CHEM-UP!
DAY 1 - 2013
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 1 of 128)
Chem Up!
An Introduction to Basic Chemistry Concepts
As you come in:
1. Please create a name plate to take to your seat.
2. Write your name on a “raffle ticket” to leave at the
front desk.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 2 of 128)
Welcome!
Please introduce
yourself to your
neighbors. Some
activities will
require working in
groups of two to
three.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 3 of 128)
Course Overview
Day 1
• Measurements
Day 2
• Atoms and Elements
Day 3
• Bonds and Intermolecular Forces
Day 4
• Reactions and Organic Molecules
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 4 of 128)
SKILLS TO HELP YOU SUCCEED
Before Class
During
Class
After Class
• Course Expectations
• Using your Textbook Wisely
• Note taking Skills for Science Courses
• Active Class Participation
• Study Techniques
• Creating Study Aids
• Resources
We will cover these topics in addition
to reviewing Chemistry!
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 5 of 128)
AGENDA FOR DAY 1
Measurements
•Scientific Notation
•Measured vs. Exact Numbers
•Significant Figures
•Calculations & Rounding
•Units of Measurement
•Prefixes
•Conversion Factors and Problem Solving
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 6 of 128)
Measurements
1) Scientific Notation
Learning Goal Write a number in
scientific notation.
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Scientific Notation
Scientific notation is used to write very large or
very small numbers such as
• the width of a human hair,
0.000 008 m, which is also
written as 8 × 10−6 m
• the number of hairs on a
human scalp,100 000,
which is also written as 1 × 105 hairs
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 8 of 128)
Writing Numbers in Scientific Notation
• A number written in scientific notation
contains a coefficient and a power of ten.
coefficient
power
unit
of ten
1.5
× 102
m
• The coefficient is at least 1 but less than 10.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 9 of 128)
Writing Numbers in Scientific Notation
• The number of spaces moved to obtain a
coefficient between 1 and 10 is shown as a
power of ten.
52 000. = 5.2 × 104
move decimal 4 spaces left
0.003 78 = 3.78 × 10−3
move decimal 3 spaces right
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 10 of 128)
Some Powers of Ten
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The Academic Support Center @ Daytona State College (Chem-Up 1, Page 11 of 128)
Comparing Numbers in Standard and
Scientific Notation
Standard Format
Scientific Notation
Diameter of the Earth
12 800 000 m
1.28 × 107 m
Mass of a human
68 kg
6.8 × 101 kg
Diameter of a virus
0.000 000 3 cm
3 × 10−7 cm
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 12 of 128)
Scientific Notation and Calculators
You can enter a number written in scientific
notation on many calculators using the EE or
EXP key.
© 2014 Pearson Education, Inc.
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Scientific Notation and Calculators
When a calculator display appears in scientific
notation, it is shown as a number between 1 and
10, followed by a space and the power (exponent).
© 2014 Pearson Education, Inc.
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Scientific Notation and Calculators
On many scientific calculators, a number is
converted to scientific notation, using the
appropriate keys.
0.000 52 2nd or 3rd function key SCI
Key
Key
= 5.2 −04 or 5.2−04 = 5.2 × 10−4
Calculator display
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 15 of 128)
Guide to Writing a Number in Scientific
Notation
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 16 of 128)
Learning Check
Write the following number in the correct
scientific notation, 0.000 058 g.
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Solution
Write the following number in the correct
scientific notation, 0.000 058 g.
Step 1 Move the decimal point to obtain a
coefficient that is at least 1 but less
than 10.
0.000 058
5.8
(The decimal moves 5 places to the right, giving a
coefficient of 5.8)
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 18 of 128)
Solution
Write the following number in the correct
scientific notation, 0.000 058 g.
Step 2 Express the number of places moved
as a power of 10.
Moving the decimal 5 places to the right
gives a power of −5.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 19 of 128)
Solution
Write the following number in the correct
scientific notation, 0.000 058 g.
