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Pre-AP Chemistry Semester 1 Review Guide
2012-13
Extra credit on exam (10 points) will be given for handwriting or hand printing (legibly) the answers to this
review guide on a separate piece of paper in complete sentences. You must show work on math related
questions. You must number the responses. Example for #1: incorrect response, “it has mass and takes up
space”; correct response, ”matter is anything that has mass and takes up space”. Responses are due by
Tuesday, January 15 at the beginning of class for full credit.
M
V
c  
D
E  h
c  3x10
Useful equations and constants:
h  6.63x10 34 J  s
8
m
s
Some equations will be provided on the exam. Bring a calculator. There will be no sharing of calculators during
the exam. You may need a calculator for about 6-8 questions (multiple choice and problem)
Tentative Format. You will be notified of any changes as we get closer.
Multiple choice questions:
124
1 point each
Short Answer: (polyatomic ions)
15
1 point each
Problems:
3
2 points each
Total points: 145
(20% of semester grade)
Chapter 1
Matter and Change (21 questions)
1.
What is matter?
2.
What are physical properties?
3.
What are chemical properties?
4.
Vertical columns in the periodic table are called what? What can you say about elements in a vertical
column?
5.
Horizontal rows in the periodic table are called:
6.
Which group of elements is very unreactive?
7.
What is the difference between an intensive and extensive physical property?
8.
What is an atom?
9.
Describe the four states of matter
10.
Describe how particles behave in solids, liquids, and gases.
11.
How can you tell if a physical or chemical change has occurred?
12.
Which of the following can be separated by physical means: elements, compounds, mixtures, or pure
substances?
13.
What is mass?
14.
What is a compound?
15.
What is a pure substance? What are the two kinds of pure substances?
16.
What is a mixture?
17.
The distinct parts of a mixture are called what?
18.
What is the difference between a homogeneous and heterogeneous mixture?
19.
What is another name for a homogeneous mixture?
20.
What is the difference between a reactant and a product?
21.
What happens to energy when a substance changes state?
22.
How are metals and nonmetals different?
Pre-AP Chemistry Semester Review Guide 2012-13
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Chapter 2
Measurements and Calculations (23)
23.
What is a unit? Give examples.
24.
The SI standard units for length and mass are what?
25.
What is a model and how can models be represented?
26.
The unit m3 measures:
length, mass, volume, or density?
27.
What are the symbols for the metric units used to measure mass and length?
28.
How are the unit prefixes g, mg, and kg related?
29.
What are precision and accuracy and what is the difference between precision and accuracy?
30.
When determining the number of significant digits in a measurement, when are zeroes significant?
31.
Describe the rules of significant figures
32.
What is the difference between a quantitative and qualitative value?
33.
To determine density, the quantities that must be measured are what?
34.
What type of property is density?
35.
What is the volume of a substance that has a density of 40 g/cm3 and a mass of 80 g?
36.
What are the steps in the scientific method?
37.
How many minutes are in a day?
38.
How can you tell the difference between variables that are directly proportional and inversely proportional?
What do their graphs look like?
Chapter 3
Atoms: The Building Blocks of Matter (25)
39.
Briefly describe Dalton’s atomic theory.
40.
Why are atoms electrically neutral?
41.
What are the three fundamental particles of an atom called and what are their charges? What are their
relative masses? Which atom’s average atomic mass is used for comparison to all other atoms?
42.
What is the law of conservation of mass?
43.
Explain the results of Thompson’s experiments with cathode ray tubes.
44.
What is the law of definite proportions?
45.
What are isotopes?
46.
What determines an atom’s atomic number?
47.
What determines an atom’s atomic mass?
48.
What is molar mass? How many grams are in 5.2 moles of copper?
49.
What is a mole? How many moles are 54 g of Al?
50.
What is Avagadro’s number? How many atoms are in 8 g of oxygen?
51.
What is the law of multiple proportions?
52.
What did Rutherford’s experiment show?
53.
What is the most common isotope of hydrogen? What is it called?
54.
