Chapter 8

Write the electron configurations for \(P\) and \(C l\) using both spdf notation and orbital box diagrams. Describe the relationship between each atom's electron configuration and its position in the periodic table.

Write the electron configurations for \(\mathrm{Mg}\) and \(\mathrm{Ar}\) using both spdf notation and orbital box diagrams. Describe the relation of the atom's electron configuration to its position in the periodic table.

Using spdf notation, write the electron configurations for atoms of chromium and iron, two of the major components of stainless steel.

Using spdf notation, give the electron configuration of vanadium, \(V\), an element found in some brown and red algae and some toadstools.

Depict the electron configuration for each of the following atoms using spdfand noble gas notations. (a) Arsenic, As. A deficiency of As can impair growth in animals even though larger amounts are poisonous. (b) Krypton, Kr. It ranks seventh in abundance of the gases in the earth's atmosphere.

Using spdfand noble gas notations, write electron configurations for atoms of the following elements and then check your answers with Table 8.3. (a) Strontium, Sr. This element is named for a town in Scotland. (b) Zirconium, Zr. The metal is exceptionally resistant to corrosion and so has important industrial applications. Moon rocks show a surprisingly high zirconium content compared with rocks on earth. (c) Rhodium, Rh. This metal is used in jewelry and in catalysts in industry. (d) Tin, Sn. The metal was used in the ancient world. Alloys of tin (solder, bronze, and pewter) are important.

Use noble gas and spdf notations to depict electron configurations for the following metals of the third transition series. (a) Tantalum, Ta. The metal and its alloys resist corrosion and are often used in surgical and dental tools. (b) Platinum, Pt. This metal was used by pre-Columbian Indians in jewelry. It is used now in jewelry and for anticancer drugs and industrial catalysts.

The lanthanides, once called the rare earth elements, are really only "medium rare." Using noble gas and spdf notations, depict reasonable electron configurations for the following elements. (a) Samarium, Sm. This lanthanide is used in magnetic materials. (b) Ytterbium, Yb. This element was named for the village of Ytterby in Sweden, where a mineral source of the element was found.

The actinide americium, Am, is a radioactive element that has found use in home smoke detectors. Depict its electron configuration using noble gas and spdf notations.

Predict reasonable electron configurations for the following elements of the actinide series of elements. Use noble gas and spdf notations. (a) Plutonium, Pu. The element is best known as a byproduct of nuclear power plant operations. (b) Curium, Cm. This actinide was named for Madame Curie (page 57)

Using orbital box diagrams, depict an electron configuration for each of the following ions: (a) \(\mathrm{Mg}^{2+},\) (b) \(\mathrm{K}^{+}\) (c) \(\mathrm{Cl}^{-},\) and \((\mathrm{d}) \mathrm{O}^{2-}\).

Using orbital box diagrams, depict an electron configuration for each of the following ions: (a) \(\mathrm{Na}^{+},\) (b) \(\mathrm{Al}^{3+}\) (c) \(\mathrm{Ge}^{2+},\) and \((\mathrm{d}) \mathrm{F}^{-}\).

Using orbital box diagrams and noble gas notation, depict the electron configurations of (a) \(\mathrm{V},\) (b) \(\mathrm{V}^{2+},\) and \((\mathrm{c}) \mathrm{V}^{5+}\) Are any of the ions paramagnetic?

Using orbital box diagrams and noble gas notation, depict the electron configurations of (a) \(\mathrm{Ti},\) (b) \(\mathrm{Ti}^{2+},\) and (c) Ti \(^{4+} .\) Are any of the ions paramagnetic?

Manganese is found as \(\mathrm{MnO}_{2}\) in deep ocean deposits. (a) Depict the electron configuration of this element using the noble gas notation and an orbital box diagram. (b) Using an orbital box diagram, show the electrons beyond those of the preceding noble gas for the \(2+\) ion. (c) Is the \(2+\) ion paramagnetic? (d) How many unpaired electrons does the \(\mathrm{Mn}^{2+}\) ion have?

Nickel generally forms \(2+\) ions but alkaline batteries have \(\mathrm{Ni}^{3+}\) ions in \(\mathrm{NiOOH} .\) Using orbital box diagrams and the noble gas notation, show electron configurations of these ions. Are either of these ions paramagnetic?

