Math Review for Chemistry
Name: __________________________________________
Unit 1: Introduction to Chemistry
Monday
Tuesday
1
2
8 Video 1.2
Density Lab
9 Video 1.3
Density Lab Quiz
15 Video 1.6
Phys/Chem Lab
16 HW packet due
Phys/Chem Lab
Quiz
Wednesday
3
Chemistry Pre-Test
Thursday
4
Chemistry Pre-Test
10
Signs of Reaction
Lab
17
11 Video 1.4
Signs of Reaction
Lab Quiz
18
Unit 1 Exam Part 1
Multiple Choice
Friday
5 Video 1.1
Signed Papers and
sign into website
Safety Quiz
12 Video 1.5
19
Unit 1 Exam Part 2
Short Answer
Notes:
 Every schedule will be color coded. Red is for announced quizzes or tests (there may be pop quizzes). Green
is for Lab (lab quizzes will always be the next day). Purple is for homework. Blue is for reminders.
 Please take time to navigate the website and edpuzzle homework site.
www.chemisme.com
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Math Review for Chemistry
Key Ideas
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Matter is classified as a pure substance or as a mixture of substances. (3.1q)
The three phases of matter (solids, liquids, and gases) have different properties. (3.1kk)
A pure substance (element or compound) has a constant composition and constant properties
throughout a given sample, and from sample to sample. (3.1r)
Elements cannot be broken down by chemical change. (3.1u)
Mixtures are composed of two or more different substances that can be separated by physical
means. When different substances are mixed together, a homogeneous or heterogeneous mixture
is formed. (3.1s)
The proportions of components in a mixture can be varied. Each component in a mixture retains
its original properties. (3.1t)
Differences in properties such as density, particle size, molecular polarity, boiling point and
freezing point, and solubility permit physical separation of the components of the mixture. (3.1nn)
A solution is a homogeneous mixture of a solute dissolved in a solvent. The solubility of a solute in
a given amount of solvent is dependent on the temperature, the pressure, and the chemical
natures of the solute and solvent. (3.1oo)
Energy can exist in different forms, such as chemical, electrical, electromagnetic, thermal,
mechanical, and nuclear. (4.1a)
Heat is a transfer of energy (usually thermal energy) from a body of higher temperature to a body
of lower temperature. Thermal energy is the energy associated with the random motion of atoms
and molecules. (4.2a)
Temperature is a measurement of the average kinetic energy of the particles in a sample of
material. Temperature is not a form of energy. (4.2b)
The concepts of kinetic and potential energy can be used to explain physical processes that
include: fusion (melting), solidification (freezing), vaporization (boiling, evaporation),
condensation, sublimation, and deposition. (4.2c)
A physical change results in the rearrangement of existing particles in a substance. A chemical
change results in the formation of different substances with changed properties. (3.2a)
Chemical and physical changes can be exothermic or endothermic. (4.1b)
The structure and arrangement of particles and their interactions determine the physical state of a
substance at a given temperature and pressure. (3.1jj)
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Math Review for Chemistry
Metric
Use Reference Tables C and D to help you answer the following questions about the metric system.
1. Give the unit used to describe the following:
a.
Mass
_______
d. Time:
______
b.
Volume
_______
e. Temperature:
______
c.
Energy
_______
f.
______
Pressure:
2. Complete the following number line by adding the prefixes that pertain to the marked values:
3. If a substance weighs 2.00 grams and you need the mass in kilograms, will the number appear to become
smaller or larger? Explain your answer.
4. If a liquid has a volume of 5800 mL and you need the mass in Liters, will the number appear to become
smaller or larger? Explain your answer.
5. If a substance has a mass of 0.00235 grams and you need the mass in milligrams, will the number appear
to become smaller or larger? Explain your answer.
