General Chemistry
Unit 3 Review Sheet – Atomic Structure and the Periodic Table
The unit test will consist of approximately 40 multiple choice and 10 short answer/short essay.
Basic Atomic Structure
 know basic information about the subatomic particles (p+, n0, e-) location, charge, relative mass, significance
 be able to determine basic information about elements using just the nuclide or ion symbol and the periodic table
 distinguish between atomic number, atomic mass, mass number, and isotopes
 understand how to distinguish between isotopes, and how isotopes relate to the atomic mass of an element
 know the main contribution of each experiment you read about (cathode ray tube  electron is a particle; Thompson’s
cathode ray tube  atom has a substructure; electrons are negatively charged; Millikin’s oil drop exp.  determine
the mass of an electron; Rutherford’s gold foil exp.  positive charges and most of mass in center of atom)
 be able to describe and draw a simple model of the Bohr atom; relate the Bohr model to atomic spectra
 distinguish between the ground state and the excited state; relate this to what you did/saw in lab
 understand what is meant by “quantized energy”
Quantum Theory
 apply what you learned about quantum theory
 be able to define an orbital
 be able to figure out the # of orbitals and electrons at each sublevel (s,p,d, and f) and at each energy level (1, 2, 3…)
 describe the general arrangement of the elements in the modern periodic table with regard to electron configurations
(where are the s, p, d, and f blocks? how do periods and groups relate to the quantum numbers?)
 understand and be able to apply the Aufbau Principle, Pauli Exclusion Principle, and Hund’s Rule
 use the periodic table to determine filling order and to write electron configurations for atoms
 write electron configurations for ions, be able to predict the charge based on location on the periodic table
 understand what constitutes a stable electron configuration and how electrons gain/lose electrons to achieve stability
 determine the number of valence electrons and draw electron dot structures
The Periodic Table and Periodic Law
 understand the periodic law
 be able to locate important groups of elements on the periodic table
 know basic characteristics of important element groups on the periodic table
 be able to distinguish between metals, metalloids, and nonmetals
 understand each of the following: atomic size, metallic character, ionization energy, electronegativity
 be able to briefly describe and explain both trends (down a group and across a period) for each of the above
 be able to briefly describe and explain the relationship between atomic versus ionic size
Unit 3 Review Answers
1. 18
6. valence electrons
11.
12; 24.305 amu;
24
16.
blue; green;
yellow; red
21.
more
26.
inert/unreactive/s
table
31.
(3)
36.
any element in
group 14 or 16
2. lose
7. 2;8
12.
excited
state
17.
orbital
3. (4)
8. 41Ca or 4120Ca
13.
ground
state
18.
3;1;5
4. (1)
9. 2 gained
14.
(2)
5. kernel
10.
9;10;9;19
15.
(4)
19.
6
20.
fourth
22.
s;p
27.
noble
gases
32.
(4)
37.
[Kr]5s2
23.
28.
2
noble gases
24.
29.
K (potassium)
two;3s
25.
30.
Ga (gallium); 1
(3)
33.
(1)
38.
[Ar]4s23d10
6
4p
34.
39.
(3)
ion
41.
no two electrons
in the same atom have
the same set of 4
quantum #s
46.
semimetals/metall
oids
51.
electronegativity
42.
electrons
fill lower
energy levels
first
47.
decreases
43.
period;grou
p/ family
44.
ductile,
malleable, good
conductor, solid @
room T
49.
decreases
35.
(3)
40.
electrons fill
equal energy orbitals
with parallels spins
before doubling up
45.
brittle, poor
conductor, any state
of matter @ room T
52.
fluorine;
higher
53.
Br2, I2, N2,
Cl2, H2, O2, F2
48.
8
54.
N
50.
lower left
55.
K, C, He