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Ch 41: Quantum Mechanics II: Atomic Structure
Young & Freedman Calc - University Physics 15th Edition
Young & Freedman Calc15th EditionUniversity PhysicsISBN: 9780135159552Not the one you use?Change textbook
All textbooksYoung & Freedman Calc 15th EditionCh 41: Quantum Mechanics II: Atomic StructureProblem 35a
Chapter 40, Problem 35a

The doubly charged ion N2+ is formed by removing two electrons from a nitrogen atom. What is the ground-state electron configuration for the N2+ ion?

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Identify the atomic number of nitrogen (N), which is 7. This means a neutral nitrogen atom has 7 electrons.
Write the ground-state electron configuration for a neutral nitrogen atom. The configuration is: 1s² 2s² 2p³.
Understand that the N²⁺ ion is formed by removing two electrons from the neutral nitrogen atom. Electrons are removed from the outermost shell first, which in this case is the 2p orbital.
Remove two electrons from the 2p orbital. The new electron configuration becomes: 1s² 2s² 2p¹.
Verify the final configuration: The N²⁺ ion now has 5 electrons, and the configuration 1s² 2s² 2p¹ reflects the ground state of the ion.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It is represented using a notation that indicates the number of electrons in each subshell, following the Aufbau principle, Pauli exclusion principle, and Hund's rule. Understanding electron configuration is essential for predicting chemical behavior and bonding properties.
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Ionization

Ionization is the process of removing one or more electrons from an atom or molecule, resulting in the formation of an ion. In the case of N2+, two electrons are removed from a neutral nitrogen atom, which has an atomic number of 7. This process alters the electron configuration and affects the ion's chemical properties.
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Ground State

The ground state of an atom refers to the lowest energy configuration of its electrons. In this state, electrons occupy the lowest available energy levels according to the principles of quantum mechanics. For ions like N2+, determining the ground state configuration is crucial for understanding their stability and reactivity in chemical reactions.
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Related Practice
Textbook Question

The energies of the 4s4s, 4p4p, and 4d4d states of potassium are given in Example 41.1041.10. Calculate ZeffZ_{eff} for each state. What trend do your results show? How can you explain this trend?

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Textbook Question

The 5s5s electron in rubidium (Rb) sees an effective charge of 2.771e2.771e. Calculate the ionization energy of this electron.

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Textbook Question

The energies for an electron in the KK, LL, and MM shells of the tungsten atom are −69,500-69,500 eV, −12,000-12,000 eV, and −2,200-2,200 eV, respectively. Calculate the wavelengths of the KαK_{\(\alpha\)} and KβK_{\(\beta\)} x rays of tungsten.

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Textbook Question

Estimate the energy of the least strongly bound level in the LL shell of N2+.

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Textbook Question

Calculate the energy difference between the ms=12m_{s}=\(\frac\)12 ('spin up') and ms=−12m_{s}=-\(\frac\)12 ('spin down') levels of a hydrogen atom in the 1s1s state when it is placed in a 1.451.45 T magnetic field in the negative zz-direction. Which level, ms=12m_{s}=\(\frac\)12 or ms=−12m_{s}=-\(\frac\)12, has the lower energy?

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