Step 3 Write the product of the coefficient
multiplied by the power of 10 with
the unit.
5.8 × 10−5 g
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 20 of 128)
Learning Check
Select the correct scientific notation for each.
1. 0.000 008
(a) 8 × 106
(b) 8 × 10−6 (c) 0.8 × 10−5
2. 72 000
(a) 7.2 × 104 (b) 72 × 103 (c) 7.2 × 10−4
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 21 of 128)
Solution
Select the correct scientific notation for each.
1. 0.000 008
(Move the decimal 6 places to right.)
(b) 8 × 10−6
2. 72 000
(Move the decimal 4 places to the left.)
(a) 7.2 × 104
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 22 of 128)
Learning Check
Write each as a standard number.
1. 2.0 × 10−2
(a) 200
(b) 0.0020
2. 1.8 × 105
(a) 180 000
(c) 0.020
(b) 0.000 018 (c) 18 000
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 23 of 128)
Solution
Write each as a standard number.
1. 2.0 × 10−2
(c) 0.020
2. 1.8 × 105
(a) 180 000
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 24 of 128)
Time For Lesson 1
Scientific Notation
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Measurements
2) Measured Numbers and Significant Figures
Learning Goal Identify a number as measured
or exact; determine the number of significant
figures in a measured number.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 26 of 128)
Measured Numbers
A measuring tool
• is used to determine a quantity such as the
length or the mass of an object
• provides numbers for a measurement called
measured numbers
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The Academic Support Center @ Daytona State College (Chem-Up 1, Page 27 of 128)
Reporting Length
To report the length of an object
• observe the numerical values of the marked
lines at the end of the object
• estimate the last digit by visually dividing the
space between the smallest marked lines
This estimated number is the final digit that is
reported for a measured number.
© 2014 Pearson Education, Inc.
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Reporting Length – 4.5 cm
• The end of the object is between the 4-cm and
5-cm marks.
• Estimate that the end is halfway between the
4-cm and 5-cm marks and report the value as
4.5 cm.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 29 of 128)
Reporting Length – 4.55 cm
• The metric ruler is marked at every 0.1 cm.
• You can now estimate that the length is
halfway between the 4.5-cm and 4.6-cm marks
and report the value as 4.55 cm.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 30 of 128)
Learning Check
. 8. . . . . . . . 9. . . . . . . .
10.
. cm
What is the length of the red line?
(A) 9.0 cm
(B) 9.03 cm
(C) 9.04 cm
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The Academic Support Center @ Daytona State College (Chem-Up 1, Page 31 of 128)
Solution
. 8. . . . . . . . 9. . . . . . . .
10.
. cm
The length of the line could be reported as
(B) 9.03 cm
(C) 9.04 cm
The estimated digit may be slightly different.
Both readings are acceptable.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 32 of 128)
Exact Numbers
Exact numbers are
• those numbers obtained by counting items
• definitions that compare two units in the same
measuring system
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Exact Numbers
Exact numbers are not measured, do not have a
limited number of significant figures, and do not
affect the number of significant figures in a
calculation.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 34 of 128)
Significant Figures
In a measured number, the significant figures,
(SFs) are all the digits, including the estimated
digit.
• All nonzero numbers are
counted as significant
figures.
• Zeros may or may or may not be significant,
depending on the position in the number.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 35 of 128)
Counting Significant Figures
All nonzero numbers in a measured number are
significant.
Measurement
38.15 cm
5.6 ft
65.6 lb
122.55 m
Number of
Significant Figures
4
2
3
5
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The Academic Support Center @ Daytona State College (Chem-Up 1, Page 36 of 128)
Zeros Between Digits
Zeros between nonzero digits are significant.
Measurement
50.8 mm
2001 min
0.0702 lb
0.40505 m
Number of
Significant Figures
3
4
3
5
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 37 of 128)
Zeros, Decimal Numbers
Zeros at the end of decimal numbers are
significant.
