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Chapter 10: Problem 119

Write the electron configuration of the cyanide ion \(\left(\mathrm{CN}^{-}\right) .\) Name a stable molecule that is isoelectronic with the ion.

Short Answer

Expert verified
The electron configuration of the cyanide ion (CN-) is \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{2}\]. A stable molecule that is isoelectronic with the CN- ion is Silicon (Si).

Step by step solution

01

Determine the Atomic Numbers

The atomic number of Carbon (C) is 6 and Nitrogen (N) is 7. Hence the total number of electrons in cyanide ion CN- before considering the negative charge is \(6+7 = 13\). Given that it is an anion, it gains an extra electron due to the negative charge bringing the total to 14.
02

Write the Electron Configuration

Using the Aufbau principle, we know that the extra electrons are added to the highest energy level first before lower ones in subsequent phase. Thus the electron configuration index for CN- would be: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{2}\].
03

Identify the Isoelectronic Stable Molecule

A molecule is isoelectronic with CN- if it has the same number of electrons. The neutral atom with 14 electrons is Silicon (Si, atomic number 14), so Silicon is isoelectronic with CN-.

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Most popular questions from this chapter

Sketch the shapes of the following molecular orbitals: \(\sigma_{1 s}, \sigma_{1 s}^{\star}, \pi_{2 p},\) and \(\pi_{2 p}^{\star} .\) How do their energies compare?

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Which of these species has a longer bond, \(\mathrm{B}_{2}\) or \(\mathrm{B}_{2}^{+} ?\) Explain in terms of molecular orbital theory.
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