1. 1 Properties of Matter What is matter? Matter is anything that has mass and volume.

2. 2 Measuring Matter Volume of a liquid –Graduated cylinder- read from bottom of meniscus Volume of solid –Length X Width X Height Volume of Irregular Shaped Objects –Water Displacement Indirect Measuring –Large objects-take a core sample and use a formula –Small objects-weigh 100 and then divide weight by 100 to get one small objects weight

3. 3 Classification of Matter MATTER Has mass and volume PHASES Solid, liquid, gas or plasma PROPERTIES PHYSICAL CHEMICAL MADE UP OF Element, compound or mixture

4. 4 Phases of Matter SOLID, LIQUID, GAS, or PLASMA

5. 5 Solids - definite shape and volume l Atoms are held close together by strong bonds l Movement is slow l Crystalline Solids (crystals) - atoms are arranged in regular fashion (geometric) Ex. - ice, salt, diamonds l Amorphous Solids - atoms LACK a regular arrangement Ex. - rock, glass, wax Phases of Matter

6. 6 Phases of Matter - Continued Liquids - NO definite shape but definite volume l Bonds are weaker and atoms are spaced apart l They take the shape of container they are in l Examples: oil, water, syrup, OJ, milk

7. 7 Phases of Matter - Continued Gases - NO definite shape OR volume l Bonds are weakest and atoms far apart l Expands to fill the container they are in Examples - air, oxygen, smoke

8. 8 Plasma Gas like mixture of + and – charged particles l Movement very rapid (10,000˚C) l 99% of mass of our solar system l Examples: Sun, Stars and Lightning Phases of Matter - Continued

9. 9 Classifying Matter Physical Properties are those that can be observed without changing the identity of the substance Chemical Properties are those that describe how a substance changes into other new substances

10. 10 PROPERTIES OF MATTER PHYSICAL CHEMICAL Size Shape Texture Color Phase Conductor Ductile Malleable Shiny/luster Density Mass Tasteless Flammability Changes color Reacts with Combustible Corrosive Volatile Explosive Dissolves Odorless Hardness Brittle Tensile strength Fluid Viscosity Elasticity Buoyant Melting point Freezing point Boiling point

11. 11 Physical Properties of Matter Viscosity – Measure of the material’s resistance to flow High-viscosity liquids take longer to flow Example: Ketchup when comparing to water Low-viscosity liquids flow easier Example: Tomato Juice flows easier than ketchup Temperature raising-viscosity decreases except in gases. 

12. 12 Physical Properties of Matter – Cont. Elasticity – Measure of ability to be stretched and then return to its original size. Example:Rubber Bands, Elastic, and Playground Balls Question: Which ball would you rather play basketball?

13. 13 Malleability – Ability to be hammered into sheets Example: Gold &Silver Coins, Aluminum Foil and Soda Cans Physical Properties of Matter – Cont.

14. 14 Brittleness – measures a material’s tendency to shatter upon impact Example: Sulfur, Calcium and Glass Hardness – Resistance to breaking or scratching Example: diamonds Physical Properties of Matter – Cont.

15. 15 Luster – shininess Example: Gold, Silver, Mercury Ductility – ability to be pulled into wires Example: Most metals (Copper, Silver) Physical Properties of Matter – Cont.

16. 16 Physical Properties of Matter – Cont. Tensile Strength- Measure of how much pulling, or tension, a material can withstand before breaking Property of fibers, ropes, cables, girders DuPont Kevlar-5 times tensile strength of steel

17. 17 Melting Point – Temperature at which a solid changes to a liquid Example: Ice  water Freezing Point – Temperature at which a liquid changes to a solid Example: Water  Ice (0°C) Physical Properties

18. 18 Boiling Point – Temperature at which a liquid changes into a gas Example: Water  vapor (100˚ C) Physical Properties

19. 19 Density – The amount of mass in a given volume How tightly packed the atoms or molecules are in a substance Formula to calculate density is: Density = Mass Volume Units are expressed as: g/mL or g/L for liquids (remember the graduated cylinder) g/cm 3 for solids Physical Properties of Matter – Cont.

20. 20 Density of a Fluid Fluid- Any matter that is able to flow Liquids and gases Density of a liquid might be different from the density of the same solid Most materials are denser in solid phase than their liquid phase Exception- Water-freezes with air spaces so it is less dense and floats. Density of liquid water is 1 g/ml

21. 21 Buoyancy – Upward force a fluid exerts on an object Determines whether the object will sink or float Example: Buoyancy of water keeping you afloat while swimming Physical Properties of Matter – Cont.

