Name____________________
Date
Period
Chapter 3 Matter and Change
SECTION 3.1 Matter
30 points this page
In your textbook, read about elements and atomic structure.
Use each of the terms below just once to complete the passage.
atom
electrons
element
neutrons
nucleus
protons
A(n) (1) _________________ is a substance that cannot be broken
down into simpler substances. A(n) (2) _________________is the
smallest particle of matter having all that element’s characteristics. It is
made up of smaller particles. The (3) _________________is made
up of protons and neutrons. Small particles that have mass and positive
electrical charges are (4) ______________________. Particles
that have about the same mass as protons, but that are electrically neutral
185 points
Isotope or Different Element?
In each of the following statements, you are given a pair of elements and important
information about each. Use this information to determine if the pair of elements are
isotopes or different elements. Indicate your answer in the space provided. Explain.
1. Element D has 6 protons and 7 neutrons.
Element F has 7 protons and 7 neutrons.
2. Element J has 27 protons and 32 neutrons.
Element L has 27 protons and 33 neutrons.
3. Element X has 17 protons and 18 neutrons.
Element Y has 18 protons and 17 neutrons.
are (5) _________________. Surrounding the nucleus of an atom
4. Element Q has 56 protons and 81 neutrons.
Element R has 56 protons and 87 neutrons.
are tiny particles called (6) _________________, which have little
mass, but have negative electrical charges that are exactly the same
magnitude as the positive charges of protons.
5. Element T has an atomic number of 20 and an atomic mass of 40.
Element Z has an atomic number of 20 and an atomic mass of 41.
In your textbook, read about atomic structure and isotopes.
Complete each statement.
6. Element P has an atomic number of 92 and an atomic mass of 238
Element S has 92 protons and 143 neutrons
7. The number of protons in an atom’s nucleus is the
________________.
8. When atoms of the same element have different mass numbers, they
are known as _________________of that element.
9. The spontaneous process through which unstable nuclei emit radiation
is called _________________.
10. A(n) _________________represents the area in an atom
where an electron is most likely to be found.
11. An atom that gains or loses an electron and has an electric charge is
called a(n) _________________.
12. The combined number of protons and neutrons is the
In your textbook, read about electrons in energy levels and isotopes.
(5 points)
7. How many electrons can be held in the innermost energy level of
atoms?
8. Many elements are mixtures of_________________.
9. Which electrons in an atom determine the chemical behavior of
different elements?
10. Describe the likelihood of elements with a full outermost energy level
to combine chemically with other elements.
_________________.
13. The _________________is the average of the mass numbers
of the isotopes of an element.
11. The identity of an element is defined by its number of
_________________.
Page 1
SECTION 3.2 Combining Matter
25 points this page
In your textbook, read about different types of bonds, chemical reactions,
and mixtures.
For each item write the word from section 3.2
__m_____________ 1.
_________________ 2.
_________________ 3.
In your textbook, read about chemical bonds.
Complete the table below by writing the type or types of chemical bond found
in the type of matter on the left. Use the following types of chemical bonds:
covalent, ionic, metallic.
A combination of two or more
components that retain their identity
Matter
The attraction of two atoms for a
shared pair of electrons that hold the
atoms together
14. Hydrogen gas (H2)
composed of atoms of two or more
different elements that are chemically
combined
Type of Chemical Bond Present
13. Sugar Molecule (C6H12O6)
15. Magnesium oxide (MgO)
16. Copper Metal on Capitol Dome
17. Table salt (NaCl)
18. Carbon dioxide (CO2)
_________________ 4.
A solution containing a substance that
produces hydrogen ions (H+) in water
_________________ 5.
Bond in which valence electrons are
shared by all atoms
_________________ 6.
Composed of two or more atoms held
together by covalent bonds
_________________ 7.
A homogeneous mixture
_________________ 8.
The attractive force between two ions of
opposite charge
19. H2O
In your textbook, read about chemical reactions and mixtures.
