1. States of Matter

2. Matter Matter – anything that has mass and takes up space Everything around us Mass: measurement that reflects the amount of matter (usually in grams) Volume: the amount of space something takes up Chemistry – the study of matter and the changes it undergoes

3. Four States of Matter Solids particles vibrate but can’t move around fixed shape fixed volume incompressible

4. Four States of Matter Liquids particles can move around but are still close together variable shape fixed volume Virtually incompressible

5. Four States of Matter Gases particles can separate and move throughout container variable shape variable volume Easily compressed Vapor = gaseous state of a substance that is a liquid or solid at room temperature

6. Four States of Matter Plasma particles collide with enough energy to break into charged particles (+/-) gas-like, variable shape & volume stars, fluorescent light bulbs, TV tubes

7. Bunsen Burner

8. Physical Properties Physical Property can be observed without changing the identity of the substance

9. Physical Properties Physical properties can be described as one of 2 types: Extensive Property depends on the amount of matter present (example: length, mass, volume) Quantitative data Intensive Property depends on the identity of substance, not the amount (example: scent, density) Qualitative data

10. Chemical Properties Chemical Property describes the ability of a substance to undergo changes in identity

11. Physical vs. Chemical Properties Which property is it? melting point flammable density magnetic tarnishes in air physical chemical physical chemical

12. Physical Changes Physical Change changes the form of a substance without changing its identity properties remain the same Examples: cutting a sheet of paper, breaking a crystal, all phase changes

13. Phase Changes – Physical Evaporation = Condensation = Melting = Freezing = Sublimation = Deposition= Liquid -> Gas Gas -> Liquid Solid -> Liquid Liquid -> Solid Solid -> Gas Gas -> Solid

14. Phase Change Graph Temp, o C Solid only, Q = m ΔT C psolid Q = mol x ΔH fusion Solid & liquid Liquid only Q= m ΔT C pliquid Q = mol x ΔH vapor Liquid & gas Time, min Temperature vs. Time Gas Only

15. Energy cannot multitask! Energy either -raises the temperature or -is used to break bonds IT CAN’T DO BOTH AT THE SAME TIME

16. Chemical Changes Process that involves one or more substances changing into a new substance Commonly referred to as a chemical reaction New substances have different compositions and properties from original substances

17. Chemical Changes Signs of a Chemical Change change in color or odor formation of a gas formation of a precipitate (solid) change in light or heat

18. Physical vs. Chemical Changes What type of change? rusting iron dissolving in water burning a log melting ice grinding spices chemical physical chemical physical

19. Exothermic- heat energy EXITS the system - ex. Combustion, evaporation of water - surroundings usually feel warmer

20. Endothermic- heat energy ENTERS the system - ex. Cold packs, melting ice - surroundings usually feel cooler

21. What Type of Change?    

23. Law of Conservation of Mass Although chemical changes occur, mass is neither created nor destroyed in a chemical reaction Mass of reactants equals mass of products mass reactants = mass products A + B  C

24. Building blocks of matter Atom: Composed of protons, electrons, and neutrons Smallest particle of matter that can be identified as one element Molecules: A collection of atoms chemically bonded together May be element or compound

25. Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yes no Can it be chemically decomposed? noyes Is the composition uniform? noyes

26. Pure Substances Element composed of identical atoms EX: copper wire, aluminum foil

27. Pure Substances Compound composed of 2 or more elements in a fixed ratio properties differ from those of individual elements EX: table salt (NaCl)

28. Mixtures  Variable combination of 2 or more pure substances. HeterogeneousHomogeneous

29. Mixtures Solution homogeneous very small particles particles don’t settle EX: rubbing alcohol

30. Mixtures Heterogeneous medium-sized to large-sized particles particles may or may not settle EX: milk, fresh- squeezed lemonade

31. Mixtures Examples: tea muddy water fog saltwater Italian salad dressing Answers: Solution Heterogeneous Solution Heterogeneous

33. Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yes no Can it be chemically decomposed? noyes Is the composition uniform? noyes

34. Matter Flowchart Examples: graphite pepper sugar (sucrose) paint soda element hetero. mixture compound hetero. mixture solution