Leader: Katie
Course: Chem 163
Supplemental Instruction
Instructor: Bonaccorsi
Iowa State University
Date: February 22, 2011
1. Of the following transitions in the Bohr hydrogen atom, the _______ transition results in
the emission of the highest-energy photon.
a) n = 1  n = 6
b) n = 6  n = 1
c) n = 6  n = 3
d) n = 3  n = 6
e) n = 1  n = 4
Practice Test for Exam 2
2. The n = 1 shell contains _______ p orbitals. All the other shells contain ________ p
orbitals.
a) 3,6
b) 0,3
c) 6,2
d) 3,3
e) 0,6
3. In general, as you go across a period in the periodic table from left to right:
1) the atomic radius _______; and
2) the first ionization energy _______.
a)
b)
c)
d)
decreases, increases
increases, decreases
decreases, decreases
increases, increases
4. Of the following species, __________ has the largest radius.
a) Rb+
b) Sr2+
c) Br d) Kr
e) Ar
5. In the Lewis symbol for a fluorine atom, there are _________ paired and __________
unpaired electrons.
a)
b)
c)
d)
e)
4,2
4,1
2,5
6,1
0,5
Supplemental Instruction
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6. Given the electronegativities below, which covalent single bond is most polar?
Element:
H
C
N
O
Electronegativity:
2.1
2.5
3.0
3.5
a)
b)
c)
d)
e)
C-H
N-H
O-H
O-C
O-N
7. Write the electron configurations for the following elements and ions in the standard
form and Noble Gas notation.
a) Arsenic
b) Silicon
c) Stable Silver ion
d) Stable Fluorine ion
8. Draw an energy diagram for an atom with 29 electrons. Identify the atom.
9. Draw the Lewis Symbol for the following atoms and compounds.
a) Br -
b) N
c) CO3 2-
d) CH2O
10. What is the frequency of electronmagnetic radiation that has a wavelength of 0.53m?
11. What is the wavelength (in nm) of a photon that has an energy of 4.38 x 10-18J?
12. Draw a 3s orbital, 2p orbital, and 5d orbital.
13. Describe the differences between ionic and covalent bonding.
14. Which of the following substances are ionic and which are molecular?
a) Cl2
b) HCl(g)
c) NaCl
d) Mg(ClO2) 2
e) CH3OH (methanol)
f) Fe(NO3) 3
g) Pb(C2H3O2) 2