Measurement
50.80 km
200. min
40.00 g
Number of
Significant Figures
4
3
4
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 38 of 128)
Zeros, Nondecimal Numbers
Zeros at the end of nondecimal numbers are not
significant.
Measurement
44 000 km
810 cm
6 150 000 g
Number of
Significant Figures
2
2
3
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 39 of 128)
Zeros, Scientific Notation
Zeros in the coefficient of numbers written in
scientific notation are significant.
Measurement
4.90 × 103 m
8.0 × 10–3 kg
6.0330 × 10–5 L
Number of
Significant Figures
3
2
5
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 40 of 128)
Zeros, Scientific Notation
Keep only the significant zeros when writing
numbers in scientific notation.
Measurement
500. g
400 000 m
0.300 cm
Scientific
Notation
Number of
Significant
Figures
5.00 × 102 g
3
4 × 105 m
1
3.00 × 10−1 cm
3
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 41 of 128)
Rules for Significant Figures
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 42 of 128)
Learning Check
State the number of significant figures in each of
the following measurements:
A. 0.030 m
B. 4.050 L
C. 0.0008 g
D. 2.80 m
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 43 of 128)
Solution
State the number of significant figures in each of
the following measurements:
A. 0.030 m
2 SF
B. 4.050 L
4 SF
C. 0.0008 g
1 SF
D. 2.80 m
3 SF
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 44 of 128)
Learning Check
1. Which answer contains three significant
figures?
(a) 0.4760
(b) 0.00476
(c) 4.076 × 103
2. All the zeros are significant in
(a) 0.00307 (b) 25.300
(c) 2.050 × 103
3. The number of significant figures in
5.80 × 102 is
(a) one
(b) two
(c) three
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 45 of 128)
Solution
1. Which answer contains three significant
figures?
(b) 0.00476
2. All the zeros are significant in
(b) 25.300
(c) 2.050 ×103
3. The number of significant figures in
5.80 × 102 is
(c) three
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 46 of 128)
Time For Lesson 2 (Part A)
Significant Figures
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 47 of 128)
Measurements
3) Significant Figures in Calculations
Learning Goal Adjust calculated answers
to give the correct number
of significant figures.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 48 of 128)
Significant Figures Calculations Video
http://www.youtube.com/watch?v=kB2szfcwu1A
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 49 of 128)
Rounding Off
In calculations
• calculated answers are usually rounded off
• rounding rules are used to obtain the correct
number of significant figures
1. If the first digit to be dropped is 4 or less, then it and
all following digits are simply dropped from the
number.
2. If the first digit to be dropped is 5 or greater, then the
last retained digit is increased by 1.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 50 of 128)
Learning Check
Adjust the following calculated answers to give
answers with three significant figures:
A. 824.75 cm
B. 0.112486 g
C. 8.2 L
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 51 of 128)
Solution
Adjust the following calculated answers to give
answers with three significant figures:
A. 824.75 cm
825 cm
B. 0.112486 g
C. 8.2 L
0.112 g
8.20 L
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 52 of 128)
Addition and Subtraction with Measured
Numbers
In addition or subtraction, the final answer is
written so that it has the same number of decimal
places as the measurement having the fewest
decimal places.
For example,
2.367
+ 34.1
36.467
36.5
Thousandths place
Tenths place
Calculator display
Answer, rounded off to tenths place
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 53 of 128)
Learning Check
For each calculation, round the answer to give the
correct number of digits.
1. 235.05 + 19.6 + 2 =
(a) 257
(b) 256.7
2. 58.925 – 18.2 =
(a) 40.725 (b) 40.73
(c) 256.65
(c) 40.7
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 54 of 128)
Solution
1.
235.05
Hundredths place
+19.6
Tenths place
+ 2
Ones place
256.65 rounds to 257
answer (a)
2.
