1. Matter

2. Stuff that objects are made of Anything that has mass and volume 3 Types –Elements –Compounds –Mixtures

3. Phases of Matter Solids Liquids Gases Animation

4. Solids Definite Shape and Volume Strong Intermolecular Forces Particles are close together Particles are arranged in neat, orderly lines Particles do move – shake, vibrate –AnimationAnimation High melting and boiling points Designated by (s) Examples: –Au (s), Fe (s), H 2 O (s)

5. Liquids Indefinite Shape Definite Volume Midrange Intermolecular Forces Particles are somewhat close together Flow freely Designated by (l) Examples: –B–Br (l), Hg (l), H 2 O (l)

6. Gases NO definite Shape or Volume –Particles will spread out to fill the shape and volume of a container Weak Intermolecular Forces Particles are far apart Particles are very disorganized Particles quickly move all over Low melting and boiling points Designated by (g) Examples: –Ne (g), O 2(g), H 2 O (g)

7. Melting and Boiling Points Use Reference Table S to find the melting and boiling points of a solid, a liquid, and a gas ElementMelting PointBoiling Point Solid Liquid Gas

8. Write a general statement about how boiling point relates to phase.

9. Physical Properties –Characteristics that can be observed without changing the identity of the substance (no new substance is formed) Examples: Color, Hardness, melting point Physical Changes –Changes that occur without changing the identity of the substance Examples: Cutting, Ripping, Phase Changes

10. Chemical Properties –Characteristics that canNOT be observed without changing the identity of the substance (a new substance is formed) Examples: Reactivity, Flammability Chemical Changes –A change that results in a new substance Examples: Burning, Rusting Physical/Chemical Change Song

11. Physical/Chemical Examples Indicate if each of the following is physical or chemical 1. The boiling point of water is 100 o C. 2. Antacids will neutralize stomach acid. 3. Diamonds will cut glass. 4. Most metals conduct electricity. 5. The density of NH 3 is 0.77g/L. 6. Solution A and B are reacted together and a precipitate (solid) is formed. 7. 2 H 2 (g) + O 2 (g) → 2 H 2 O(l) 8. H 2 O(l) → H 2 O(g)

12. Classification of Matter  All matter can be classified as one of the following: –Elements –Compounds –Mixtures

13.  All matter can be described as: –Homogeneous – uniform throughout –Heterogeneous – different throughout  Classify the following as homogeneous or heterogeneous 1.A glass of water 2.Italian salad dressing 3.Turkey and gravy 4.Milk 5.Orange juice with pulp 6.Orange juice without pulp

14. Substances  Type of Matter – Element, Compound  All samples have identical properties and composition They are homogeneous They are homogeneous

15. Elements Composed entirely of atoms with the same atomic number Composed entirely of atoms with the same atomic number Cannot be decomposed Cannot be decomposed Found on the Periodic Table Found on the Periodic Table Begin with a capital letter Begin with a capital letter Homogeneous Homogeneous Examples: Cu, Fe, O 2, Ne Examples: Cu, Fe, O 2, Ne –Diatomic Element = contains two of the same atoms (O 2, H 2 )

16. Compounds Composed of at least 2 different elements Composed of at least 2 different elements Elements are chemically combined (bonded) Elements are chemically combined (bonded) Homogeneous Homogeneous

17. Compounds Can be decomposed (by chemical means) into 2 or more elements Can be decomposed (by chemical means) into 2 or more elements –Electrolysis, Reactions The properties of the component elements are usually very different from the properties of the compound The properties of the component elements are usually very different from the properties of the compound Combined in a definite ratio Combined in a definite ratio –In Sodium Chloride (NaCl) the Na and Cl must combine in a 1:1 ratio Examples: MgO, H 2 O, NaCl Examples: MgO, H 2 O, NaCl –Binary Compound = contains 2 different elements

18. Compare and contrast elements and compounds. ElementsCompounds Both

19. Mixtures Combination of 2 or more substances Combination of 2 or more substances No chemical change occurs (No bond is formed) No chemical change occurs (No bond is formed)

20. Mixtures Parts retain their individual properties Parts retain their individual properties Can be separated by physical means Can be separated by physical means –Filtering, Magnetism, Distillation, Density Can combine in varying ratios Can combine in varying ratios –The amount of salt in salt water can vary

21. Mixtures Can be heterogeneous Can be heterogeneous –Concrete, Dirt, Chocolate Chip Cookie Can be homogeneous Can be homogeneous –Gases (Air) –Aqueous Solutions – a solution made with water NaCl(aq) = salt is dissolved in water NaCl(aq) = salt is dissolved in water

22. Law of Conservation of Matter Matter cannot be created or destroyed

23. Law of Conservation of Mass Mass cannot be created or destroyed The mass before a reaction must be equal to the mass after the reaction

24. Law of Conservation of Energy Energy cannot be created or destroyed The amount of energy remains constant, however it may transfer forms http://www.youtube.com/watch?v=uyN9y0BEMqc

25. Exothermic Reactions Heat is released Heat is a product Surroundings will feel warm

26. Endothermic Reactions Heat is absorbed Heat is a reactant Surroundings will feel cold