91Ó°ÊÓ

In the Bohr model of the atom, are the electrons in shells closer to the nucleus higher or lower in energy than electrons in shells farther from the nucleus? Explain.

What is the total number of \(p\) -subshell electrons for each of the following atoms: \(\mathrm{P}, \mathrm{Mg}\), Se, \(\mathrm{Zn} ?\)

Rank visible light, gamma rays, X-rays, radio/ television waves, infrared radiation, and ultraviolet light in order of (a) increasing wavelength and (b) increasing energy.

Draw a simple Bohr model (no subshells) for an oxygen atom. How many electrons are in the valence shell? How many more electrons can be put into the valence shell?

Explain the major difference between the orbits in the Bohr model of the atom and the orbitals in the quantum mechanical model of the atom.

The second ionization energy of an atom is the minimum energy required to remove an electron from the \(+1\) cation of the atom, and it is always larger than the first ionization energy. Why is this so? (Hint: Think of atomic electrons as clouds, and each electron must "look" through every other electron cloud in the atom to "see" (feel) the nucleus.)

Predict the formula for the compound aluminum nitride made from the elements aluminum and nitrogen, and explain how you made your prediction.

True or false: Photons of green light have a higher frequency than photons of blue light. True or false: Photons of blue light have a longer wavelength than photons of orange light.

Of the following atoms, which has the largest first ionization energy? (a) \(\mathrm{Br}\) (b) \(\overline{\mathrm{O}}\) (c) \(\mathrm{C}\) (d) \(\mathrm{P}\) (e) I

Of the following transitions in the Bohr hydrogen atom, which transition results in the emission of photons with the shortest wavelength? (a) \(n=1 \rightarrow n=6\) (b) \(n=4 \rightarrow n=1\) (c) \(n=9 \rightarrow n=5\) (d) \(n=3 \rightarrow n=6\) (e) \(n=5 \rightarrow n=9\)