Textbook Question
What is the systematic name for each of the following ions?
(c) [Co(CO3)3]3-
(d) [Pt(en)2(SCN)2]2+
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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
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McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.38b
McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.38bChapter 21, Problem 21.38b
Predict the number of unpaired electrons for each of the following.
(c) Mn3+
(d) Cr2+
Verified step by step guidance1
Step 1: Determine the electron configuration of the neutral atom. For Mn (Manganese), the electron configuration is [Ar] 4s2 3d5. For Cr (Chromium), the electron configuration is [Ar] 4s1 3d5.
Step 2: Remove electrons to account for the positive charge. For Mn3+, remove three electrons. The first two electrons are removed from the 4s orbital, and the third electron is removed from the 3d orbital, resulting in the electron configuration [Ar] 3d4. For Cr2+, remove two electrons. The first electron is removed from the 4s orbital, and the second electron is removed from the 3d orbital, resulting in the electron configuration [Ar] 3d4.
Step 3: Determine the number of unpaired electrons by looking at the electron configuration. For Mn3+, there are four unpaired electrons in the 3d orbital. For Cr2+, there are also four unpaired electrons in the 3d orbital.
Step 4: Remember that unpaired electrons are responsible for the magnetic properties of an atom or ion. The more unpaired electrons, the stronger the magnetic properties.
Step 5: Practice predicting the number of unpaired electrons for different atoms and ions to become more comfortable with this process.
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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. For transition metals, this involves filling the 3d and 4s orbitals according to the Aufbau principle, Hund's rule, and the Pauli exclusion principle. Understanding the electron configuration of an element is crucial for predicting its chemical properties, including the number of unpaired electrons.
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Electron Configuration Example
Unpaired Electrons
Unpaired electrons are electrons that occupy an orbital alone rather than in pairs. The presence of unpaired electrons in an atom contributes to its magnetic properties and reactivity. In transition metals, the number of unpaired electrons can be determined by examining the electron configuration and identifying how many electrons are in the d orbitals without a partner.
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Oxidation States
Oxidation states indicate the degree of oxidation of an atom in a compound, reflecting the number of electrons lost or gained. For transition metals, oxidation states can affect the electron configuration significantly. For example, Mn in Mn3+ has lost three electrons, which alters its electron configuration and the number of unpaired electrons compared to its neutral state.
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Related Practice
Textbook Question
For each of the following complexes, describe the bonding using valence bond theory. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons.
(b) [Ag(NH3)2]+
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Textbook Question
Cobalt(III) trifluoroacetylacetonate, Co(tfac)3, is a sixcoordinate, octahedral metal chelate in which three planar, bidentate tfac ligands are attached to a central Co atom:
(b) Diastereoisomers A and B have dipole moments of 6.5 D and 3.8 D, respectively. Which of your diastereoisomers is A and which is B?
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Textbook Question
Give a valence bond description of the bonding in each of the following complexes. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons.
(b) [NiBr4]2- (tetrahedral)
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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.
(b) If NiCl2L2 is paramagnetic and Ni(NCS)2L2 is diamagnetic, which of the two complexes is tetrahedral and which is square planar?
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Textbook Question
Look at the location in the periodic table of elements A, B, C, and D. What is the electron configuration of the transition metal in each of the following ions?
(a) A2+
(b) B+
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