Properties of Matter

Properties of Matter • Objective 2.1: Students will know the difference between matter and non-matter.http://antoine.frostburg.edu/chem/senese/101/matter/slides/index.shtml Matter: anything that has mass and takes up space (volume). Properties: shape, color, texture, size, luster, etc. Non-matter: heat, light, microwaves (forms of energy)

Kinetic Theory and Matter • How does the kinetic theory explain the observed properties of matter? Brainstorm how this works. What does kinetic theory contribute to our understanding? (2.8.1, 2.8.5) Outside-In: Clearing up how cloud droplets freeze http://www.sciencenews.org/articles/20021130/fob3.asp 2.2 THE STUDENT WILL USE SIMPLE MODELS TO EXPLAIN OBSERVED PROPERTIES OF MATTER (5,7)

h http://antoine.frostburg.edu/chem/senese/101/matter/slides/index.shtml

http://www.st-andrews.ac.uk/~ctab/AS1002/Lecture_Notes/lecture_8.pdfhttp://www.st-andrews.ac.uk/~ctab/AS1002/Lecture_Notes/lecture_8.pdf

Solids, Liquids, Gases, Plasmas • How are these types of matter different or similar to each other? • How can you distinguish among them? • How would you define a property? 2.3 THE STUDENT WILL DIFFERENTIATE AMONG THE PROPERTIES OF SOLIDS, LIQUIDS, GASES AND PLASMAS. (11,12)

http://antoine.frostburg.edu/chem/senese/101/matter/slides/index.shtmlhttp://antoine.frostburg.edu/chem/senese/101/matter/slides/index.shtml

Properties • Extensive: related to the amount of mass present. Examples include: mass, volume, length. Extensive properties change as the amount of a particular substance changes. • Intensive: are unique to the substance. Sometimes called “fingerprints” of a substance. Examples include: density, boiling point, melting point, color, smell, etc.

Solids, Liquids, Gases • Solids: Sulfur, graphite, salt crystals, copper metal. Amorphous solids: gum, rubber, glass • Liquids: water, alcohol, glycerin • Gases: oxygen, nitrogen, helium, etc.

Characteristics • Solids: • Retain their shape • Are virtually incompressible • Do not flow • Experience very slow diffusion • Gases: • Assume volume and shape of container • Are compressible • Flow • Diffuse rapidly • Liquids: • Assume shape of container • Does not expand to fill container • Flows readily • Diffuses slowly

Gases and the Kinetic Molecular Theory • How do gases compress or expand? • Where are gases found? • What are their behaviors when temperatures change or pressures change? • What is temperature and what is pressure? Why Baseballs Fly Further at Higher Altitudes http://www.usatoday.com/weather/tg/wbasebal/wbasebal.htm Understanding Air Density and Its Effects http://www.usatoday.com/weather/wdensity.htm

Solids • According to Kinetic Molecular Theory, particles in a solid occupy fixed positions (well-defined arrangements). Particles are close together. Diamond, pyrite, amethyst, quartz. Melting points occur at a specific temperature. • The attractive forces are strong enough to hold them in place. They are not compressible. • Amorphous solids have no orderly arrangements. No well-defined faces and shapes. Melting points occur over a range of temperatures.

Liquids • According to Kinetic Molecular Theory, particles in a liquid have more attractions between them than in a gas which holds the particles together. • They are denser and far less compressible than in a gas. • The attractive forces are not strong enough to let them move away from each other, so any liquid can be poured.

Plasmas • Plasmas: Theoretically, 99% of the universe is made of plasma. • Plasma: no definite shape or volume and contains broken particles. They conduct electricity and is affected by magnetic fields. • Found in lightning, fire and aurora borealis. Artificial plasma is in fluorescent lights and plasma balls (created by passing electric charges through gases).

