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# Properties of matter ppt

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### Transcript of "Properties of matter ppt"

1. 1. Properties of MatterCh. 2
2. 2. Quick Review Matter is anything that: a) has mass, and b) takes up space Mass = a measure of the amount of ―stuff‖ (or material) the object contains (don’t confuse this with weight, a measure of gravity) Volume = a measure of the space occupied by the object
3. 3. States of Matter1) Solid- matter that can not flow (definite shape) and has definite volume.2) Liquid- definite volume but takes the shape of its container (flows).3) Gas- a substance without definite volume or shape and can flow.  Vapor- a substance that is currently a gas, but normally is a liquid or solid at room temperature. (Which is correct: ―water gas‖, or ―water vapor‖?)4) Plasma- Ionized gas that contains positive ions and electrons
4. 4. Drawing the States of Matter Solid Liquid Gas
5. 5. States of Matter Result of a Definite Definite Temperature Will it Compress? Volume? Shape? Increase? SmallSolid YES YES Expansion NO SmallLiquid YES NO Expansion NO LargeGas NO Expansion NO YES
6. 6. The 6 Phase Changes1. Melting: Solid to Liquid2. Freezing: Liquid to Solid3. Evaporation: Liquid to Gas4. Condensation: Gas to Liquid5. Sublimation: Solid to Gas6. Deposition: Gas to Solid
7. 7. Describing MatterProperties used to describe matter can beclassified as: 1) Extensive – depends on the amount of matter in the sample - Mass, volume, calories are examples 2) Intensive – depends on the type of matter, not the amount present - Hardness, Boiling Point
8. 8. Is Density Intensive orExtensive?
9. 9. PropertiesWords that describe matter (adjectives)Physical Properties- a property that can be observed and measured without changing the material’s composition.Examples- color, hardness, m.p., b.p.
10. 10. PropertiesChemical Properties- a property that can only be observed by changing the composition of the material.Examples- ability to burn, decompose, ferment, react with, etc.
11. 11. Physical ChangePhysical change will change the visible appearance, without changing the composition of the material.Can be reversible, or irreversible Boil, melt, cut, bend, split, crack Is boiled water still water? ***ALL 6 PHASE CHANGES ARE PHYSICAL CHANGES!***
12. 12. Chemical ChangeChemical Change - a change where a new form of matter is made. Rust, burn, decompose, ferment
13. 13. Signs of a Chemical Change1. Gas production2. Precipitate formation3. Energy production (light, sound)4. Change in Temperature5. Change in color6. Change in chemical or physical property
14. 14. Chemical vs. Physical ChangeAsk yourself: Is anything new being made?
15. 15. 3 Types of Matter1. Elements2. Compounds3. Mixtures a. Heterogeneous b. Homogeneous (Solutions)
16. 16. Pure Substances Pure substances can be either  Elements  Compounds
17. 17. 1. ElementsSimplest kind of matterCannot be broken down any simpler and still have properties of that element!All one kind of atom. Atoms– the smallest particle or unit of an element that has the properties of that element.
18. 18. 2. CompoundsSubstances that can be broken down only by chemical methods When broken down, the pieces have completely different properties than the original compound. Made of two or more atoms, chemically combined (not just a physical blend!)
19. 19. 3. Mixtures Mixtures are a physical blend of at least two substances; have variable composition. Every part keeps it’s own properties. They can be either:
20. 20. 3. Mixtures (cont.) 1) Heterogeneous – the mixture is not uniform in composition Ex. Chocolate chip cookie, gravel, soil.
21. 21. 3. Mixtures (cont.) 2) Homogeneous - same composition throughout; called ―solutions‖ • Kool-aid, air, salt water
22. 22. More on Homogenous (solutions) Mixed molecule by molecule, thus too small to see the different parts Can occur between any state of matter: gas in gas; liquid in gas; gas in liquid; solid in liquid; solid in solid (alloys), etc. Most common solutions consist of 1 or more substances dissolved (the dissolved ―stuff‖ is called the solute) in a liquid (called the solvent) If the solvent is water—aqueous solution A true solution will never separate or settle out on its own.
23. 23. Ways of Separating Mixtures Differences in physical properties can be used to separate mixtures.1) Filtration - separates a solid from the liquid in a heterogeneous mixture (by size)2) Distillation – separates a solution by boiling pointsThere are other ways as well: magnets, evporationchromotography
24. 24. Law of Conservation ofMass/Matter
25. 25. During any chemical reaction, the mass of the products (right side of arrow) is always equal to the mass of the reactants (left side of arrow).All the mass can be accounted for: Burning of wood results in products that appear to have less mass as ashes; where is the rest?
26. 26. Example ProblemWhen methane gas burns, and reacts andcombines with oxygen to produce carbondioxide and water vapor. If 4 grams ofmethane reacts with 16 grams of oxygen toproduce 11 grams of carbon dioxide, howmuch water vapor is produced?
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