If 8 g of element A combine with 20 g of element B, then 16 g of element A combine with ____g of
element B. Does this illustrate the law of definite or multiple proportions?
Chapter 4 (32)
55.
Visible light, X rays, infrared radiation, and radio waves all have the same ____________________.
56.
Electromagnetic radiation behaves like a ______________________ as it travels through space and a
____________________ when it is absorbed by solid matter.
57.
Describe the properties of electromagnetic radiation (speed, frequency, and wavelength).
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58.
64.
65.
66.
According to the particle model of light, certain kinds of light cannot eject electrons from metals because
they don’t have enough _____________________.
The emission of electrons from metals that have absorbed photons is called what?
A quantum of electromagnetic energy is called a(n) __________________________
The energy of a photon, or quantum, is related to its _________________________
A bright-line spectrum of an atom is caused by the energy released when electrons [jump to / fall from] a
higher energy level.
For an electron in an atom to change from the ground state to an excited state, what must happen to the
electron?
If electrons in an atom have the lowest possible energies, the atom is in the ______________________
Bohr's model of the atom works best in explaining the line spectra of what element?
How many quantum numbers are needed to describe the energy state of an electron in an atom?
67.
Name the quantum numbers and what they represent.
68.
Louis de Broglie's research suggested that electrons should be considered as _________________ confined
to the space around an atomic nucleus.
Which model of the atom explains the orbitals of electrons as waves?
A 3-dimensional region outside the nucleus where an electron can most probably be found is called an
____________________
The size and shape of an electron cloud are most closely related to the electron's __________________
With the quantum model of the atom, scientists have come to believe that determining an electron's exact
location around the nucleus is _______________________________.
An electron for which n = 4 has more ____________ than an electron for which n = 2.
What is the main difference between a 1s orbital and a 2s orbital?
What are the letter designations for the first four sublevels with the number of orbitals and number of
electrons that can be accommodated in each sublevel?
How many possible orbital shapes can the 1st, 2nd, 3rd, and 4th energy level have?
A single orbital in any energy level or sublevel can hold how many electrons?
What is the Aufbau principle, Hund’s rule, and the Pauli exclusion principle?
Write the electron configuration and orbital diagram for oxygen. Write the shorthand notation.
What is an octet? Which sublevels are filled with electrons when an element is said to have an octet of
electrons in its highest energy level?
Calculate the frequency of a wave with a wavelength of 3.00 cm
Calculate the mass of 5.00 moles of NaCl
59.
60.
61.
62.
63.
69.
70.
71.
72.
73.
74.
75.
76.
77.
78.
79.
80.
81.
82.
Chapter 5 (23)
83.
Identify the alkali metals, alkali earth metals, halogens, noble gases, actinides, and lanthanides on the
periodic table. Which one of these is radioactive?
84.
How are elements ordered on the periodic table?
85.
How did Mendeleev and Mosley differ in the ordering of elements on the P.T.?
86.
Describe periodic trend of atomic radius size.
87.
The periodic law allows some properties of elements to be predicted based on what?
88.
What is electronegativity?
89.
How many elements are in a period in which only the s and p orbitals are filled?
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90.
91.
92.
93.
94.
95.
96.
Where are metals and nonmetals located on the P.T.?
Why is hydrogen placed separately from other elements on the P.T.?
In nature, alkali metals occur as ____________________
Which group of nonmetals is the most reactive?
The first electrons to be removed when a d-block element forms ions are from which block?
What is the difference between anions and cations?
What are the electrons involved in chemical bonding called?
Know your polyatomic ions (11)
Extra credit on exam given as follows:
8-10 points
Handwritten on separate paper, state the question, answer in complete sentences, show calculations
where applicable. Answers numbered. All questions answered legibly.
1-7 points
Handwritten on separate paper, question not stated, no complete sentences, calculations not shown,
but questions answered. Depending on quality and number of questions answered. (teacher
determines quality)
0 points.
Answers written on this sheet and any typed responses.
DO NOT TYPE, DO NOT ANSWER ON THIS SHEET.
Pre-AP Chemistry Semester Review Guide 2012-13
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