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Unit One:
Introduction to
Chemistry
0
Unit One:
Introduction to Chemistry
Table of Contents:
Pg. 1
Table of Contents
Pg. 2
What is Chemistry?
Pg. 3
Laboratory Work
Pg. 4-5
Laboratory Equipment
Pg. 6
Laboratory Safety
Pg. 7
Chem. Lab Background Info
Pg. 8-10
Lab One: Physical and Chemical Changes
Pg. 11-12
Measuring
Pg. 12-13
Significant Figures (assignment on Pg. 18-19)
Pg. 14
Scientific Notation
Pg. 15-16
SI Prefixes (Pg. 20 is the assignment)
Pg. 17
Unit Conversion (Pg. 21 is the assignment)
1
What is Chemistry?
What is Chemistry?
 Brainstorm: http://www.polleverywhere.com/free_text_polls/NjYxMDc3NTgz
 Chemistry is everything. It is all around us.
Def’n: Chemistry is the study of the composition and properties of ____________________________.
What is matter?
 Matter has two general properties: it occupies ____________________________ and has
____________________________.
 The mass of an object is the quantity of ____________________________ in that object (not to be
confused with weight (weight changes as ____________________________ changes, but mass does
not).
 The space that matter occupies is called its ____________________________.
 A property of matter that combines volume and mass is ____________________________.
 Phases of matter:
Areas of Chemistry (only a few):
 Analytical Chemistry: ____________________________ substances.
 Biochemistry: Study of ____________________________ organisms.
 Bio Technological Chemistry: Creating and modifying ____________________________ material.
 Inorganic Chemistry: Study of ____________________________ compounds structures and
properties.
 Organic Chemistry: Study of ____________________________ and it’s compounds.
2
Laboratory Work
The Scientific Method:

Scientific method is the process that scientists follow in order to perform
____________________________ to investigate the world around them.

The scientific method:
o Gather information through ____________________________
o Define the ____________________________
o Create a ____________________________
o _________________________ an experiment to test the hypothesis
o ____________________________ and observe the experiment
o ____________________________ data from experiment
o Modify of create new ____________________________
Lab Report Outline:
o ____________________________: (title of the experiment)
o ____________________________: (purpose)
o ____________________________: (what you expect)
o ____________________________: (step by step or “see procedure…”)
o ____________________________: (observations and measurements)
o ____________________________/ ____________________________: (show work, answer Q’s, explain
observations)
o ____________________________: (discuss findings, summarize experiment)
o Possible Sources of ____________________________ (things that may have occurred to
prevent precise or accurate results)
3
Lab Reports
Purpose
/2
Hypothesis
/3
Materials and
Procedure
/2
Data and
Observations
/15
Analysis
/15
Conclusion
/5
Sources of Error
/3
Format
/5
A
(100%-80%)
Purpose describes the
reason for doing the
experiment
B
(80%-60%)
Purpose describes
part of the reason for
the experiment
Hypothesis is
educated, gives
expectations and
relates to purpose
Materials / Procedure
are referenced
properly
Hypothesis is
uneducated or
unrelated to the
purpose
Reference has an
error in reference
Observations are
detailed and include
information of before
during and after the
experiment
Observations are not
detailed or don’t
include information
from before, during
and after the reaction
Analysis explains
observations, and
answers questions
Analysis answers
questions but doesn’t
completely explain
observations
Answers purpose,
relates to hypothesis
and is correct.
Answers purpose or
relates to hypothesis
and is correct
Has more than 2
correct sources of
error
Neat, headings, ruler
used, name and
partner (s) included.
Has 2 correct sources
of error
Neat, but may not be
formatted properly
/50
C
(60%-50%)
Purpose doesn’t
describe the
reason for doing
the experiment
Hypothesis is
uneducated and
unrelated to the
purpose
Reference is
incorrectly
referenced
D
(50% or less)
no purpose
Observations are
not detailed and
don’t include
information from
before, during, or
after reaction
Analysis does not
explain
observations and
questions are
answered
incorrectly
Doesn’t answer
purpose/
hypothesis, or is
incorrect
Has less than 2
correct sources of
error
A little messy but
proper formatting
Observations do
not exist
No hypothesis
No procedure or
materials
Analysis
contains very
little analytical
information or
does not exist
Doesn’t exist
Has no sources
of error
Messy and not
properly
formatted.
4
Name:_________________________________
Laboratory Equipment
Match the following pictures of laboratory equipment with the names on the next page by putting
the appropriate letter in the blank beside the names.
5
1. Beaker ________

