Physical Science Semester 1 Review
Name:____________________ Period:_____
Chapter 1: Science Skills (answer questions 1-22 on page 29 for extra practice.)
1. What are the branches of natural science?
2. What are the typical steps in as scientific method?
3. How does a scientific law differ from a scientific theory?
4. What are three types of variables in a controlled experiment?
5. Why do scientists use scientific notation?
6. What system of units do scientists use for measurements?
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7. List the SI units for mass, length, and temperature.
8. What is the equation for converting Celsius into Kelvin? (Hint: K = ?)
9. List four different ways scientists organize data.
10. What does a given point represent on a line graph?
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Chapter 2: Properties of Matter (answer questions 1-22 on page 63 for extra practice.)
1. What is the definition of a pure substance?
2. Give three examples of elements.
3. How is a compound different from an element?
4. What are the two types of mixtures? Give an example of each.
5. Give an example of a colloid.
6. Give three examples of physical properties.
7. What are two ways of separating mixtures?
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8. Give an example of a physical change that is reversible and a physical change that is irreversible.
9. Give two examples of chemical properties.
10. List the three ways of recognizing chemical changes.
11. How do chemical changes differ from physical changes?
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Chapter 3: States of Matter (answer questions 1-24 on page 95 for extra practice.)
1. What are the three states of matter defined in terms of shape and volume?
2. What is pressure?
3. What three factors affect gas pressure?
4. How does increasing the temperature affect the pressure of a contained gas?
5. What is the equation for Charles’s Law?
6. What happens to the pressure of a gas if its volume is reduced?
7. What is the equation for Boyle’s Law?
8. How does increasing the number of particles of a contained gas affect its pressure?
9. What is the equation for the combined gas law?
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10. What are the six common phase changes?
11. Which three phase changes are exothermic?
12. Which three phase changes are endothermic?
13. What is the difference between evaporation and boiling?
14. What happens to the temperature of a substance during a phase change?
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Chapter 4: Atomic Structure (answer questions 1-23 on page 121 for extra practice.)
1. What was Dalton’s Atomic Theory?
2. What evidence did J.J. Thompson provide about the structure of an atom?
3. What did Rutherford discover about the structure of an atom?
4. What are the three subatomic particles? Give the charge and relative mass of each.
5. Where are each of the subatomic particles located in an atom?
6. What does atomic number tell you about an element?
7. How is mass number calculated?
8. How are the isotopes of an element different from one another?
9. What do protons and neutrons have in common? How are they different?
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10. How can atoms be neutral if they contain charged particles?
11. What is the difference between atoms of oxygen-16 and oxygen-17?
12. Explain why it isn’t possible for an atom to have a mass number of 10 and an atomic number of 12.
13. What property to protons and electrons have that neutrons do not?
14. When is an electron likely to move from one energy level to another?
15. What model do scientists use to describe how electrons move around the nucleus?
16. What does an electron cloud represent?
17. What does it mean if an atom is in its ground state?
18. What happens when an electron moves from an excited state back down to the ground state?
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Chapter 5: The Periodic Table (answer questions 1-23 on page 153 for extra practice.)
1. Who developed the first periodic table?
2. How did Mendeleev arrange his periodic table?
3. How did the discovery of new elements such as gallium demonstrate the usefulness of Mendeleev’s
table?
4. Why did Mendeleev leave spaces in his table?
5. What is the periodic law?
6. Where are periods located in the periodic table? Where are groups located?
7. How the is the atomic mass of an element calculated?
8. What are the three classes of elements?
9. What are three properties of metals?
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10. Where are metals located on the periodic table?
11. What are two properties of nonmetals?
12. Where are nonmetals located on the periodic table?
13. Where are metalloids located on the periodic table?
14. What is a valence electron?
15. Why do elements in the same group have similar properties?
16. What is the name of the Group 1A elements? How many valence electrons does each one have?
17. What is the name of the Group 2A elements? How many valence electrons does each one have?
18. What is the name of the Group 7A elements? How many valence electrons does each one have?
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19. What is the name of the Group 8A elements? How many valence electrons does each one (except
helium) have?
