1. CH. 2 - MEASUREMENT
Units of Measurement

2. A. Number vs. Quantity
Quantity - number + unit
UNITS MATTER!!

3. CH. 2 - MEASUREMENT
II. Using Measurements

4. A. Accuracy vs. Precision
Accuracy - how close a measurement is to the accepted value
Precision - how close a series of measurements are to each other
ACCURATE = CORRECT
PRECISE = CONSISTENT

5. A. Accuracy vs. Precision

6. B. Percent Error Indicates accuracy of a measurement your value
given value

7. B. Percent Error % error = 2.9 %
A student determines the density of a substance to be 1.40 g/mL. Find the % error if the accepted value of the density is 1.36 g/mL.
% error = 2.9 %

8. C. Significant Figures Indicate precision of a measurement.
Recording Sig Figs
Sig figs in a measurement include the known digits plus a final estimated digit
2.31 cm

9. C. Significant Figures 739 5085 2.60 Counting Sig Figs
Digits from 1-9 are always significant.
Zeros between two other sig figs are always significant
One or more additional zeros to the right of both the decimal place and another sig digit are significant
Count all numbers EXCEPT:
Leading zeros
Trailing zeros without a decimal point -- 2,500
739
5085
2.60

10. Counting Sig Fig Examples
C. Significant Figures
Counting Sig Fig Examples
4 sig figs
3 sig figs
3. 5,280
3. 5,280
3 sig figs
2 sig figs

11. C. Significant Figures (13.91g/cm3)(23.3cm3) = 324.103g 324 g
Calculating with Sig Figs
Multiply/Divide - The # with the fewest sig figs determines the # of sig figs in the answer.
(13.91g/cm3)(23.3cm3) = g
4 SF
3 SF
3 SF
324 g

12. C. Significant Figures 3.75 mL + 4.1 mL 7.85 mL 3.75 mL + 4.1 mL
Calculating with Sig Figs (con’t)
Add/Subtract - The # with the lowest decimal value determines the place of the last sig fig in the answer.
3.75 mL mL
7.85 mL
3.75 mL mL
7.85 mL
224 g
+ 130 g
354 g
224 g
+ 130 g
354 g
 7.9 mL
 350 g

13. C. Significant Figures Calculating with Sig Figs (con’t)
Exact Numbers do not limit the # of sig figs in the answer.
Counting numbers: 12 students
Exact conversions: 1 m = 100 cm
“1” in any conversion: 1 in = 2.54 cm

14. C. Significant Figures Practice Problems 5. (15.30 g) ÷ (6.4 mL)
4 SF
2 SF
= g/mL
 2.4 g/mL
2 SF g g
 18.1 g
18.06 g

15. D. Scientific Notation
A way to express any number as a number between 1 and 10 (coefficient) multiplied by 10 raised to a power (exponent)
Number of carbon atoms in the Hope diamond
460,000,000,000,000,000,000,000
4.6 x 1023
Mass of one carbon atom g
2 x g
coefficient
exponent

16. D. Scientific Notation 65,000 kg  6.5 × 104 kg
Converting into Sci. Notation:
Move decimal until there’s 1 digit to its left. Places moved = exponent.
Large # (>1)  positive exponent Small # (<1)  negative exponent
Only include sig figs.

17. D. Scientific Notation Practice Problems 7. 2,400,000 g 8. 0.00256 kg
9. 7  10-5 km
 104 mm
2.4  106 g
2.56  10-3 kg km
62,000 mm

18. D. Scientific Notation Calculating with Sci. Notation
(5.44 × 107 g) ÷ (8.1 × 104 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

19. D. Scientific Notation Practice Problems 4  1010 cm2 6.9  10-2 kg2
11. (4 x 102 cm) x (1 x 108cm)
12. (2.1 x 10-4kg) x (3.3 x 102 kg)
13. (6.25 x 102) ÷ (5.5 x 108)
14. (8.15 x 104) ÷ (4.39 x 101)
15. (6.02 x 1023) ÷ (1.201 x 101)
6.9  10-2 kg2
1.1 x 10-6
1.86 x 103
5.01 x 1022

