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REGENTS CHEMISTRY
Name___________________________
Mrs. Murray
Chemistry, period______
Date________________
Unit 1: Matter
Text Book
 Chapter 2 Analyzing Data, pages32-58
 Chapter 3 Matter- Properties and Changes, pages 70-90
A. Scientific Notation/ Standard Notation:
Change the following numbers to standard notation.
1) 4.47 x 103
2) 1.683 x 105
3) 6.800 x 10-3
4) 3.6 x 10-4
5) 5.3 x 102
6) 5.4 x 10-1
7) 3.69 x 102
8) 5.1 x 10-6
9) 9.9 x 101
10) 4.953 x 10-2
Convert the following to scientific notation
1) 1200
2) 57000
3) 3.798
4) 6790
5) 87400
6) 916089
7) 4213
8) 50009
9) 8.71
10) 2000000
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REGENTS CHEMISTRY
B. Measurements
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REGENTS CHEMISTRY
What volume (in mL) is indicated on each of the
graduated cylinders?
C. Conversions
Express the following numbers in scientific notation and convert .
SHOW ALL WORK.
1. 489,600 minutes converted to seconds
2. 0.00397 years converted to days
3. 0.47 kilometers converted to meters
4. 647 joules converted to kilojoules
*5. 849,000 kilometers converted to centimeters
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REGENTS CHEMISTRY
D. Temperature Conversions
1. Complete the following chart. Show all calculations.
C
K
0C
450 K
294 K
25°C
225 K
-40°C
2. What does temperature measure?
3. What is the absolute temperature scale? Why is it called that?
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REGENTS CHEMISTRY
E. Significant Figures

When are zeros significant?

When are zeros not significant?
Determine the number of significant figures in the following numbers.
1. 0.02
2. 0.020
___________
6. 5,000.0 ____________
___________
7. 6,051,000 ____________
3. 501
___________
8. 0.0005____________
4. 501.0
___________
9. 0.1020____________
5. 5,000
___________
10. 10,001 ____________
Perform the following operations expressing the answer in the correct number of significant
figures. State the rule next to the answer.
11. 1.35 m x 2.467 m = ______________
12. 1,035 m + 42.98 m = _____________
13. 12.01 mL + 35.2 mL + 6 mL = _______________
14. 55.46 g - 28.9 g = _____________
15.0.021 cm x 3.2 cm x 100.1 cm = _______________
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REGENTS CHEMISTRY
F. Density Problems: Show all work.
1. What is the mass of an object whose density is 12 g/mL and occupies a volume of 4 mL?
2. A piece of metal has a mass of 22.7 g. It occupies a volume of 2.00 cm3. What is the density
of the lead?
3. What is the volume of an object whose density is 20g/mL and has a mass of 10 g?
4. A piece of lead has a mass of 302g. What volume does it occupy?
5. An aliquot of ethyl alcohol (density = 0.79 glmL ) occupies a volume of 30 mL. What is the
mass of the ethyl alcohol?
6. The density of silver is 10.5 glcm3. What mass would occupy a volume of 24.0 cm3 ?
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REGENTS CHEMISTRY
G: Classification
Define in your own words:
Substance –
Mixture –
Solution-
Using the classification flowchart from your notes, classify each of the following. Initially
determine if the example is homogeneous or heterogeneous. Then identify final chemical
classification as element, compound, solution or heterogeneous mixture.
Matter
Heterogeneous or
Homogeneous
Final Classification
Water
Carbon
Soil
Pure Air
Carbon Dioxide (CO2)
Table Salt (NaCl)
Sugar dissolved in
water
Homogenized Milk
Stone
Orange Juice
Lead
Oxygen Gas
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REGENTS CHEMISTRY
H: Physical and Chemical Properties
Define in your own words:

Physical Property –

Chemical Property –
Classify the following property as either chemical or physical by putting a check in the
appropriate column.
Physical Property
Chemical Property
1. blue color
2. density
3. flammability
4. solubility
5. reacts with acid to form H2
6. supports combustion
7. sour taste
8. melting point
9. reacts with water to form a gas
10. reacts with a base to form water
11. hardness
12. boiling point
13. can neutralize a base
14. luster
15. odor
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REGENTS CHEMISTRY
I. Physical and Chemical Changes
Define in your own words:

Physical Change –

Chemical Change –
Classify the following as being a physical or chemical change.
Physical
1.
Sodium hydroxide dissolves in water.
2.
Hydrochloric acid reacts with potassium
Chemical
hydroxide to produce a salt, water and heat.
3.
A pellet of sodium is sliced in two.
4.
Water is heated and changed to steam.
5.
Potassium chlorate decomposes to potassium
chloride and oxygen gas.
6.
Iron rusts.
7.
When placed in H2O, a sodium pellet catches on
fire as hydrogen gas is liberated and sodium
hydroxide forms.
8.
Evaporation.
9.
Ice melting.
10.
Food is digested in the stomach.
11.
A tire is inflated with air.
12.
Grass growing in a lawn.
13.
Pancakes cooking on a griddle.
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Wood rotting.
15.
Sugar dissolves in water.
16.
Milk sours.
17.
Water is absorbed by a paper towel.
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REGENTS CHEMISTRY
J: Percent Error - Show all work.
1. A student measured the volume of her soda before she drank it for her midmorning snack.
She measured the volume of the 12 oz. bottle to be 14 oz. Calculate percent error.
2. Clyde was directed to mass a 500.00 g mass on the balance. After goofing off for ten
minutes, he quickly massed the object and reported 458.21 g. Calculate percent error.
3. Drew was told to measure 50 cm of copper wire to use in an experiment. Since his ruler only
measured to 45 cm he used this amount of wire and his experiment was a failure. Calculate
percent error.
4. Will was assigned to determine the density of a sample of nickel metal. When he finished, he
reported the density of nickel as 5.59 g/ml. Calculate percent error.
5. An experiment to determine the volume of a "mole" of a gas was assigned. Barry didn't read
the experiment carefully and concluded the volume was 18.7 liters, but knew he should
have obtained 22.4 liters. Calculate percent error.
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REGENTS CHEMISTRY
K: DBQ - HOW DENSE ARE YOU?
Water has a density of 1.00 g/cm3. The average adult has a
density of 0.97 g/cm3. The 0.97 value means that in fresh water,
most people float about 97% underwater and 3% above water.
It’s a little easier to float in saltwater with 95% under the surface
and 5% above water. In either case, it doesn’t leave much of us
sticking out of the water! And for those with near-zero body fat—like young adult males in good
shape—floating is an even greater challenge! Now if we had noses on top of our heads, like
whales do, we could stop worrying about drowning.
Fact: Anyone who can float on his or her back can remain afloat indefinitely. Or one can float
face down in the water, expend a little energy by taking a few strokes every 20 seconds or so
while lifting the head to take a few breaths—a technique called treading water. Using this
technique people have stayed afloat for long periods of time.
So why do so many people drown in deep water? Currents and water temperatures are certainly
important factors, but many people who find themselves in deep water panic and expend energy
trying to keep their faces continually above water. As they tire, they gasp for air and begin to
swallow water. This extra water weight only adds to their total density, and soon they must exert
even more effort to stay afloat. With more and more swallowed water, their density increases
until they sink below the surface and drown.
1. If the mass of a person is 2.85 x 103 grams, what volume will they occupy? Express your
answer to the correct number of significant figures.
2. When a person treads water, how often does a person need to take a stroke? Convert this
measurement to minutes.
3. What happens to a persons density as they begin to drown? What causes the change in
density?
4. If a student conducted an experiment and determined the density of water to be 1.04 g/cm3,
calculate the percentage of error.
5. How many significant figures are there in the experimentally determined value of the density
of water?
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REGENTS CHEMISTRY
Unit 1 REVIEW: Matter
1. A correct scientific measurement is taken when all digits are read off the equipment + 1
approximation digit added to the end.
2. Convert from one measurement system to another... especially metrics using proportions or
King Henry Doesn't Usually Drink Chocolate Milk
3. Temperature measures average kinetic energy of a substance. Conversions...
K = °C + 273
*** found on REFERENCE TABLE T***
4. Significant Figures identify how many digits were actually measured. The rules:
 all non-zero digits are significant
 zeroes between non zero digits count
 zeroes at the beginning of a value NEVER COUNT
 zeroes at the end of a value count only if there is a decimal point ( no point...no count)


When adding and subtracting values... record answer according to least precise
measurement…lowest measured decimal place.
When multiplying and dividing values... record answer according to least precise
measurement …to the lowest measured sig figs.
5. Density is a physical property.
 Density for elements is found on REFERENCE TABLE S.
 Density = Mass / Volume **** formula given on REFERENCE TABLE T.
6. Matter can be classified according to composition:
Is it homogeneous or heterogeneous?
oIf it is heterogeneous... we do not study these
If it is homogeneous…Is it pure?
oIf it is not pure…it is a mixture…SOLUTION. Mixtures can vary in composition.
oIf it is pure it is called a SUBSTANCE.
oA pure substance can not vary in composition...it's composition is DEFINITE.
oA pure substance that can be decomposed is a COMPOUND.
oA pure substance that can not be broken down is an ELEMENT.
*** Be able to draw pictures and identify similarities and differences between
elements, compounds and mixtures.
7. Properties and changes in matter can be physical or chemical.
 Physical properties and changes can be observed or measured.
 Chemical properties and changes can be seen thru chemical reactions.
8. Calculate percentage of error. Formula on Reference Table T.
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