6. Convert the following:
a. 900 km
=
__________ m
h. 568 mm
=
__________ m
b. 200 kg
=
__________ g
i. 52 mg
=
__________ g
c. 5.00 m
=
__________ km
j. 0.025 J
=
__________ mJ
d. 7000 J
=
__________ kJ
k. 0.859 s
=
__________ ms
e. 800 cm
=
__________ m
l. 0.0256 m
=
__________ um
f. 20 cg
=
__________ g
m. 0.000589g =
__________ ng
g. 2.0 L
=
__________ cL
n. 0.00005987 m=
__________ pm
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Math Review for Chemistry
Metric
1. Determine the number of mm in 1600 m.
2. Determine the number of m in 1600 mm.
3. Determine the number of mm 14.3 cm.
4. Convert 5.2 cm of MG ribbon into mm of ribbon.
5. Convert 0.049 kg of sulfur to g.
6. Convert 0.020kg of tine to mg.
7. Convert 150mg of aspirin to g of aspirin.
8. Convert 2500 mL of HCl to L of HCl.
9. Convert 4.75 cm to m.
10. Convert 5.698 Kg to mg.
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Math Review for Chemistry
Scientific Notation
Scientific notation is used to express numbers that are very large or small. An example is 6.02x1023
which is a large number called a “mole” in chemistry. It means 6.02 times 10 twenty three times; or
602000000000000000000000! The number 6.02 is the “base number”, which must be between 1 and 10. The
number 23 is the “exponent” which represents the number of place the decimal moved to get the base number
between 1 and 10.
Another number, 5.12x10-5 is a small number. The exponent is negative which really means the 5.12 is
divided by 10 five times. So the rule is if the exponent is positive the real number is large and if the exponent is
negative the real number is small.
Convert the following numbers into scientific notation:
1)
3,400
_______________________________
2)
0.000023
_______________________________
3)
101,000
_______________________________
4)
0.010
_______________________________
5)
45.01
_______________________________
6)
1,000,000
_______________________________
7)
0.00671
_______________________________
8)
4.50
_______________________________
Convert the following numbers into standard notation:
9)
2.30 x 104
_______________________________
10)
1.76 x 10-3
_______________________________
11)
1.901 x 10-7
_______________________________
12)
8.65 x 10-1
_______________________________
13)
9.11 x 103
_______________________________
14)
5.40 x 101
_______________________________
15)
1.76 x 100
_______________________________
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Math Review for Chemistry
Significant Figures Introduction
1. A student finds the mass of a solid using 4 balances. Explain his findings in terms of precision and accuracy.
Data
Mass 1
45.698 grams
Mass 2
45.7 grams
Mass 3
45.69842 grams
Mass 4
45.9 grams
2. A beaker has marks every 50mL. A cylinder has marks every 10mL. A pipette has marks every 1mL. Is the
pipette the most accurate or precise tool? Explain your answer.
3. Sally measures 11mL of water in the beaker described in question 2. Henry measures 11mL in the pipette
described in question 2. When they add their water together in one cup, do they have exactly 22mL combined?
Why or why not?
In order to report the most precise and accurate data possible we must learn to count significant figures.
When measuring a substances mass, volume, etc. the device requires you to measure “one place beyond.”
All the numbers you report count as a significant figure sig fig) except leading zeros and sometimes the
trailing zeros. Let’s investigate:
Example 1: A piece of aluminum has a mass of 0.0521 grams which had 3 sig figs. This is not 5 sig
figs because if we convert that mass to mg the mass becomes 52.1 mg. Again the number has 3 sig figs
which shows it didn’t get any more precise. Proof that leading zeros never count.
Example 2: A beaker of water contains 520 mL which has 2 sig figs. The trailing zero doesn’t count this
time because if we convert to liters the volume is .52 L. The trailing zero was not measured. If we want
to show that it was exactly 520 mL we would report it as 520. mL with a decimal point. That way if we
convert to liters it is .520L.
