Textbook Question
Draw the structure of all isomers of the octahedral complex [NbX2Cl4]- (X- = NCS-), and identify those that are linkage isomers.
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Ch.21 - Transition Elements and Coordination Chemistry
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 21, Problem 21.39
Predict the number of unpaired electrons for each of the following.
(a) Sc3+
(b) Co2+
Verified step by step guidance1
Determine the electron configuration of the neutral atom for each element.
For Scandium (Sc), the atomic number is 21, so the electron configuration is [Ar] 3d^1 4s^2.
For Cobalt (Co), the atomic number is 27, so the electron configuration is [Ar] 3d^7 4s^2.
Remove electrons according to the charge of the ion. For Sc^3+, remove three electrons from the outermost orbitals, resulting in [Ar].
For Co^2+, remove two electrons from the outermost orbitals, resulting in [Ar] 3d^7. Determine the number of unpaired electrons in the 3d subshell.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electron Configuration
Electron configuration describes the distribution of electrons in an atom's orbitals. It follows the Aufbau principle, which states that electrons fill lower-energy orbitals first. Understanding the electron configuration of an element is crucial for predicting its chemical behavior, including the number of unpaired electrons.
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Electron Configuration Example
Unpaired Electrons
Unpaired electrons are those that occupy an orbital alone, without a partner of opposite spin. The presence of unpaired electrons in an atom influences its magnetic properties and reactivity. Atoms with unpaired electrons are often paramagnetic, while those with all electrons paired are diamagnetic.
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Transition Metals and Oxidation States
Transition metals can exhibit multiple oxidation states due to their ability to lose different numbers of d electrons. The oxidation state affects the electron configuration and, consequently, the number of unpaired electrons. For example, Scandium (Sc) in the +3 oxidation state loses three electrons, while Cobalt (Co) in the +2 state loses two, altering their electron configurations.
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Related Practice
Textbook Question
Which of the following complexes can exist as enantiomers? Draw their structures.
(a) [Cr(en)3]3+
(b) cis-[Co(NH3)Cl]2+
(c) trans-[Co(en)2(NH3)Cl]2+
(d) [Pt(NH3)3Cl3]+
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Textbook Question
Predict the crystal field energy-level diagram for a linear ML2 complex that has two ligands along the :
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Textbook Question
Constitutional isomers of a ruthenium(II) coordination compound are shown below.
(a) Give the formula and name for structures 1-3.
(b) Which structures are linkage isomers?
(c) Which structures are ionization isomers?
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Textbook Question
Nickel(II) complexes with the formula NiX2L2, where X− is Cl− or N-bonded NCS− and L is the monodentate triphenylphosphine ligand P(C6H5)3, can be square planar or tetrahedral.
(a) Draw crystal field energy-level diagrams for a square planar and a tetrahedral nickel(II) complex, and show the population of the orbitals.
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Textbook Question
Assign a systematic name to each of the following ions.
(a) [AuCl4]-
(b) [Fe(CN)6]4-
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