1. Chapter 2 “Matter and Change” p. 38

2. Describing Matter Properties:
Extensive – depends on amt of matter in sample
- ex’s. mass, volume, calories, magnetism
Intensive – depends on type of matter, not amt.
Hardness, Density, B.P.
All samples of same substance have same intensive prop’s. (same composition)

3. Identifying Substances
Physical Properties- observed & measured w/o changing composition
color, hardness, m.p., b.p.
Chemical Properties- observed by changing comp of material
ability to burn, decompose, ferment, react w/, etc.

4. Solid- cannot flow (definite shape & volume)
States of matter
Solid- cannot flow (definite shape & volume)
Liquid- definite vol - takes shape of container (flows)
Gas- w/o definite vol or shape & flows
Vapor- gaseous but normally liquid or room temp
water “gas”, or water “vapor”?

5. Three Main Phases – page 41

6. States of Matter Definite Volume? Definite Shape? Solid Liquid Gas
Result of a Temperature Increase?
Definite Volume?
Definite Shape?
Will it Compress?
Small Expans.
Solid
YES
YES
Not easily
Small Expans.
Liquid
Not easily NO
YES
Large Expans.
Gas NO NO
YES

7. 4th state: Plasma - formed at hi temps; ionized phase of matter (Sun)

8. Sublime
Condense
Freeze
Evaporate
Melt
Solid
Liquid
Gas

9. Physical vs. Chemical Change
Physical change changes visible appearance w/o changing comp of material
Boil, melt, cut, bend, split, crack
Is boiled water still water?
Reversible, or irreversible
Chemical change - change where new substance formed
Rust, burn, decompose, ferment

10. Section 2.2 Mixtures p. 44 Mixture - physical blend of 2+ components
Heterogeneous – uniform in comp
Choc chip cookie, gravel, soil
Homogeneous - same comp thruout
(solutions)
Kool-aid, air, salt water
Every part keeps own prop’s

11. Solutions - homogeneous mixtures
Mixed molecule by molecule, so too small to see diff pts
occurs btwn any state of matter: gas-gas; liquid-gas; gas-liquid; solid-liquid; solid-solid (alloys)
Steel (Fe, Cr & Ni)

12. Phase?
“phase” describes any pt of sample w/ uniform comp of properties
A homogeneous mixture consists of a single phase
A heterogeneous mixture consists of two or more phases.
Note Figure 2.6, page 45

13. Differences in physical props used to separate mixtures
Separating Mixtures
Some by physical means: rocks & marbles, iron filings & sulfur (magnet)
Differences in physical props used to separate mixtures
Filtration - separates solid from liquid in hetero mix. (by size) – Figure 2.7, page 46

14. Separation of a Mixture
Distillation: takes advantage of different boiling pts.
NaCl boils at 1415 oC
H2O boils at 100 oC
Mg boils at 1107 oC

15. Separation of a Mixture
Components of dyes such as ink may be separated by paper chromatography.
Forensic Ink Analysis
Chromatography video

16. Applications of Chromatography
2 Greek words:
chroma "color" and “graphein "to write"
Biological labs:
ID amino acids
detects drugs in urine
Environmental labs:
ID contaminants in waste oil
pesticides in groundwater
test drinking water & test air quality
Pharmaceutical companies
prepare quantities of extremely pure materials.
Food industry
ID contaminants like aflatoxin
naturally occurring toxin produced by fungus

17. Sec 2.3 Elements & Compounds p. 48
Substances are either: a) elements, or b) compounds

19. Compounds v.s. Mixtures

20. Which is it?
Compound
Mixture
Element

21. Chemical Change Heat & light often indicate chem chg
A “chemical change” chg producing matter w/ diff. comp than original matter
1+ substances are converted into different substances.
Heat & light often indicate chem chg

22. Classification of Matter

23. Symbols & Formulas 118 elements 1 - 2 letter symbol
1st letter CAP; 2nd letter lowercase
B, Ba, C, Ca
Some names Latin
Table 2.2, page 52
cmpds have formula
H2O, NaCl, C12H22O11

24. Sec 2.4 Chemical Rxns p. 53 Chemical Changes
Chemical property - ability of substance to undergo specific chem change
Fe + O = rust
rusting - chem prop of Fe
During chem chge comp of matter always changes

25. Chemical Rxns are…
When 1+ substances changed into new substances
Reactants- start w/
Products- end w/
Products have NEW PROPS diff from reactants
Arrow points from reactants to new products

26. Recognizing Chemical Changes
Energy absorbed/released (temp changes hotter/colder)
Color changes
Gas production (bubbling, fizzing, or odor change; smoke)
precipitate forms - solid separates from solution (won’t dissolve)
Irreversibility - not easily reversed
Some ex’s not chem – boiling water bubbles, choc syrup in milk, etc.

27. Law of conservation of mass
During any chem rxn, product mass = reactant mass
All mass accounted for:
Burning wood results in products that appear to have less mass (ashes)….
CO2 & H2O vapor
Law of conservation of mass

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

29. Using your online textbook:
Due by Friday 9/22:
Page 42 #1-7  
Page 47 #11-16
Page 52 #20-27
Page 55 #28-34