A containder like a cup. May be heated.
2. Buret/ Test Tube Clamp ________

To fasten to the ring stand as a support
for apparatus
3. Burette ________

Used to withdraw and measure
volumes of solutions in titrations.
Marked with milliliter scale.
4. Crucible and Cover ________

To heat small amounts of solid
materials with high temperature
5. Double Burette Clamp ________

To hold burettes when titrating
6. Erlemeyer Flask ________

A container that may be heated
7. Evaporating Dish ________

A container for small amounts of liquid
being evapoorated
8. Florence Flask ________

A container that may be heated
9. Forceps ________

To pick up or hold small objects
10. Funnel ________

To hold filter paper. May be used in
pouring.
11. Graduated Cylinder ________

To measure volume of a liquid
12. Iron Ring ________

To fasten to the ring stand as a support
for apparatus
13. Laboratory/ Bunsen Burner ________

To heat chemicals in beakers or test
tubes
14. Medicine Dropper ________

To transfer small amounts of liquid.
15. Mortar and Pestle ________

To grind chemicals to a powder
16. Pinch Clamp ________

To clamp a rubber connector
17. Pipestem Triangle ________

To support the crucible
18. Plastic Wash Bottle ________

To dispense distilled water
19. Ring Stand ________

A support with many uses
20. Rubber Connector ________

To connect parts of apparatus
21. Spatula ________

To transfer solid chemicals in weighing
22. Stirring Rod ________

To stir combinations of materials. To
use in pouring liquids.
23. Test Tube ________

A container that may b heated
24. Test Tube Brush ________

To scrub glass apparatus ________
25. Test Tube Holder ________

To hold a test tube
26. Test Tube Rack ________

To hold test tubes in an upright position
27. Tongs ________

To pick up and hold apparatus
28. Volumetric Flask ________

Used in preparation of solutions
29. Watch Glass ________

May be used as a beaker cover. May be
used in evaporating very small amounts
of liquid.
30. Wire Gauze ________

To spread the heat of a flame
6
Lab Safety
REMEMBER: Marks will be deducted for not following proper safety procedures during
the lab, so make sure you understand each rule!
1. Safety goggles must be worn at all times during a lab. This rule must be followed not matter what
you are doing during the lab period.
2. Contact lenses are not allowed. Even when worn under safety goggles, since fumes from the
chemicals can get under them and cause serious injuries or blindness. If this is a problem, please
contact me ahead of time.
3. Closed toe shoes and long pants must be worn in the lab. Sandals and shorts are not allowed.
4. Long hair must be tied back when using open flames.
5. Eating and drinking are strictly prohibited in the classroom, since it is a chemistry classroom and
there may be traces of toxic chemicals in the classroom.
6. No unauthorized experiments are to be performed. If you are curious about trying a procedure not
covered in the experimental procedure, consult with your instructor.
7. Never taste anything. Chemistry is not a subject where you are allowed to lick the spoon.
8. Never directly smell any gas. Any smelling of gas that is required must by done by means of wafting.
9. Coats, backpacks, etc. should be left at your locker or desk, never on the lab benches or within the
area of the experiment.
10. Always wash your hands before leaving lab (with soap).
11. Learn where the safety and first-aid equipment is located.
12. Notify the instructor immediately in case of an accident.
13. Consider all chemicals to be hazardous.
14. Know what chemicals you are using. Be sure to carefully read the label twice before taking anything
from a bottle.
15. Excess reagents are never to be returned to stock bottles, as this will contaminate the stock bottles.
If you take too much, dispose of the excess. (The proper technique is to put less than required in your
flask or weigh boat and slowly add more, until you reach the desired amount)
16. Many common reagents, for example, alcohols and acetone, are highly flammable. Do not use them
anywhere near open flames.
17. Always pour acids into water. If you pour water into acid, the heat of reaction may cause the water
to explode into steam, sometimes violently, and the acid will splatter.
18. If chemicals come into contact with your skin or eyes, flush immediately with abundant amounts
of water and consult with your instructor.
19. Never point a test tube or any vessel that you are heating at yourself or your neighbour.
20. Dispose of chemicals properly. Always consult your instructor before pouring any chemicals down
the sink.
21. Clean up all broken glassware immediately and dispose of the broken glass properly.
22. Never leave burners unattended. Turn them off whenever you leave your workstation. Be sure that
the gas is shut off at the bench rack when you leave the lab.
23. Beware of hot glass--it looks exactly like cold glass.
7
Background Information for Chemistry Labs
Qualitative vs. quantitative:

Qualitative is using ____________________________ to observe and quantitative is using
____________________________ to observe. The first lab we will do is a ____________________________
lab because we just use our senses to observe instead of taking measurements.
Physical Change vs. Chemical Change:

Physical change: Change of ____________________________ or ____________________________ without
changing the actual makeup of the substance.
o ex:

Chemical change: Change in the chemical ____________________________ of a substance. Not
easily ____________________________.
o signs that a chemical change has occurred:

*____________________________ change,

*____________________________ produced,

*____________________________ produced,

*change in ____________________________,

*____________________________ produced,

*____________________________ change,

____________________________ change (often shown by a change in volume),

change in ____________________________ point or ____________________________
point,

change in electrical ____________________________,

change in ____________________________ (DON'T EVER TEST)
*easiest (and safest) to observe
Properties of Matter:
Physical Properties


We can observe physical properties without the ____________________________ identity of
the substance being changed (observed with senses).
Examples of Physical Properties that could be observed:
Chemical Properties

Chemical properties can only be observed when a chemical ____________________________
takes place.

Examples of Chemical Properties that could be observed:
8
Name:
Period:
Lab Partner:
Date:
Lab One: Physical and Chemical Changes
Introduction:
A good understanding of material things requires and understanding of the physical and
chemical characteristics of matter. Such characteristics are familiar to you, and physical and
chemical changes are part of your everyday experience. However, you may not yet have a clear
idea of the difference between a physical change and a chemical change. You may not yet know
exactly how a chemical change is distinguished from a physical change. The purpose of this
experiment is to clarify these important distinctions.
The physical properties of a substance are those properties that can be observed and
measured without changing the composition of the substance. Because they depend on there
being no change in composition, physical properties can be used to describe and identify
substances.
The chemical properties of a substance are those properties that can only be observed
when the substance is undergoing a change in composition.
In a physical change, only physical state of a sample of matter is altered. In chemical
changes, new substances, of different chemical composition are produced. A process in which a
chemical change takes place is called a chemical reaction. The observable signs that a chemical
change has occurred are as follows:

