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Chapter 18: Problem 7

Discuss the variation of ionisation potential across a transition series.

Short Answer

Expert verified
Generally, ionisation potential increases across a transition series due to increased nuclear charge. However, exceptions exist in the case of chromium and copper where the ionisation potential is lower due to entering of the last electron into the inner d-orbital resulting in increased stability and hence, lower ionisation potential.

Step by step solution

01

Understanding the Trend

In general, across a transition series, the ionisation potential increases. This is due to the increase in nuclear charge as you move across the series. This increased nuclear charge results in stronger attraction between the nucleus and the outermost electron. This means that more energy (higher ionisation potential) is required to remove this electron.
02

Identifying the Exceptions

There are exceptions to this general trend. The ionisation potential of chromium and copper is less than that of their preceding elements (iron, cobalt and nickel). This is due to the fact that in these elements (chromium and copper), the last electron enters the inner d-orbital instead of the outer s-orbital, resulting in increased stability and hence, lower ionisation potential.
03

Understanding the Cause of Exceptions

The lowered ionisation potential in the case of chromium and copper is due to the symmetry and increased stability provided by a completely filled or half-filled d-subshell. These configurations result in lower energy and hence, lower ionisation potential.

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Most popular questions from this chapter

Explain the following properties of transition elements: (a) Catalytic properties (b) Magnetic properties

Give reasons for the following: (a) Scandium forms colourless and diamagnetic compounds (b) Transition metals show variable oxidation state (c) Transition metals form complexes (d) Transition metals act as a catalyst

What are the characteristic properties of transition elements?

Why do copper and chromium have exceptional electronic configuration.

Give reasons for the following (a) \(\mathrm{Mn}^{2+}\) shows the maximum magnetic character among the divalent ions of \(3 d\) -transition series. (b) \(\mathrm{Cu}^{+}\) is diamagnetic but \(\mathrm{Cu}^{2+}\) is paramagnetic. (c) Transition metals have high electrode potential but they are not good reducing agents. (d) Alkali metals are more reactive than transition metals
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