Phase Changes • What is meant by a phase? • How do we understand phase change? • How do we understand the changes which occur during the phase change? (3.8.2) • All phase changes are accompanied by changes in energy and pressure. http://id.mind.net/~zona/mstm/physics/mechanics/energy/heatAndTemperature/changesOfPhase/changeOfState.html http://www.usatoday.com/weather/wwatphse.htm 2.4 THE STUDENT WILL INVESTIGATE AND DESCRIBE HOW ALL PHASE CHANGES ARE ACCOMPANIED BY CHANGES IN ENERGY AND PRESSURE. (4,5,6,7)

Heterogeneous vs. Homogeneous • Heterogeneous mixtures contain different substances which can be physically separated (see the heterogeneous rock, raisin bread). • Homogeneous mixtures contain substances which are all in the same phase or contain all the same substance (air, copper, sodium chloride, bronze). 2.5 THE STUDENT WILL INVESTIGATE AND DESCRIBE THE DIFFERENCES BETWEEN HOMOGENEOUS AND HETEROGENEOUS MIXTURES. (4,5,7)

Heterogeneous Matter http://www.fotosearch.com/BDX115/bxp26795/

Homogeneous Matter Snowflake Bromine gas http://theodoregray.com/PeriodicTable/Elements/035/ http://www.jericho-underhill.com/09l.htm Diamond Copper(II)Sulfate Pentahydrate http://www.seawhy.com/xlcuso4.html

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Separating Substances • Using properties of substances, we can separate mixtures based on the different physical and chemical properties (2.8.2). This is the basis for using unknowns in labs. • What types of properties can be used?

Solutions, Suspensions, Colloids • Solutions: homogeneous mixtures which pass through filter paper unchanged, do not settle on standing and show no Tyndall Effect. • Suspensions: heterogeneous mixtures which do not pass through filter paper, settle upon standing, and can show a Tyndall Effect. • Colloids: heterogeneous mixtures which pass through a filter paper unchanged, do not settle upon standing and have a Tyndall Effect. 2.6 THE STUDENT WILL DIFFERENTIATE AMONG MIXTURES, SOLUTIONS, SUSPENSIONS, AND COLLOIDS. (11,12)

Examples of Tyndall Effects In liquids the Tyndall Effect can be easily seen by using a laser pointer. If you dilute milk to Where it is almost clear, or if you have any type of sol, such as colloidal silver, then the beam of the laser can be easily seen as it travels through the liquid. http://www.silver-lightning.com/tyndall/

The Tyndall Effect is caused by reflection of light by very small particles in suspension in a transparent medium. It is often seen from the dust in the air when sunlight comes in through a window, or comes down through holes in clouds. It is seen when headlight beams are visible on foggy nights, and in most X-File episodes when Moulder and Sculley check out some dark place with flashlights. Tyndall Effect http://www.silver-lightning.com/tyndall/

Examples of colloids Aerosols: Man-made: Aerosol sprays, insecticide spray, smog. Natural: Fog, clouds. Solid aerosol:Natural: Smoke, dust. Foam:Man-made: Shaving lather, whipped cream. Emulsions:Natural: Milk. Man-made: Mayonnaise, cosmetic lotion, lubricants. Sols:Man-made: Paint, ink, detergents, rubber (a latex - also occur naturally) Solid Foams: Man-made: Marshmallow, styrofoam, insulation, cushioning. Gels:Man-made: Butter, jelly. Solid sols:Man-made: Certain alloys. Natural: Pearl, opal. Biological macromolecules and cells may be considered to be biocolloids and many foods are also colloidal in nature. Colloids are also an important feature of the natural environment. http://www.chm.bris.ac.uk/webprojects2002/pdavies/examples.html

Solutions and Suspensions http://www.schoolscience.co.uk/content/4/physics/bama/aerosch2pg3.html

Properties of Matter http://microgravity.grc.nasa.gov/balloon/blob.htm

Chemical vs. Physical Changes • Physical changes do not alter the properties of a substance. Tearing paper, crushing rocks, pounding metals, etc. • Chemical changes alter the properties of a substance. Lighting a candle, souring of milk, baking bread.

Chemical Change - Fireworks http://www.skydreamz.com/

Physical Change - Melting http://www.sciencemuseum.org.uk/antenna/climatechange/Cip3/422.asp/

Properties of Matter