Example 3: A reaction takes 0.0025050 s which has 5 sig figs. Remember the first three zeros ar “place
holders and don’t count. If we convert to ms we get 2.5050 ms, also with 5 sig figs. The trailing zero
was measured or else the student wouldn’t have reported it. The rule is: Leading zeros never count,
trapped zeros always count they are measured) and trailing zeros count if there is a decimal.
Using the rules above, count the number of significant figures in the following measurements:
4. 3.456 L
_____
7.
0.000206 m
_____
5. 2.300 g
_____
8. 0.025600 L
_____
6. 1.258092 m
_____
9. 0.520301 J
_____
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Math Review for Chemistry
If a piece of glassware is very precise it may have a lot of sig figs, as many as 4. A less accurate piece of
glassware such as a beaker will only have 1 sig fig. If both pieces of glassware are used to measure quantities in
a lab we have to round our results to the least precise measurement. When working with measurements the
quantity with the least decimal places is the least precise. For example, if the beaker measures 10mL and a
cylinder measures 10.1mL the cylinder is more precise. If the two quantities are added together the new volume
is 20mL. The decimal must be rounded to make our answer to one sig fig. Therefore the rule is: When adding
or subtracting measurements, round your answer to the lowest number of decimal places given.
Complete the following operations and report to the correct number of significant figures.
10.
10.2 + 21
________
14.
0.023 - 0.0004
_______
11.
31.3 + 54.45 ________
15.
5.068 - 0.1
_______
12.
22.59 + 21
________
16.
45.6 - 22.12 + 11
_______
13.
0.023 + 20.1 ________
17.
0.0123 +5.689 – 0.014
_______
When performing calculations with our data sometimes we have to multiply and divide our data. In theis case,
the most precise answer is the one with the most sig figs. Since we need to round to our least precise
measurement, we should round to the least number of sig figs given. For example, if the mass of a substance is
10.0 grams 3 sig figs) and the volume is 2 mL 1 sig fig) the density is 5 g/mL also 1 sig fig). The rule is:
When multiplying or dividing measurements, round your answer to the lowest number of significant
figures given.
Complete the following operations and report to the correct number of significant figures.
18.
5.87 * 2.1
________
22.
589 / 12
_______
19.
4 * 78
________
23.
78.632 / 52.3
_______
20.
0.0235 * 9
________
24.
1569 / 24 * 2
_______
21.
0.014 * 0.01
________
25.
596 * 32 ) / 22
_______
If both types of operations are used, always follow the multiplication rules least sig figs). Finally, in scientific
notation, only the base number counts not the exponent or the 10). Use PEMDAS!
26.
22.1-10.0) / 2
________
28.
6.23x10-3/2.15x10-4
_________
27.
12.35 / 4.56-2.14)
________
29.
2.1x102 – 1.4x101) * 2
_________
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Math Review for Chemistry
Rounding Significant Figures
Unrounded Answer
Rounded Answer
1. 1.2m + 2.35m
2. 2.6358cm * 2.1cm
3. 5.681mm - 2.mm
4. 3845.2L / 25.2354L
5. 25cm + 3cm
6. 1.2m * 2m
7. 859678.2354cm – 568426.1cm
8. 5.3cm * 5.2398m * 2m
9. 45.25252nm + 45.8563nm
10. 68.23m / 38.255m
11. 10000g / 10.0g
12. 1L * 1.0L
13. 1254.1cm / 100cm
14. 0.000456m + 0.00524m
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Math Review for Chemistry
Significant Figures Worksheet
Identify the number of significant figures:
1. 3.0800
______
6. 3.200x109
______
2. 0.00418
______
7. 250
______
3. 7.19x10-5
______
8. 780,000,000
______
4. 91,600
______
9. 0.0101010
______
5. 0.0003003
______
10. 0.00800
______
Round to 3 significant figures:
1. 7.8975
______
6. 78765.085
______
2. 7976.896
______
7. 8999.99
______
3. 80.000
______
8. 1.0000
______
4. 848001
______
9. 0.008978
______
5. 7.89765x10-8
______
10. 0.000076097078
______
Solve using the proper number of significant figures:
1. 4.86097 + 90.9048
________
2. 3578.9 – 423.84
________
3. 89038.9357 + 345.98 – 89.847
________
4. 8975.8947 x 56.8
________
5.
