1. Lesson 3 Classifying Matter Classifying Matter Anything in black letters = write it in your notes (‘knowts’)

2. Matter - Anything that has mass and takes up space. Which of these things is not considered matter? Cell Phone GravityRainbow FireHappiness Light Bulb AirSound Empty Pop Bottle Have any examples of matter? Is anything NOT matter?

3. With your lab partner, write down how you could prove to someone that air has mass.

4. Matter -Anything that has mass Mass - Measure of the amount of matter in an object Matter Mass We need a better definition for mass…

5. Mass -Measure of an object’s inertia. Inertia -Resistance to change in motion. Which of the above has more inertia?

6. Volume - amount of space occupied by an object Common units of volume: mL or L (liquids) cm 3 or m 3 (solids) 1 cm 3 = 1 mL

7. mass  volume  mass volume Density = density  grams mL or cm 3 g/mL or g/cm 3 UNITS

8. The density of water is approx. 1 g/mL The density of an object normally decreases as its temperature increases. Hot air rises!!

9. States of Matter Solid Particles are packed closely together; definite shape and volume

10. Liquid Particles are close but are free to flow past one another; shape depends on container

11. Gas Particles are far apart and move freely; shape and volume depend on container; can be compressed

12. Physical Change A change in appearance but NOT in the chemical identity of a substance. The melting point of gallium metal is 30˚C. The figure shows how the heat from a person’s hand can melt a sample of gallium.

13. Phase Changes melt freeze evaporate condense sublimate deposit

14. A vapor is a gas that evaporates from a liquid. The difference between a vapor & a gas

15. The difference between evaporation & boiling Evaporation occurs only at the surface, boiling occurs throughout the liquid.

16. The white cloud is NOT steam. It is actually hot water vapor condensing to form a mist of water droplets

17. Element, Compound, or Mixture?

18. Mixture - physical blend of 2 or more things Homogeneous – same composition throughout, uniformly mixed; solutions Heterogeneous – variable composition, nonuniformly mixed; contains more than 1 phase.

19. Olive oil Vinegar Oil & Vinegar Heterogeneous (2 phases) Homogeneous

20. Separating Mixtures Filtration – separates a solid from a liquid. Liquid that passes through the filter paper

21. Distillation – separates a mixture into parts based on the boiling points of each part.

22. Element – fundamental building block of matter; made of atoms. Each element has a chemical symbol. 1 st - Capital letter 2 nd - Lowercase

23. Compound – 2 or more atoms chemically bonded in a fixed proportion. Has a chemical formula. Compounds can be broken down into simpler substances, but elements cannot. Subscript Chemical Formula H2OH2O 2 H atoms and 1 oxygen atom

24. The properties of compounds are different from the elements that form them. + Sodium (Na) Metal so reactive it reacts with water Chlorine (Cl 2 ) Toxic gas used in WWI for chemical warfare Salt (NaCl) Relatively harmless 2 poisonous substances react to form a completely benign compound that is necessary for us to live.

25. Periodic Table 7 Periods (Rows) 18 Columns (Groups or Families ) Elements in each column have similar chemical properties

26. Law of Conservation of Mass In any chemical reaction, reactant mass = product mass