1. How does it relate to your world
Intro to Chemistry
How does it relate to your world

2. Things to think about…
How many ways does chemistry apply to your life?
Of those ways, which holds the most merit?
Why do I need to know chemistry?

3. What is Chemistry?
The study of the composition of matter and the changes that matter undergoes
Matter is anything that has mass and occupies space
Affects ALL aspects of life and most natural events

4. Areas of Study Organic – study of all chemicals containing Carbon
Inorganic – study of all chemicals not containing Carbon
Biochemistry – study of the processes that take place in organisms
Analytical – study that focuses on the composition of matter
Physical – study that deals with the mechanism, the rate, and the energy transfer that occurs when matter undergoes change

5. Organic Chemistry
ALCOHOL
ETHER
BENZENE

6. Inorganic Chemistry Calcium Carbonate CaCO3 Sodium Chloride NaCl
Calcite
Halite
Quartz
Calcium Carbonate
Sodium Chloride
Silicon Oxide
CaCO3
NaCl
SiO2

7. Biochemistry
Plants!

8. Analytical Chemistry

9. Physical Chemistry

10. Pure v. Applied Pure chemistry – research for research’s sake Nylon
Applied chemistry – research for a purpose
Aspirin

11. The Scientific Method

12. Purpose
Answers why we are doing the experiment

13. Research
Research is needed to gain information on the purpose of the experiment
This information will be used to form a hypothesis

14. Hypothesis Means educated guess
This is a proposed answer to the problem developed in the purpose

15. Experiment An experiment tests your hypothesis
The experiment will contain different variables
Independent Variable – Variable that is changed
Dependent variable – measured based on the changes of the independent variable
Control – used as a comparison to measure results

16. Data Always record data in a clear, understandable way
Use charts and graphs to show data whenever possible

17. Analysis and Conclusion
Analysis is the collection of data from the experiment which should suggest a result
The conclusions states the result of the experiment and whether or not the hypothesis was correct or incorrect

18. Define the Variables for the Ants
Independent Variable =
Dependent Variable =
Control =
Length of their legs
Number of steps taken
Regular Ant

19. Talk it out… How would I find the best basketball shoe?
How would I know the best type of grass for an athletic field?
How would I know which detergent cleans clothes the best?

20. Qualitative v. Quantitative
Qualitative = qualities, properties, or descriptions
Quantitative = numbers, measurements, or calculations
Give me two examples of each

21. Accuracy v. Precision
Accuracy – a measure of how close a measurement gets to the apparent or true value of whatever is measured
Precision – a measure of how close a series of measurements are to one another

22. Por Ejemplo

23. Ejemplo dos

24. Ejemplo tres

25. Por Ejemplo

26. International System Giga G Billion 109 1,000,000,000 Mega M
Prefix
Symbol
Meaning
Multiply By:
Giga G
Billion 109
1,000,000,000
Mega M
Million 106
1,000,000
Kilo k
Thousand 103
1,000
Deci d
Tenth 10-1 .1
Centi c
Hundredth 10-2
.01
Milli m
Thousandth 10-3
.001
Micro
Millionth 10-6
Nano n
Billionth 10-9
International System

27. Measurements Length meter m Mass grams g Temperature Kelvin K Time
Quantity
Unit
Symbol
Length
meter m
Mass
grams g
Temperature
Kelvin K
Time
Second s
Amount of a substance
Mole
mol
Electric Current
Ampere A

28. Derived Units Quantity Unit Symbol Area Square meter m2 Volume
Cubic meter or Liter
m3 or L
Density
kilograms per cubic meter
kg/m3
Pressure
Pascal (kg/m*s2) Pa
Energy
Joule (kg*m2*s2) J
Frequency
Hertz (1/s) Hz
Electric Charge
Coulomb (A*s) C

29. Practice mm mg cg cm km Gg Mm ng mL kL millimeters milligrams
centigrams
centimeters
kilometers
Gigagrams
Megameters
Nanograms
Milliliters
kiloliters

30. The Estimated Digit
In chemistry we will measure materials to an estimated digit
An estimated digit is a magnitude smaller than the tool we are measuring with
We can only go one magnitude because we want to be as accurate as possible

31. Practice
3.2 cm
2.35 cm
36.3 mL

32. Scientific Notation
Written as the product of two numbers: a coefficient and 10 raised to a power
Therefore: 602,000,000,000,000,000,000,000
Equals: 6.02x1023
Or:
Equals: 7.75x10-10

33. Significant Figures
Includes all the digits that are known PLUS a last digit that is estimated when measuring
Calculations are based on significant figures!!!
Significant figures are based on a set of rules

34. Significant Figure Rules
Every nonzero digit in a reported measurement is assumed to be significant
Zeros appearing between nonzero digits are significant
Left most zeros appearing in front of nonzero digits are not significant
Zeros at the end of a number and to the right of a decimal point are ALWAYS significant

35. Significant Figure Rules
Zeros at the right most end of a measurement that lie to the left of an understood decimal point are not significant if they serve as place holders to show the magnitude of the number, if zeros are at the right of a decimal point, they are significant
Exact quantities have an unlimited amount of significant figures

36. Starting Number NO YES Infinite sig figs YES NO YES NO NO YES
Is number counted?
Infinite sig figs
Does number have a decimal?
YES NO
Are zeroes at the front?
YES
All digits except leading zeroes
Are there zeroes trailing? NO NO
YES
All numbers are sig figs
All digits except trailers

37. Examples / Practice 3 (Rule 1) 123 m 5 (Rule 4) 9.8000 x 104 m
40506 mm
22 meter sticks
98000 m
3 (Rule 1)
5 (Rule 4)
4 (Rule 2, 3, 4)
5 (Rule 2)
Unlimited (Rule 6)
2 (Rule 5)

38. On Your Own! m
143
8.750x10-2m
8765m m
0.074m
1.072m 4 2 3 5

39. Adding and Subtracting
The answer to an addition or subtraction calculation should be rounded to the same number of decimal places (not including sig figs) as the measurement with the least number of decimal places
Ex m m m =
Therefore:  369.8

40. Practice
8.3 m m
8432 m m
35.2 sec sec
52 m – m
m m
2.10 m m
1780 m m
53.6 g g
10.5 m
8420 m
2582 sec
52 m
10.9 m
2.03 m
1780 m
53.6 g

41. Multiplying and Dividing
Round the answer to the same number of sig figs as the measurement with the least amount of sig figs
Ex. 7.55m x 0.34m = 2.567m2
Therefore: 2.567m2  2.6m2

42. Practice 18m2 8.3m x 2.22m 675m 8432m / 12.5 89700 sec 35.2 sec x 2547
53.6g /
18m2
675m
89700 sec
.22m2
.29
.15m2
20000m or 2x104m
96000m or 9.6x104m

43. Conversions
Units can be converted from one to another using a conversion factor or a simple equation
Chemistry using conversions for mass, volume, and parts

44. Conversion Factors

45. Conversion Steps
Starting Unit
Conversion Factors

46. Conversion Practice 250 kPa (253.35) 2.5 atm  kPa 2000 J (1672)
400 Cal  J
75 °F  °K
356 g  lbs
250 kPa (253.35)
2000 J (1672)
3.0x102°K (296)
.784 g