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Chapter 7: Problem 83

Write the ground-state electron configurations for the following elements: \(\mathrm{B}, \mathrm{V}, \mathrm{Ni}, \mathrm{As}, \mathrm{I}, \mathrm{Au}\).

Short Answer

Expert verified
The ground-state electron configurations for the elements are: \(B: 1s^{2}2s^{2}2p^{1}\), \(V: 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{3}\), \(Ni: 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{8}\), \(As: 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{3}\), \(I: 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{5}\), and \(Au: 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{1}4f^{14}5d^{10}\).

Step by step solution

01

Understanding the Rules

Electrons in an atom are organized into shells, subshells, and orbitals. Electrons fill up shells and subshells in an order defined by the energy level and shape of the orbital. This filling order is represented by the arrows in the Aufbau diagram.
02

Writing Electron Configurations For B

To write electron configurations, follow the aufbau diagram from the lowest energy level to the highest. For \(B\) (Boron), which has 5 electrons, the electron configuration is \(1s^{2}2s^{2}2p^{1}\).
03

Writing Electron Configurations For V

For \(V\) (Vanadium), which has 23 electrons, the electron configuration is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{3}\)
04

Writing Electron Configurations For Ni

For \(Ni\) (Nickel), which has 28 electrons, the electron configuration is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{8}\)
05

Writing Electron Configurations For As

For \(As\) (Arsenic), which has 33 electrons, the electron configuration is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{3}\).
06

Writing Electron Configurations For I

For \(I\) (Iodine), which has 53 electrons, the electron configuration is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{5}\).
07

Writing Electron Configurations For Au

For \(Au\) (Gold), which has 79 electrons, the electron configuration is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{1}4f^{14}5d^{10}\).

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Most popular questions from this chapter

Some copper compounds emit green light when they are heated in a flame. How would you determine whether the light is of one wavelength or a mixture of two or more wavelengths?

An electron in a hydrogen atom is excited from the ground state to the \(n=4\) state. Comment on the correctness of the following statements (true or false). (a) \(n=4\) is the first excited state. (b) It takes more energy to ionize (remove) the electron from \(n=4\) than from the ground state. (c) The electron is farther from the nucleus (on average) in \(n=4\) than from the ground state. (d) The wavelength of light emitted when the electron drops from \(n=4\) to \(n=1\) is longer than that from \(n=4\) to \(n=2\). (e) The wavelength the atom absorbs in going from \(n=1\) to \(n=4\) is the same as that emitted as it goes from \(n=4\) to \(n=1\).

Give the values of the quantum numbers associated with the following orbitals: (a) \(2 p,\) (b) \(3 s,\) (c) \(5 d\).

What are photons? What role did Einstein's explanation of the photoelectric effect play in the development of the particle-wave interpretation of the nature of electromagnetic radiation?

(a) What is the frequency of light having a wavelength of \(456 \mathrm{nm} ?\) (b) What is the wavelength (in nanometers) of radiation having a frequency of \(2.45 \times 10^{9} \mathrm{~Hz} ?\) (This is the type of radiation used in microwave ovens.)
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