1. Measurement/Calculation
Units of Measure

2. Metric System
based on powers of ten, so it’s easy to convert between units.
Remember:
KING HENRY DANCED BEFORE DAWN COUNTING MONEY Or
KING HENRY DIED BY DRINKING CHOCOLATE MILK

3. Units Mega kilo hecto deka BASE deci centi milli micro M k h da (none)
106
105
104
103
102
101
100 or 1
10-1
10-2
10-3
10-4
10-5
10-6

4. How to use
Right
Kilo
Hecto
Deka
BASE
Deci
Centi
Milli
Left

5. Examples 20 L= _______ mL 7 kg = _______ mg 90 mm = _______ cm
Kilo
Hecto
Deka
BASE
Deci
Centi
Milli
20 L= _______ mL
7 kg = _______ mg
90 mm = _______ cm
223 mL = ________ L
0.49 hm = ______ m
20 000
9.0
0.223 49

6. SI base units Quantity Base Unit Symbol Time second s Length meter m
Mass
kilogram kg
Temperature
Kelvin K
Amount of a substance
mole
mol

7. SI derived units (derived units are calculated from base units)
Quantity
Derived Unit
Symbol
Volume: various formulas, such as LxWxH
cubic centimeters or milliliters
liters
cm3 or mL L
Density: mass divided by volume
grams per milliliter or grams per cubic centimeter
g/mL or g/cm3

8. NOTE:
1 cm3 IS EQUAL TO 1 mL!!!
And a cc is the same as a cm3

10. Measurement/Calculation
Scientific Notation/Accuracy &Precision

11. Rules to putting into Sci Not
Must have a whole number between 1- 9
If you move:
Decimal to Left…exponent is Positive
Decimal to Right...exponent is Negative

12. Examples
.0032
3.2 X 10-3
1.53 X 107

13. Examples
5.00 X 104
2.32 X10-3
50 000
5.00
.00232
2.32

14. Addition/Subtraction
Make exponents the same by moving decimal place and changing exponent
Then add/subtract and put in correct Sci Not OR
Type into your calculator
Change mode to Sci

15. Example
5.00 X 104
X 104
5.00 X 104
X 103 
5.244X 104 OR
Type into your calculator
EXP EE
EXP EE
Enter
5.00 4 3 +
2.44

16. Multiplication/Division
Multiply numbers
Add exponents
Division
Divide numbers
Subtract exponents
Then put back in correct scientific notation!

17. Example = 6.7 × 102 g/mol Type on your calculator: = 671.6049383
=0.67 X 103 g/mol
Type on your calculator:
EXP EE
EXP EE
ENTER
EXE
5.44 7 ÷
8.1 4 =
= 670 g/mol
= 6.7 × 102 g/mol

18. Accuracy and Precision
Accuracy: how close a measurement is to the true value (the “correct answer”)
Precision: how close a value is to other values in that series

20. Are the following groups of measurements accurate, precise, both, or neither?
1) Given: true mass of sample of zinc is 14.5 g
Measurements made:
13.2 g, 15.6 g, 17.9 g, 12.0 g
Given: true volume of sample of water is 33.3mL
22.4 mL, 22.2 mL, 22.4 mL, 22.3 mL
3) Given: true length of copper wire is 58.5 cm
58.4 cm, 58.5 cm, 58.5 cm, 58.4 cm

21. Quantitative: a numerical measurement (quantity)
Qualitative: a descriptive measurement (quality); does not involve numbers
Quantitative: a numerical measurement (quantity)

22. Measurement/Calculation
Significant Figures

23. Rules to Significant Figures
If it’s not 0, it counts.
Example
743.44 24 5 2

24. Rules to Significant Figures
0’s in between significant figures count.
Example
506
20405
.707 3 5 3

25. Rules to Significant Figures
All 0’s at the end past the decimal point count.
Example
2.440
784.30 4 5

26. Rules to Significant Figures
0’s as placeholders don’t count.
Example
440
0.09 2 1

27. Alternative Way
Atlantic
(Absent)
Pacific
(Present)

28. Pacific
(Present)
Atlantic
(Absent)
If the decimal is present, start on the Pacific side at the first nonzero digit and count it and all the digits to the right of it.
If the decimal is absent, start on the Atlantic side at the first nonzero digit and count it and all the digits to the left of it.

29. Adding/Subtracting Add/Subtract First
The answer has only as many decimal places as the measurement having the least number of decimal places.
Example g g g g 1 3 2
267.9 g
Answer should have 1 decimal place

30. Multiplication/Division
Mult/Divide First
The answer has only as many significant figures as the measurement with the least number of significant figures.
Example
13.78 g
11.3 mL 4 3
1.22 g\ml
= g/mL
Answer should have 3 significant figures

31. Example
15000
2030.0
0.0020 2 5

32. Measurement/Calculation
Density

33. Density
Derived unit
g/mL or g/cm3
Mass/Volume

34. D. Density V = 825 cm3 m = DV D = 13.6 g/cm3 m = (13.6 g/cm3)(825cm3)
An object has a volume of 825 cm3 and a density of 13.6 g/cm3. Find its mass.
GIVEN:
V = 825 cm3
D = 13.6 g/cm3
m = ?
WORK:
m = DV
m = (13.6 g/cm3)(825cm3)
m = g=11 200g

35. D. Density D = 0.87 g/mL V = m V = ? m = 25 g V = 25 g 0.87 g/mL
A liquid has a density of 0.87 g/mL. What volume is occupied by 25 g of the liquid?
GIVEN:
D = 0.87 g/mL
V = ?
m = 25 g
WORK:
V = m D
V = g
0.87 g/mL
V = 28.74mL = 29 mL

36. D. Density D = ? D = m V = 53.4-50 =3.4 mL m = 5.6 g D = 5.6 g 3.4 mL
A marble has a mass of 5.6 g. It is placed in a graduated cylinder with 50.0 mL of water. The water level rises to 53.4 mL. What is the density of the marble?
3.4 mL
GIVEN:
D = ?
V = =3.4 mL
m = 5.6 g
WORK:
D = m V
D = g
3.4 mL
D=1.647 g/mL = 1.6 g/mL

37. Graphing
Graphing is an important tool for expressing data so that it is easier to read and interpret
Rules for graphing:
--place the manipulated/independent variable (the one that was changed) on the x axis.
--place the dependent/responding variable (the results of that change) on the y axis.
(dry mix)
DRY
MIX
y scale = largest y value – smallest y value x scale = largest x value – smallest x value
# of lines on the y axis # of lines on the x axis
The graph should cover at least ¾ of the grid