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Chapter 7: Problem 48

Write electron configurations for the following ions, and determine which have noble-gas configurations: (a) \(\mathrm{Cr}^{3+}\), (b) \(\mathrm{N}^{3-},(\mathrm{c}) \mathrm{Sc}^{3+},(\mathrm{d}) \mathrm{Cu}^{2+}\) (e) \(\mathrm{Tl}^{+}\), (f) \(\mathrm{Au}^{+}\).

Short Answer

Expert verified
The electron configurations for the given ions are: (a) \(\mathrm{Cr}^{3+}\): \(1s²2s²2p⁶3s²3p⁶3d³\) (Not a noble-gas configuration) (b) \(\mathrm{N}^{3-}\): \(1s²2s²2p⁶\) (Noble-gas configuration) (c) \(\mathrm{Sc}^{3+}\): \(1s²2s²2p⁶3s²3p⁶\) (Noble-gas configuration) (d) \(\mathrm{Cu}^{2+}\): \(1s²2s²2p⁶3s²3p⁶3d¹⁰\) (Noble-gas configuration) (e) \(\mathrm{Tl}^{+}\): \(1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²5d¹⁰6p⁵\) (Noble-gas configuration) (f) \(\mathrm{Au}^{+}\): \(1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s¹4f¹⁴5d⁹\) (Not a noble-gas configuration) The ions with noble-gas configurations are: \(\mathrm{N}^{3-}\), \(\mathrm{Sc}^{3+}\), \(\mathrm{Cu}^{2+}\), and \(\mathrm{Tl}^{+}\).

Step by step solution

01

(a) Determine electron configuration for \(\mathrm{Cr}^{3+}\)

First, we need to find the atomic number of Chromium (Cr). From the periodic table, Cr has an atomic number of 24. In its neutral state, it has the same number of electrons; therefore, the electron configuration for Cr is: 1s²2s²2p⁶3s²3p⁶4s²3d⁵ However, Cr⁺³ has lost three electrons. When an atom loses electrons, the first electrons to be removed are from the highest energy level, which is 4s in this case. Thus, the electron configuration for Cr³⁺ is: 1s²2s²2p⁶3s²3p⁶3d³
02

(a) Identify if the electron configuration for \(\mathrm{Cr}^{3+}\) is noble-gas

Comparing this electron configuration with the noble gas configurations, we notice that it is not a noble-gas configuration because it does not end with a full set of 2, 8, 18, 32, etc. electrons in each shell or subshell.
03

(b) Determine the electron configuration for \(\mathrm{N}^{3-}\)

The atomic number of Nitrogen (N) is 7. So, the electron configuration for N is: 1s²2s²2p³ As the ion is N³⁻, it means it has gained three extra electrons (total of 10 electrons). So, the new electron configuration for \(\mathrm{N}^{3-}\) is: 1s²2s²2p⁶
04

(b) Identify if the electron configuration for \(\mathrm{N}^{3-}\) is noble-gas

Comparing this electron configuration with the noble gas configurations, we notice that it has a noble-gas configuration, which is the same as Neon (Ne). Perform similar tasks for the given ions:
05

(c) Determine electron configuration for \(\mathrm{Sc}^{3+}\)

1s²2s²2p⁶3s²3p⁶4s²3d¹
06

(c) Identify if the electron configuration for \(\mathrm{Sc}^{3+}\) is noble-gas

It has a noble-gas configuration, which is the same as Argon (Ar).
07

(d) Determine electron configuration for \(\mathrm{Cu}^{2+}\)

1s²2s²2p⁶3s²3p⁶4s¹3d¹⁰
08

(d) Identify if the electron configuration for \(\mathrm{Cu}^{2+}\) is noble-gas

It has a noble-gas configuration, which is the same as Argon (Ar).
09

(e) Determine electron configuration for \(\mathrm{Tl}^{+}\)

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²5d¹⁰6p⁵
10

(e) Identify if the electron configuration for \(\mathrm{Tl}^{+}\) is noble-gas

It has a noble-gas configuration, which is the same as Xenon (Xe).
11

(f) Determine electron configuration for \(\mathrm{Au}^{+}\)

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s¹4f¹⁴5d⁹
12

(f) Identify if the electron configuration for \(\mathrm{Au}^{+}\) is noble-gas

It does not have a noble-gas configuration. So, the ions with noble-gas configurations are: \(\mathrm{N}^{3-}\), \(\mathrm{Sc}^{3+}\), \(\mathrm{Cu}^{2+}\), and \(\mathrm{Tl}^{+}\).

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Most popular questions from this chapter

An element \(X\) reacts with oxygen to form \(\mathrm{XO}_{2}\) and with chlorine to form \(\mathrm{XCl}_{4} . \mathrm{XO}_{2}\) is a white solid that melts at high temperatures (above \(\left.1000^{\circ} \mathrm{C}\right)\). Under usual conditions, \(\mathrm{XCl}_{4}\) is a colorless liquid with a boiling point of \(58^{\circ} \mathrm{C}\). (a) \(\mathrm{XCl}_{4}\) reacts with water to form \(\mathrm{XO}_{2}\) and another product. What is the likely identity of the other product? (b) Do you think that element \(\mathrm{X}\) is a metal, nonmetal, or metalloid? Explain. (c) \(\mathrm{By}\) using a sourcebook such as the CRC Handbook of Chemistry and Physics, try to determine the identity of element \(\mathrm{X}\).

Note from the following table that the increase in atomic radius in moving from \(\mathrm{Zr}\) to \(\mathrm{Hf}\) is smaller than in moving from \(\mathrm{Y}\) to La. Suggest an explanation for this effect. \begin{tabular}{llll} \hline \multicolumn{3}{l} { Atomic Radii \((\AA)\)} \\ \hline Sc & 1.44 & \(\mathrm{Ti}\) & 1.36 \\ \(\mathrm{Y}\) & 1.62 & \(\mathrm{Zr}\) & 1.48 \\ \(\mathrm{La}\) & 1.69 & \(\mathrm{Hf}\) & 1.50 \end{tabular}

Based on their positions in the periodic table, predict which atom of the following pairs will have the smaller first ionization energy: (a) \(\mathrm{Cl}, \mathrm{Ar} ;\) (b) \(\mathrm{Be}, \mathrm{Ca}\) (c) \(\mathrm{K}\), Co; (d) \(\mathrm{S}, \mathrm{Ge} ;\) (e) Sn. Te.

Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions, identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. If such an atom does not exist, explain why. (b) \(\mathrm{Sc}^{3+}\) (d) \(\mathrm{Zn}^{2+},(\mathrm{e}) \mathrm{Sn}^{4+}\) (a) \(\mathrm{Cl}\) (c) \(\mathrm{Fe}^{2+}\)

Hydrogen is an unusual element because it behaves in some ways like the alkali metal elements and in other ways like nonmetals. Its properties can be explained in part by its electron configuration and by the values for its ionization energy and electron affinity, (a) Explain why the electron affinity of hydrogen is much closer to the values for the alkali elements than for the halogens. (b) Is the following statement true? "Hydrogen has the smallest bonding atomic radius of any element that forms chemical compounds." If not, correct it. If it is, explain in terms of electron configurations. (c) Explain why the ionization energy of hydrogen is closer to the values for the halogens than for the alkali metals. (d) The hydride ion is \(\mathrm{H}\). Write out the process corresponding to the first ionization energy of hydride. (e) How does the process you wrote in part (d) compare to the process for the electron affinity of elemental hydrogen?
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