Chapter(s)
3__
Name ______________________
Period ____
Study Packet: Matter and Change
Set I – Properties and States of Matter
1. What is the difference between mass and weight?
Mass never changes, weight depends on gravity
2. Identify whether the following is a physical or chemical property.
a) Water boils at 100oC
physical
b) Acids will react with metals to form hydrogen chemical
c) Iron will rust when left in air
chemical
d) Food will spoil when left out of the fridge.
chemical
e) The density of aluminum is 2.90 g/cm3 physical
f) A piece of glass you can see through
g) Insoluble in water
physical
physical
h) Will combine with fluorine to make fluoride compounds
chemical
3. Identify whether the following is an intensive or extensive property.
a) Water boils at 100oC
intensive
b) The density of aluminum is 2.90 g/cm3 intensive
c) The mass of a block of CO2(s) (better known as dry ice)
extensive
4. Identify the state of matter. (Assume at RT, unless otherwise stated.)
a) steam
gas
f) has high energy gas
b) apple juice
liquid
g) has moderate energy liquid
c) gasoline
liquid
h) has little energy solid
d) sand
solid
i)
e) pencil
solid
SP - Matter and Change
H2O (s)
solid
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Set II - Density
1. 6.10 g/cm3
2. 3.00 mL
3. 96g
density of 0.5
Find the density of a wooden block that has a volume of 5 cm3 & a mass of 30.5 g
What volume would a rock occupy if it had a mass of 31.2 g & a density of 10.4 g/cm3?
Calculate the mass of a wooden block that is 4 cm long, 2 cm wide, 6 cm high, & has a
g/cm3.
The same wood block is sawed perfectly in half. Determine the mass, volume and density
mass = 48 g ; volume= 24cm3; density = 05.g/cm3
4. 0.150L
How large a container, in L, would you need to hold 195 g of a liquid that has a density
of 1.3 g/cm3?
5. A jeweler suspects that a piece of gold jewelry in his collection is a fake. He knows that the density of
gold is 19.3 g/cm3. If the volume of jewelry is 6 cm3, & its mass is 109 g, is the piece fake? Yes it’s
fake! Explain. The density of the jewelry is 18.2g/cm3
6. The following table has mass & volume of some mineral samples. Calculate the density of sample B.
4g/mL
Sample
Mass (g)
Volume
(mL)
A
19.5
6.54
B
12.4
3.1
C
6.8
3.4
7. Which has a greater mass--- 10 cm3 of steel (d = 7.8 g/cm3) OR 5 cm3 of mercury (d = 13.6 g/cm3)?
Steel: 78g
Mercury: 68g
Steel is more massive
8. The density of oak is 0.7 g/cm3, & the density of pine is 0.4 g/cm3. Compare the masses of a 30 cm3
of each type of wood.
Oak: 21g
Pine: 12g
oak is more massive
9. A 500 mL glass container filled with milk has a mass of 620 g. The mass of the container is 35 g.
What is the density of the milk? Mmilk = 585g
1.17g/mL
10. What is the mass, in kg, of the carrot that has a density of 6 g/mL?
0.018kg – 0.024kg
Set III – Classification of Matter
1. Determine the following information for each material listed below. You may want to do some research for some of the
substances.
Category 1: State of Matter (Solid, Liquid, or Gas)
Category 2: Pure Substance or Mixture
Category 3: If the material is a pure substance, list whether it is an element or compound.
If the material is a mixture, list whether homogeneous or heterogeneous.
Substance
24K gold
SP - Matter and Change
Category 1
Category 2
Category 3
Solid
Pure substance
element
2
14K gold
Solid
Mixture
Homogeneous
air
Gas
Mixture
Homogeneous
brass
Solid
Mixture
Homogeneous
sugar/water solution
Liquid
Mixture
Homogeneous
sugar (C6H12O6)
Solid
Pure substance
Compound
sand/water mixture
Solid in a liquid
Mixture
Heterogeneous
hydrogen gas (H2)
Gas
Pure substance
Element
diamond
Solid
Pure substance
Element
Liquid or gas
Pure substance
Compound
aluminum
Solid
Pure substance
Element
copper sulfate (CuSO4)
Solid
Pure substances
Compound
distilled water
Liquid
Pure substance
Compound
tap water
Liquid
Mixture
homogeneous
ammonia (NH3)
2. Determine the method of separation you would use to separate each mixture (if physical separation is not possible
write – CHEMICAL SEPARATION)
a) Sugar dissolved in water
boil off the water
b) A suspension of sand and water
filter
c) Carbon dioxide
chemical separation
d) Isopropyl alcohol solution
fractional distillation
e) Iron filings in the sand
magnet
f)
chemical separation
Distilled water
g) Onions in a hamburger
pick out
Set IV -- Changes in Matter
1. Identify the name of the phase change (prior knowledge)
a) Solid  liquid
melting
d) Gas  liquid
condensation
b) Liquid  gas
vaporization
e) Gas  solid
deposition
c) Solid  gas
sublimation
f)