Explain briefly why each of the following is not a possible set of quantum numbers for an electron in an atom. In each case, change the incorrect value (or values) to make the set valid. (a) \(n=4, \ell=2, m_{\ell}=0, m_{\mathrm{s}}=0\) (b) \(n=3, \ell=1, m_{\ell}=-3, m_{s}=-\frac{1}{2}\) (c) \(n=3, \ell=3, m_{\ell}=-1, m_{\mathrm{s}}=+\frac{1}{2}\)

Explain briefly why each of the following is not a possible set of quantum numbers for an electron in an atom. In each case, change the incorrect value (or values) to make the set valid. (a) \(n=2, \ell=2, m_{\ell}=0, m_{\mathrm{s}}=+\frac{1}{2}\) (b) \(n=2, \ell=1, m_{\ell}=-1, m_{\mathrm{s}}=0\) (c) \(n=3, \ell=1, m_{\ell}=+2, m_{\mathrm{s}}=+\frac{1}{2}\)

What is the maximum number of electrons that can be identified with each of the following sets of quantum numbers? In one case, the answer is "none." Explain why this is true. (a) \(n=4, \ell=3\) (b) \(n=6, \ell=1, m_{\ell}=-1\) (c) \(n=3, \ell=3, m_{\ell}=-3\)

What is the maximum number of electrons that can be identified with each of the following sets of quantum numbers? In some cases, the answer may be "none." In such cases, explain why "none" is the correct answer. (a) \(n=3\) (b) \(n=3\) and \(\ell=2\) (c) \(n=4, \ell=1, m_{\ell}=-1,\) and \(m_{\mathrm{s}}=-\frac{1}{2}\) (d) \(n=5, \ell=0, m_{\ell}=+1\)

Depict the electron configuration for magnesium using an orbital box diagram and noble gas notation. Give a complete set of four quantum numbers for each of the electrons beyond those of the preceding noble gas.

Depict the electron configuration for phosphorus using an orbital box diagram and noble gas notation. Give one possible set of four quantum numbers for each of the electrons beyond those of the preceding noble gas.

Using an orbital box diagram and noble gas notation, show the electron configuration of gallium, Ga. Give a set of quantum numbers for the highest- energy electron.

Using an orbital box diagram and noble gas notation, show the electron configuration of titanium. Give one possible set of four quantum numbers for each of the electrons beyond those of the preceding noble gas.

Arrange the following elements in order of increasing size: \(\mathrm{Al}, \mathrm{B}, \mathrm{C}, \mathrm{K},\) and \(\mathrm{Na} .\) (Try doing it without looking at Figure \(8.11,\) and then check yourself by looking up the necessary atomic radii.)

Arrange the following elements in order of increasing size: Ca, Rb, P, Ge, and Sr. (Try doing it without looking at Figure \(8.11,\) then check yourself by looking up the necessary atomic radii.)

Select the atom or ion in each pair that has the larger radius. (a) Cl or \(\mathrm{Cl}^{-}\) (c) In or I (b) Al or \(\mathbf{O}\)

Select the atom or ion in each pair that has the larger radius. (a) Cs or Rb (b) \(\mathbf{O}^{2-}\) or \(\mathbf{O}\) (c) Br or As

Which of the following groups of elements is arranged correctly in order of increasing ionization energy? (a) \(\mathrm{C} < \mathrm{Si} < \mathrm{Li} < \mathrm{Ne}\) (c) \(\mathrm{Li} < \mathrm{Si} < \mathrm{C} < \mathrm{Ne}\) (b) \(\mathrm{Ne} < \mathrm{Si} < \mathrm{C} < \mathrm{Li}\) (d) \(\mathrm{Ne} < \mathrm{C} < \mathrm{Si} < \mathrm{Li}\)

Arrange the following atoms in order of increasing ionization energy: \(\mathrm{Li}, \mathrm{K}, \mathrm{C},\) and \(\mathrm{N}\)

Compare the elements Na, Mg, O, and P. (a) Which has the largest atomic radius? (b) Which has the most negative electron affinity? (c) Place the elements in order of increasing ionization energy.

Compare the elements \(\mathrm{B}, \mathrm{Al}, \mathrm{C},\) and \(\mathrm{Si}\) (a) Which has the most metallic character? (b) Which has the largest atomic radius? (c) Which has the most negative electron affinity? (d) Place the three elements \(B\), \(A l\), and \(C\) in order of increasing first ionization energy.

Explain each answer briefly. (a) Place the following elements in order of increasing ionization energy: \(F, O,\) and \(S\) (b) Which has the largest ionization energy: \(\mathbf{O},\) S, or Se? (c) Which has the most negative electron affinity: \(\mathrm{Se}, \mathrm{Cl}\) or Br? (d) Which has the largest radius: \(\mathbf{O}^{2-}, \mathbf{F}^{-},\) or \(\mathrm{F} ?\)

Explain each answer briefly. (a) Rank the following in order of increasing atomic radius: \(O, S,\) and \(F\) (b) Which has the largest ionization energy: \(P\), Si, S, or Se? (c) Place the following in order of increasing radius: \(\mathbf{O}^{2-}\) \(\mathrm{N}^{3-},\) and \(\mathrm{F}^{-}\) (d) Place the following in order of increasing ionization energy: Cs, Sr, and Ba.

The name rutherfordium, Rf, has been given to element 104 to honor the physicist Ernest Rutherford (page 65 ). Depict its electron configuration using spdfand noble gas notations.

Using an orbital box diagram and noble gas notation, show the electron configurations of uranium and of the uranium(IV) ion. Is either of these paramagnetic?

