1. Notes for Measurement & Matter Unit

2. Uncertainty in Measurements
Accuracy
Precision
Error
Percent Error

3. Importance of Measurements
Types of measurements
1.Qualitative
Examples:
2. Quantitative

4. Scientific Notation Rules for writing scientific notation: Examples:
a. Number must be between 1 and 9
b. Positive exponent = LARGE number
c. Negative exponent = SMALL number
Examples:
1.9 x 109 is written correctly and is a large number
19.8 x 109 is written incorrectly because it is not a number between 1 and 9
1.98 x is written correctly and is a small number

5. You will ask yourself ‘why’
Significant Figures – Why?!?
In a calculation, it is important to know which digits are significant
Last digit is uncertain (estimated or guess) because each person may see it slightly different
You will ask yourself ‘why’
all semester!

6. *Rules for calculating using sig figs
Rounding
(pg 40)
Adding and subtracting
(pg 41)
Multiplying and dividing
(pg 42)

7. The universal system modern scientists use for measurement is…

8. THE METRIC SYSTEM!!!!
FORGET THE ENGLISH SYSTEM!!!! The only time you will see the English system is when converting to metric!

9. The Systeme International (SI)
Unit
Symbol
Value
Kilo- k-
1000 or 103
Meter m
Base unit
Centi- c-
1/100 or 10-2
Milli- m-
1/1000 or 10-3
Micro- µ-
1/1,000,000 or 10-6
Nano- n-
1/1,000,000,000 or 10-9
1000 m = 1 km
1 L = 1000 mL
1 g = 100 cg

10. Measuring Length Volume Mass Equipment and units Meniscus
Weight vs. mass

11. Dimensional Analysis You have probably used without knowing it
- AKA Factor-label method
FINALLY, a reason for algebra
How do you find out how many seconds are in a day?

12. Knowing that: 1 day = 24 hours 1 hour = 60 minutes
1 minute = 60 seconds

13. So, now we can convert within and outside of the metric system
So, now we can convert within and outside of the metric system. All you need to know is the conversion factor. Answer: How many mm are in 1 in? How many cm are in 10 km? How many L are in 5 gallons?

14. PRACTICE PRACTICAR RÉPÉTER
UNIT: something that gives definition to a numerical value, e.g. mile, meters, feet, seconds, etc.
CONVERSION FACTOR: a fraction/equation in which the numerator and denominator represent the same measurement
100 cm = 1 m or cm
1 m
*Some common conversion factors:
1 in = 2.54 cm 1 mi = 5280 ft
1 lb = 454 g 1 qt = 2 pt
1 qt = L 1 gal = 4 qt
1 cc = 1cm3 = 1 mL

15. NUMERATOR: the number above the fraction lab
DENOMINATOR: the number below the fraction lab
CONSTANT: a known set of quantities
INVERT: constants given to you as conversion factors can be flipped around
100 cm or 1 m
1 m cm
PER: can refer to the fraction line
60 seconds per minute or sec
1 min

16. FYI
-For study cards!!! -Ch. 1 tutorials

17. Temperature What is temperature? Measured in scales Pg 72 #26 and 28
Absolute zero
1. 0 K ºC
K = ºC + 273
ºC = K - 273
Pg 72 #26 and 28

19. Matter & Changes

20. What is the difference between an ELEMENT and MATTER?

21. What are the properties of matter?
Read pgs 55-60

22. Matter is anything that has mass and takes up space
What’s the matter?
Matter is anything that has mass and takes up space
Composed of atoms and molecules which act like tiny particles always in motion (kinetic theory)
At higher temps, particles move faster or slower?
At the same temp, heavier particles move faster or slower?

23. What’s the matter?
Pure substances have only one kind of matter 4 states of matter in the universe Properties of matter Physical Chemical
low energy
med. energy
high energy

24. States of Matter Solids Liquids Gases
Draw 3 bubbles in your notes. Read pg and add characteristics to each bubble.
Solids
Liquids
Gases

25. Why is H2O So Special?

26. Types of Changes in Matter (p 61-63)
Physical Change
Chemical Change

27. Chemical Reactions One or more substances forms new substances
Reactants  Products
Fe + S  FeS
2H2O2  2H2O + 2O2
yields

28. Law of Conservation of Mass (p63-64)
Mass is neither created not destroyed.
Review Example Problem 3-1
Page 65 #6-9
Element cards

29. Organizing Matter (p 66-67)
A mixture is a physical blend of 2+ substances
There are 2 types:
1. Heterogeneous
2. Homogeneous
Solutions

30. Organizing Matter (p 68-69)
How can these mixtures be separated?

31. Organizing Matter (p 70-71)
What is a pure substance?
Element:
-Ex:
Compound:

32. Organizing Matter

33. Physical Properties (p 56)
What is a physical property?
What is an extensive property?
What is an intensive property?

34. What are physical and chemical changes?
Review!
What are physical and chemical changes?

35. What are the techniques chemists use for separating mixtures?

36. Chromatography
- marker chromatography
- paper chromatography of plant pigment