58.925
–18.2
40.725
Thousandths place
Tenths place
rounds to 40.7
answer (c)
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 55 of 128)
Multiplication and Division with Measured
Numbers
In multiplication and division, the final answer is
written to have the same number of significant
figures (SFs) as the measurement with the fewest
SFs.
For example,
24.65 × 0.67
4 SF
2 SF
= 16.5155 
Calculator
17
Final answer (2 SF)
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 56 of 128)
Adding Significant Zeros
When the calculator answer is a small whole
number and more significant figures are needed,
we can add one or more zeros.
For example,
= 4

4.00
3 SF Calculator Final answer (3 SF)
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 57 of 128)
Learning Check
Give an answer for each with the correct number
of significant figures.
1. 2.19 × 4.2 =
(a) 9
(b) 9.2 (c) 9.198
2. 2.54 × 0.0028 =
0.0105 × 0.060
(a) 11.3
(b) 11
(c) 0.041
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 58 of 128)
Solution
Give an answer for each with the correct number
of significant figures.
1. 2.19 × 4.2
=
(b) 9.2
2. 2.54 × 0.0028 =
0.0105 × 0.060
(b) 11
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 59 of 128)
Time For Lesson 2 (Part B)
Significant Figures
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 60 of 128)
Measurements
4) Units of Measurement
Learning Goal Write the names
and abbreviations for the metric
or SI units used in measurements
of length, volume, mass,
temperature, and time.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 61 of 128)
Units of Measurement Video
http://youtu.be/ddtEz4DRojo
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 62 of 128)
The International System of Units (SI)
Chemists use the metric system and the
International System of Units (SI) for
measurement when they
• measure quantities
• do experiments
• solve problems
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Units of Measurement and Their
Abbreviations
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Length
Length is measured in
• units of meters (m) in both the metric and
SI systems
• units of centimeters (cm) by chemists
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Length
Useful relationships between units of length
include:
1 m = 1.094 yd
1 m = 39.37 in.
1 m = 100 cm
2.54 cm = 1 in.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 66 of 128)
Volume
Volume, the space occupied by a substance,
• is measured using units of m3 in the SI system
• is commonly measured in liters (L) and
milliliters (mL) by chemists
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The Academic Support Center @ Daytona State College (Chem-Up 1, Page 67 of 128)
Volume
Useful relationships between units of volume
include:
1 m3 = 1000 L
1 L = 1000 mL
1 mL = 1 cm3
1 L = 1.057 qt
946.3 mL = 1 qt
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 68 of 128)
Mass
The mass of an object, a
measure of the quantity of
material it contains,
• is measured on an
electronic balance
• has the SI unit of
kilogram (kg)
• is often measured by
chemists in grams (g)
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Mass
Useful relationships between units of mass
include:
1 kg = 1000 g
1 kg = 2.205 lb
453.6 g = 1 lb
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Temperature
Temperature, a measure of how hot
or cold an object feels,
• is measured on the
Celsius (ºC) scale
• is measured on the
Kelvin (K) scale in the
SI system
• is 18 ºC or 64 ºF on this
thermometer
© 2014 Pearson Education, Inc.
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Time
Time is based on an atomic clock and is
measured in units of seconds (s) in both the
metric and SI systems.
© 2014 Pearson Education, Inc.
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Learning Check
For each of the following, indicate whether the unit
describes
(a) length, (b) mass, or (c) volume
1.
2.
3.
4.
A bag of onions has a mass of 2.6 kg.
A person is 2.0 m tall.
A medication contains 0.50 g of aspirin.
A bottle contains 1.5 L of water.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 73 of 128)
Solution
For each of the following, indicate whether the unit
describes
(a) length, (b) mass, or (c) volume
1.
2.
3.
4.
A bag of onions has a mass of 2.6 kg.
A person is 2.0 m tall.