5.78x10-9) 7.789x104)
________
6.
9.856x108)/ 5.8x10-6)
________
7.
76.9478 + 7865.9) x 6.780 – 5.76)
________
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Math Review for Chemistry
Significant Figures Practice
Count the number of Significant figures:
Round to three significant figures:
12
Math Review for Chemistry
Density Introduction
1. Reference table S gives the densities of many elements. Which of the first 10 elements is the least dense?
2. Which of the first ten elements has the greatest density?
3. Generally, what phase are all elements in that have low densities? What phase has high densities?
4. Bubbles in soda rise to the surface. Explain this in terms of density.
5. Sand in the ocean always settles to the ocean floor. Explain this in terms of density.
6. A drop of water and a pool of water both have a density of 1 g/mL. Is density intensive or extensive?
7. A sample of sulfur has a mass of 28.5 grams. What is this sample’s volume in mL?
8. A sample of oxygen has a mass of 16.0 grams, what is the volume of the sample in Liters?
9. A balloon is filled with helium to a volume of 2.00L. What is the mass of the helium in gram?
10. A lead cube with a length of 2.2cm has what volume? Mass?
11. A pure elemental gas has a mass of 0.018 g and a volume of 20.0 mL. What gas could it be?
12. A pure metallic liquid has a mass of 162.6 g and a volume of 12mL. What element could it be?
13. A student finds the mass of a sample of copper to be 130.0 grams and measure the volume to be 15.0 cm3.
What is the student’s percent error?
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Math Review for Chemistry
Density Practice
1. The density of silver (Ag) is 10.5 g/cm3. Find the mass of Ag that occupies 965 cm3 of space.
2. A 2.75 kg sample of a substance occupies a volume of 250.0 cm3. Find its density in g/cm3.
3. Under certain conditions, oxygen gas O2) has a density of 0.00134 g/mL. Find the volume occupied by
250.0 g of O2 under the same conditions.
4. Find the volume that 35.2 g of carbon tetrachloride (CCl4) will occupy if it has a density of 1.60 g/mL.
5. The density of ethanol is 0.789 g/mL at 20oC. Find the mass of a sample of ethanol that has a volume of
150.0 mL at this temperature.
6. 30.0 g of each of the following acids are needed. Find the volume of each that must be measured out in a
graduated cylinder.
A. hydrochloric acid ( HCl), density = 1.164 g/mL
B. sulfuric acid (H2SO4), density = 1.834 g/mL
C. nitric acid (HNO3), density = 1.251 g/mL
7. A rectangular block of lead (Pb) measures 20.0 mm X 30.0 mm X 45.0 mm. If the density of Pb is 11.34
g/cm3, calculate the mass of the block.
8. A cube of gold Au) has a side length of 1.55 cm. If the sample is found to have a mass of 71.9 g, find the
density of Au.
Temperature Conversions
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Math Review for Chemistry
1) Convert 83 °C to Kelvin
2) How many Celsius degrees separate the freezing and boiling points of water? _______
What are these two temperatures? ________ & _________
3) What is the lowest possible temperature in °C? _________
4) How many Kelvin separate the freezing and boiling points of water? ______
What are these two temperatures? ________ & ________
5) What is the lowest possible temperature in Kelvin? __________
6) Using the temperature conversion formula on Table T in your Reference Tables, convert the following
temperatures to either Celsius or Kelvin.
383 K
80C
323K
10 C
10K
7) Using Table S in your reference table what temperature does Sulfur melt at?
8) Using table S, what is the freezing point of Silver (Ag)?
