Chapter 7

Why is the fifth ionization energy of carbon so much larger than its fourth?

Why is the first ionization energy of aluminum less than the first ionization energy of magnesium?

For sulfur, write an equation for the change associated with (a) its first electron affinity and (b) its second electron affinity. How should they compare?

Why does Cl have a more exothermic electron affinity than F? Why does Br have a less exothermic electron affinity than \(\mathrm{Cl}\) ?

Why is the second electron affinity of an atom always endothermic?

Ozone protects the earth's inhabitants from the harmful effects of ultraviolet light arriving from the sun. This shielding is a maximum for UV light having a wavelength of \(295 \mathrm{nm}\). What is the frequency in hertz of this light?

The meter is defined as the length of the path light travels in a vacuum during the time interval of \(1 / 299,792,458\) of a second. It is recommended that a helium-neon laser is used for defining the meter. The light from the laser has a wavelength of \(632.99139822 \mathrm{nm}\). What is the frequency of this light, in hertz?

In New York City, radio station WCBS broadcasts its FM signal at a frequency of 101.1 megahertz \((\mathrm{MHz})\). What is the wavelength of this signal in meters?

Calculate the energy in joules of a photon of red light having a frequency of \(4.0 \times 10^{14} \mathrm{~Hz}\). What is the energy of one mole of these photons?

Calculate the energy in joules of a photon of green light having a wavelength of \(563 \mathrm{nm}\).

In the spectrum of hydrogen, there is a line with a wavelength of \(410.3 \mathrm{nm}\). (a) What color is this line? (b) What is its frequency? (c) What is the energy of each of its photons?

Use the Rydberg equation to calculate the wavelength in nanometers of the spectral line of hydrogen for which \(n_{2}=5\) and \(n_{1}=2\). (Report your answer using three significant figures.) In what region of the electromagnetic spectrum would this line be found? Would we be expected to see the light corresponding to this spectral line? Explain your answer.

Calculate the wavelength and energy in joules of the spectral line produced in the hydrogen spectrum when an electron falls from the tenth Bohr orbit to the fourth. (Report your answer using three significant figures.) \(\mathrm{In}\) which region of the electromagnetic spectrum (UV, visible, or infrared) is the line?

Calculate the energy in joules and the wavelength in nano- meters of the spectral line produced in the hydrogen spectrum when an electron falls from the fourth Bohr orbit to the first. (Report your answer using three significant figures.) In which region of the electromagnetic spectrum (UV, visible, or infrared) is the line?

What is the letter code for a subshell with (a) \(\ell=1\) and (b) \(\ell=3 ?\)

What is the letter code for a subshell with (a) \(\ell=2\) and (b) \(\ell=4 ?\)

What is the value of \(\ell\) for (a) a \(p\) orbital and (b) a \(g\) orbital?

What are the values of \(n\) and \(\ell\) for the subshells: (a) \(3 s\) (b) \(5 d ?\)

Give the values of \(n\) and \(\ell\) for the subshells: (a) \(4 p\), (b) \(6 f\).

For the shell with \(n=6\), what are the possible values of \(\ell ?\)

What values of \(\ell\) are possible for a shell with \(n=4 ?\)

What is the value of \(n\) for a shell if the largest value of \(\ell\) is 5 ?

What are the possible values of \(m_{\ell}\) for a subshell with (a) \(\ell=1\) and (b) \(\ell=3 ?\)

If the value of \(\ell\) for an electron in an atom is 5 , what are the possible values of \(m_{\ell}\) that this electron could have?

If the value of \(m_{\ell}\) for an electron in an atom is \(-4,\) what is the smallest value of \(\ell\) that the electron could have? What is the smallest value of \(n\) that the electron could have?

How many orbitals are there in an \(h\) subshell \((\ell=5) ?\) What are the possible values of \(m_{\ell} ?\)

Give the complete set of quantum numbers for all of the electrons that could populate the \(2 p\) subshell of an atom.

Give the complete set of quantum numbers for all of the electrons that could populate the \(3 d\) subshell of an atom.

