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Chapter 6: Problem 75

Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations: (a) \(\mathrm{Cs},(\mathbf{b}) \mathrm{Ni},(\mathbf{c}) \mathrm{Se},(\mathbf{d}) \mathrm{Cd},(\mathbf{e}) \mathrm{U},(\mathbf{f}) \mathrm{Pb}\)

Short Answer

Expert verified
The condensed electron configurations for the given atoms are: (a) Cesium (Cs): \([Xe]6s^1\) (b) Nickel (Ni): \([Ar]4s^2 3d^8\) (c) Selenium (Se): \([Ar]4s^2 3d^{10} 4p^4\) (d) Cadmium (Cd): \([Kr]5s^2 4d^{10}\) (e) Uranium (U): \([Rn]7s^2 5f^3 6d^1\) (f) Lead (Pb): \([Xe]6s^2 4f^{14} 5d^{10} 6p^2\)

Step by step solution

01

(a) Cs (Cesium) Electron Configuration

: To find the condensed electron configuration of Cesium: 1. Identify the noble gas that comes before Cs: The noble gas before Cs is Xenon (Xe) with an atomic number of 54. 2. Write down the noble-gas core abbreviation: [Xe] 3. Add the electron configuration for Cs after the noble gas abbreviation: Cs has an atomic number of 55. The electron configuration after Xe is 6s1. So, the condensed electron configuration for Cesium is: \([Xe]6s^1\)
02

(b) Ni (Nickel) Electron Configuration

: To find the condensed electron configuration of Nickel: 1. Identify the noble gas that comes before Ni: The noble gas before Ni is Argon (Ar) with an atomic number of 18. 2. Write down the noble-gas core abbreviation: [Ar] 3. Add the electron configuration for Ni after the noble gas abbreviation: Ni has an atomic number of 28. The electron configuration after Ar is 4s2 3d8. So, the condensed electron configuration for Nickel is: \([Ar]4s^2 3d^8\)
03

(c) Se (Selenium) Electron Configuration

: To find the condensed electron configuration of Selenium: 1. Identify the noble gas that comes before Se: The noble gas before Se is Argon (Ar) with an atomic number of 18. 2. Write down the noble-gas core abbreviation: [Ar] 3. Add the electron configuration for Se after the noble gas abbreviation: Se has an atomic number of 34. The electron configuration after Ar is 4s2 3d10 4p4. So, the condensed electron configuration for Selenium is: \([Ar]4s^2 3d^{10} 4p^4\)
04

(d) Cd (Cadmium) Electron Configuration

: To find the condensed electron configuration of Cadmium: 1. Identify the noble gas that comes before Cd: The noble gas before Cd is Krypton (Kr) with an atomic number of 36. 2. Write down the noble-gas core abbreviation: [Kr] 3. Add the electron configuration for Cd after the noble gas abbreviation: Cd has an atomic number of 48. The electron configuration after Kr is 5s2 4d10. So, the condensed electron configuration for Cadmium is: \([Kr]5s^2 4d^{10}\)
05

(e) U (Uranium) Electron Configuration

: To find the condensed electron configuration of Uranium: 1. Identify the noble gas that comes before U: The noble gas before U is Radon (Rn) with an atomic number of 86. 2. Write down the noble-gas core abbreviation: [Rn] 3. Add the electron configuration for U after the noble gas abbreviation: U has an atomic number of 92. The electron configuration after Rn is 7s2 5f3 6d1. So, the condensed electron configuration for Uranium is: \([Rn]7s^2 5f^3 6d^1\)
06

(f) Pb (Lead) Electron Configuration

: To find the condensed electron configuration of Lead: 1. Identify the noble gas that comes before Pb: The noble gas before Pb is Xenon (Xe) with an atomic number of 54. 2. Write down the noble-gas core abbreviation: [Xe] 3. Add the electron configuration for Pb after the noble gas abbreviation: Pb has an atomic number of 82. The electron configuration after Xe is 6s2 4f14 5d10 6p2. So, the condensed electron configuration for Lead is: \([Xe]6s^2 4f^{14} 5d^{10} 6p^2\)

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Most popular questions from this chapter

Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (a) \(1 s^{2} 2 s^{2},(\mathbf{b}) 1 s^{2} 2 s^{2} 2 p^{4}\) (c) \([\operatorname{Ar}] 4 s^{1} 3 d^{5},(\mathbf{d})[\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{4}\)

The following do not represent valid ground-state electron configurations for an atom either because they violate the Pauli exclusion principle or because orbitals are not filled in order of increasing energy. Indicate which of these two principles is violated in each example. (a) 1\(s^{2} 2 s^{2} 3 s^{1}\) (b) \([\mathrm{Xe}] 6 s^{2} 5 d^{4}(\mathbf{c})[\mathrm{Ne}] 3 s^{2} 3 d^{5} .\)

The series of emission lines of the hydrogen atom for which \(n_{1}=3\) is called the Paschen series. (a) Determine the region of the electromagnetic spectrum in which the lines of the Paschen series are observed. (b) Calculate the wavelengths of the first three lines in the Paschen series - those for which \(n_{1}=4,5,\) and \(6 .\)

Indicate whether energy is emitted or absorbed when the following electronic transitions occur in hydrogen: (a) from \(n=2\) to \(n=6,(\mathbf{b})\) from an orbit of radius 4.76\(\hat{\mathrm{A}}\) to one of radius \(0.529 \mathrm{A},(\mathbf{c})\) from the \(n=6\) to the \(n=9\) state.

Molybdenum metal must absorb radiation with a minimum frequency of \(1.09 \times 10^{15} \mathrm{s}^{-1}\) before it can eject an electron from its surface via the photoelectric effect. (a) What is the minimum energy needed to eject an electron? (b) What wavelength of radiation will provide a photon of this energy? (c) If molybdenum is irradiated with light of wavelength of \(120 \mathrm{nm},\) what is the maximum possible kinetic energy of the emitted electrons?
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