91Ó°ÊÓ

What is meant by an atom's valence shell?

According to Bohr, why do atoms in the same group in the periodic table have similar chemical properties?

Explain how the Bohr model of the atom accounts for the existence of atomic line spectra.

What would happen to the electron in a groundstate hydrogen atom if the atom were given \(5.1 \mathrm{eV}\) of energy?

Regarding the representative elements: (a) What does knowing the group number tell you about an element's valence electrons? (b) What does knowing the period number tell you about an element's valence electrons?

The electron in a hydrogen atom relaxes from the \(n=4\) shell to some lower- energy shell. The light emitted during the relaxation has a wavelength of \(1772.6 \mathrm{~nm}\). By calculating the energy of this light, determine the shell to which the electron relaxed. \(\left[1 \mathrm{eV}=1.602 \times 10^{-19} \mathrm{~J}\right]\)

What was the experimental evidence that supported the existence of subshells? Explain how this evidence suggested subshells.

(a) What is the numbering system used to label shells? (b) What is the lettering system used to label subshells? (c) How many subshells are there in a given shell?

Bohr solved the potassium problem by putting its last electron where? How did he justify this?

Write the electron configuration for the following elements without using the noble gas abbreviated form (use the periodic table to assist you). (a) \(\bar{B}\) (b) \(\mathrm{Sc}\) (c) \(\mathrm{Co}\) (d) Se (e) \(\mathrm{Ru}\)