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Chapter 8: Problem 87

The following electron configurations correspond to the ground states of certain elements. Name each element. (a) \([\mathrm{Rn}] 7 s^{2} 6 d^{2} ;\) (b) \([\mathrm{He}] 2 s^{2} 2 p^{2} ;\) (c) \([\mathrm{Ar}] 3 d^{3} 4 s^{2}\) (d) \([\mathrm{Kr}] 4 d^{10} 5 s^{2} 5 p^{4} ;\) (e) \([\mathrm{Xe}] 4 f^{2} 6 s^{2} 6 p^{1}\)

Short Answer

Expert verified
The elements corresponding to these electron configurations are: (a) Thorium (Th); (b) Carbon (C); (c) Vanadium (V); (d) Tellurium (Te); (e) Thulium (Tm).

Step by step solution

01

Identity The Noble Gas Core

The electron configurations are given with a noble gas core, represented by the symbol of the noble gas in square brackets. For example, in (a) \([\mathrm{Rn}] 7 s^{2} 6 d^{2}\), Rn stands for Radon, which has 86 electrons. This is the inert gas core for this element.
02

Count the Additional Electrons

Count the number of electrons outside the noble gas core. In the previous example, the number of additional electrons is \(7s^{2}\) or 2 electrons and \(6d^{2}\) or 2 electrons. Adding these to the 86 electrons of the noble gas core gives a total of 90 electrons.
03

Identify the Element

The element is identified by its atomic number, which is equal to the total number of electrons in the neutral atom. An atom with 90 electrons is thorium (Th).
04

Repeat the Process

Repeat the process for each of the electron configurations given in the assignment.

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Most popular questions from this chapter

Without doing detailed calculations, indicate which of the following electromagnetic radiations has the greatest energy per photon and which has the least: (a) \(662 \mathrm{nm}\) (b) \(2.1 \times 10^{-5} \mathrm{cm} ;\) (c) \(3.58 \mu \mathrm{m} ;\) (d) \(4.1 \times 10^{-6} \mathrm{m}\).

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