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Chapter 23: Problem 19

Define the following terms: stereoisomers, geometric isomers, optical isomers, and plane-polarized light.

Short Answer

Expert verified
Stereoisomers are isomers with different spatial arrangement of atoms. Geometric isomers, a type of stereoisomer, have the same atoms but different positions due to restricted rotation around a bond. Optical isomers, another type of stereoisomers, are non-superimposable mirror images of each other. Plane-polarized light refers to light waves oscillating in one plane, often used in determining optical activity of substances.

Step by step solution

01

Defining Stereoisomers

Stereoisomers are a type of isomers where the atoms have the same connectivity but different spatial arrangements. They are molecules composed of the same atoms and bonds but differ in the 3D orientation of the atoms in space.
02

Defining Geometric Isomers

Geometric isomers, also known as cis-trans isomers, are a type of stereoisomers. They occur when the rotation around a certain bond is restricted or prevented. This restriction allows the same atoms to occupy different positions in space without breaking any bonds, hence creating different isomers.
03

Defining Optical Isomers

Optical isomers, also known as enantiomers, are a type of stereoisomers. They are pair of molecules which are non-superimposable mirror images of each other. This means, there is no possible orientation or rotation where all the atoms in two optical isomers will align.
04

Defining Plane-Polarized Light

Plane-polarized light refers to light waves that oscillate in a single plane. When light passes through a polarizer (like a polarizing filter), it becomes plane-polarized. This property of light is crucial in determining the optical activity of substances.

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Most popular questions from this chapter

Copper is also known to exist in the +3 oxidation state, which is believed to be involved in some biological electron-transfer reactions. (a) Would you expect this oxidation state of copper to be stable? Explain. (b) Name the compound \(\mathrm{K}_{3} \mathrm{CuF}_{6}\) and predict the geometry of the complex ion and its magnetic properties. (c) Most of the known Cu(III) compounds have square planar geometry. Are these compounds diamagnetic or paramagnetic?

The \(K_{\mathrm{f}}\) for the complex ion formation between \(\mathrm{Pb}^{2+}\) and EDTA \(^{4-}\) $$ \mathrm{Pb}^{2+}+\mathrm{EDTA}^{4-} \rightleftharpoons \mathrm{Pb}(\mathrm{EDTA})^{2-} $$ is \(1.0 \times 10^{18}\) at \(25^{\circ} \mathrm{C} .\) Calculate \(\left[\mathrm{Pb}^{2+}\right]\) at equilibrium in a solution containing \(1.0 \times 10^{-3} M \mathrm{~Pb}^{2+}\) and \(2.0 \times 10^{-3} M \mathrm{EDTA}^{4-}\)

For the same type of ligands, explain why the crystal field splitting for an octahedral complex is always greater than that for a tetrahedral complex.

Define the following terms: coordination compound, ligand, donor atom, coordination number, and chelating agent.

Aqueous copper(II) sulfate solution is blue in color. When aqueous potassium fluoride is added, a green precipitate is formed. When aqueous potassium chloride is added instead, a bright-green solution is formed. Explain what is happening in these two cases.
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