Chapter 7

Choose the larger atom in each pair: (a) Al or Ar; (b) \(\mathrm{Tl}\) or In.

Place the following in order of expected increasing size: Ge, As, \(\mathrm{Sn}, \mathrm{Sb}\).

Place the following in order of increasing size: \(\mathrm{N}^{3-}, \mathrm{Mg}^{2+},\) \(\mathrm{Na}^{+}, \mathrm{Ne}, \mathrm{F}^{-}, \mathrm{O}^{2-}\)

Choose the larger particle in each pair: (a) \(\mathrm{Na}\) or \(\mathrm{Na}^{+}\) (b) \(\mathrm{Co}^{3+}\) or \(\mathrm{Co}^{2+} ;\) (c) \(\mathrm{Cl}\) or \(\mathrm{Cl}^{-}\).

Choose the larger particle in each pair: (a) \(S\) or \(S^{2-}\); (b) \(\mathrm{Al}^{3+}\) or \(\mathrm{Al} ;\) (c) \(\mathrm{Au}^{+}\) or \(\mathrm{Au}^{3+}\).

Choose the atom with the larger ionization energy in each pair: (a) \(B\) or \(\mathrm{N} ;\) (b) Se or \(S ;\) (c) \(\mathrm{Cl}\) or Ge.

Choose the atom with the larger ionization energy in each pair: (a) Li or Rb; (b) Al or \(\mathrm{F} ;(\mathrm{c}) \mathrm{F}\) or \(\mathrm{C}\)

Choose the atom with the more exothermic electron affinity in each pair: (a) I or Br; (b) Ga or As.

Choose the atom with the more exothermic electron affinity in each pair: (a) \(S\) or \(A s ;\) (b) \(S\) i or \(N\).

Use the periodic table to select the element in the following list for which there is the largest difference between the second and third ionization energies: \(\mathrm{Na}, \mathrm{Mg}, \mathrm{Al}, \mathrm{Si}, \mathrm{P}, \mathrm{Se}, \mathrm{Cl}\).

Use the periodic table to select the element in the following list for which there is the largest difference between the fourth and fifth ionization energies: \(\mathrm{Na}, \mathrm{Mg}, \mathrm{Al}, \mathrm{Si}, \mathrm{P}\) Se, Cl.

The human ear is sensitive to sound ranging from 20.0 to \(2.00 \times 10^{4} \mathrm{~Hz}\). The speed of sound is \(330 \mathrm{~m} / \mathrm{s}\) in air, and \(1500 \mathrm{~m} / \mathrm{s}\) under water. What is the longest and the shortest wavelength that can be heard (a) in air and (b) under water?

Which of the following electronic transitions could lead to the emission of light from an atom? \(1 s \longrightarrow 4 p \longrightarrow 3 d \longrightarrow 5 f \longrightarrow 4 d \longrightarrow 2 p\)

Suppose students gave the following orbital diagrams for the \(2 s\) and \(2 p\) subshell in the ground state of an atom. What, if anything, is wrong with them? Are any of these electron distributions impossible? (a) \(\begin{array}{lll}\text { (a) } & \text { (11) (11) } & \text { (b) (1) (1) }\end{array}\) (c) (1) (1) (1) (d) (11) (1) (1)

How many electrons are in \(p\) orbitals in an atom of gallium?

Use orbital diagrams to illustrate what happens when an oxygen atom gains two electrons. On the basis of what you have learned about electron affinities and electron configurations, why is it extremely difficult to place a third electron on the oxygen atom?

For an oxygen atom, which requires more energy, the addition of two electrons or the removal of one electron?

Write out the orbital diagram of \(N\) in the ground state. Without adding any more orbitals, write out all the different excited state electron configurations that can be written for \(\mathrm{N}\).

Our understanding of the quantum mechanical atom has been developing since the early 1900 s. Has quantum mechanics had any effect on the daily lives of people?