9) Using table S, what is the boiling point of Mercury (Hg)?
10) Using Table S, if room temperature is 22C, is Bromine a solid, liquid, or gas?
Matter Activity
Station Number/
Description/Observations
Classification
How do you know?
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Math Review for Chemistry
Identity of Substance
(Element,
Compound,
Homogeneous Mixture,
Heterogeneous Mixture)
1
2
3
4
5
6
7
8
9
10
11
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Math Review for Chemistry
12
13
14
Questions:
1. How could you tell a substance is an element?
2. What phases can elements be in?
3. How could you tell a substance is a compound?
4. What phases can compounds be in?
5. How could you tell a sample is a mixture?
6. What phases can mixtures be in?
7. How do you know the difference between a homogeneous and heterogeneous mixture?
Matter
Anything that has mass and volume (takes up space)
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Math Review for Chemistry
CAN be separated by
PHYSICAL means
Can NOT be separated
by physical means
PURE SUBSTANCES
(each piece looks the same
– PURE!)
-each piece has exact same
composition.
Can NOT be separated
by chemical means
ELEMENT (simplest
form of matter)
Example: Na, Cl2
MIXTURES (each piece is
different – not pure)
Same
Separated by
composition
chemical means,
throughout
only
Different
composition
throughout
COMPOUND or
MOLECULE
(2+ different elements
chemically combined)
HOMOGENEOUS
MIXTURE (uniform
throughout—distinct
pattern)
HETEROGENEOUS
MIXTURE (not
uniform throughout—
a pattern)
Example: NaCl (table
salt), H2O (water)
Example: saltwater,
iced tea
Example: Italian
dressing, concrete, soil,
chocolate chip cookie
Homo = same
Hetero = opposite
Particle
Diagram
Particle
Diagram
Particle
Diagram
Particle
Diagram
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Math Review for Chemistry
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Math Review for Chemistry
Matter Practice
Classify each of the following with the combination of terms listed below.
pure substance – element
mixture – homogeneous
pure substance – compound
mixture – heterogeneous
1. HCl (aq)
2. sugar (C11H22O11)
3. KBr (s)
4. Soil
5. Cl2 (g)
6. water
7. CH2(OH)2 (aq)
8. Sodium
9. Hg (l)
10. iron oxide
11.NH3 (l)
12. salt water
13. Matter that is composed of two or more different elements chemically combined in a fixed proportion is
classified as
(1) a compound
(2) an element
(3) a mixture (4) a solution
14. A compound differs from an element in that a compound
(1) is homogeneous
(2) has a definite composition
(3) has a definite melting point
(4) can be decomposed by a chemical reaction
15. A compound differs from a mixture in that a compound always has a
(1) homogeneous composition
(2) maximum of two elements
(3) minimum of three elements
(4) heterogeneous composition
16. A heterogeneous material may be
(1) an element
(2) a compound
(3) a pure substance
(4) a mixture
17. Which statement is an identifying characteristic of a mixture?
(1) a mixture can consist of a single element
(2) a mixture can be separated by physical means
(3) a mixture must have a definite composition by weight
(4) a mixture must be homogeneous
18. Which must be a mixture of substances?
(1) solid
(2) liquid
(3) gas
(4) solution
19. Which substance can be decomposed by chemical means?
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Math Review for Chemistry
(1) aluminum
(2) octane
(3) silicon
(4) xenon
20. Which substance can be decomposed by chemical means?
(1) ammonia
(2) oxygen
(3) phosphorus
(4) silicon
21. Which substance can not be broken down by a chemical reaction?
(1) ammonia
(2) argon
(3) methane
(4) water
22. Two substances, A and Z, are to be identified. Substance A can not be broken down by a chemical change.
Substance Z can be broken down by a chemical change. What can be concluded about these substances?
(1) Both substances are elements.
(2) Both substances are compounds.