A medication contains 0.50 g of aspirin.
A bottle contains 1.5 L of water.
(b)
(a)
(b)
(c)
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 74 of 128)
Learning Check
Identify the measurement that has an SI unit.
1. John’s height is _____.
(a) 1.5 yd
(b) 6 ft
(c) 2.1 m
2. The mass of a lemon is _____.
(a) 12 oz
(b) 0.145 kg
(c) 0.6 lb
3. The temperature is _____.
(a) 85 ºC
(b) 255 K
(c) 45 ºF
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 75 of 128)
Solution
Identify the measurement that has an SI unit.
1. John’s height is______.
(c) 2.1 m
2. The mass of a lemon is _____.
(b) 0.145 kg
3. The temperature is _____.
(b) 255 K
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 76 of 128)
Measurements
5) Prefixes and Equalities
Learning Goal Use the numerical
values of prefixes to write a
metric equality.
© 2014 Pearson Education, Inc.
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Prefixes
In the metric and SI systems of units, a prefix
attached to any unit increases or decreases its
size by some factor of 10.
The relationship of a prefix to a unit can be
expressed by replacing the prefix with its
numerical value.
1 kilometer (1 km) = 1000 meters
© 2014 Pearson Education, Inc.
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Metric, SI Prefixes that Increase
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Metric, SI Prefixes that Decrease
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Measuring Length, Prefixes
When the prefix centi is used with the unit meter,
it becomes a centimeter, a length that is onehundredth of a meter (0.01 m).
When the prefix milli is used with the unit meter,
it becomes a millimeter, a length that is onethousandth of a meter (0.001 m).
© 2014 Pearson Education, Inc.
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Measuring Length, Equalities
An equality shows the relationship between two
units that measure the same quantity.
For example, 1 m is the same length as
100 cm. The equality is written as:
1 m = 100 cm
= 1 × 102 cm
1 m = 1000 mm
= 1 × 103 mm
1 cm = 10 mm
= 1 × 101 mm
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Measuring Volume
A volume of 1 L or smaller is common in the
laboratory. When a liter is divided into
10 equal parts, each is called a deciliter (dL).
1 L = 10 dL
= 1 × 101 dL
1 L = 1000 mL = 1 × 103 mL
1 dL = 100 mL = 1 × 102 mL
© 2014 Pearson Education, Inc.
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Measuring Volume
The cubic centimeter (cm3 or cc) is the volume
of a cube with the dimensions
1 cm × 1 cm × 1 cm.
A cube measuring 10 cm on each side has a volume of 1000 cm3, or 1 L;
a cube measuring 1 cm on each side has a volume of 1 cm3, 1cc, or 1 mL.
© 2014 Pearson Education, Inc.
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Measuring Volume
A cubic centimeter has the same
volume as a milliliter.
1 cm3 = 1 cc = 1 mL
A cube measuring 10 cm on each side has a volume of 1000 cm3, or 1 L;
a cube measuring 1 cm on each side has a volume of 1 cm3, 1cc, or 1 mL.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 85 of 128)
Measuring Mass
When measuring the mass of
• your body, the mass is measured in
kilograms (kg)
• laboratory samples, mass is reported in grams,
milligrams (mg), or micrograms (μg)
1 kg = 1000 g = 1 × 103 g
1 g = 1000 mg = 1 × 103 mg
1 mg = 1000 μg = 1 × 103 μg
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 86 of 128)
Measuring Mass, Equalities
Equalities can be written for mass in the metric
(SI) system.
When metric equalities are used, 1 gram is the
same mass as 1000 mg and 0.001 kg.
