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Chapter 23: Problem 8

Why is the number of common oxidation states for the elements at the beginning and those at the end of the first transition series less than for elements in the middle of the series?

Short Answer

Expert verified
The elements at the beginning and end of a series have fewer oxidation states because their 'd' orbitals are either empty or filled, causing 'd' electrons to be tightly bound and not readily participate in bonding. This is different from elements in the middle of the series which have more electrons in their 'd' orbitals, hence, more available electrons for bonding resulting in more common oxidation states.

Step by step solution

01

Understanding Transition Elements

Transition elements are the elements that are located in the d-block of the periodic table. These elements are characterized by their variable oxidation states.
02

Defining Oxidation States

Oxidation state is a concept in chemistry that allows the counting of electrons transferred to or from a substance in a redox reaction. The oxidation state can be a positive, negative, or zero number.
03

Explaining Oxidation States in Transition Elements

In a transition series, the number of oxidation states corresponds to the number of electrons in the outer 'd' orbitals that can participate in bond formation. This is why elements in the middle of a transition series typically have more common oxidation states, because they have more 'd' electrons that can be involved in forming bonds.
04

Explaining Lower Oxidation States at the Beginning and End

Elements at the beginning and end of a transition series have fewer common oxidation states as the 'd' orbital is empty or filled at the start, and at the end of the series, the 'd' electrons are tightly bound and do not readily participate in bonding.

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Most popular questions from this chapter

Complete and balance the following equations. If no reaction occurs, so state. (a) \(\operatorname{TiCl}_{4}(\mathrm{g})+\mathrm{Na}(1) \stackrel{\Delta}{\longrightarrow}\) (b) \(\mathrm{Cr}_{2} \mathrm{O}_{3}(\mathrm{s})+\mathrm{Al}(\mathrm{s}) \stackrel{\Delta}{\longrightarrow}\) (c) \(\mathrm{Ag}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \longrightarrow\) (d) \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}(\mathrm{aq})+\mathrm{KOH}(\mathrm{aq}) \longrightarrow\) (e) \(\mathrm{MnO}_{2}(\mathrm{s})+\mathrm{C}(\mathrm{s}) \stackrel{\Delta}{\longrightarrow}\)

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