Colour change

Gas produced

Solid produced

Energy Change
o Change in heat
o Light produced

Odor change
Purpose:
Students will observe properties of several substances and decide whether changes in matter are
physical or chemical.
Equipment:
Scissors
Spatula
Evaporating dish
Test tubes
Test tube stopper
Materials:
Magnesium ribbon (0.5 cm)
Copper (II) sulfate crystals
Hydrochloric acid (5mL,
0.2M)
Copper (I) chloride solution
Distilled water
Sheet of paper
Sodium bicarbonate
5% Acetic acids solution
Sodium chloride
Aluminum foil
Lead (II) nitrate solution
Potassium iodide solution
9
Procedure:
Note: Because this is a qualitative experiment observations are very important so make sure you include as
many detailed observations as possible.
BE SURE TO CLEAN YOUR AREA BEFORE YOU LEAVE EACH STATION
Investigation A:
1. Examine a piece of aluminum (Al) foil and identify at least three physical properties.
2. Add a small amount of copper (I) chloride solution to a test tube. Identify some
physical properties of the solution.
3. Roll the Al foil into a small loose ball and place it in the copper (I) chloride solution.
Describe the results.
Investigation B:
1. Obtain a scoop of sodium chloride and identify some physical properties of sodium
chloride.
2. Add a small amount of distilled water to a test tube and identify some physical
properties of water.
3. Place a small portion of the sodium chloride in the water. Describe the results.
4. Transfer about one-half of the salt solution you prepared to an evaporating dish (or
beaker) and place the dish out to dry. Allow the water to evaporate completely.
Describe the results (tomorrow).
Investigation C:
1. Examine a small piece of magnesium ribbon (0.5 cm) and identify at least three physical
properties.
2. Add a small amount of 0.2M solution of Hydrochloric Acid to a test tube. Describe the
physical properties.
3. Add the piece of magnesium ribbon to the hydrochloric acid solution. Describe the
results.
Investigation D:
1. Select several small crystals of copper (II) sulfate (CuSO4) and identify some physical
properties.
2. Place a small amount (~1 cm) of distilled water (H2O) and place it in a test tube.
Identify some physical properties.
3. Drop the CuSO4 crystals into the water. Stopper the test tube and shake the contents to
promote interaction of particles. Describe the results.
10
Investigation E:
1. Obtain a sheet of paper. Examine it and identify some physical properties
2. Using a pair of scissors cut the paper in such a way that you end up with a hole in the
paper large enough to slip your hand entirely through. Describe the results.
Investigation F:
1. Measure out a 1/2 scoop of sodium bicarbonate. Identify some physical properties.
Place the baking soda in a test tube.
2. Using a graduated cylinder, measure 5 mL of 5% acetic acid solution and identify some
physical properties.
3. Transfer the acetic acid to the test tube containing the sodium bicarbonate and allow
them to mix (DO NOT STOPPER). Describe the results.
Investigation G:
1. In a test tube, measure out a small amount of lead (II) nitrate solution and identify some
physical properties.
2. Identify some physical properties of potassium iodide.
3. Add a small amount of potassium iodide to the lead (II) nitrate. Record your
observations.
Data Analysis:
1. State in your own words the difference between physical and chemical properties. Give an
example of each that has not been mentioned in this experiment.
2. State in your own words the difference between a chemical change and a physical change.
Don’t forget your paragraph explaining your observations.
Conclusions:
For each change you observe, indicate whether the change was physical or chemical in nature.
Give reasons for you answer.
Don’t forget your sources of error
11
Measuring
Math and Measurements:

Chemistry math is different from regular math in that in chemistry we use
____________________________ and in math we use exact numbers. Because a measurement is
never 100% accurate (because of _________________________ _________ _____________________), there
is error to account for. In order to make sure that the answers to our mathematical
problems are not more or less accurate than the ____________________________ involved, we use
sig figs.
Precision vs. Accuracy

Precision: Ability to reproduce the ____________________________ result. Error in precision
(Random Error) occurs with poor ____________________________.

Accuracy: Ability to get the ____________________________ result. Error in accuracy (Systematic
Error) occurs with poor ____________________________ (calibration).
Ex. A piece of metal is known to have a mass of 18.01 g. When a student made three attempts to
determine the mass of the metal, the following results were obtained:
a) 18.00 g
b) 18.03 g
c) 18.02 g
Are these results accurate, precise, or both?
SI Units (Système International):

Remember that Units are important! SI Units are the units that are the most widely used
units. SI Units are base units. This means all other units can be derived from the base SI
Units.
o
o
o
o
Length- ______________________ : m
Mass- ______________________: kg
Time- ______________________: s
Electric current- ____________: A
o Temperature- ____________________: K
o Amount of substance- _________________: mol
o Luminous intensity- _____________________: cd
12
How to Measure:

When measuring you always estimate ______________________ digit.
Example 1:
Example 2:
Significant Figures