1 kg = 1000 g
1 g = 1000 mg
1 mg = 0.001 g
1 mg = 1000 µg
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 87 of 128)
Metric Conversions Video
http://youtu.be/ptoig7YfPHw
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 88 of 128)
Learning Check
Indicate the unit that completes each of the
following equalities:
1. 1000m = ________
(a) 1mm
(b) 1 km
(c) 1 dm
2. 0.01m = _________
(a) 1 mm
(b) 1 cm
(c) 1 dm
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 89 of 128)
Solution
Indicate the unit that completes each of the
following equalities:
1. 1000 m = _____
(b) 1 km
2. 0.01 m = _____
(b) 1 cm
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 90 of 128)
Learning Check
Complete each of the following equalities:
1. 1 kg = _____
(a) 10 g
(b) 100 g
2. 1 mm = _____
(a) 0.001 m
(b) 0.01 m
(c) 1000 g
(c) 0.1 m
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 91 of 128)
Solution
Complete each of the following equalities:
1. 1 kg = _____
(c) 1000 g
2. 1 mm = _____
(a) 0.001 m
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 92 of 128)
Measurements
6) Writing Conversion Factors
Learning Goal Write a conversion
factor for two units that describe
the same quantity.
© 2014 Pearson Education, Inc.
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Equalities on Food Labels
The contents of packaged foods
• are listed in both metric and U.S. units
• indicate the same amount of a substance in two
different units
In the United States, the contents of many packaged
foods are listed in both U.S. and metric units.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 94 of 128)
Writing Conversion Factors
Equalities
• use different units to describe the same quantity
• can be between units of the metric system, or
U.S. units, or between metric and U.S. units
1m
= 1000 mm
1 lb
= 16 oz
2.205 lb = 1 kg
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The Academic Support Center @ Daytona State College (Chem-Up 1, Page 95 of 128)
Writing Conversion Factors
Two Conversion Factors for the Equality
60 min = 1 h
Numerator 
Denominator 
These conversion factors are read as 60 minutes per
hour and 1 hour per 60 minutes. The per means
“divide.”
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 96 of 128)
Writing Conversion Factors
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Metric Conversion Factors
We can write conversion factors for any metric
relationship.
Both conversion factors represent the same
quantity; one is just the inverse of the other.
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Metric – U.S. System Conversion Factors
We can write conversion factors between the
U.S. system and metric quantities.
© 2014 Pearson Education, Inc.
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Conversion Factors with Powers
Sometimes we can use a conversion factor that is
squared or cubed.
Distance = length
Area
= length × length = length2
Volume = length × length × length = length3
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The Academic Support Center @ Daytona State College (Chem-Up 1, Page 100 of 128)
Conversion Factors with Powers
To square the equality 1 m = 100 cm, we square
both the number and the unit on each side.
Equality: 1 m = 100 cm
Area: (1 m)2 = (100 cm)2 or 1 m2 = (100)2 cm2
Conversion factors:
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Conversion Factors with Powers
Both the number and the unit must be squared.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 102 of 128)
Learning Check
Write conversion factors for each pair of units:
A. liters and milliliters
B. meters and kilometers
© 2014 Pearson Education, Inc.
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Solution
Write conversion factors for each pair of units:
A. liters and milliliters (1 L = 1000 mL)
B. meters and kilometers (1 km = 1000 m)
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 104 of 128)
Learning Check
Write the equality and conversion factors for the
relationships between the following units:
A. grams – milligrams
B. square inches – square centimeters
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 105 of 128)
Solution
Write the equality and conversion factors for the
relationships between the following units:
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Equalities, Conversion Factors in Problems
An equality may also be stated within a problem
that only applies to that problem.
1. The car travels at 85 km/h
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Equalities, Conversion Factors in Problems
2. The tablet contains 500 mg Vitamin C.
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Conversion Factors, Percentage Ppm
and Ppb
When scientists represent very small quantities,
they use ppm and ppb.
© 2014 Pearson Education, Inc.
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Conversion Factors, Percentage Ppm
and Ppb
A percent (%) is written as a conversion factor
by choosing a unit and expressing the numerical
relationship of the parts of this unit to 100 parts
of the whole.
