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Electron Configurations for a Group What is the

Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro ISBN: 9780321809247 1

Solution for problem 1PE Chapter 6.8SE

Chemistry: A Molecular Approach | 3rd Edition

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Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro

Chemistry: A Molecular Approach | 3rd Edition

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Problem 1PE

Electron Configurations for a Group What is the characteristic valence electron configuration of the group 7 A elements, the halogens? A certain atom has an ns2np6 electron configuration in its outermost occupied shell. Which of the following elements could it be? (a) Be (b) Si (c) I (d) Kr (e) Rb

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Solution: Here, we are going to identify the element having outermost electronic 2 6 configuratio n s . Step1: The distribution of electrons in different orbitals is known as electronic configuration of the atom. The filling of orbitals are governed by the following rules: a) Aufbau principle: The Aufbau principle states that in the ground state(lowest energy state) of an atom, an electron enters the orbital of lowest energy first and subsequent electrons are fed in the order of increasing energies. The orbital should be filled in the following sequence: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, ………. b) Pauli’s exclusion principle: According to this principle an orbital can accommodate maximum of two electrons and these must have opposite spins. c) Hund’s rule of maximum multiplicity: According to this rule, electron pairing will not take place in orbitals of same energy(subshell) until each orbital is singly filled. For example, there are three p- orbitals(p , p andx yof thez - subshell in a principal energy level. According to Hund’s rule, each of the three p-orbitals must get one electron of parallel spin before any one of them receives the second electron of opposite spin. The three rules are applied simultaneously to get the electronic configuration. In writing the electronic configuration, an orbital is shown by using its proper symbol.The number of electrons present in an orbital is shown as the right-hand superscript of the symbol of the orbital. 1 For example, the electronic configuration of hydrogen is 1s . This means that the single electron in hydrogen occupies the s orbital present in the principal energy level n = 1. Similarly the electronic configuration of other elements are written. Furthermore, for simplicity a common convention is used. In this, the detailed electronic configuration of the noble gas core preceding the valence shell is represented by the symbol of the noble gas in square brackets. Then, the configuration of the valence shell is written after the symbol. For example, the electronic configuration of sodium may be written as Na(Z = 11) : [Ne]3s Step2: n np 6is a fulfilled configuration, i.e., all the orbitals are completely occupied. Out of all the elements in the periodic table, only the noble gases have all fully occupied orbitals as shown below: Thus, the correct option is (d). -----------------

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Chapter 6.8SE, Problem 1PE is Solved
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Textbook: Chemistry: A Molecular Approach
Edition: 3
Author: Nivaldo J. Tro
ISBN: 9780321809247

The full step-by-step solution to problem: 1PE from chapter: 6.8SE was answered by , our top Chemistry solution expert on 02/22/17, 04:35PM. Since the solution to 1PE from 6.8SE chapter was answered, more than 885 students have viewed the full step-by-step answer. This textbook survival guide was created for the textbook: Chemistry: A Molecular Approach, edition: 3. The answer to “Electron Configurations for a Group What is the characteristic valence electron configuration of the group 7 A elements, the halogens? A certain atom has an ns2np6 electron configuration in its outermost occupied shell. Which of the following elements could it be? (a) Be (b) Si (c) I (d) Kr (e) Rb” is broken down into a number of easy to follow steps, and 51 words. Chemistry: A Molecular Approach was written by and is associated to the ISBN: 9780321809247. This full solution covers the following key subjects: electron, configuration, elements, Group, atom. This expansive textbook survival guide covers 82 chapters, and 9454 solutions.

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