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Orbital Diagrams and Electron Configurations Draw the

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

Solution for problem 1PE Chapter 6.7SE

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

Orbital Diagrams and Electron Configurations Draw the orbital diagram for the electron configuration of oxygen, atomic number 8. How many unpaired electrons does an oxygen atom possess? How many of the elements in the second row of the periodic table (Li through Ne) will have at least one unpaired electron in their electron configurations? (a) 3 (b) 4 (c) 5 (d) 6 (e) 7

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Solution: Here, we are going to find the elements in the second row having at least one unpaired electron in their electronic configurations. 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 , x ay p ) z the p - 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. Step2: The elements of second row are Lithium(Li), Beryllium(Be), Boron(B), Carbon(C), Nitrogen(N), Oxygen(O), Fluorine(F) and Neon(Ne) The electronic configuration of the second row elements are given below: Step3: From the above table, it is clear that, the elements having unpaired electrons are Lithium, Boron, Carbon, Nitrogen, Oxygen and Fluorine. Therefore, number of elements in the second row having at least one unpaired electron in their electronic configurations is 6. Thus, the correct option is (d). -------------------

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Chapter 6.7SE, Problem 1PE is Solved
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Textbook: Chemistry: A Molecular Approach
Edition: 3
Author: Nivaldo J. Tro
ISBN: 9780321809247

This full solution covers the following key subjects: electron, orbital, oxygen, configurations, unpaired. This expansive textbook survival guide covers 82 chapters, and 9454 solutions. The answer to “Orbital Diagrams and Electron Configurations Draw the orbital diagram for the electron configuration of oxygen, atomic number 8. How many unpaired electrons does an oxygen atom possess? How many of the elements in the second row of the periodic table (Li through Ne) will have at least one unpaired electron in their electron configurations? (a) 3 (b) 4 (c) 5 (d) 6 (e) 7” is broken down into a number of easy to follow steps, and 64 words. This textbook survival guide was created for the textbook: Chemistry: A Molecular Approach, edition: 3. The full step-by-step solution to problem: 1PE from chapter: 6.7SE was answered by , our top Chemistry solution expert on 02/22/17, 04:35PM. Since the solution to 1PE from 6.7SE chapter was answered, more than 522 students have viewed the full step-by-step answer. Chemistry: A Molecular Approach was written by and is associated to the ISBN: 9780321809247.

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