2. 1

3.  Matter: anything that:  has mass and  takes up space  Mass:  a measure of the amount of “stuff” (or matter) the object contains.  (don’t confuse this with weight, a measure of gravity. Ex your weight on the moon is 1/6 here but your mass is the same!)  Volume:  a measure of the space taken up by the object Ex. Sun has 1.3 million times Earth’s volume and  Found with V = lxwxh or graduated cylinder. 2

4.  Density :  How squeezes or compressed the matter is.  Density Formula: d = m / V Density? 3

5.  Words that describe matter (adjectives)  Physical Properties:  a property that can be observed and measured without changing the material’s composition, A.K.A. formula or what it is.  Ex: color, density, hardness, melting/boiling point  Chemical Properties:  a property that can only be observed by changing the composition of the material leaving a new compound and formula  Examples- ability to burn, decompose, ferment, react with, etc. 4

6.  Physical Science: Properties of Matter Video Physical Science: Properties of Matter Video 5

7. 1)Solid: matter that can not flow (definite shape) and has definite volume.  Usually densest, slowest, low energy 2)Liquid: definite volume but takes the shape of its container (flows).  Usually mid density, mid speed, mid energy 3)Gas: a substance without definite volume or shape and can expand to any size.  Usually low density, fast speed, high energy 6

8. 7

9. States of Matter Solid Liquid Gas Definite Volume? YES NO Definite Shape? YES NO Result of a TemperatureI ncrease? Small Expans. Large Expans. Will it Compress? NO YES 8

10.  Physical change will change the visible appearance, without changing the composition of the material.  Boil, melt, cut, bend, split, crack  Is water vapor still water?  Can be reversible, or irreversible  Chemical change - a change where a new form of matter is formed.  Rust, burn/combust, decompose/rot ferment, react with. 9

11. A change in which one or more substances are converted into different substances. Heat and light are often evidence of a chemical change. 10

12. 1)Energy is absorbed or released (temperature changes hotter or colder) 2)Color changes 3)Gas production (bubbling, fizzing, or odor change; smoke) 4)formation of a precipitate - a solid that separates from solution (won’t dissolve) 5)Irreversibility - not easily reversed But, there are examples of these that are not chemical – boiling water bubbles, etc. 11

13. http://videos.howstuffworks.com/discovery/29395-assignment-discovery-elements-compounds- and-mixtures-video.htm 12

14. ‘ Pure ’ Substances are either: a) elements, or b) compounds 13

15.  simplest kind of matter  cannot be broken down anymore and still have properties of that element  all one kind of atom. 14

16.  Currently, there are 118 elements  Elements have a 1 or two letter symbol, and compounds have a formula.  An element’s first letter always capitalized; if there is a second letter, it is written lowercase: B, Ba, C, Ca, H, He  Start learning the elements names and symbols on your chart! Element quizzes!  Some names come from Latin or other languages; Fe ferrous-Iron; Au aurum-> gold 15

17.  Some elements exist and are ONLY stable by pairing with another atom of the same element—> diatomic elements 16

18.  substances that can be broken down only by chemical methods  made of two or more atoms, chemically combined (not just a physical blend or mix!)  can be broken down into simpler substances by chemical means (elements cannot)  H2O  NaCl  SiO2 17

19.  Quite different properties than their component elements.  Due to a CHEMICAL CHANGE, the resulting compound has new and different properties: Table sugar – carbon, hydrogen, oxygen Sodium chloride – sodium, chlorine Water – hydrogen, oxygen 18

20.  2 or more atoms may be chemically bonded in two different ways: 1. ionic bonding 2. covalent bonding 3. Metallic bonding****** 19

21.  Ionic bonding  metal chemically bonded with another nonmetal  electrons are transferred metalnonmetal 20

22.  Covalent bonding  nonmetal chemically bonded with another nonmetal  electrons are shared nonmetal nonmetal 21

23.  Mixtures are a physical blend of at least two substances; have variable composition. They can be either: 1)Heterogeneous mixture– the mixture is not uniform in composition Chocolate chip cookie, gravel, soil. 2)Homogeneous mixture - same composition throughout; called “solutions” Kool-aid, air, salt water  Every part keeps it’s own properties. 22

24. CompoundMixture Made of one kind of material Made of more than one kind of material Made by a chemical change Made by a physical change Definite composition Variable composition 23 material Made by composition

25. Element Compound Mixture 24

26.  Heterogeneous Mixture  uneven distribution of components  colloids and suspensions  EX: granite 25

27.  Colloid  medium-sized particles  Tyndall effect - particles scatter light (looks cloudy)  Light test.  particles never settle  EX: milk 26

28.  Suspension  large particles  particles scatter light  particles will settle (needs to be shaken)  EX: fresh-squeezed lemonade  OJ 27

29.  Mixed molecule by molecule, thus too small to see the different parts They are dissolved into each other!  Can occur between any state of matter: gas in gas; liquid in gas; gas in liquid; solid in liquid; solid in solid (alloys), etc.  Thus, based on the distribution of their components, solutions can also be called called homogeneous phases or heterogeneous phases. 28

30.  Some can be separated easily by physical means: rocks and marbles, iron filings and sulfur (use magnet)  Differences in physical properties can be used to separate mixtures.ex density, melting/boiling points, size, etc.  Filtration - separates a solid from the liquid in a heterogeneous mixture (by size) 29

31. Components of some solutions with colored compounds such as ink may be separated by paper chromatography. Molecular mass for each compound is different so they can’t travel the same distance. 30 Large molecules Small molecules

32. Distillation: takes advantage of different boiling points. NaCl boils at 1415 o C 31

33.  The ability of a substance to undergo a specific chemical change is called a chemical property. iron plus oxygen forms rust, so the ability to rust is a chemical property of iron  During a chemical change (also called chemical reaction), the composition of matter always changes.  This indicates a chemical ‘reaction’ 32

34.  When one or more substances are changed into new substances.  Reactants- the stuff you start with  Products- what you make  The products will have NEW PROPERTIES different from the reactants you started with  Arrow points from the reactants to the new products  EX CH4 + O2  CO2 + H2O  EX Fe + O2  Fe2O3 33

35.  chemical reactions video from discovery education chemical reactions video from discovery education  You tube reactions  http://www.youtube.com/watch?v=VVxWucoVn 9A&noredirect=1 http://www.youtube.com/watch?v=VVxWucoVn 9A&noredirect=1 34

36.  During any chemical reaction, the mass of the products is always equal to the mass of the reactants.  All the mass can be accounted for:  Burning of wood results in products that appear to have less mass as ashes; where is the rest?  Law of conservation of mass 35

37. - Page 55 reactants = product 43.43 g Original mass = 43.43 g Final mass 36