Significant figures (sig figs) are the number of digits in a number or measurement that are
_______________________________. Sig figs are important in order to calculate answers to
problems using measurements. Sig figs are used so that when you are performing
calculations using measured values the answer is only as _____________________________ as the
measurements used.
Sig fig rules:
1. All _____________________________ digits are significant.
Ex. 384 has _______ sig figs
2. All zeros _____________________________ non-zero digits are significant.
Ex. 1,002 has ______ sig figs
3. Zeros before the _____________________________ non-zero digit are not significant
Ex. 0.0020901 has ______ sig figs
4. Zeros after the _________________________ non-zero digit may be significant (they are
significant if the number has a decimal).
Ex. 0.00200 has _______ sig figs
Ex. 200 has ______ sig figs
13
Note: If you want the zeros after the last non-zero digit to be significant, you should write the number in
scientific notation. For example if 200 should have 3 sig figs instead of 1, it should be written as 2.00 x 102.

Examples:
1. 315=
4. 300.=
7. 0.01350=
2. 305=
5. 0.135=
8. 0.013050=
3. 300=
6. 0.1350=
Calculations with sig figs:
Adding and Subtracting with Sig Figs

When adding and subtracting, the answer will have the same number of
_____________________________ or places as the digit with the least number of decimals/places.

Examples:
o 0.135 + 0.01 =
o 350 + 315 =
Multiplying and Dividing with Sig Figs

When multiplying and dividing with sig figs, the answer will have the same number of
_____________________________ as the number in the question with the least number of sig figs.

Example:
o 0.43986 x 0.10 =
When combining multiplying/dividing with adding/subtracting

Use _____________________________ and do not round until the end (just keep track of the
number of sig figs each number has using underlining of subscripts)

Example:
o 0.31 + 4.00 x 3.6498
Why don’t you round until the end?
[(1.35+4.36) x (0.970x4.31)] x [(6.71x 5.98) /
(0.10+3.31)]
[(1.35+4.36) x (0.970x4.31)] x [(6.71x 5.98) /
(0.10+3.31)]
[5.710 x 4.1807] x [40.1258 / 3.410]
[5.71 x 4.18] x [40.1 / 3.41]
23.8718 x 11.767097
23.9 x 11.8
=280.9018 = 281
=282
Assignment on pg. 18-19
14
Scientific Notation

Do you know what has a mass of 5,973,600,000,000,000,000,000,000 kg?
It's the _____________________________!

Do you know what has a mass of 0.00000000000000000000000000000091093826 kg. ?
This is the mass of an _____________________________!

Scientists have developed a shorter method to express very _____________________________ or
very _____________________________ numbers. This method is called scientific notation.

Scientific Notation is based on powers of the base number _____________________.

Scientific Notation: an easier way to write a long number... instead of writing
602200000000000000000000 we write _____________________________

This means that we multiply 6.022 by 1023.
o Remember: 1023 means 10x10x10x10x10x10x10x10x10x10x10x10x10x10x
10x10x10x10x10x10x10x10x10.

The mass of the earth would be written as _____________________________kg.

The mass of an electron would be written as _____________________________kg.
If the number is big (greater than 1) the exponent will be _____________________________.
If the number is small (less than 1) the exponent will be _____________________________.
Examples:
Ex 1. Write 3.378x 105 in standard notation.
Ex 2. Write 2.87 x 10-8 in standard notation.
When writing a number in scientific notation, there must only be _______________ non-zero digit
to the left of the decimal. Be sure to keep the same number of significant figures.
Examples:
Ex 1. Write 0.000430 in scientific notation.
Ex 2. Write 283,000 in scientific notation.
Note: In your assignments, use scientific notation for numbers >999 and <0.001
15
SI Prefixes

SI= _____________________________ _____________________________– French

SI Prefixes change the _____________________________ of the number (using units) without
changing the actual _____________________________ of the number.
o Ex. 1000g=1kg, so instead of writing 1000g we could just write _____________kg.
o Also useful in calculations:
Ex. if I am traveling 50 meters per second, how many kilometers per hour is
that? In this question we need to be able to convert meters to kilometers.

The SI Prefixes can be found on the chart titled “SI prefix Chart”.