Examine equations A and B below. Then answer the questions.
(A) 2H2 + O2 → 2H2O
(B) H2CO3 → H+ + HCO3–
______ 20. Which equation represents the formation of water?
_________________ 9.
The forces that hold the elements
together in a compound
_s______s________ 10. A solid homogeneous mixture
_________________ 11. A solution characterized by the
formation of hydroxide ions (OH )
_________________ 12. The change of one or more substances
into other substances
Page 2
______ 21. Which equation represents the formation of an acid
solution?
______ 22. How many atoms of oxygen (O) are on both sides of
equation A?
______ 23. How many atoms of hydrogen (H) are on both sides of
equation A?
______ 24. How many atoms of hydrogen (H) are on both sides of
equation B?
______ 25. In which equation are carbonic acid molecules broken
apart into hydrogen ions and bicarbonate ions?
SECTION 3.3 States of Matter
25 points this page
In your textbook, read about the cycles of matter and the different states of matter.
For each statement below, determine if the statement is correct. If correct write the
word correct on the line, if not correct, use proofreading marks to make it correct.
______
1. Most solids have a crystalline structure in which the
particles are arranged in regular geometric patterns.
______
2. Hot, highly ionized, electrically conducting gas is called
plasma.
______
3. The change of state from solid to gas without an
intermediate liquid state is called evaporation.
______
4. A glass is a solid that consists of densely packed atoms
arranged at random.
______
______
5. The change from a solid to a liquid is called condensation.
______
______
7. There are only three states of matter in the universe.
In your textbook, read about changes of state.
Examine the diagram below. Then answer the questions.
6. The process of changing from a liquid to a gas is called
sublimation.
8. Matter cannot be created or destroyed.
In your text book, read about the states of matter.
Complete the table by filling in the missing information.
13. What change of state is represented by arrow A?
The States of Matter
14. What change of state is represented by arrow B?
State of
Matter
9.
Definition of State
Hot, highly ionized, electrically
conducting gases
Example
Lightning, neon sign, the Sun,
other stars
15. What change of state is represented by arrow C?
16. What change of state is represented by arrow D?
10. Liquid
17. What change of state is represented by arrow E?
11.
12.
Made of densely packed particles
arranged in a definite pattern; has
both a definite shape and volume
18. How is thermal energy involved in the processes of melting and
evaporation?
Helium
19. How is thermal energy involved in the processes of freezing and
condensation?
Page 3
Vocabulary Review
atom atomic mass
ionic bond solution
35 points this page
chemical reaction condensation electron
nucleus plasma valence electrons radioactive decay
Write in the word that best completes the statement or answers the
question. Use page 78 in your textbook. (16 points)
1. The basic building blocks of matter are _________.
Write the word from the box that best matches the definition. (11 points)
2. The nucleus of an atom is made up of
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________ and ____________,
1. The outermost electrons of an atom
2. The center of an atom
3. Hot, highly ionized, electrically conducting gas
4. The smallest particle of an element that keeps its characteristics
5. The change from a gas to a liquid
6. A homogeneous mixture
7. The change of one or more substances into other substances
8. The attractive force between two ions of opposite charge
9. A tiny particle with a negative electrical charge
10. The average of the mass numbers of an element’s isotopes
11. When unstable nuclei emit radiation spontaneously
Fill in the blank with a word that makes the statement correct. (8 points)
12. The combined number of protons and neutrons is the ____________
13. An ____________represents the area in an atom where an electron is most likely
to be found.
3. Many elements are mixtures of ____________
with a different atomic mass.
4. Chemical behavior is determined by the number of
____________located in the outermost energy level.
5. Solutions containing a substance that produces hydrogen
ions (H+) in water are ____________.
6. A combination of two or more components that retain
their identity is a(n) ____________
7. Densely packed arrangements of particles that take the
shape of their containers are____________
8. What type of bonding takes place when Na+ and Cl–
combine to form NaCl? ____________
9. Salt water is a ____________of salt and water.
14. A(n) ____________is the attraction of two atoms for a shared pair of electrons
10. Soil is an example of a heterogeneous __________.
that holds the atoms together.
