1. Matter chapter 16 & 23 Mass occupies space Pure substances and mixtures

2. Types of properties of Matter chapter 17 Physical –determined without changing identity of the substance Chemical –determined only by changing the identity of the substance -hardness -elasticity -brittleness -malleable -tensile strength -density -buoyancy -viscosity

3. Matter exists in 3 phases Gas –no definite shape or volume, compressible, low density Liquid -no definite shape but has a definite volume, incompressible, medium density Solid –definite shape and volume, incompressible, high density

4. Phase change Liquid to gas (vaporization) Gas to liquid (condensation) Solid to liquid (melting) Liquid to solid (freezing) Solid to gas (sublimation) Gas to solid (deposition)

5. Matter contains Energy = capacity to do work Potential energy –stored energy do to position Kinetic energy –energy due to motion Types of energy Mechanical –motion Electrical –motion Nuclear –motion Solar –sun Sound -compression on air Heat Chemical Chemical energy –potential form Heat energy –kinetic form

7. Typical changes that Matter can undergo Physical –does not alter the identity of the substance Chemical –does alter the identity of the substance

8. Mixtures Variable compositions Heterogeneous and Homogenous Both can be broken down by physical means Heterogeneous –different make up within and could be uneven throughout the different parts (water and dirt)(5% dirt or 10% dirt or 50% dirt, and who knows how much water?) Homogenous –same make up throughout the different parts (water and sugar)(10%sugar and 10%sugar and 10% sugar everywhere throughout) = solution = amount of sugar can change 10% sugar or 20% sugar or 30% sugar etc., but then the amount of water would too in the different parts if you split it up.

9. Pure substance Same composition throughout -means the substance is made of the same materials throughout and has the same amount of those materials throughout Could be an element or compound

10. Pure Substances.compounds – Composed of elements chemically combined (billions of them) -Chemical formulas –represented by symbols, can’t be broken down physically but can be broken down chemically -if you cut it apart, it would have the same amount of elements present in both pieces (if you cut apart a tootsie roll, both pieces are still a tootsie roll)

11. Pure substances Element –basic unit of matter -111known elements -92 are naturally occurring -others are man made -cannot be broken down further either by physical or chemical means -represented by symbols –one letter symbol = capitalized -two letter symbol = first letter capitalized second is small

12. Matter broken down Atom Smallest particle with all the properties of an element Basic unit of an element Molecule Smallest unit of a compound with all of the properties of the compound Basic unit of a compound

13. Measuring temperatures of atoms and molecules Temperature measures the average velocity of an atom or molecule Higher temperature = faster the velocity Energy in matter can be measured by the heat it contains or gives off SI Unit = Joule, common unit is calorie 1 calorie = 4.184 Joules 1 Kcal = 1,000 calories

14. Conservation of Matter and Energy Law of Conservation of matter -total amount of matter and energy in the Universe is constant. Matter cannot be created or destroyed Einstein E =mc 2 –unit of energy (mass) x (speed of light) 2, during all chemical reactions, there will be no change of the amount of energy or matter in the Universe Law of Conservation of Mass –no detectable change in mass in a chemical reaction

15. Identify and Memorize (look on Internet or inside back cover of your book) ALB CaC ClCu HeH FPb MgHg NO PK NaS