freezing
Liquid  solid
2. There are two types of vaporization: boiling and evaporation. What is the difference?
Boiling occurs throughout the liquid and evaporation occurs at the surface of the liquid
3. Identify whether the following is a physical or chemical change.
a) melting butter physical
b) b) shattering a window
physical
c) combustion of gasoline chemical
SP - Matter and Change
d) CO2(s)  CO2(g) physical
e) burning a candle chemical
f)
painting a table physical
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g) baking a cake chemical
i)
K2O + H20  2KOH chemical
h) dissolving salt in water physical
4. When 400 g of wood are burned, 270 g of gas are produced. What is the mass of ash left? 130g
5. Consider the reaction below and complete the table.
magnesium + oxygen  magnesium oxide
Reaction
A
B
C
D
E
Mass of Mg (g)
5.0
6.5
13.6
19
10.8
Mass of O2 (g)
3.3
4.3
9.0
12.5
37.4
Mass of MgO (g)
8.3
10.8
22.6
31.5
48.2
6. Determine whether the following are endothermic or exothermic changes.
a) boiling water
endothermic
b) sweat drying on your skin
endothermic
c) water condensing on a glass endothermic
d) 2Mg + O2 + heat  2MgO endothermic
e) water freezing to become ice exothermic
f) C6H12O6 + O2  CO2 + H2O + heat
exothermic
g) CO2 + H2O + energy  C6H12O6 + O2
endothermic
Test Review: Matter and Change
Objectives to be tested include, but are not exclusive to
 Define: chemistry, matter, endothermic, exothermic, pure substance, mixture
o Science is the use of evidence to develop testable explanations and predictions of natural phenomena.
o Chemistry – the study of matter and it’s changes.
o Matter – has mass and volume
o Endothermic – absorbs heat, substance gets warmer
o Exothermic – gives off heat, substance gets cooler
o Pure substance – can not be broken down by physical means (has a chemical formula)
o Mixture – physical blend of substances.
 Homogeneous – uniform composition. INCLUDES SOLUTIONS and ALLOYS
 Heterogeneous – non.uniform composition. Includes suspensions & colloids
 Identify and relate properties of 3 states of matter
o Solids, liquids, gases. See chart from notes
 Distinguish between physical and chemical properties/physical and chemical changes
o Go through notes and book and make a list of all physical/chemical properties and changes
 Identify a substance as pure substance (element or compound) or mixture (homogeneous or heterogeneous)
o Element – occupies one box on the periodic table
o Compound – a combination of elements put together in a formula. Not to be mixed up with alloys which
are a homogeneous mixture of elements
o Mixture – see number 1, letter H
 State and apply laws of conservation of mass/energy
SP - Matter and Change
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Law of conservation of mass
 Make sure the mass of the reactants is equal to the mass of the products
o Law of conservation of energy – energy can not be created nor destroyed
List the indicators of a chemical reaction
o Temperature change (exo/endothermic)
o Color change (like rusting)
o Formation of gas (like in the balloon activity)
o Formation of precipitation
o Light is formed
Understand the meaning of density (intensive property) and be able to calculate it from mass and volume data
density = mass/volume
density does not change as the amount of a substance changes
Distinguish between atom, molecule, compound, element
o Atom – one unit of an element
o Molecule – more than one atom
o Compound – combination of elements put together in a formula
o Element – one box on the periodic table
Determine number of atoms in a chemical formula
a. Subscripts indicate the number of atoms of that particular element
o




Practice
1. Provide an example of matter and of something that is not matter.
Matter: book; non-matter: light
2. Determine
a)
b)
c)
d)
whether the following are describing a physical property or chemical property:
metallic sodium is soft enough to be cut with a knife Physical
cork floats on water
Physical
when water is heated above 100C a gas is evolved. Physical
when sodium comes in contact with water, a gas is evolved. Chemical
3. Determine
a)
b)
c)
d)
whether the following is describing a physical change or chemical change:
evaporation of nail polish remover Physical
hard-boiling an egg Chemical
digesting food Chemical
chewing food Physical (the act of breaking up the food only)
4. Identify the following as a
a) ham sandwich
b) S8
c) pool water
d) SO2
element, compound, homogeneous mixture, or heterogeneous mixture:
Heterogeneous mixture
Element
Homogeneous (assuming no floating debris)
Compound
5. If 32 g of sulfur combines with 32 g of oxygen, when heated, to form solid sulfur dioxide, what mass of sulfur
dioxide is produced? Identify the reactants and products in this reaction. Is this reaction endothermic or exothermic?
Mass of sulfur dioxide produced = 64 g
Reactants = sulfur and oxygen
Exothermic
6. When potassium bromide dissolves, it is an endothermic process. Would the test tube feel cool or warm? Cold
7. List 2 intrinsic properties and 2 extrinsic properties.
Intrinsic: density, boiling point, melting points
Extrinsic: mass, volume
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