• For example, a person has 18% body fat
by mass.
• Equality: 18 mass units of fat per
100 mass units of body mass
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 110 of 128)
Measurements
7) Problem Solving Using Unit Conversions
Learning Goal Use conversion
factors to change from one unit
to another.
© 2014 Pearson Education, Inc.
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Problem-Solving Process
The problem-solving process begins by
analyzing the problem in order to
• identify the given unit and needed unit
• write a plan that converts the given unit to the
needed unit
• identify one or more conversion factors that
cancel units and provide the needed unit
• set up a calculation
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 112 of 128)
Setting up the Problem
Suppose you need to convert 18.2 mm to meters.
• First, identify the given and needed units.
Given: 18.2 mm
Need: meters
• Write a plan that will convert the given unit to
the needed unit.
millimeter
Given
Conversion
factor
meters
Need
© 2014 Pearson Education, Inc.
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Setting up the Problem
• Look for the connection between millimeters
and meters.
1 m = 1000 mm
• From this equality, we can write two
conversion factors.
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Setting up the Problem
• Select the conversion factor that cancels the
given unit, which is the millimeter.
• Complete the calculation and round off to the
needed significant figures.
millimeters
conversion factor
meters
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 115 of 128)
Guide to Problem Solving Using Conversion
Factors
© 2014 Pearson Education, Inc.
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Learning Check
• How many minutes are in 2.5 h?
© 2014 Pearson Education, Inc.
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Solution
How many minutes are in 2.5 h?
Step 1 State the given and needed quantities.
Given: 2.5 h
Need: minutes
Step 2 Write a plan to convert the given
unit to the needed unit.
hours
Given
Conversion factor
minutes
Need
© 2014 Pearson Education, Inc.
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Solution
How many minutes are in 2.5 h?
Step 3 State the equalities and conversion
factors.
1 h = 60 min
Step 4 Set up the problem to cancel units
and calculate.
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Using Two or More Conversion Factors
• Often, two or more conversion factors are
required to obtain the unit needed for the answer.
Unit 1  Unit 2  Unit 3
• Additional conversion factors are placed in the
setup to cancel each preceding unit.
Given unit × factor 1 × factor 2 = needed unit
© 2014 Pearson Education, Inc.
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Sample Problem
How many minutes are in 1.4 days?
Step 1 Given 1.4 days Need minutes
Step 2 Plan days  hours  minutes
Step 3 Equalities 1 day = 24 h
1 h = 60 min
Conversion Factors
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 121 of 128)
Sample Problem
How many minutes are in 1.4 days?
Step 4 Set up problem, cancel units.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 122 of 128)
Learning Check
A bucket contains 4.65 L water. How many
gallons of water is that?
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 123 of 128)
Solution
A bucket contains 4.65 L water. How many
gallons of water is that?
Step 1 Given 4.65 L
Need gallons
Step 2 Plan liters  quarts  gallons
Step 3 Equalities 1 L = 1.057 qt
1 gal = 4 qt
Conversion Factors
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 124 of 128)
Solution
Step 4 Set up problem, cancel units.
© 2014 Pearson Education, Inc.
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 125 of 128)
Time For Lesson 3
Unit Conversions & Dimensional
Analysis
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 126 of 128)
SNEAK PEEK…AGENDA FOR DAY 2
Atoms & Elements
•Elements & Symbols
•The Periodic Table
•Atoms
•Atomic # and Mass #
•Isotopes
•Valence Electrons
•Ions
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 127 of 128)
Questions
Compiled by
J. Picione (Chemistry Faculty)
D. Leonard, R. Wendt, J. Brown, E. Scott, and A. Kandefer (Learning Specialists)
The Academic Support Center @ Daytona State College
http://www.daytonastate.edu/asc/ascsciencehandouts.html
The Academic Support Center @ Daytona State College (Chem-Up 1, Page 128 of 128)