(3) Substance A is an element and substance Z is a compound.
(4) Substance A is a compound and substance Z is an element.
23. Which terms are used to identify puresubstances?
(1) an element and a mixture
(2) an element and a compound
(3) a solution and a mixture
(4) a solution and a compound
24. Two different samples decompose when heated. Only one of the samples is soluble in water. Based on this
information, these two samples are
(1) both the same element
(2) two different elements
(3) both the same compound
(4) two different compounds
25. Tetrachloromethane, CCl4, is classified as a
(1) compound because the atoms of the elements are combined in a fixed proportion
(2) compound because the atoms of the elements are combined in a proportion that varies
(3) mixture because the atoms of the elements are combined in a fixed proportion
(4) mixture because the atoms of the elements are combined in a proportion that varies
21
Math Review for Chemistry
Drawing Particle Arrangements
Draw a diagram of a:
pure diatomic
element
pure diatomic
compound
mixture of
two elements
mixture of
an element &
a compound
mixture of
two diatomic
elements &
a compound
1.) In terms of composition/type of atoms, what is the difference between a monatomic element, a diatomic
element, and a diatomic compound?
2.) Use the following key for parts a-c.
a.) 8 atoms of element X in gaseous form
= element X
= element Z
b.) 4 molecules of compound X2Z in liquid form
c.) Homogeneous mixture of element Z with element X (10 atoms of each element).
22
Math Review for Chemistry
Phases and Phase Changes
Directions: Using the boxes provided below as your container, place six circular molecules in each container
representing the given phase. Then on each line with the arrow label which phase change is occuring. Last fill in
the chart below about phases using the words provided in the parenthesis.
SOLID (s)
LIQUID (l)
Solid
GAS (g)
Liquid
Gas
Shape
(Has a fixed shape or
takes the shape of the
container)
Volume
(Has a fixed volume or
takes the volume of the
container)
Density
(high or low)
Particle arrangement
(rigid or free)
Attraction
(particles are highly
attracted and close or
weakly attracted and
spread out)
23
Math Review for Chemistry
Unit 1 Review
Regents Chemistry
METRIC
1. Using tables on page one of your reference table you should be able to identify which unit is used to measure
each quantity and you should be able to convert between units using the prefixes. Locate the prefix assigned to
the measurement unit that you are starting with and then find the prefix that you want to convert to. Count the
number difference between the factors and then move your decimal that many places.
a. Identify the unit used for each quantity:
(1) mass
_________
(4) temperature
__________
(2) volume
_________
(5) length
__________
(3) energy
_________
(6) time
__________
b. Convert the following:
(1) 568 mL to L
___________________
(2) 0.00897 g to mg
___________________
(3) 45700 mm to km ___________________
2. Density is the measurement of mass divided by volume. A substance’s density can help identify it. For
example, water’s density is 1.00g/mL. Substances float in water of they have low densities, and sink when their
densities are greater than 1.00 g/mL.
a. Calculate the density of 5.00 gram sample of an unknown substance, which has a volume of
5.15mL.
b. Using table S, identify the unknown substance in question (a) above. __________________________
c. Calculate the mass of a substance with a density of 2.50 g/mL and a volume of 23.0mL.
d. Calculate the volume of a metal rectangle with a height of 2.0cm, a length of 3.0cm, and a width
of 1.0cm.