20. Chemistry Binder Organization
Chemistry Binder: (8 tabs)
Reference:
Administrative papers (policies & procedures, etc)
Chemistry reference handouts (Periodic Table, Chemical Reference Sheet, etc)
Notes
Filler Paper for lecture notes
Handouts or worksheets to supplement textbook
Divided by chapter or unit – there are 7 separate sections for the first semester

21. M V D = E. Derived Units 1 cm3 = 1 mL 1 dm3 = 1 L
Combination of base units.
Volume (m3 or cm3)
length  length  length
1 cm3 = 1 mL
1 dm3 = 1 L
D = M V
Density (kg/m3 or g/cm3)
mass per volume

22. F. Density
Mass (g)
Volume (cm3)

23. F. 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 = 11,200 g

24. F. 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 = 29 mL

25. Homework
Complete Worksheet “Using Measurements – Chapter 2”: due Monday (skip section on Dimensional Analysis – we will learn this next week  )
Study for test tomorrow

26. Conversion Factors Problems
Dimensional Analysis
Conversion Factors
Problems

27. A. Problem-Solving Steps
1. Analyze
2. Plan
3. Compute
4. Evaluate

28. B. Dimensional Analysis
A tool often used in science for converting units within a measurement system
Conversion Factor
A numerical factor by which a quantity expressed in one system of units may be converted to another system

29. B. Dimensional Analysis
The “Factor-Label” Method
Units, or “labels” are canceled, or “factored” out

30. B. Dimensional Analysis
Steps:
1. Identify starting & ending units.
2. Line up conversion factors so units cancel.
3. Multiply all top numbers & divide by each bottom number.
4. Check units & answer.

31. C. Conversion Factors Example: 1 in. = 2.54 cm
Fractions in which the numerator and denominator are EQUAL quantities expressed in different units
Example: in. = 2.54 cm
Factors: 1 in and cm
2.54 cm in.

32. How many minutes are in 2.5 hours?
Conversion factor
cancel
2.5 hr x
60 min
1 hr
= 150 min
By using dimensional analysis / factor-label method, the UNITS ensure that you have the conversion right side up, and the UNITS are calculated as well as the numbers!

33. C. Conversion Factors 1. Liters and mL 2. Hours and minutes
Learning Check:
Write conversion factors that relate each of the following pairs of units:
1. Liters and mL
2. Hours and minutes
3. Meters and kilometers
1 L
1000 mL
1 hr
60 min
1000 m
1 km

34. D. Dimensional Analysis Practice
You have $7.25 in your pocket in quarters. How many quarters do you have?
7.25 dollars quarters
1 dollar X
= 29 quarters

35. D. Dimensional Analysis Practice
How many seconds are in 1.4 days?
Plan: days hr min seconds
1.4 days x 24 hr x 60 min x 60 sec =
1 day 1 hr min
sec
sec

36. D. Dimensional Analysis Practice
How many milliliters are in 1.00 quart of milk? qt mL
1.00 qt
1 L
1.057 qt
1000 mL
1 L
= 946 mL 

37. D. Dimensional Analysis Practice
You have 1.5 pounds of gold. Find its volume in cm3 if the density of gold is 19.3 g/cm3. lb
cm3
1.5 lb
1 kg
2.2 lb
1000 g
1 kg
1 cm3
19.3 g
= 35 cm3

38. D. Dimensional Analysis Practice
5) Your European hairdresser wants to cut your hair 8.0 cm shorter. How many inches will he be cutting off? cm in
8.0 cm
1 in
2.54 cm
= 3.1 in

39. D. Dimensional Analysis Practice
6) Roswell football needs 550 cm for a 1st down. How many yards is this? cm yd
550 cm
1 in
2.54 cm
1 ft
12 in
1 yd
3 ft
= 6.0 yd

40. D. Dimensional Analysis Practice
7) A piece of wire is 1.3 m long. How many 1.5-cm pieces can be cut from this wire? m
pieces
1.3 m
100 cm
1 m
1 piece
1.5 cm
= 86 pieces

41. D. Dimensional Analysis Practice
How many liters of water would fill a container that measures 75.0 in3?
in3 L
75.0 in3
(2.54 cm)3
(1 in)3
1 L
1000 cm3
= 1.23 L