22. 22 Buoyancy Buoyancy force is LESS then object’s weight, object will SINK Buoyancy force is EQUAL to the object’s weight, object will FLOAT Buoyancy force is MORE then object’s weight, object will FLOAT IN AIR

23. 23 Archimedes's Principle Greek mathematician, 3 rd century BC Principle states-The buoyancy force on an object in a fluid is equal to the weight of the fluid displaced by the object Buoyancy of Gasses Balloon floats because it displaces a very large volume of air Volume of air displaced weighs more than the balloon

24. 24 Classification of Matter

25. 25 Classification of Matter Matter can be divided into 2 categories: SUBSTANCES & MIXTURES Substances can NOT be separated into different kinds of matter by physical means. Mixtures can be separated into different kinds of matter by physical means.

26. 26 What are substances? – Elements Any substance in which all the atoms in a sample are alike, one kind of matter Examples: Carbon, Sodium and Oxygen – Compounds 2 or more elements chemically combined in a fixed ratio (subscript) Usually has different appearance from elements that make it up Examples: Water – H 2 O and Salt - NaCl Classification of Matter In science, substances are limited to elements and compounds.

27. 27 Classification of Matter Atom-smallest possible particle of an element Molecule- smallest possible particle of a compound

28. 28 What are mixtures ? 2 or more substances that can be separated by physical means Do not always contain the same amounts of the different substances that make them up –Homogeneous same throughout, particles so tiny that cannot be seen, don’t settle out or scatter light Examples: milk, salt water and cola –Heterogeneous a mixture in which different materials can be easily distinguished Suspension-visible particles settle-muddy water Examples: Sand/water, Italian salad dressing, pizza and dry soups Classification of Matter

29. 29 Changes in Matter MATTER PHYSICAL CHANGES CHEMICAL CHANGES NUCLEAR CHANGES

30. 30 Changes in Matter Melting Freezing Boiling Evaporation Cutting Splitting Chopping Sublimation Chemical reaction Photosynthesis Respiration Digestion of food PhysicalChemical Nuclear Fission Fusion

31. 31 Physical vs. Chemical Change Physical Change - Does NOT create a new substance, affects only the physical properties. Appearance changes – not chemical makeup A change in size, shape or form (phases of matter).

32. 32 Physical Change Vaporization- process at which a liquid changes to a gas by increasing the temperature to the liquids boiling point Example: water boils to form steam at 100° C

33. 33 Physical Change Evaporation- process at which a liquid changes to a gas. The liquid is not boiling. Example: A puddle drying up or sweat drying

34. 34 Physical Change Condensation – Process at which a gas becomes a liquid Gas cooled below its boiling point Example: water vapor  water, dew in the morning, glass of ice tea in hot weather.

35. 35 Physical change Sublimation – When a solid changes directly to a gas The matter doesn’t melt Example:snow, dry ice and glaciers Deposition- Gas changes directly into a solid Ex. Fire extinguisher

36. 36 Chemical Change - A change in which a NEW substance is created End products are chemically different from the original. Chemical Change Corrosive-dissolving away of a metal-rusting

37. 37 Four Signs or Evidence of a Chemical Change Gas forms Permanent color change Heat/or light energy is given off Precipitate forms. A precipitate is an insoluble substance that forms out of solution.

38. 38 Identify the following as physical or chemical change. Ice cube melting. Slicing an apple into pieces. Physical vs. Chemical Change Wood burning. People eating.

39. 39 Changes in Matter - Continued Exotic Super Hot Nucleus of atom comes apart Particle accelerates Exotic Super Cold Below -270˚ C Superfluids from gases

40. 40 Charles’ Law Jacques Charles, French scientist (1742-1823) Law states-volume of a gas increases when temperature increases and reverse, volume of gas decreases when temperature decreases. V 1 / T 1 = V 2 / T 2 –Temperature must be in Kelvin degrees (+273)

41. 41 Boyle’s Law Robert Boyle-British scientist (1627-1691) Law states-as pressure of a gas increases, its volume decreases proportionately and reverse pressure of gas decreases, its volume increases proportionately. P 1 V 1 = P 2 V 2 Pascal-unit for pressure (Pa) (kPa)