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Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

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Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 7.4, Problem 1CYU
Textbook Problem
4721 views

Depict the electron configurations for V2+, V3+, and Co3+. Use orbital box diagrams and the noble gas notation. Are any of the ions paramagnetic? If so, give the number of unpaired electrons.

Interpretation Introduction

Interpretation:

The electronic configurations forV2+, V3+, and Co3+ions and orbital box diagrams and the noble gas notation and its paramagnetic properties have to be identified.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons (e-) of a given molecule or respective atoms in atomic or molecular orbitals.

Paramagnetic: The Paramagnetic properties are due to the presence of unpaired electrons, and from the realignment of the electron paths caused by the external magnetic field.

Diamagnetic properties: In diamagnetic materials all the electron are paired so there is no permanent net magnetic moment per atom.

Explanation of Solution

Electronic configuration of Vanadium atom: It has two electrons in the (4s) orbitals and three electrons in 3d orbitals, the electrons filling method presented below.

AtomicnumberofVanadium(V)= 23spdfwith noble gas notation=[Ar]3d34s2Orbitalboxnotation       = [Ar]3d34s2

Electronic configuration of Vanadium (II) ion: When (V) was oxidized to V2+ions, it lost for two electrons in outermost (4s) orbitals.

  spdfwith noble gas notation=[Ar]3d34s0Orbitalboxnotation       = [Ar]3d34s0

Electronic configuration of Vanadium (III) ion: Again the Vanadium (III) ion is formed by removing even one electron from Vanadium (II) ion of d-orbitals as shown below,

  spdfwith noble gas notation=[Ar]3d24s0Orbitalboxnotation       = [Ar]3d24s0

Electronic configuration of cobalt atom: It has two electrons in the (4s) orbitals and (7) electrons in 3d orbitals, the electrons filling method presented below

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Chapter 7 Solutions

Chemistry & Chemical Reactivity
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