Electrons in Atoms
For the 1987 Copyright of The Addison Wesley Textbook
2) Calculate the wavelength of a radio wave with the frequency of 93.1 x 10^6 s^-1.
3) Explain the difference between an orbit and an orbital.
4) What is the maximum number of electrons that can go into the following sublevels?
a) 2s b) 5s c) 3p d) 4d e) 4f f) 4p g) 5d h) 5f
5) Write the electron configurations for the following atoms:
a) boron b) chlorine c) zinc d) phosphorous e) manganese f) calcium
6) How does the the organization of the periodic table correspond to the scale and structure
represented by electron energy levels?
7) Picture two hydrogen atoms. The electron in the first hydrogen atom is in the n = 1 level.
The electron in the second hydrogen atom is in the n = 4 level.
a) Which atom has the ground state electron configuration?
b) Which atom can emit electromagnetic radiation?
c) In which atom is the electron in a larger orbital?
d) Which atom has a lower energy?
8) If the electromagnetic radiation used to send television signals has a frequency of
3.0 x 10^9 Hz, what is its wavelength?
9) An amateur radio operator transmits radio waves with a wavelength of 10 meters. What
is teh energy of a single photon of this radio wave?
10) Write the electron configuration for lutetium.
