Ch.6 - Electronic Structure of Atoms

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.6 - Electronic Structure of Atoms

Problem 73c

Chapter 6, Problem 73c

(c) What does each box in an orbital diagram represent?

Verified step by step guidance

Understand that an orbital diagram is a visual way to represent the electron configurations of atoms or ions.

Recognize that each box in an orbital diagram represents an orbital, which is a region in an atom where there is a high probability of finding electrons.

Note that each orbital can hold a maximum of two electrons, which must have opposite spins, as indicated by arrows pointing in opposite directions (up and down).

Identify that the arrangement of boxes follows the order of increasing energy levels and sublevels, starting from the lowest energy (1s) to higher energies (2s, 2p, 3s, etc.).

Realize that the filling of these orbitals by electrons in the boxes follows the Pauli Exclusion Principle and Hund's Rule, ensuring that electrons occupy the lowest energy orbitals available and that electrons in the same sublevel occupy different orbitals before pairing up.

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Key Concepts

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

Orbital Diagrams

Orbital diagrams are visual representations of the electron configurations of atoms. Each box in the diagram corresponds to an atomic orbital, which can hold a maximum of two electrons with opposite spins. These diagrams help illustrate how electrons are distributed among the various orbitals in an atom, following the principles of quantum mechanics.

Quantum Mechanics

Quantum mechanics is the branch of physics that describes the behavior of matter and energy at the atomic and subatomic levels. It introduces concepts such as wave-particle duality and quantization of energy levels, which are essential for understanding how electrons occupy orbitals and the shapes and orientations of these orbitals in an atom.

Pauli Exclusion Principle

The Pauli Exclusion Principle states that no two electrons in an atom can have the same set of four quantum numbers. This principle is crucial for understanding the arrangement of electrons in orbitals, as it dictates that each box in an orbital diagram can hold a maximum of two electrons, each with opposite spins, ensuring that the electron configuration adheres to this fundamental rule.

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Textbook Question

(a) What are 'valence electrons'?

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Textbook Question

What is the maximum number of electrons that can occupy each of the following subshells? a. 3p, b. 5d, c. 2s, d. 4f.

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Textbook Question

For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: a. nitrogen

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Textbook Question

What is the maximum number of electrons in an atom that can have the following quantum numbers? a. n = 3, ml = -2; b. n = 4, l = 3; c. n = 5, l = 3, ml = 2; d. n = 4, l = 1, ml = 0.

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Textbook Question

For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: c. chlorine

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