.aspx
Brightstorm Kinetic-Molecular Theory: Phase Change (4:16)
Phase changes are the transformations from one state of matter to another due to thermodynamics. The processes of phase change between solid and liquid are called melting and freezing. Phase changes between liquid and gas are vaporization and condensation. Phase changes between gas and solid are deposition and sublimation. Phase changes can be spontaneous or non-spontaneous.
(begin)3.3 PowerPoint (48 slides) & NoteGuide http://websites.pdesas.org/mgolenberke/2011/10/29/372260/file.aspx
Day 9 – 3.3 vocab quiz?
Finish 3.3 PowerPoint & NoteGuide
3.3 Study Workbook http://websites.pdesas.org/mgolenberke/2011/10/29/372276/file.aspx
More Brightstorm if time:
Brightstorm Kinetic-Molecular Theory: Phase Diagrams (6:10)
Phase diagrams graphically depict the state of matter in varying temperatures and pressures. The x-axis of a phase diagram is always temperature while the y-axis is always pressure. There is a point on a phase diagram called the triple point at which all three phases of matter exist simultaneously.
Brightstorm Kinetic-Molecular Theory: Boiling Point (3:40)
Boiling point is the particular temperature where vapor pressure equals to of a liquid equals to the surrounding environmental liquid. At this temperature the liquid begins to bubble as liquid below the surface turns to gas and escapes upwards.
Brightstorm Kinetic-Molecular Theory: Vapor Pressure (2:26)
Vapor pressure is the pressure caused by the evaporation of liquids. Three common factors that influence vapor press are surface area, intermolecular forces and temperature. The vapor pressure of a molecule differs at different temperatures.
Day 10
Collect homework
Chapter 3 WordWise http://websites.pdesas.org/mgolenberke/2011/10/29/372301/file.aspx
Correct 3.3
Review for Test http://www.phschool.com/webcodes10/index.cfm?fuseaction=home.gotoWebCode&wcprefix=cca&wcsuffix=1030
Day 11 Chapter 3 Test