20. Which group of elements is the least reactive?
21. Why is hydrogen located in a group with reactive metals?
22. What happens to the reactivity of nonmetals within a group from the top of the group to the bottom?
23. What happens to the reactivity of metals within a group from the top of the group to the bottom?
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Chapter 6: Chemical Bonds (answer questions 1-25 on page 187 for extra practice.)
1. When is an atom stable?
2. What does an electron dot diagram show?
3. What happens to electrons in an ionic bond?
4. Ionic bonds form between which two types of elements (metals, nonmetals, metalloids)?
5. What are three properties of ionic compounds?
6. What happens to electrons in a covalent bond?
7. Covalent bonds form between two of what type of element (metals, nonmetals, metalloids)?
8. What is a polar covalent bond?
9. What are the seven diatomic elements?
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10. Which type of compounds have prefixes in their names?
11. When are Roman numerals used in naming compounds?
12. What is a polyatomic ion?
13. How is it possible for two different ionic compounds to contain the same elements?
14. How many potassium ions are needed to bond with a phosphate ion?
15. Name the following ionic compounds:
a. LiCl
d. PbSO4
b. BaO
c. Na3N
16. Name the molecular compounds with these formulas:
a. P2O5
b. CO
17. What is the formula for the ionic compound formed from potassium and sulfur?
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Chapter 7: Chemical Reactions (answer questions 1, 2, 4, 5, 6, 8, 11, 12, and 14 on page 223 for extra
practice.)
1. What is the law of conservation of mass?
2. Why does a chemical equation need to be balanced?
3. Balance the following equation and identify the type(s) of reaction: Na + Cl2  NaCl
4. Write a balanced chemical equation for the formation of magnesium oxide, MgO, from magnesium
(Mg) and oxygen gas (O2), and identify the type(s) of reaction.
5. What are the five types of chemical reactions? Include the general equation with each.
6. What occurs in an oxidation-reduction reaction?
7. What doe LEO stand for? What does GER stand for?
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8. Balance each of the following reactions and identify these reactions as synthesis, decomposition, single
replacement, double replacement, or combustion.
a. Pb(NO3)2 + HCl  PbCl2 + HNO3
b. C2H6 + O2  CO2 + H2O
c. Ca + HCl  CaCl2 + H2
d. SO2 + O2  SO3
9. Explain the difference between a single-replacement reaction and a double-replacement reaction.
10. What occurs in an endothermic reaction? How would it feel if you touched it?
11. What occurs in an exothermic reaction? How would it feel if you touched it?
12. What is the law of conservation of energy?
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Chapter 10: Nuclear Chemistry (answer questions 1-5, 8-21 on page 319 for extra practice.)
1. What happens during nuclear decay?
2. What are three types of nuclear radiation? Give the symbol for each.
3. How does nuclear radiation affect atoms?
4. What devices can detect nuclear radiation?
5. Write a balanced nuclear equation for the alpha decay of throrium-232.
6. Write a balanced nuclear equation for the beta decay of carbon-14.
7. Determine the product of alpha decay for americium-241.
8. Determine the product of beta decay for strontium-90.
9. What is background radiation? List some of its sources.
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10. What is the effect of beta decay on the composition of a nucleus?
11. What is half-life?
12. How can scientists determine the age of an object that contains carbon-14?
13. If a radioactive sample has decayed until only 1/8th of the original sample remains unchanged, how
many half-lives have elapsed?
14. What type of nuclear radiation is emitted when carbon-14 decays?
15. What is fission?
16. What is fusion?
17. What is a chain reaction?
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18. Under what conditions does the strong nuclear force overcome the repulsive effect of electric forces in
the nucleus?
19. What property of fission makes it a useful reaction?
20. What particles are affected by strong nuclear forces?
21. What must happen in order for a nuclear chain reaction to occur?
22. How do products of a fusion reaction differ from the products of a fission reaction?
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