Textbook Question
Assign a systematic name to each of the following ions.
(a) [AuCl4]-
(b) [Fe(CN)6]4-
1
views
Ch.21 - Transition Elements and Coordination Chemistry
McMurry8th EditionChemistryISBN: 9781292336145
Not the one you use?Change textbookSelect a different textbook
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
All textbooks
McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.27b
McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.27bChapter 21, Problem 21.27b
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+
Verified step by step guidance1
Step 1: Identify the atomic number of the transition metal. The atomic number is the number of protons in an atom, which also equals the number of electrons in a neutral atom. You can find this information in the periodic table.
Step 2: Write the electron configuration for the neutral atom. The electron configuration describes the distribution of electrons in an atom's electron shells. It follows the Aufbau principle, which states that electrons fill the lowest energy levels first. For example, the electron configuration of a neutral atom of iron (Fe), which is a transition metal with an atomic number of 26, is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶.
Step 3: Adjust the electron configuration for the ion. When a transition metal ion loses electrons, it first loses the electrons in the highest energy level (the outermost shell). In the case of a Fe²⁺ ion, it would lose the two 4s electrons, resulting in the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶.
Step 4: Repeat steps 1-3 for each ion. Remember that the charge of the ion indicates the number of electrons lost (for positive ions) or gained (for negative ions).
Step 5: Keep in mind that some transition metals can have exceptions to the Aufbau principle due to the stability of half-filled or fully filled d sub-levels. For example, chromium (Cr) and copper (Cu) have electron configurations that differ from what would be predicted by the Aufbau principle.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
4mWas this helpful?
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. For transition metals, the electron configuration can be complex due to the involvement of d orbitals, and it is crucial to understand how to write configurations for both neutral atoms and their ions.
Recommended video:
Guided course
01:33
Electron Configuration Example
Ionic Charge and Electron Loss
Ionic charge indicates the number of electrons an atom has lost or gained to form an ion. For example, a 2+ charge means the atom has lost two electrons. In transition metals, the loss of electrons typically occurs from the outermost s and d orbitals, which is essential for determining the correct electron configuration of the resulting ion.
Recommended video:
Guided course
01:53Formal Charge
Periodic Table and Transition Metals
The periodic table organizes elements based on their atomic number and electron configurations. Transition metals are found in groups 3 to 12 and are characterized by their ability to form variable oxidation states. Understanding the position of elements A, B, C, and D in the periodic table helps predict their electron configurations and the behavior of their ions.
Recommended video:
Guided course
01:23Transition Metal Example
Related Practice
Textbook Question
Two first-series transition metals have three unpaired electrons in complex ions of the type [MCl4]2-.
(a) What are the oxidation state and the identity of M in these complexes?
(b) Draw valence bond orbital diagrams for the two possible ions.
(c) Based on common oxidation states of first-series transition metals (Figure 21.6), which ion is more likely to exist?
<QUESTION REFERENCES FIGURE 21.6>
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?
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)
Textbook Question
Tell how many diastereoisomers are possible for each of the following complexes, and draw their structures.
(c) [Cu(H2O)4Cl2]+
(d) Ru(NH3)3I3
Textbook Question
Assign a systematic name to each of the following ions.
(c) [Fe(H2O)5NCS]2+
(d) [Cr(NH3)2(C2O4)2]-
1
views