1. IB/Accelerated Chemistry
Larry J. Scheffler
Lincoln High School
1600 SW Salmon
Portland, OR 97205

2. IB/Accelerated Chemistry
Instructor : Mr. Larry J. Scheffler
Web:
Instructor : Mr. Larry J. Scheffler
Web:
Copy this web address and set a bookmark on your web browser. You will be using this site all year 2

3. Class Information Form
Your Name
Code name (use something that you will remember, I will
post grades under that name)
Address
Telephone Number
School ID Number
Year in School
Check previous math and science classes
Check computer experience and skills
Answer the four questions that follow 3

4. IB Chemistry 1-2 Agenda Periods 1 , 3, and 5 Information forms
Brief overview of the course
Access to information on the internet
Class Policies
Safety contracts
Chemical Hazards
Scientific Methods
Assignments 4

5. IB Chemistry 1-2 Assignments
Tomorrow: Read the Lab Density Determination
Begin reading through
Next week: Read chapter 1 in textbook
Tuesday Sept 15: Return signed the PPS Safety Agreement and read thoroughly the chemical hazards handout 5

6. Introduction to Chemistry
The study of matter and its relationships
The study of materials and how they
interact
The Central Science 6

7. Chemistry Topics Include
Atomic Theory
Periodic Table
Bonding
Formulas and Stoichiometry
States of matter
Calorimetry / Thermodynamics
Solutions
Kinetics
Equilibrium
Acids and Bases
Oxidation Reduction 7

8. Is Chemistry Hard??
Maybe! --- but you will develop skills that are valuable for the rest of your life! 8

9. Is Chemistry Hard?? Well maybe but you will develop skills
that are valuable for the rest of your life
These include:
Abstract Thinking
Critical Thinking
Analysis
Logic
Math Skills 9

10. Is Chemistry Hard?? Well maybe but you will develop skills
that are valuable for the rest of your life
These include:
Problem Solving
Communication
Time Management
Hazards Management
Abstract Thinking
Critical Thinking
Analysis
Logic
Math Skills 10

11. Chemical Hazards Hazard Criteria
A Threshhold Limit value of less than 500 ppm
A Lethal dose (LD50) less than 500mg per kg
Readily polymerizable
Flashpoint less than 140oF
A strong oxidizer or reducing agent
Highly corrosive
Carcinogen, mutagen,or teratogen
Radioactive
See the handout for more definitions and criteria for chemical hazards 11 11

12. Scientific Methods Always based on observation and experimentation
Observable and reproducible evidence are required to support conclusions 12

13. Scientific Method Investigation process - Preliminary observations
- Formulation of a hypothesis
Design experiments to test the hypothesis
Evaluate and interpret data
Draw appropriate conclusions 13 13

14. Scientific Methods
The scientific method is not necessarily a chronological order that scientists always follow.
But remember ………..
Scientific information is always based on evidence. The emphasis is always on information that we can gain from observations and experiments 14

15. Hypothesis, Theory and Law
A Hypothesis is a tentative explanation or expected result based on past evidence and experience
A Theory is an explanation of a phenomona based on the results of scientific experimentation.
A Law is a principle that can be observed repeatedly in the world over a long period of time 15

16. Matter Has both volume and mass Exists in various states: Solid Liquid
Gas
Plasma 16

17. Forms of Matter
Element
Compound
Mixture
Homogeneous
Heterogeneous 17

18. Elemental Composition of the Earth

19. Properties of Matter Physical - Chemical - Extensive - Intensive -
Color
Density
Melting point
How the substance reacts with other substances
Depend on the amount of material
Independent of the amount of material 19

20. Density Definition Formula Ratio of mass to volume D = Mass/ volume
Density is an intensive property. It is constant for most solids and liquids, but it depends on the pressure and temperature for a gas
Definition
Formula 20

21. Physical and Chemical Changes
A change in state or shape. Affects the physical properties but retains the properties of the substance
Undergoes a chemical reaction. A new substance is formed with new physical and chemical properties 21

22. Problem Solving Density
If you solve the formula correctly the units will match
D = m/V = g/cm3
M = DV = (g/cm3) /(cm3) = g
V = m/D =(g)/(g/cm3) = cm3
Formulas
Density = Mass/volume
D = m/V
M = DV
V = m/D
Units
Density = g/cm3
Mass = grams or g
Volume = cubic centimeters or cm3

23. Temperature Scales Kelvin Celsius Fahrenheit Boiling point of water.
100 oC
212 oF
Freezing point
273 K
32 oF
Absolute Zero.
0 K
-273 oC
-460 oF 23

24. Temperature Conversions
Fahrenheit to Celsius
oC = 5/9 ( oF - 32)
Celsius to Fahrenheit
oF = 9/5 oC
Celsius to Kelvin
K = oC +273 24

25. Measurement
Measurements in the laboratory will normally be made using the metric system and SI units where feasible 25

26. Measurement Issues Uncertainty Accuracy Precision Error
Significant Figures
Scientific Notation 26

27. Uncertainty in Measurements
All measurements are limited by the instruments used to make them
The uncertainty of a measurement depends on the quality with which a measurement is made
The uncertainty depends on the precision and accuracy of the measurement 27

28. Accuracy and Precision
Accuracy is the degree of closeness of a measured or calculated quantity to its actual (true) value.
Precision is also called reproducibility or repeatability. It is the degree to which further measurements or calculations show the same or similar results.
In other words
Accuracy refers to the proximity of a measurement to the true value of a quantity.
Precision refers to the proximity of several measurements to each other. 28

29. Accuracy and Precision
A measurement may be either accurate or precise, both or neither. 29

30. Significant Figures
A measurement is always limited by the precision of the
Instrument. An understanding of significant figures is important to express the appropriate precision of a measurement
Only zeros can be non-significant digits
There are two cases where a zero may be non significant:
Zeros at the end of numbers greater
than 1 that do not refer to a precise count
Zeros in front of the first non zero digit in
numbers less than 1 30

31. Significant Figures
The zeros shown in red are not significant. The number is precise to 4 significant digits
With numbers having a zero at the end the number of significant figures depends on the precision with which the number is known.
one significant digit. The number is known to the nearest ten thousand.
three significant digits. The number is known to the nearest hundred.
five significant digits. The number is known to the nearest unit. 31

32. Scientific Notation
Large numbers are hard to visualize. Scientific notation writes numbers in two parts: a number between 1 and 10 and a power of 10
Examples
3.00 x 108 rather than
4.82 x rather than 32

33. Error
The error in a measurement refers to the degree of fluctuation in a measurement. It is usually expressed as a + value
Example: a measurement of a mass from the scale could be recorded as g g.
It is often helpful to record measurements as relative error or percent error 33