Chapter 7

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 relationship 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, \(\mathrm{V},\) an element found in some brown and red algae and some toadstools.

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

Using spdf and noble gas notations, write electron configurations for atoms of the following elements. (Try to do this by looking at the periodic table but not at Table \(7.3 .\) ) (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 preColumbian Indians in jewelry. Now it is still used in jewelry but it is also the basis for anticancer drugs and catalysts (such as those in automobile exhaust systems).

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.

Americium, Am, is a radioactive element isolated from spent fuel in nuclear reactors and used in home smoke detectors. Depict its electron configuration using noble gas and spdf notations.

Predict 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 by-product of nuclear power plant operations. (b) Curium, Cm. This actinide was named for Marie Curie (page 72 ).

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) \(n=4, \ell=3, m_{\ell}=1\) (b) \(n=6, \ell=1, m_{\ell}=-1, m_{\mathrm{s}}=-1 / 2\) (c) \(n=3, \ell=3, m_{c}=-3\)

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 \(m_{\mathrm{s}}=+1 / 2\) (d) \(n=5, \ell=0, m_{\ell}=-1, m_{\mathrm{s}}=+1 / 2\)

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 one possible 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.

The effective nuclear charge, \(Z^{*},\) is the net force of attraction experienced by the outermost electron in an atom. Which of the following statements best describes how \(Z^{*}\) varies among the elements of the second period (Li to \(\mathrm{F}\) )? (a) regular increase from Li to \(\mathrm{F}\) (b) regular decrease from Li to \(\mathrm{F}\) (c) general increase from Li to F, but with exceptions

Which of the following statements correctly describes the value of the effective nuclear charge, \(Z^{*},\) felt by (a) the \(2 s\) electron at a large distance from a Li atom? (i) \(\quad Z^{*}\) equals 1 (ii) \(Z^{*}\) is between 1 and 3 (iii) \(Z^{*}\) equals 3 (b) the \(2 s\) electron at its most probable distance from the nucleus of a Li atom? (i) \(\quad Z^{*}\) equals 1 (ii) \(Z^{*}\) is between 1 and 3 (iii) \(Z^{*}\) equals 3

List the first five orbitals (the five orbitals in an atom at lowest energy) in order of filling, according to the Aufbau principle.

The values of \(n\) and \(\ell\) are useful to determine the order of filling (Aufbau principle). Use \(n\) and \(\ell\) to determine which orbital, \(4 f, 5 d,\) or \(6 s,\) will fill first.

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

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

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

Using orbital box diagrams and noble gas notation, depict the electron configurations of (a) Ti, (b) \(\mathrm{Ti}^{2+},\) and \((\mathrm{c}) \mathrm{Ti}^{4+} .\) Is the element or 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 \(\mathrm{Mn}^{4+}\) (c) Is \(\mathrm{Mn}^{4+}\) paramagnetic? (d) How many unpaired electrons does the \(\mathrm{Mn}^{4+}\) ion have?

One compound found in alkaline batteries is NiOOH, a compound containing \(\mathrm{Ni}^{3+}\) ions. When the battery is discharged, the \(\mathrm{Ni}^{3+}\) is reduced to \(\left.\mathrm{Ni}^{2+} \text { ions [as in } \mathrm{Ni}(\mathrm{OH})_{2}\right] .\) Using orbital box diagrams and the noble gas notation, show electron configurations of these ions. Are either of these ions paramagnetic?

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 \(7.5 ;\) 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 \(7.5 ;\) then check yourself by looking up the necessary atomic radii.

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

Select the atom or ion in each pair that has the larger radius. (a) Cs or Rb (b) \(\mathrm{O}^{2-}\) or \(\mathrm{O}\) (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: Li, \(\mathrm{K}, \mathrm{C}_{r}\) and \(\mathrm{N}\).

Compare the elements \(\mathrm{Na}, \mathrm{Mg}, \mathrm{O},\) and \(\mathrm{P}\) (a) Which has the largest atomic radius? (b) Which has the most negative electron attachment enthalpy? (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 attachment enthalpy? (d) Place the three elements \(\mathrm{B}, \mathrm{Al}\), and \(\mathrm{C}\) in order of increasing first ionization energy.

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

Identify the element that corresponds to each of the simplified photoelectron spectral data given below. (Energy data taken from D. A. Shirley, R. L. Martin, S. P. Kowalczyk, F. R. McFeely, and L. Ley: "Core-electron binding energies of the first thirty elements," Physical Review B, Vol. 15, pp. 544-552, \(1977 .)\) (a) There are peaks at energies corresponding to \(1079,70.8,38.0,5.14 \mathrm{eV},\) corresponding to 2 \(2,6,\) and 1 electrons, respectively. (b) There are peaks at energies corresponding to \(4043,443,351,48.4,30.1,\) and \(6.11 \mathrm{eV},\) corre- sponding to \(2,2,6,2,6,\) and 2 electrons, respectively. (c) There are peaks at energies corresponding to \(5475,638,524,77,47,12,\) and \(7.3 \mathrm{eV},\) corre- sponding to \(2,2,6,2,6,3,\) and 2 electrons, respectively.

The red color of rubies is the result of the substitution of some \(\mathrm{Cr}^{3+}\) ions for \(\mathrm{Al}^{3+}\) ions in solid \(\mathrm{Al}_{2} \mathrm{O}_{3}\). (a) Using spáf notation with the noble gas notation, write the electron configuration for the Cr atom and for the \(\mathrm{Cr}^{3+}\) ion? (b) Is \(\mathrm{Cr}^{2+}\) paramagnetic? Is \(\mathrm{Cr}^{3+} ?\) (c) The radius of the \(\mathrm{Cr}^{3+}\) ion is \(64 \mathrm{pm}\). How does this compare with the radius of the \(\mathrm{Al}^{3+}\) ion?

The deep blue color of sapphires comes from the presence of \(\mathrm{Fe}^{2+}\) and \(\mathrm{Ti}^{4+}\) in solid \(\mathrm{Al}_{2} \mathrm{O}_{3}\). Using \(s p d\) notation with the noble gas notation, write the electron configuration for each of these ions.

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?

Element \(109,\) now named meitnerium (in honor of the Austrian-Swedish physicist, Lise Meitner \([1878-1968]),\) was produced in August 1982 by a team at Germany's Institute for Heavy lon Research. Depict its electron configuration using spdf and noble gas notations. Name another element found in the same group as meitnerium.

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

The magnet in the following photo is made from neodymium, iron, and boron. (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 attachment enthalpy in Group 7A (f) the element whose electron configuration is \([\mathrm{Ar}] 3 d^{10} 4 s^{2}\)

Arrange the following atoms in order of increasing ionization energy: \(\mathrm{Si}, \mathrm{K}, \mathrm{P},\) and \(\mathrm{Ca}\)

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

Answer the questions below about the elements A and \(\mathrm{B},\) which have the electron configurations shown. $$ \mathrm{A}=[\mathrm{Kr}] 5 s^{1} \quad \mathrm{B}=\left[\mathrm{Ar} | 3 d^{10} 4 \mathrm{s}^{2} 4 p^{4}\right. $$ (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 attachment enthalpy? (d) Which element has the larger atomic radius? (e) What is the formula for a compound formed between A and B?

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.