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Ch.23 - Transition Metals and Coordination Chemistry
All textbooksBrown 14th EditionCh.23 - Transition Metals and Coordination ChemistryProblem 11
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Chapter 23, Problem 11

Complete the exercises below. The lanthanide contraction explains which of the following periodic trends? a. The atomic radii of the transition metals first decrease and then increase when moving horizontally across each period. b. When forming ions, the period 4 transition metals lose their 4s electrons before their 3d electrons. c. The radii of the period 5 transition metals (Y–Cd) are very similar to the radii of the period 6 transition metals (Lu–Hg).

Verified step by step guidance
1
Step 1: Understand the concept of lanthanide contraction. The lanthanide contraction refers to the phenomenon where the atomic radii of the lanthanide series elements decrease progressively with increasing atomic number, despite having similar electron configurations.
Step 2: Analyze how lanthanide contraction affects periodic trends. The contraction is due to poor shielding of the nuclear charge by the f-electrons, leading to a stronger attraction between the nucleus and the outer electrons.
Step 3: Evaluate option (a). Consider how the atomic radii of transition metals change across a period. This trend is more related to the filling of d-orbitals and not directly explained by lanthanide contraction.
Step 4: Evaluate option (b). Consider the electron configuration of period 4 transition metals and how they lose electrons. This behavior is due to energy considerations of 4s and 3d orbitals, not lanthanide contraction.
Step 5: Evaluate option (c). Compare the radii of period 5 and period 6 transition metals. The lanthanide contraction causes the radii of period 6 transition metals to be similar to those of period 5, as the contraction offsets the expected increase in size.
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Related Practice
Open Question
Complete the exercises below. a. A compound with formula RuCl₃ • 5H₂O is dissolved in water, forming a solution that is approximately the same color as the solid. Immediately after forming the solution, the addition of excess AgNO₃ (aq) forms 2 mol of solid AgCl per mole of complex. Write the formula for the compound, showing which ligands are likely to be present in the coordination sphere.
Textbook Question

Which of these crystal-field splitting diagrams represents:

a. a weak-field octahedral complex of Fe³⁺ ,

b. a strong-field octahedral complex of Fe³⁺ 

c. a tetrahedral complex of Fe³⁺

d. a tetrahedral complex of Ni²⁺ (The diagrams do not indicate the relative magnitudes of ∆. ) [Find more in Section 23.6.]

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Textbook Question

In the linear crystal-field shown here, the negative charges are on the z-axis. Using Figure 23.28 as a guide, predict which of the following choices most accurately describes the splitting of the d orbitals in a linear crystal-field? [Find more in Section 23.6.]                                                                                                                                                

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Open Question
Complete the exercises below. Which periodic trend is partially responsible for the observation that the maximum oxidation state of the transition-metal elements peaks near groups 7B and 8B? a. The number of valence electrons reaches a maximum at group 8B. b. The effective nuclear charge increases on moving right across each period. c. The radii of the transition-metal elements reach a minimum for group 8B, and as the size of the atoms decreases it becomes easier to remove electrons.
Open Question
Complete the exercises below. For each of the following compounds, determine the electron configuration of the transition-metal ion. a. TiO, b. TiO₂, c. NiO, d. ZnO.
Open Question
Among the period 4 transition metals (Sc–Zn), which elements do not form ions with partially filled 3d orbitals?