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Chapter 4 Column Notes: Arrangement of Electrons in Atoms: Answer all parts of each question. Use
the text, figures and captions as resources.
Section 4-1: The Development of a new Atomic Model
1. How was the development of the Atomic
Model advanced by the study of light?
2. What is electromagnetic radiation? What
is the electromagnetic spectrum?
3. Looking at Figure 1, what are the
different types of electromagnetic
radiation?
4. When there is no air (a vacuum), what is
the speed of gamma rays? Of X-rays? Of
ultraviolet light? Of visible light? What is
the speed of all electromagnetic
radiation?
5. What is a wavelength? What is the unit
for wavelengths?
6. What is frequency? What is the unit of
frequency? What are the two ways of
expressing this unit?
7. What is the mathematical relationship
between wave frequency and
wavelength? What does the symbol c
stand for? What is its value for
electromagnetic radiation?
8. What does the word emission mean with
respect to the photoelectric effect?
9. What does minimum frequency mean
with respect to the photoelectric effect?
10. What did Max Planck suggest to explain
the photoelectric effect? What new term
did he propose to link energy to an
atom?
11. Explain Planck’s equation relating energy
and frequency, including what each
variable represents. (Nobel Prize)
12. According to Planck’s equation, which
electromagnetic radiation (Figure 1) has
the most energy? The least?
13. What term did Einstein use to describe a
quantum of energy? How did he use this
term to explain the photoelectric effect?
(Nobel Prize)
14. What is the ground state of an atom?
Excited state? Describe what happens
when an atom goes from the excited to
the ground state. What can you see?
15.
What is a line-emission spectrum?
A continuous spectrum?
Relate Niels Bohr’s model of the atom
(Figure 8) to the colored lines of the
hydrogen emission spectrum (Figure 5)
(Nobel Prize). What did he call the paths of
electrons around the nucleus?
16. What are the Lyman, Balmer and Paschen
spectral series?
17. What does the word emission mean with
respect to Bohr’s model?
18. What were the flaws of Bohr’s model?
Section 4-2 The quantum model of the atom
19. How did De Broglie relate the electron to
waves? How did this extend Bohr’s model
of the electron? (Nobel Prize)
20. Why did Heisenberg say it is difficult to
locate an electron? (Nobel Prize)
21. How did Schrodinger’s equation support
the concept of quantization of electron
energies? (Nobel Prize)
22. What is the modern atomic theory
called? What is its main concept?
23. How does Figure 11 portray an atomic
orbital?
24. Compare and contrast the orbital model
to Bohr’s orbit model of electron
location?
25. What is the purpose of quantum
numbers?
26. Name the 4 quantum numbers and the
characteristic they describe.
27. What do the n numbers represent?
Which n number represents electrons
closest to the nucleus? Electrons with
highest energy?
28. What do each of these symbols
represent: s, p, d, f
Section 4-3 Electron Configurations
29. Why do electrons tend to be arranged in
the ground state electron configuration?
30. What rule does the Pauli exclusion
principle describe? How is the spin
quantum number critical to this rule?
31. What does Hund’s rule say about electron
configuration? Why is this rule necessary?
32. Write the ground state electron
configuration for magnesium using the
three types of notation. (indicate which is
which)
33. What is the ‘highest occupied energy
level’? What are ‘inner shell electrons’?
34. How does electron configuration tell you
which is the highest occupied energy
level?
35. What is the noble-gas configuration?
36. For the element iron:
a.
b.
c.
d.
Write the complete electron configuration
How many electron-containing orbitals does
iron have?
How many of these orbitals are completely
filled?
How many unpaired electrons are in the iron
atom?
37. What do all elements in each group have
in common with respect to electron
configuration?