To convert from units with one SI prefix to another SI prefix, we write an equation such that
the units are:
Steps to Follow:
1. Start by writing down what you are trying to _____________________________.
2. Draw your _____________________________ sign and the _____________________________ line
3. Put the units you are trying to get rid of in the _____________________________ of the
conversion factor.
4. Put the units you are trying to end up with in the _____________________________ of the
conversion factor.
5. Fill your numbers in for the conversion factor. Remember the numerator need to
_____________________________ the denominator.
o Example 1: Convert 3287.3g to kilograms
o Example 2: Convert 43.38mL to kiloliters
Funny SI Prefixes
o Time between slipping on a peel and smacking the pavement = 1 bananosecond
o 1 millionth of a mouthwash = 1 microscope
Assignment on pg. 20
16
SI Prefix Charts
To convert from unit m, L, s, or g to a unit with an SI prefix from the table below,
you will need to move the decimal to the left.
Peta
Tera
Giga
Mega
Kilo
Hecto
Deca
Unit
1Pm=
1013m
1Tm=
1012m
1Gm=
109m
1Mm=
106m
1km=
103m
1hm=
102m
1dam=
101m
Meter
1PL=
1013L
1TL=
1012L
1GL=
109L
1ML=
106L
1kL=
103L
1hL=
102L
1daL=
101L
Liters
1Ps=
1013s
1Ts=
1012s
1Gs=
109s
1Ms=
106s
1ks=
103s
1hs=
102s
1das=
101s
Second
1Pg=
1013g
1Tg=
1012g
1Gg=
109g
1Mg=
106g
1kg=
103g
1hg=
102g
1dag=
101g
Gram
To convert from unit m, L, s, or g to a unit with an SI prefix from the table below,
you will need to move the decimal to the right.
Unit
Deci
Centi
Milli
Micro
Nano
Pico
Femto
Meter
1dm=
10-1m
1cm=
10-2m
1mm=
10-3m
1 µm=
10-6m
1nm=
10-9m
1pm=
10-12m
1fm=
10-15m
Liters
1dL=
10-1L
1cL=
10-2L
1mL=
10-3L
1 µL=
10-6L
1nL=
10-9L
1pL=
10-12L
1fL=
10-15L
Second
1ds=
10-1s
1cs=
10-2s
1ms=
10-3s
1 µs=
10-6s
1ns=
10-9s
1ps=
10-12s
1fs=
10-15s
Gram
1dg=
10-1g
1cg=
10-2g
1mg=
10-3g
1 µg=
10-6g
1ng=
10-9g
1pg=
10-12g
1fg=
10-15g
17
Unit Conversions
(Similar to SI Prefixes)

We use the ___________________________ _____________________ method to perform unit conversions.

Using conversion factors to change the units may not seem like the easiest way, but it will
help you in the future when we learn stoichiometry.

