1. Chapter 1 Chemical Foundations

2. `
If data/observations do not support your hypothesis, you must start over

3. SI Base Units Quantity Unit Symbol Length meter m Mass kilogram kg
Time second s
Electric current ampere A
Temperature Kelvin K
Amount of substance mole mol
Luminous intensity candela cd

4. How do we get from one unit to another unit?
Dimensional Analysis- converting from one unit to another
Use a conversion factor Ratio
1m = 100cm= 1000mm
Do a couple of examples from the practice worksheet.
Have students work selected examples for homework. Check answers the next day by putting them on the overhead transparency.

5. Using Scientific Measurements
Significant Figures- those digits known with certainty plus one estimated digit
Rules for Determining Sig. Figs.
a. All nonzero digits are significant
b. Zeros between nonzero digits are sig.
c. Zeros appearing in front of all nonzero digits are not significant
d. Zeros at the end of a number and to the right of a decimal point are significant
e. Zeros at the end of a number may or may not be significant. Depends if there is a decimal.
Percent error was defined in the lab.
Examples:
145= 3 sig fig.
1024= 3 sf
40.7= 3 sf
87009= 5 sf
.0056= 2 sf
.00009= 1 sf
.00306= 3 sf
85.00= 4 sf
= 10 sf
2000 = 1 sf
2000. = 4 sf

6. Cont. Rounding Rules greater than 5, increase by 1
less than 5, stay the same
5 followed by nonzero digit(s), increase by 1
5, not followed by nonzero digit(s), and preceded by an odd digit, increase by 1
5, not followed by nonzero digit(s), and the preceding s.f. is even, stay the same
Examples:rounder to 3 S.F.
42.68  42.7
17.32 17.3
 27.9
4.635  4.64
78.65  78.6

7. Cont. Addition or subtraction
the answer must have the same # of digits to the right of the decimal point as there are in the measurement having the fewest digits to the right of the decimal point
Multiplication and division
the answer will have the same number of significant figures as the measurement with the fewest number of sig. figs.
Add/sub example
 2 digits
 5 digits
 2.89
Mult./division example
 5 SF
x  3 sf
 121

8. Cont. Scientific Notation uses the form, M x 10n
M is a number greater than or equal to one but less that 10
n is a whole number
1. Determine M by moving the decimal pt. to the left/right so that only 1 nonzero digit remains to the left of the decimal pt.
2. Determine n by counting the number of places you moved the decimal pt. If you moved it left, n is positive. If you moved it right, n is negative.
chemistry deals with very large and very small numbers
To make it easier we use scientific notation
x 10-4
x 100
23,000, x 107

9. Temperature TK= TC + 273.15 TC= TK - 273.15 TF= TC • 9/5 + 32
TC = (TF –32) • 5/9
Widely used scales are Fahreheit, celsius, and Kelvin

10. Density D= m/v States Of Matter 1. Solid fixed volume and shape
2. Liquid  fixed volume, variable shape
3. Gas  variable volume and shape
4. Plasma high temperature physical state in which atoms lose their electrons
Plasma is found in a fluorescent bulb

11. Classification of Matter
Pure Substances
- made of only one kind of atom or molecule
a. Elements- contains only one kind of atom or molecules
examples of molecules are N2, O2
b. Compounds- 2 or more elements chemically combined
examples: NaCl, CO
Nitrogen and oxygen are diatomic
Allotrope different forms of an element
Example: carbon, graphite, diamond
oxygen, ozone

12. Classification cont. Mixtures
- a blend of 2 or more pure substances physically mixed together
a. Homogeneous Mixture- uniform in composition
also known as a Solution(small particles)
Colloid-contains intermediate sized particles
b. Heterogeneous Mixture- not uniform throughout
Suspension-separates into layers over time
Mixtures can be separated physically
Cannot be represented by a chemical formula
Proportions varies
Examples of solutions- tap water, Kool Aid, soda
Examples of colloids- milk, gels, foams
Examples of suspension- salad dressings, “shake well’

13. Separation of Mixtures
Magnetism
Filter
Evaporation
Centrifuge
Decant
Chromatography
Distillation
Density
-metal from nonmetal
Liquids and particles smaller that filter pores
Filtrate- substance collected
Liquids evaporates and leaves solid behind
Separates matter of different densities
Pour off liquid and leave solid behind
Separates components of a solution
Separates substances with dif. Boiling points
Ratio of mass tp volume

14. Lesson Plans Day 1: Intro. To class: guidelines,books, etc.
Individual notes:
PHEOC
SI base units(7)
Dimensional analysis
Density

15. continued States of matter
Classification of matter- find handout, define on sheet
Separation of mixtures methods
Day 2 and 3
Show slides 5-9
HW. P : 24,26,28,30,36,48,54,60,68,80

16. Cont.
Day 4
Lab
Day 5
Ch. 1 Test