The rare earth elements, or lanthanides, commonly exist as \(3+\) ions. Using an orbital box diagram and noble gas notation, show the electron configurations of the following elements and ions. (a) Ce and \(\mathrm{Ce}^{3+}\) (cerium) (b) Ho and \(\mathrm{Ho}^{3+}\) (holmium)

A neutral atom has two electrons with \(n=1\), eight electrons with \(n=2,\) eight electrons with \(n=3,\) and two electrons with \(n=4 .\) Assuming this element is in its ground state, supply the following information: (a) atomic number (b) total number of s electrons (c) total number of \(p\) electrons (d) total number of \(d\) electrons (e) is the element a metal, metalloid, or nonmetal?

Which of the following is not an allowable set of quantum numbers? Explain your answer briefly. \(n \quad \ell \quad m_{\ell} \quad m_{\mathrm{s}}\) \(\begin{array}{lllll}\text { (a) } & 2 & 0 & 0 & -\frac{1}{2}\end{array}\) \(\begin{array}{lllll}\text { (b) } & 1 & 1 & 0 & +\frac{1}{2}\end{array}\) \(\begin{array}{lllll}\text { (c) } & 2 & 1 & -1 & -\frac{1}{2}\end{array}\) \(\begin{array}{lllll}\text { (d) } 4 & 3 & +2 & -\frac{1}{2}\end{array}\)

A possible excited state for the \(\mathrm{H}\) atom has an electron in a 4p orbital. List all possible sets of quantum numbers \((n, \ell\) \(m_{\ell},\) and \(m_{s}\) ) for this electron.

The magnet in the photo is made from neodymium, iron, and boron. (IMAGE NOT COPY) (a) Write the electron configuration of each of these elements using an orbital box diagram and noble gas notation. (b) Are these elements paramagnetic or diamagnetic? (c) Write the electron configurations of \(\mathrm{Nd}^{3+}\) and \(\mathrm{Fe}^{3+}\) using orbital box diagrams and noble gas notation. Are these ions paramagnetic or diamagnetic?

Name the element corresponding to each characteristic below. (a) the element with the electron configuration \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3}\) (b) the alkaline earth element with the smallest atomic radius (c) the element with the largest ionization energy in Group \(5 \mathrm{A}\) (d) the element whose \(2+\) ion has the configuration \([\mathrm{Kr}] 4 d^{5}\) (e) the element with the most negative electron affinity in Group 7A (f) the element whose electron configuration is \([\mathrm{Ar}] 3 d^{10} 4 s^{2}\)

Arrange the following atoms in the order of increasing ionization energy: Si, K, P, and Ca.

Rank the following in order of increasing ionization energy: Cl, \(\mathrm{Ca}^{2+}\), and \(\mathrm{Cl}^{-}\). Briefly explain your answer.

Answer the questions below about the elements \(A\) and \(B\), which have the electron configurations shown. $$A=[K r] 5 s^{1} \quad B=[A r] 3 d^{10} 4 s^{2} 4 p^{4}$$ (a) Is element A a metal, nonmetal, or metalloid? (b) Which element has the greater ionization energy? (c) Which element has the less negative electron affinity? (d) Which element has the larger atomic radius?

Answer the following questions about the elements with the electron configurations shown here: $$A=[A r] 4 s^{2} \quad B=[A r] 3 d^{10} 4 s^{2} 4 p^{5}$$ (a) Is element A a metal, metalloid, or nonmetal? (b) Is element B a metal, metalloid, or nonmetal? (c) Which element is expected to have the larger ionization energy? (d) Which element has the smaller atomic radius?

Which of the following ions are unlikely to be found in a chemical compound: \(\mathrm{Cs}^{+}, \mathrm{In}^{4+}, \mathrm{Fe}^{6+}, \mathrm{Te}^{2-}, \mathrm{Sn}^{5+},\) and \(\mathrm{I}^{-} ?\) Explain briefly.

Place the following elements and ions in order of decreasing size: \(\mathrm{K}^{+}, \mathrm{Cl}^{-}, \mathrm{S}^{2-},\) and \(\mathrm{Ca}^{2+}\).

Answer each of the following questions: (a) Of the elements S, Se, and Cl, which has the largest atomic radius? (b) Which has the larger radius, Br or \(\mathrm{Br}^{-} ?\) (c) Which should have the largest difference between the first and second ionization energy: Si, Na, P, or Mg? (d) Which has the largest ionization energy: \(\mathrm{N}, \mathrm{P}\), or As? (e) Which of the following has the largest radius: \(\mathrm{O}^{2-}\) \(\mathrm{N}^{3-},\) or \(\mathrm{F}^{-} ?\)

The following are isoelectronic species: \(\mathrm{Cl}^{-}, \mathrm{K}^{+},\) and \(\mathrm{Ca}^{2+}\) Rank them in order of increasing (a) size, (b) ionization energy, and (c) electron affinity.