1. Place the following types of electromagnetic radiation in order of increasing energy and label
them on the spectrum below
a. infrared
d. orange light
b. x-rays
e. ultraviolet
c. blue light
f. radio waves
2. One type of electromagnetic radiation has a frequency of 200 MHz, another has a wavelength
of 225 nm, and another type has photons with energy equal to 4.20 x 10-19 J. Identify each type
of radiation and put them in order of increasing energy and frequency.
3. The ionization energy of gold is 890.1 kJ/mol (the amount of energy needed to remove a mole
of electrons from atoms on the surface of gold metal). What is the maximum wavelength of light
that can remove an electron from a gold atom?
4. It takes 208.4 kJ to remove 1 mole of electrons from atoms on the surface of rubidium metal.
If rubidium is irradiated with 254 nm light, what is the maximum kinetic energy the released
electrons can have?
5. Calculate the deBroglie wavelength for:
a. an electron with a velocity 20% the speed of light (me = 9.1 x 10-31 kg)
b. a 1.00 kg ball thrown at a speed of 10 m/s
6. Calculate the wavelength of light associated with the following transitions in a hydrogen atom:
(state whether it is an absorption or emission)
a. n = 2 → n = 3
b. n = 4
→
n=1
1. Fill in the table:
Quantum #
Name
n
Meaning
Possible values
l
ml
ms
2. Which of the following are incorrect? Why?
2s
3f 7s
8p
1p
5p 2d
4f
2p
1d
3. Sketch the orbitals 1s, 2s, 2px, 2py, and 2pz . Give the quantum numbers for each orbital and
identify any nodes.
4. How many orbitals can have the following designation? What about electrons?
a. n = 2
b. n=3, l = 2
c. n = 4, l = 2, ml = -1
d. 6d
e. 4fxyz
5. Write electron configurations for:
a. O
b. Ne
c. Ca
d. Zn
e. Br
f. Cr
g. Cu
6. How many unpaired electrons are present in each of the following?
a. P
b. Mg2+
c. Fe
d. S2e. Al
7. Which of the following correspond to an excited state? If so,write the correct ground state
configuration.
a. 1s22s22p53s1
b. [Ne]3s23p4
c. [Ar]4s13d5
d.[Kr]5s24d85p1
e. [Ar]4s23d104p3
8. In a hydrogen atom, all the orbitals in a given energy level are degenerate. Describe what this
means.
9. Calculate the energy (in kJ/mol) required to remove the electron in the ground state for each:
a. H
b. Li2+
1. Use the Heisenberg uncertainty principle to calculate:
a. the uncertainty in velocity (∆v) of an electron whose position is known to within 0.2 nm.
b. the uncertainty in position of a 0.15 kg baseball whose velocity is known to within 0.3 m/s.
2. Define:
a. ψ
b. ψ2
3. Draw ψ and ψ2 for the first three energy levels for an electron in a one-dimensional box of
length “L”. Indicate any nodes.
4. Assume you have an electron in a one-dimensional box of length 4.00 x 10-11 m. Calculate the
wavelength of light needed to excite the electron from the ground state to energy level n=5.
(me = 9.11 x 10-31 kg)
5. Which has a higher ground state energy, an electron in a box of length 10-6 m or in a box of
length 10-10 m?
6. Consider an electron in a one-dimensional box. It is known that photons of wavelength 8080
nm are capable of exciting the electron from the n=2 to the n=3 energy level. What is the length
of the box?
1. Put the following in order of increasing size:
a. P, N, As
b. Rb, Na, Al
c. Ca2+, S2-, Cl-, Ar
2. Put the following in order of increasing ionization energy:
a. O, S, Se
b. Ni, P, F
c. O, O-, O23. Put the following in order of decreasing (least to most exothermic) electron affinity:
a. C, O, Li
b. C, Si, In
c. Cl, Br, I
4. Put the following in order of increasing electronegativity:
a. B, Al, Mg
b. As, Cl, S
c. C, F, Cl
5. Put the following bonds in order of increasing polarity:
a. C-N, C-O, C-C
b. H-F, H-Cl, H-Br
c. Al-Cl, Si-Cl, P-Cl
Rules for Lewis Structures:
1. find the total number of valence electrons in the molecule
2. form single bonds between atoms (two electrons per bond)
3. arrange the remaining electrons to satisfy the duet rule for hydrogen and the octet rule for
second-row elements
6. Draw Lewis structures for the following. Show resonance where applicable.
a. H2O
c. HCN (carbon is central atom)
b. NCl3
d. CO2
e. SO2
f. CO32-
g. H2CO (carbon is central atom)
h. NH4+
i. NO3-
j. SO3
For the following, draw two Lewis structures, one which satisfies the octet rule and one which
minimizes formal charge.
a. POCl3
b. SO3
Draw Lewis structures for the following molecules, which are exceptions to the octet rule.
a. PCl5
b. BeF2
c. XeI4
d. BBr3