1. Chemistry deals with the properties of matter.
Matter is anything that has mass and takes up space (volume)
This and that fjalkdfja
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2. Chemistry is the study of matter and the changes that it undergoes
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. Any substance with a definite composition
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
Potassium permanganate KMnO4, Glycerol C3H5(OH)3,

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. Weight is the effect of Earth’s gravity on a mass
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. 4

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

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 21

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 Vs. Base Acid: pH of less than 7 Base: pH of more 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

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… 28

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 30

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