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Chapter 1- Metric System, Unit Conversion, and the Scientific Method
1. Vocabulary terms:
independent variable
dependent variable
control variable
length
mass
volume
hypothesis
scientific method
2. The metric system is easy to use because it is based on factors of what?
3. Complete the following chart. Know the prefix, symbol, and meaning of each.
deka
Prefix
h
Symbol
Meaning
deci
m, L, g
c
1,000
0.001
4. Be able to convert units of measurement.
Example: (a) 1,000 kg = ______ g
(b) 1865cm = _______m
(c) 7452.87 g = _________ kg
(d) 24 L = __________ mL
5. How do you convert Celsius to Fahrenheit and Fahrenheit to Celsius.
Examples: (a) 16° C = _______ ° F
(b) 48 ° F = _______ ° C
6. What is the formula for calculating the volume of a solid?
(a) What is the volume of a box that has a length of 5 m, width of 2 m and a height of 5 m?
(b) What is the volume of a block that measures 12 cm by 10 cm by 5 cm?
(c) The unit for volume is the length of all the sides to the (2nd or 3rd) power.
7. What is the formula for calculating the density of an object? Will the following objects sink or
float?
(a) What is the density of an object with a volume of 13 mL and a mass of 9 grams?
(b) What is the density of an object with a mass of 20 g and a volume of 18 cm³?
8. What are the 7 steps to the scientific method? The last step is to ________________.
Chapters 15 and Chapter 22- Classification of Matter
1. Be sure you know the definitions of the following terms:
Solute
Nonelectrolyte
Element
Solvent
Compound
Polar
Heterogenous Mixture
Nonpolar
Homogenous Mixture
Saturated Solution
Solution
Unsaturated Solution
Colloid
Supersaturated Solution
Tyndall Effect
Ion
Electrolyte
Alloy
Physical Change
Physical Property
Chemical Change
Chemical Property
Suspension
2. List names and symbols for three elements found in group 12 of the periodic table.
3. What is the difference between heterogenous and homogenous mixtures? Name a few examples
of each.
4. List 2 examples of colloids and explain why colloids produce the “Tyndall Effect”.
5. List 1 example of a suspension. Will suspensions produce the “Tyndall Effect”?
6. Explain the difference between a physical property and a chemical property.
7. Identify the solvent and the solute in 3 different types of solutions.
8. List one example of a solid, liquid, and gaseous solution.
9. What is the difference between a saturated solution and an unsaturated solution in
terms of the ratio of solvent vs. solute?
10. What two things must you do in order to dissolve a gas in a liquid?
11. List three examples of electrolytes and three examples of non electrolytes.
12. List 6 physical and 6 chemical changes and be able to differentiate between the two.
13. What 3 things can you do in order for solid solutes to dissolve more quickly in a
solvent?
14. Water is the universal ________________. (solute/solvent)
Chapters 17 and 19- Atomic Structure and Periodic Table
1. Be sure you know the definitions of the following terms:
Atom
Proton
Isotope
Atomic number
Neutron
metal
Atomic mass
Electron
nonmetal
Period
Quark
metalloid
Group
Periodic Table
2. What are the three parts of the atom? Identify the location of each part, and the charge
of each subatomic particle.
3. Describe the difference between periods and groups. (Which one tells you outer-level
electrons and which tells you the number of energy levels?)
4. Name three elements in each group. State which group they are found in, the period in
which they are located, and how many protons, neutrons, and electrons are found in each
element.
5. Know the locations and label the names for the following groups: 1, 2, 3-12, 13, 14,
15, 16, 17, 18
What makes the elements in each group similar?
6. How many quarks have been identified by scientists?
7. Classify Nitrogen, Boron, and Chlorine as a metal, metalloid, or nonmetal. How many
outer electrons does each have?
8. Classify 2 solid, 2 liquid, 2 gaseous, and 2 synthetic elements on the periodic table.
9. Electron dot diagrams show how many _________________ electrons an element has.
10. Each inner energy level of an atom has a maximum number of ____________ it can hold.
11. Dot diagrams are used to represent ____________ _______________.
12. Neutrons carry a ___________________ charge.
13. A chemical symbol represents the ________________ of an element.
14. Horizontal rows of the periodic table are called _______________.
15. Atoms of the same element with different numbers of neutrons are called ____________.
16. A certain atom has 26 protons, 26 electrons, and 30 neutrons. Its mass number is ________.
17. A certain atom has an atomic number of 20 and a mass number of 41. How many protons
does it have?
18. How many neutrons would an element with an atomic number of 17 and an atomic mass of
35 have?
Chapter 20 and 21 Naming Compounds and Chemical Reactions
1. What is the formula for the binary compound formed between aluminum and oxygen?
2. Three transitional metals in Group 12 of the periodic table are _______________.
3. Given the compound Li3N , what is the oxidation number for nitrogen?
4. A combustion reaction must have________________ included in the reactants.
5. The elements that make up a compound and the exact number of atoms of each element in a
unit of the compound can be shown in a __________________.
6. A chemical bond that occurs when atoms share electrons is a(n) ________________ bond.
7. What is the correct name of the following chemical formula: N2O4?
8. How many electrons are needed in the outer energy levels of most atoms for the atom to be
chemically stable?
9. Balance the following equations and name the type of reaction:
Mg + N2  Mg3N2
CaCO3 → CaO +
CO2
10. How many Chlorine atoms are present in the compound Ca(ClO3)2?
11. How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2?
12. What is the name of the compound with the formula NaCl?
13. Why do the noble gases NOT form compounds readily?
14. In a chemical formula, the number of each type of atom in the compound is shown by
numbers called _______________.
15. What is the correct formula for magnesium oxide?
16. A(n) _________________ chemical equation has the same number of atoms of each element
on each side of the equation.
17. An element with an atomic number of 35 and an atmic mass of 80 would have _____protons,
______electrons, and _______neutrons.
18. What type of reaction is shown in the following chemical equation: 2H2O → 2H2 + O2?
19. Each substance to the right of the arrow in a chemical equation is a ________________.
20. An atom that has a +2 oxidation number has ______________________
21. The __________ _____________ tells you how many electrons an atom must gain, lose, or
share to become stable.
22. Numbers that precede symbols and formulas in a chemical equation are ______________.
23. A chemical reaction in which two or more substances combine to form another substance is
called a ___________________.
24. According to the law of conservation of mass, if two atoms of hydrogen are on the reactant
side, how many atoms of hydrogen must be part of the product?
Chapter 18 Nuclear Power and Radiation
1. The most penetrating type of radiation is the _________________.
2. The stability of an isotope nucleus depends on the ______________.
3. The three types of nuclear radiation in increasing order of penetrating power are:
4. Radioactive tracers are useful in ___________ _____________.
5. Both fusion and fission reactions produce __________________.
6. One type of radioactive device that indicates the intensity of radiation with a clicking
sound that increases in frequency as more radiation is present is a(n)
_______________________.
7. When the strong force is not sufficient to hold unstable nuclei together permanently,
the nucleus starts to __________________.
8. Which element is most likely to be produced during a nuclear fusion reaction in the
Sun?
9. The majority of the mass of an atom is located in the __________________.
10. Unranium-238 has a half-life of 4.5 billion years. If you have a 50 gram sample of uranium238, how much is left after 9 billion years?