Chemistry Unit 1- Matter Study Guide
Unit Essential Questions
Why can intensive properties be used to identify substances?
a. How do you know if something is matter?
i.
Why do we place matter into different categories?
b. How can matter change?
i.
How do physical changes differ from chemical changes?
c. What information can we gather about all forms of matter?
i.
How are physical properties different from chemical properties?
ii.
It's called chemistry so why are physical properties studied anyway?
Unit Learning Goals
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Describe density as a physical property that depends only on the type of substance, not the amount of
substance (intensive property)
Distinguish between elements, compounds, and mixtures (heterogeneous and homogeneous)
Explain why elements and compounds are pure substances but mixtures are not
Sort particulate models of elements, compounds, and mixtures into their respective categories
Calculate the mass, volume, and density of an object from real world data, such as: a plot of mass
versus volume to calculate the density of a substance
Predict whether an object floats or sinks in a liquid
Plan and conduct an experiment to classify properties of matter as intensive
Demonstrate how intensive properties can be used to identify a compound
Classify changes in matter as either the result of a chemical change or a physical change
Provide evidence or clues that a chemical change has taken place
EQ - How do you know if something is matter?
1. What is the chemistry definition of matter?
2. Provide 3 examples and 3 non-examples of matter.
EQ – Why do we place matter into different categories?
3. Complete the following concept map using the word bank listed below;
WORD BANK - gas , formation of bubbles, element, ability to react with acid, boiling, solid, change in
temperature, malleability, homogenous, corroding , burning, cutting, heterogeneous, formation of a
precipitate, color change, compound, rusting
4. Describe how pure substances are different from mixtures.
5. Label the following particulate models as either pure substances (PS) or mixtures (M)
6. For the pure substances above, add an additional label indicating whether it is an Element (E) or a
Compound (C).
7. What is the difference between a heterogeneous mixture and a homogeneous mixture? Give an
example of each.
8. What is the difference between an element and a compound? Give two examples of each.
EQ - How can matter change?
9. List the two main ways in which matter can change.
10. Provide 2 examples of EACH of the changes listed above.
11. Describe how each of the changes listed above differ from each other.
12. Read each scenario. Decide whether a physical or chemical change has occurred and give evidence for
your decision. The first one has been done for you to use as an example.
Scenario
a
Umm! A student removes a loaf of bread hot from
the oven. The student cuts a slice off the loaf and
spreads butter on it.
b
Your friend decides to toast a piece of bread, but
leaves it in the toaster too long. The bread is black
and the kitchen if full of smoke.
c
You forgot to dry the bread knife when you
washed it and reddish brown spots appeared on it.
d
You blow dry your wet hair.
e
You blow dry your wet hair.
f
You take out your best silver spoons and notice
that they are very dull and have some black spots.
g
A straight piece of wire is coiled to form a spring.
h
Food color is dropped into water to give it color.
i
Chewing food to break it down into smaller
particles represents a _________ change, but the
changing of starch into sugars by enzymes in the
digestive system represents a
___________change.
j
In a fireworks show, the fireworks explode giving
off heat and light.
Physical or
Chemical
Change?
Physical
Evidence…
No change in substances.
No unexpected color
change, temperature
change or gas given off.
13. Does the following diagram represent a physical or chemical change? Explain your choice.
14. Two colorless solutions are mixed and a yellow solid appears. What kind of change is this? Give
reasons for your answer.
15. Write a T for true and an F for false.
_____ a. Color change is evidence that a chemical change may have occurred.
_____ b. Fizzing or foaming is evidence that a chemical change may have occurred.
_____ c. Production of sound is evidence that a chemical change may have occurred.
_____ d. Production of heat or light is evidence that a chemical change may have occurred.
_____ e. Production of an odor is evidence that a chemical change may have occurred.
_____ f. Chemical changes cannot be reversed by physical changes.
EQ - What information can we gather about all forms of matter?
16. Classify each of the properties listed below as physical or chemical. For physical properties further
classify the property as extensive or intensive.