11. Solutions containing a substance that produces
15. An atom that gains or loses an electron is a charged particle called an ________.
hydroxide ions (OH-) in water are ____________.
16. A(n) ____________is a substance that cannot be broken down into simpler
substances.
12. ____________ bonds form from shared electrons
between atoms.
17. A tiny particle that has mass and a positive electrical charge is a ____________
13. Tomatoes have a pH of 4. They are considered to be
18.
____________are solutions characterized by the formation of hydroxide ions
____________.
(OH).
19. The process of changing from a liquid into a gas is called ____________.
Page 4
14. Air is an example of a homogeneous __________.
15. Changes of state involve thermal __________.
Understanding Main Ideas
40 points this page
Study the diagram, which shows the formation of the compounds calcium fluoride
and nitrogen gas. Then answer the questions.
Thinking Critically
Use the information from the periodic table to complete the table below. Then
answer the questions that follow.
Element
1. Which compound is formed by ionic bonding? Explain.
Number
of Protons
Number
of Neutrons
1. Oxygen
8
2. Fluorine
10
Number
of Electrons
Atomic
Number
Atomic Mass
(rounded off)
3. Neon
2. Which compound is formed by covalent bonding? Explain.
3. How many electrons are in the fourth level of a calcium atom?
4. The isotopes neon-20 and neon-22 have the same chemical properties.
Explain why.
4. Which atom forms an ion by the loss of electrons?
5. The atomic number of chlorine is 17. Draw all the electrons for an
atom of chlorine in the following diagram. Make sure that the
electrons are in the appropriate energy levels.
Page 5
20
30 points this page
Applying Scientific Methods
Two students are presented with a problem in science class. They
need to identify specific compounds in an unknown mixture. This
“mystery” mixture could include one or more of the following
compounds: cornstarch, baking powder, powdered sugar. All of these
compounds are white and are difficult to distinguish by using sight alone.
To analyze the mixture, the students must first find ways to identify
the individual compounds. Their teacher gives them four test tubes;
distilled water; samples of cornstarch, baking powder, and powdered
sugar; dropper bottles; iodine solution; white vinegar; a shallow pan; a
candle, and matches.
The students place small amounts of cornstarch, baking powder,
powdered sugar, and a few drops of water in separate piles in the shallow
pan. They add a drop of vinegar to each sample and record what happens
in a data table. Only the baking soda shows any change. It begins to fizz
as a result of a gas being given off.
Then the students place small amounts of each compound on the pan a
second time. This time, they add a drop of iodine to each sample and
record their results. Only the sample of cornstarch turns blue.
Finally, the students place a small amount of each compound in three
separate test tubes. They use a lit candle to gently heat the bottom of each
test tube. Only the sugar shows any signs of melting. The other
compounds are unaffected.
After finding the
three unique
ways described
above of water
testing
Distilled
for each
compound, the
Cornstarch
students then
repeat all three
Sugar
tests on the
mystery mixture.
The following
Baking
soda
data table shows
their
results.
Mystery
mixture
Answer the
questions that
follow.Material
Tested
Page 6
Addition of
Vinegar
Addition of
Iodine
Heated with
Candle
No change
No change
Boiled
No change
Turns blue
No change
No change
No change
Melts
Fizzing takes
place
Fizzing takes
place
No change
No change
Turns blue
No change
1. Did the students conduct quantitative (numerical) or qualitative
(descriptive) research? Explain your answer, using examples from the
students’ investigation.
2. Was a control used in this experiment? Explain your answer.
3. What safety rules should the students have followed when heating the
compounds and mixture?
4. Which compound or compounds were present in the mystery
mixture? Explain how you arrived at your conclusion.
5. How would you determine if all three compounds were absent from
the sample?
6. Why would tasting the mystery mixture NOT be an appropriate way
of identifying its components?