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?Sketch the shape and orientation of the following types of orbitals: (a) \(p_{x}\), (b) \(d_{z^{2}}\), (c) \(d_{x^{2}-y^

Chemistry: The Central Science | 14th Edition | ISBN: 9780134414232 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus ISBN: 9780134414232 1274

Solution for problem 6.64 Chapter 6

Chemistry: The Central Science | 14th Edition

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Chemistry: The Central Science | 14th Edition | ISBN: 9780134414232 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus

Chemistry: The Central Science | 14th Edition

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Problem 6.64

Sketch the shape and orientation of the following types of orbitals:

(a) \(p_{x}\),

(b) \(d_{z^{2}}\),

(c) \(d_{x^{2}-y^{2}}\).

Text Transcription:

p_x,

d_z2,

d_x2 - y2

Step-by-Step Solution:

Step 1 of 5) The bonding between manganese and oxygen is not always ionic. Manganese(VII) oxide, Mn2O7, is a green liquid that freezes at 5.9 °C, an indication that covalent rather than ionic bonding dominates. The change in the oxidation state of manganese is responsible for the change in bonding. In general, as the oxidation state of a metal increases, so does the degree of covalent bonding. When the oxidation state of the metal is highly positive (roughly speaking, +4 or larger), we can expect significant covalency in the bonds it forms with nonmetals. Thus, metals in high oxidation states form molecular substances, such as Mn2O7, or polyatomic ions, such as MnO4 - and CrO4 2 - , rather than ionic compounds. Sum the valence electrons from all atoms, taking into account overall charge. Use the periodic table to help you determine the number of valence electrons in each atom. For an anion, add one electron to the total for each negative charge. For a cation, subtract one electron from the total for each positive charge. Do not worry about keeping track of which electrons come from which atoms. Only the total number is important.

Step 2 of 2

Chapter 6, Problem 6.64 is Solved
Textbook: Chemistry: The Central Science
Edition: 14
Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
ISBN: 9780134414232

Since the solution to 6.64 from 6 chapter was answered, more than 222 students have viewed the full step-by-step answer. Chemistry: The Central Science was written by and is associated to the ISBN: 9780134414232. The full step-by-step solution to problem: 6.64 from chapter: 6 was answered by , our top Chemistry solution expert on 10/03/18, 06:29PM. This textbook survival guide was created for the textbook: Chemistry: The Central Science, edition: 14. The answer to “?Sketch the shape and orientation of the following types of orbitals: (a) \(p_{x}\), (b) \(d_{z^{2}}\), (c) \(d_{x^{2}-y^{2}}\).Text Transcription:p_x, d_z2, d_x2 - y2” is broken down into a number of easy to follow steps, and 22 words. This full solution covers the following key subjects: . This expansive textbook survival guide covers 29 chapters, and 2820 solutions.

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?Sketch the shape and orientation of the following types of orbitals: (a) \(p_{x}\), (b) \(d_{z^{2}}\), (c) \(d_{x^{2}-y^