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Ch.6 - Electronic Structure of Atoms
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.6 - Electronic Structure of AtomsProblema 67b
Capitolo 6, Problema 67b

(b) If we add one electron to form the He atom, would your answer to part (a) change?

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Identify the original atom or ion discussed in part (a) and its electron configuration.
Understand that adding one electron to the He atom would change its electron configuration and potentially its stability.
Consider the effect of adding an electron on the atomic radius and the overall charge of the atom.
Analyze how the change in electron configuration affects the chemical properties of the atom, such as reactivity and ionization energy.
Conclude whether these changes would alter the answer provided in part (a) based on the properties discussed.

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Atomic Structure

Atomic structure refers to the arrangement of protons, neutrons, and electrons within an atom. In the case of helium (He), it has two protons and two neutrons in its nucleus, with two electrons orbiting around it. Understanding atomic structure is crucial for analyzing how adding or removing electrons affects the atom's properties and behavior.
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Atom Structure

Ionization and Electron Configuration

Ionization involves the addition or removal of electrons from an atom, leading to the formation of ions. When an electron is added to a neutral helium atom, it becomes a negatively charged ion (He-). This change in electron configuration can significantly alter the atom's chemical properties and reactivity, which is essential for answering the question.
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Electron Configuration Example

Chemical Properties of Elements

The chemical properties of elements are determined by their electron configurations, particularly the arrangement of valence electrons. Adding an electron to helium changes its electron configuration, which can influence its reactivity and interactions with other elements. Understanding these properties is vital for predicting how the atom will behave in different chemical contexts.
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Chemical Properties
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Domanda del libro di testo

Two possible electron configurations for an Li atom are shown here. (c) In the absence of an external magnetic field, can we say that one electron configuration has a lower energy than the other? If so, which one has the lowest energy?

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(a) For an He+ ion, do the 2s and 2p orbitals have the same energy? If not, which orbital has a lower energy?

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(b) Would you expect it to require more or less energy to remove a 3s electron from the chlorine atom, as compared with a 2p electron?

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(a) The average distance from the nucleus of a 3s electron in a chlorine atom is smaller than that for a 3p electron. In light of this fact, which orbital is higher in energy?

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(b) Identify the number of nodes; that is, identify places where the electron density is zero, in the 2px orbital; in the 3s orbital.

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(d) For the hydrogen atom, list the following orbitals in order of increasing energy: 3s, 2s, 2p, 5s, 4d.

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