In an atom of barium, how many electrons have (a) \(\ell=0\) and \((\mathbf{b}) m_{\ell}=1 ?\)

Give the electron configurations of (a) \(S,\) (b) \(K\), (c) \(\mathrm{Ti}\) and (d) Sn. (c) \(\mathrm{Ni}\)

Write the electron configurations of (a) As, (b) Cl, and (d) \(S i\).

Which of the following atoms in their ground states are expected to be paramagnetic: (a) \(\mathrm{Mn}\) (b) As, (c) S, (d) Sr, (e) \(\mathrm{Ar}\) ?

Which of the following atoms in their ground states are expected to be diamagnetic: (a) Ba, (b) Se, (c) \(\mathrm{Zn}\) (d) Si?

How many unpaired electrons would be found in the ground state of (a) \(\mathrm{Mg}\), (b) \(\mathrm{P}\), and \((\mathbf{c}) \mathrm{V}\) ?

How many unpaired electrons would be found in the ground state of (a) \(\mathrm{Cs},(\mathbf{b}) \mathrm{S},\) and \((\mathbf{c}) \mathrm{Ni}\) ?

Write the abbreviated electron configurations for (a) Ni, (b) \(\mathrm{Cs},(\mathbf{c}) \mathrm{Ge}\) (d) \(\mathrm{Br}\), and \((\mathrm{e}) \mathrm{Bi} .\)

Write the abbreviated electron configurations for (a) Al, (b) Se, (c) \(\mathrm{Ba}\) (d) \(\mathrm{Sb},\) and \((\mathrm{e}) \mathrm{Gd}\)

Draw complete orbital diagrams for (a) Mg and (b) Ti.

Draw complete orbital diagrams for (a) As and (b) Ni.

Draw orbital diagrams for the abbreviated configurations of (a) \(\mathrm{Ni},(\mathbf{b}) \mathrm{Cs},(\mathbf{c}) \mathrm{Ge},\) and \((\mathbf{d}) \mathrm{Br}\)

Draw orbital diagrams for the abbreviated configurations of \((\) a \() \mathrm{Al},(\mathbf{b}) \mathrm{Se},(\mathbf{c}) \mathrm{Ba},\) and \((\mathbf{d}) \mathrm{Sb}_{-}\)

What is the value of \(n\) for the valence shells of (a) Sn, (b) \(\mathrm{K},(\mathbf{c}) \mathrm{Br},\) and \((\mathbf{d}) \mathrm{Bi}\) ?

What is the value of \(n\) for the valence shells of (a) Al, (b) Se, (c) \(\mathrm{Ba},\) and (d) \(\mathrm{Sb}\) ?

Give the configuration of the valence shell for (a) Na, (b) \(\mathrm{Al},(\mathbf{c}) \mathrm{Ge},\) and \((\mathbf{d}) \mathrm{P}\)

Give the configuration of the valence shell for (a) \(\mathrm{Mg}\) (b) \(\mathrm{Br}\) (c) \(\mathrm{Ga}\), and \((\mathbf{d}) \mathrm{Pb}\).

Draw the orbital diagram for the valence shell of (a) Na, (b) \(\mathrm{Al},(\mathbf{c}) \mathrm{Ge},\) and \((\mathbf{d}) \mathrm{P}\)

Draw the orbital diagram for the valence shell of (a) \(\mathrm{Mg}\), (b) \(\mathrm{Br},(\mathbf{c}) \mathrm{Ga},\) and (d) \(\mathrm{Pb}\).

If the core electrons were \(100 \%\) effective at shielding the valence electrons from the nuclear charge and the valence electrons provided no shielding for each other, what would be the effective nuclear charge felt by a valence electron in (a) \(\mathrm{Na}\) (b) \(S,(\mathbf{c}) \mathrm{Cl} ?\)

If the core electrons were \(100 \%\) effective at shielding the valence electrons from the nuclear charge and the valence electrons provided no shielding for each other, what would be the effective nuclear charge felt by a valence electron in (a) \(\mathrm{Mg}\), (b) \(\mathrm{Si}\), (c) \(\mathrm{Br}\) ?

Choose the larger atom in each pair: (a) \(\mathrm{Mg}\) or \(\mathrm{S} ;\) (b) As or Bi.