Chapter 6
Name ______________________
Electronic Structure of Atoms
Concept Development Exercises
1.
What is the wavelength, , of the electromagnetic radiation possessing a frequency,
 = 4.6 x 1015 Hz?
2.
A. According to Max Planck’s proposal, energy is quantized. What does that mean?
B. Einstein proposed that light itself is quantized. What do we call those smallest
pieces of radiant energy?
C. How much energy, in joules, do the photons of red light ( = 656 nm) possess?
How many electron-volts do these photons possess?
3.
Consider the visible line spectrum of hydrogen. What does each line in the spectrum
represent?
4.
Niels Bohr developed a solar system model of the atom (1913) that explained the
emission of light from excited atoms. What is the relationship between a
permissible orbit and the level of energy possessed by a hydrogen atom in this
model?
5.
In 1925 Louis deBroglie proposed that if light has a dualistic nature, sometimes
behaving as a wave and sometimes as a particle, then perhaps matter can behave in
much the same way. He proposed that any piece of matter moving with a speed has
an associated wavelength, which can be computed as follows:
h

mv
A. Compute the wavelength of an electron moving with a speed of 5 x 106 m/s.
B. What type of EM radiation would have the same wavelength?
6.
The wave nature of electrons created the way for Heisenberg and Scrodinger to
develop the science of quantum mechanics. The solution of Schrodinger’s wave
equation led to establishment of quantum numbers that specify the energies and
probable whereabouts of electrons in atoms.
A. Define the four quantum numbers: n, l, ml, and ms.
n:
l:
ml:
ms:
7.
How many electrons can occupy an s orbital? How about a set of p, d, or f orbitals?
8.
What are the quantum numbers associated with each electron in a nitrogen atom?
9.
State the aufbau principle:
10. Distinguish between an energy level and a sublevel.
11. Write the electron configuration for atoms of
A. lithium, Li:
B. sodium, Na:
C. potassium, K:
D. rubidium, Rb:
E. cesium, Cs:
12. What do the electron configurations of the alkali metals have in common?
13. Why are the noble gases so noble?
14. Draw the shell diagrams for atoms of
A. fluorine
B. chlorine
C. bromine
15. Identify the s-blocks, p-blocks, d-blocks, and f-blocks of the periodic table.
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