Property
Color
Combustibility
Hardness
Density
Mass
Melting point
Ductility
Volume
Reactivity with acid
Odor
Weight
Malleability
Tendency to corrode
Physical or Chemical
Intensive or Extensive
17. Identify each of the following as an example of a physical property or a chemical property.
a. Silver tarnishes when it comes in contact with hydrogen sulfide in the air.
b. A banana is yellow.
c. A sheet of copper can be pounded into a bowl.
d. Barium melts at 725 C.
e. Gasoline is flammable.
f. A diamond is the hardest natural substance.
g. Helium does not react with any other element.
h. A bar of lead is more easily bent than is a bar of aluminum of the same size.
i.
Potassium metal is kept submerged in oil to prevent contact with oxygen or water.
j.
An apple will turn brown is left in oxygen.
k. Diamond dust can be used to cut or grind most other materials.
l.
Acid in tomato sauce can corrode aluminum foil.
m. Rocks containing carbonates can be identified because they fizz when hydrochloric acid is applied.
n. A piece of charcoal, which is mostly the substance carbon, glows red, gives off heat, and becomes a
gray ash.
18. Classify the following examples as intensive or extensive properties of matter.
a) Your pencil is yellow. _______________________________
b) Your watch is 12cm long. _______________________________
c) Your t‐shirt is made of cotton. _______________________________
d) The mass of a basketball is 0.62 kg. _______________________________
e) The outer covering of the ball is rubber. ______________________________
19. Sticking a thermometer into a glass of clear liquid will not reveal what the liquid is. Under what
conditions could you measure the temperature of the material to get useful information about its
identity?
20. Circle the following unit(s) that could be used for density. (HINT: 1 mL also equals 1 cm 3)
g/mL
L/g
kg/cm3
mL/cm3
g/cm
21. In a glass of ice water, the ice cubes are on top of the water. What can you say about the density of
solid water in relation to the density of liquid water?
22. A rock has a mass of 127 g and displaces 32.1 mL of water. What is the density of the rock?
23. The density of gold is 19.32 g/mL. You have a shiny, gold-colored bar of metal which weighs 57.3 g and
has a volume of 4.7 mL. Is your metal bar pure gold? ___________ (YES or NO)
24. The density of aluminum is 2.7 g/mL. What is the volume of 8.1 grams?
25. You have 250 mL of ethanol that has a density of 0.78 g/mL. What is the mass of the liquid?
26. Three balloons are each filled with a different gas: hydrogen (0.0899 g/L), carbon dioxide (1.977
g/L), and helium (0.1785 g/L). The balloons are released into the air. Which balloon will float the
highest in the air (air has a density of 1.29 g/L)? __________________________________
27. Density is an _______________________ property and is used to determine the
______________________ of a substance.
28. You are on a scientific exploration that has lead you deep into uncharted territory, weeks away from
civilization. Your bumbling assistant has forgotten to label the containers of clear liquid that you have
brought with you to conduct your investigations and you are thirsty. You need water to survive. You
know from the supply list and safety sheets that two of the clear liquids are poisonous if ingested. You
need to figure out which of the three is water without tasting them. From your knowledge of
chemistry, you also know that all substances have properties that can be used to identify them. Design
an experiment to determine which container is water and thus, safe to drink. Because of the rigorous
terrain you only have access to basic lab equipment such as; a scale, thermometer, matches, graduated
cylinders, tape measure, syringe and a beaker. From the safety sheets you also know the following
about each of the liquids
Properties
Chemical formula H2O
C2H6OS
C2H6O2
Molar mass
18.01 g/mol
78.13 g/mol
62.07 g·mol−1
Appearance
Colorless liquid
Colorless liquid
Colorless liquid
Odor
None
None
None
Density
Liquid: 1 g/cm3
Liquid: 1.1004 g/cm3
Liquid: 1.1132 g/cm3
Melting point
0 °C
19 °C
−12.9 °C
Boiling point
100 °C
189 °C
197.3 °C