In order for us to change the units without changing the _____________________________ of the
number we must make the conversion factor (units we want/units we have)= __________. If
the numerator equals the denominator, then the conversion factor will equal 1.
Remember: the conversion factor must equal 1.
1.
2.
3.
4.
5.
Start by writing down what you are trying to convert.
Draw your multiplication sign and the division line
Put the units you are trying to get rid of on the denominator of the conversion factor.
Put the units you are trying to end up with in the numerator of the conversion factor.
Fill your numbers in for the conversion factor. Remember the numerator need to equal
the denominator.
o Example 1: Convert 3.12 hours to minutes
o Example 2: Convert 0.569 pounds to grams
1 pound = 0.45359kg, 1kg = 1000g
o Example 3: How far does light travel in 1 year? (speed of light is 3.00 x 108 m/s)
o Example 4: Convert 5.0 m/s to km/hr?
Assignment on pg. 21
18
19
Name:_______________________________________
Significant Figures Assignment
Figure out the answers to the questions below. Match the number of significant figures (sig figs) in
your answer to the corresponding letter in the chart below. Then enter the corresponding letter
into the appropriate blank to figure out the joke below. Be sure to explain your answers (as shown
below).
Hint: You do not necessarily have to figure out the answer to the question, you just have to figure
out how many sig figs the answer will have.
W __ __ __ __ __ __ __ __ __ __
1
2
3
4
5
6
7
8
9
__ __ __ __ __ __ __ __ __ __ ?
10 11
12 13 14
15 16
17 18 19 20 21
__ __ __ __ __ __ __ __
22 23 24 25
26 27 28 29
1=C
5=A
9=G
13-Y
17=R
21=K
25=U
2=I
6=D
10=L
14=N
18=F
22=M
26=V
3=T
7=H
11=Z
15=S
19=X
23=P
4=E
8=O
12=B
16=W
20=J
24=Q
1. Example: 042879.43789349870 x 0.0000094292834793248789
(16 sig figs)
x
(17 sig figs) = (16 sig figs)
16 sig figs in the answer means the corresponding letter is “W”, so “W” goes in the blank #1 above.
2. How many sig figs?
0.0004293090
3. How many sig figs?
890.00
4. How many sig figs?
8.90 x 105
5. How many sig figs in the answer? 95.097 + 205.90709
6. How many sig figs in the answer? 587.982523 - 587.9795
7. How many sig figs in the answer? 2497.2498 / 439.639
8. How many sig figs? 1000000099.0
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9. How many sig figs in the answer? 3.57 + 22.2380
10. How many sig figs in the answer? 792736201.193834800 x 11116540098.866544
11. How many sig figs? 00089.000500
12. How many sig figs? 900100089.000500
13. How many sig figs in the answer? 304.01 + 45.2039489
14. How many sig figs in the answer? 680690.876809098 + 273.0293828
15. How many sig figs? 0.00000900
16. How many sig figs in the answer? 39800291/13092813.10938
17. How many sig figs? 1.000 x 106
18. How many sig figs in the answer? (3.46 - 3.15) x 6.95
19. How many sig figs in the answer? 48392.9300 / 39301.293049
20. How many sig figs in the answer? (8329.23 + 8987.2791) x 29384.9837
21. How many sig figs in the answer? (3.46 + 3.15) / 6.95
22. How many sig figs? 10008700.650000
23. How many sig figs in the answer? (4.19-4.09) x (4.19+4.09)
24. How many sig figs? 0.000000009
25. How many sig figs in the answer? (6.98+5.78) X (8.90+9.07)
26. How many sig figs in the answer? 68890965.8600 / 7654430096543224.67
27. How many sig figs in the answer? 5064.67 x 0.8701
28. How many sig figs? 5680000.000 x 1015
29. How many sig figs in the answer? (18.99/1.055)+(12.04/0.980) 12.3
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Name:_______________________________________
SI Prefix Conversion Assignment
Perform the calculations required to complete the following unit conversions. Be sure to use scientific
notation where appropriate.
1. Convert 170.4 m to cm
2. Convert 564 Dag to g
3. Convert 49 Hg to g
4. Convert 600 L to KL
5. Convert 0.0923 m to mm
6. Convert 210 cL to dL
7. Convert 4.51x 103 s to ms
8. Convert 45700 cg to Kg
9. Convert 24.6 KL to L
10. Convert 82.4 nm to m
11. Convert 0.0293 ms to ns
12. Convert 58 ds to ms
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Name: ______________________________________
Unit Conversions Assignment
Here is some info you may need in order to answer these questions (we will assume that any
number without a decimal is an exact number and therefore has infinite sig figs):
1 foot=0.3048 m=12 inches=30.48 cm= 0.333333333yards=0.00018939miles
1 mile=1.609344km
1 lightyear=9.4607x1015m
1cm3=1ml=1x10-6m3
1 pound = 0.45359 Kg
1US gallon=3.785411 litres
1. If you had a ruler that was 12 inches how many kilometers would that be?
2. If you were traveling 102 km/hour, how many miles/hour would that be?
3. If you travelled 200km on a 50 liter tank, how many miles per gallon (US) are you getting?
4. How many light-years tall are you? (use scientific notation)
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