e. If the metal in question (d) above is iron, calculate the mass. (Hint: density is on table S)
24
Math Review for Chemistry
SCIENTIFIC NOTATION
3. Scientific Notation is used to represent very small or very large numbers. Convert the following to scientific
notation:
a. 0.00000345
____________________________
b. 1098000000
____________________________
c. 0.000345
____________________________
d. 0.000005677
____________________________
SIGNIFICANT FIGURES
4. All whole numbers 1-9 count. Preceding zeros never count, trapped zeros always count, and trailing zeros
count IF THERES A DECIMAL before the zero. Count the number of significant figures:
5678
0.09809
0.00345
0.0712
0.0987
10000
10200
102.0986
5. When rounding, your answer can only be as precise as your least precise measurement. When adding or
subtracting numbers, round your answer to the lowest decimal place given. When multiplying or dividing,
round your answer to the least number of significant figures. Calculate and round to the correct number of
significant figures:
a. 4.567 + 1.2 = _____________
d. 67065/87.2 = ________________
b. 678.345-234.98 = ______________
e. (54.0-32.34)/1.202 = ________________
c. 45 x789 = _____________
f. 3.108*(98.70-8.20) = __________________
ELEMENTS, COMPOUNDS, AND MIXTURES
6. Matter is anything that has a mass and takes up space. An element is the simplest form of matter, which
cannot be broken down any further. Elements are listed on Table S and the periodic table. Their symbols start
with an uppercase letter.
a. Which of the following is not matter? _____________________
Magnesium
Calcium Carbonate
Salt water
Heat
b. Which of the above is an element? _____________________
25
Math Review for Chemistry
7. Compounds are composed of two or more elements. They can only be decomposed chemically. Elements
and compounds are also known as substances.
a. Which of the choices in number one was a compound? ________________________
b. How can compound be broken down? __________________________________________________
c. Which of the choices in question one are substances? ______________________________________
8. Mixtures are physical combinations of two or more substances (elements and/or compounds). Mixtures can
be homogeneous (completely mixed, cannot see the parts) or heterogeneous (unevenly mixed, can see the
parts). Mixtures can be separated by physical means. Label each as homogeneous or heterogeneous:
Sand: ____________________
Brass: ______________________________
Milk: ____________________
Oil and water: ________________________
9. Compounds must be separated chemically but mixtures can be separated easily using physical methods.
a. Match each method with its name.
Distillation
Filtration
Decant
Chromatography
Separated by differences in particle size
To pour off the top layer of an uneven mixture
Separated by differences in boiling point.
Just a test for purity
b. Which of the above processes only work if the mixture is heterogeneous? _____________________
10. Mixtures are composed of solutes that dissolve and solvents that do the dissolving. The solute should be the
smaller quantity.
a. In iced tea, what is the solute? ___________________ solvent? ________________________
b. In air, name a solute: _________________
c. Do all solvents have to be water? Explain. _______________________________________________
SOLIDS, LIQUIDS, AND GASES
11. A solid has a definite shape and volume. Solids are arranged in a geometric pattern. Liquids have a definite
volume but take the shape of the container they are in. Gases have an indefinite shape and volume; they take the
shape and volume of the container. Gases are easily compressed.
a. Draw particle diagrams for a solid, liquid, and a gas using at least 5 particles:
b. Which has a definite shape?
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Math Review for Chemistry
HCl(g)
H2O(l)
Cu(s)
c. Which has a definite volume?
LiF(g)
Br2(l)
Mg(s)
12. Vapors are the gas phase of substances that are normally solid or liquid at room temperature. Which can be
a vapor?
Carbon dioxide ______
Water _____
Oxygen _____
13. Phase changes occur when heat is given to or taken from a sample. For each of the following, give the
phases involved and if it is endothermic or exothermic.
Evaporation
___________________________
__________________________
Melting
___________________________
__________________________
Deposition
___________________________
__________________________
Boiling
___________________________
__________________________
Condensation
___________________________
__________________________
Sublimation
___________________________
__________________________
CHANGES IN THE LAB
14. Physical changes are changes where the substance retains its properties. Chemical changes will make
substances change into new substances and change properties.
a. Label the following as physical (P) or chemical (C) properties:
Texture
____
flammability ____
boiling point:
____
Odor
____
color
chemical composition:
____
____
b. Label the following as physical (P) or chemical (C) changes:
Corrosion: ____
melting:
____
mixing:
____
Freezing:
cutting:
____
decaying:
____
____
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