CHEM 5013 - Applied Chemical Principles
Suggested problems for Quiz #8 on Thursday November 14th
1. Explain in your own words the processes of absorption and emission of light by an
atom. That is, what is happening at the atomic level?
Absorption – Electron absorbs energy from an incident photon and this pushes the
electrons to excited (higher energy) states
Emission – The electrons return to ground state (lowest energy level) and while doing
so, emit an amount of energy equal to the amount absorbed. This energy is seen as
light
2. What is the wavelength of microwave radiation whose frequency is 1.315x10 9 Hz?
Report your answer in nanometers.
λ = c/v = 3 x 108 m/s
1.315 x 109 /s
= 0.228 m x
1 nm
1 x 10-9 m
= 2.28 x 108 nm
3. What is the energy (in Joules) of a photon corresponding to the microwave radiation
in question #2?
E = hv = (6.63 x 10-34 J▪s) ( 1.315 x 109 Hz) =
8.72 x 10-25 J
4. Mercury vapor lamps are increasingly being phased out in the United States. One wavelength
of emission provided by a mercury vapor lamp is known as the G-Line (the violet colored line)
and has a wavelength of 435.8 nm. Calculate the energy in a single photon of light emitted
at the G-line of a mercury vapor lamp.
435.8 nm x (1x10-9m/1 nm) = 4.358 x 10-7 m
E = h c / λ = (6.63 x 10-34 J▪s) (3 x 108 m/s)
=
4.56 x 10-19 J
4.358 x 10-7 m
5. Provide the following:
a. The full ground state electron configuration for an atom of Tin
1s22s22p63s23p64s23d104p65s24d105p2 (50 total electrons)
b. The orbital diagram for an atom of Iron
1s2 2s2
2p6
3s2
3p6
4s2
3d10
6. Give two different possible orbital diagrams for the 1s22s22p4 configuration of an atom
of oxygen, one of which corresponds to the ground state.
1. GROUND STATE ORBITAL DIAGRAM
2. EXCITED STATE ORBITAL DIAGRAM
ANYTHING ELSE
1s2
2s2
2p4
7. Which of the following possible orbital diagrams are allowed and which are not
according to the Pauli Exclusion Principle? For those that are not allowed, explain
why they are not allowed. (1 pt each)
a.
b.
1s
2s
2p
1s
ALLOWED – Just not ground state
c.
2s
2p
NOT ALLOWED – only allowed to
have 2 electrons in 2s orbital
d.
1s
2s
2p
NOT ALLOWED – same spin on 2
Electrons in 1s orbital
1s
2s
2p
ALLOWED – Just not ground state
8. Which of the following electron configurations is possible? For those that are not
possible, explain why they are not possible.
a. 1s22s12p6
b. 1s22s22p63s23p63d7
Possible but not Ground State
c. 1s22s22p8
Not possible – can only have 6
electrons in a p subshell
Possible
d. 1s22s32p63s13d9
Not possible – can only have 2
electrons in s subshell