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Chapter 24: Problem 69

Explain the important distinction between each of the following pairs: (a) coordination number and oxidation number; (b) monodentate and polydentate ligands; (c) cis and trans isomers; (d) dextrorotatory and levorotatory compounds; (e) low-spin and highspin complexes.

Short Answer

Expert verified
A: Coordination number refers to the total number of ligands attached to a central atom, oxidation number indicates the degree of oxidation or reduction of an atom. B: Monodentate ligands bind at a single point, polydentate ligands bind at multiple points. C: In cis isomers, functional groups are on the same side; in trans, on opposite sides. D: Dextrorotatory compounds rotate light clockwise, levorotatory counterclockwise. E: High spin complexes maximize total spin by occupying all orbitals singly first, low spin complexes minimize total spin by pairing electrons in lower energy orbitals first.

Step by step solution

01

Distinction A

Coordination number refers to the total number of ligands that are directly attached to a metal ion in a complex ion or a compound, while the oxidation number is a concept in chemistry that indicates the degree of oxidation or reduction of an atom in a chemical compound.
02

Distinction B

Monodentate ligands are ligands that bind to a central atom at a single point, usually through one atom. Polydentate ligands, on the other hand, bind to a central atom at multiple points. They are often referred to as chelating ligands due to the way they 'hold' the central atom like a claw.
03

Distinction C

Cis and trans isomers are terms used to describe the orientation of functional groups within a molecule. In cis isomers, functional groups are on the same side of the molecule. In trans isomers, functional groups are on opposite sides of the molecule.
04

Distinction D

Dextrorotatory and levorotatory compounds refer to the direction in which these compounds rotate plane-polarized light. Dextrorotatory substances rotate light clockwise, and are denoted by a positive rotation angle. Levorotatory substances rotate light counter clockwise and are denoted by a negative rotation angle.
05

Distinction E

Low-spin and high-spin complexes refer to the differences in electron configuration in transition metal complexes. A high-spin complex is one where the electrons prefer to occupy all orbitals singly before any pairing occurs, maximizing the total spin. A low-spin complex is one where electron pairing occurs in lower energy orbitals before the higher energy ones are occupied, minimizing total spin.

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Most popular questions from this chapter

Explain the following observations in terms of complex-ion formation. (a) \(\mathrm{Al}(\mathrm{OH})_{3}(\mathrm{s})\) is soluble in \(\mathrm{NaOH}(\mathrm{aq})\) but insoluble in \(\mathrm{NH}_{3}(\mathrm{aq})\) (b) \(\mathrm{ZnCO}_{3}(\mathrm{s})\) is soluble in \(\mathrm{NH}_{3}(\mathrm{aq}),\) but \(\mathrm{ZnS}(\mathrm{s})\) is not. (c) The molar solubility of AgCl in pure water is about \(1 \times 10^{-5} \mathrm{M} ;\) in \(0.04 \mathrm{M} \mathrm{NaCl}(\mathrm{aq}),\) it is about \(2 \times 10^{-6}; \mathrm{M}\) but in \(1 \mathrm{M} \mathrm{NaCl}(\mathrm{aq}),\) it is about \(8 \times 10^{-5} \mathrm{M}\).

In your own words, describe the following terms or symbols: (a) coordination number; (b) \(\Delta_{\mathrm{o}} ;\) (c) ammine complex; (d) enantiomer.

Write equations to represent the following observations. (a) A quantity of \(\mathrm{CuCl}_{2}(\mathrm{s})\) is dissolved in concentrated HCl(aq) and produces a yellow solution. The solution is diluted to twice its volume with water and assumes a green color. On dilution to ten times its original volume, the solution becomes pale blue. (b) When chromium metal is dissolved in \(\mathrm{HCl}(\mathrm{aq}), \mathrm{a}\) blue solution is produced that quickly turns green. Later the green solution becomes blue-green and then violet.

What are the coordination number and the oxidation state of the central metal ion in each of the following complexes? Name each complex. (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\) (b) \(\left[\mathrm{AlF}_{6}\right]^{3-}\) (c) \(\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]^{2-}\) (d) \(\left[\operatorname{CrBr}_{2}\left(\mathrm{NH}_{3}\right)_{4}\right]^{+}\) (e) \(\left[\operatorname{Co}(\text { ox })_{3}\right]^{4-}\) (f) \(\left[\mathrm{Ag}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}\right]^{3-}\)

Draw plausible structures corresponding to each of the following names. (a) pentamminesulfatochromium(III) ion (b) trioxalatocobaltate(III) ion (c) triamminedichloronitrito-O-cobalt(III)
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