Chemistry deals with the properties of matter.

1. Chemistry deals with the properties of matter. • Matter is anything that has mass and takes up space (volume)

2. Chemistry and Matter Chemistry is the study of matter and the changes that it undergoes You depend on Chemicals everyday for: Cooking, Film, Laundry, Asprin

3. What is a Chemical? Any substance with a definite composition

4. Physical states of matter • There are three states of matter • Solids • Liquids • Gasses

5. States of Matter • States of matter can be changed by a change in temperature or pressure • Solid – definite shape and volume, particles slightly vibrate, incompressible, dense • Liquid – no definite shape, definite volume, particles flow freely, slightly compressible, less dense • Gas – no definite shape or volume, particles are not confined and move continuously, very compressible, least dense • *vapor – gaseous state of a substance that is solid or liquid at room temp

6. Chemical reactions describe how matter behave. • Chemical reaction: The process by which elements and/or compounds interact with one another to form new substances

7. Chemical reaction ------ Carbon dioxide + water + energy ----Sugar + oxygen Reactants Products

8. Exothermic reaction • Rxn. in which energy is released • Potassium permanganate & glycerol

9. Endothermic reaction • A reaction in which energy is absorbed • barium hydroxide solid with ammonium chloride cause water to freeze.

11. Stop

12. Matter • Anything that has a mass and volume

13. Mass and Weight Weight is the effect of Earth’s gravity on a mass Mass - same no matter where an object is located Weight changes as the amount of gravity changes.

14. Units of Measurement • SI units are metric system which uses seven base units • The 4 you need to know now are meter, kilogram, second, Kelvin • SI units range from very small to large measurements. • Area , volume, pressure, weight are derived units - which means they are a combination of base units

15. Conversion for SI units KATHY HOW DOES MY DOG CATCH MICE K = Kilo H = Hecta D = Deca M = meter/liter/gram d = deci c = centi m = milli These are the common ones T = Tera G = Giga M = Mega K = Kilo ~ m = milli m = micro n = nano But we went both higher and lower ;~)

16. Jordan’s mnemonic device • Tell Granny Melisa Kites Hovering Don’t make due ‘cause my mom’s napping

17. Conversion • 1 foot = 12 inches • 3 feet = 1 yard • 1 inch = 2.54 cm • 5280 feet = 1 mile • 1Km = 10 Dm • 1 Km = 100 Hm • 1 Km = 1000 m • 1 m = 100 cm • 1 m = 1000 mm • 1 cm = 10 mm

18. Making measurements • Length – the straight line distance between any two points • Mass – measure of the quantity of matter in an object • Volume – a measure of space such as the capacity of a container • Weight – the force with which gravity pulls on a quantity of matter

19. Physical Properties • Can be observed without changing the composition of a substance • Ex – size, shape, color, mass, volume, length, density, boiling point, melting point, freezing point, state of matter, hardness, smell, taste, Cutting, crushing, bending, dissolving

20. Chemical Properties • Totally changes the identity of the substance; Only observed through chemical reactions • Ex. Corrosive, combustible, ability to react with a substance, inability to react, explode, rust, oxidize, tarnish, ferment, rot, cook • Indicators of a chemical rxn: temperature change, odor change, color change, formation of a precipitate, gas produced

21. What is the nature of matter Element – cannot be broken down into a simpler substance (ex: oxygen, hydrogen) Atom – smallest particle that has property of an element

22. Compound – made of more than one element (ex: water;h2o) • Molecule – a neutral group of atoms held together by covalent bonds

23. Allotrope • One of a number of different forms of an element • Ex. O2 and O3;graphite, diamond, Buckyball, Bucky tube

24. Compounds • Substance composed of two or more different elements • Covalent vs. Ionic • Acid and Base • Organic or inorganic

25. Covalent Vs. Ionic • Covalent compounds share electrons • EX. Water, sugar and oxygen • Ionic compound – compounds that has an electric charge. • Ex. Table salt

26. Acid: pH of less than 7 Ex. Aspirin pH=2.7 Tastes sour Turns blue litmus paper red Base: pH of more than 7 Ex. Ammonia pH=11.6 Tastes bitter and feels slippery Turns red litmus paper blue Reacts with acid to produce salt Acid Vs. Base

27. Organic Vs. Inorganic • Organic compounds: contain carbon, hydrogen, oxygen and other trace elements • Inorganic compound: generally do not have carbon

28. Chemical Formulas Tells what elements & how many atoms of each element are found in a substance Ex: Indigo = C16H10N2O2 Each molecule has 16 carbon atoms, 10 hydrogen atoms,etc…

29. Pure substance • Any matter that has a fixed composition and definite properties (water) • Pure substance such as water can not be broken down by physical action such as boiling, melting or grinding

30. Types of Mixtures Homogeneous – (same) mixture that is uniformly mixed Heterogeneous (different) – mixture where substances are not uniformly mixed

31. Heterogeneous and Homogeneous • Heterogeneous Mixture – Like Sand in water • Homogeneous Mixture – Like Salt in water

32. Miscible vs. Immiscible Miscible and immiscible refers to liquid Miscible - two liquids dissolve in each other Ex: Alcohol and water Immiscible – a heterogeneous mixture

33. Separating mixtures • React a substance and remove it via filtration technique