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Chapter 20: Problem 1

What distinguishes a transition metal from a representative metal?

Short Answer

Expert verified
Transition and representative metals are distinguished based on their placement in the periodic table, electron arrangements, physical properties, and chemical behaviors. Transition metals, found in the d block of the periodic table, have two electrons in the outer shell and up to ten in an inner shell, are generally hard with high densities, form colored compounds, and can exist in multiple oxidation states. In contrast, representative metals, found in the s and p blocks, have varied numbers of electrons in their outer shells, are softer with lower densities, and typically exist in a single oxidation state.

Step by step solution

01

Understand Definitions

First, understand what a representative metal is and what a transition metal is. Representative metals, also known as main-group metals, belong to the s and p blocks of the periodic table. Transition metals belong to the d block.
02

Distinguish Based on Electron Arrangements

Transition metals have two electrons in the outer energy level and up to ten in the inner level. Representative metals vary in the number of electrons in their outer shell, but always have their s and possibly p orbitals filled.
03

Discuss Physical Properties

Next, compare the physical properties of the two types of metals. Transition metals are usually hard and have high densities, while representative metals are softer with lower densities.
04

Compare Chemical Behaviors

Compare the chemical behaviors of these metals. Transition metals often form colored compounds and have several oxidation states. Simultaneously, representative metals typically exist in a single oxidation state.

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Most popular questions from this chapter

Briefly describe the crystal field theory. Define the following terms: crystal field splitting, high-spin complex, low-spin complex, spectrochemical series.

Copper is also known to exist in +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?

What are the systematic names for these ions and compounds: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right]^{+},\) (b) \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3},\) (c) \(\left[\mathrm{Co}(\mathrm{en})_{2} \mathrm{Br}_{2}\right]^{+},\) (d) \(\mathrm{Fe}(\mathrm{CO})_{5} ?\)

Which of these hydrated cations are colorless: \(\mathrm{Fe}^{2+}(a q), \mathrm{Zn}^{2+}(a q), \mathrm{Cu}^{+}(a q), \mathrm{Cu}^{2+}(a q), \mathrm{V}^{5+}(a q)\) \(\mathrm{Ca}^{2+}(a q), \mathrm{Co}^{2+}(a q), \mathrm{Sc}^{3+}(a q), \mathrm{Pb}^{2+}(a q) ?\) Explain your choice.

As we read across the first-row transition metals from left to right, the +2 oxidation state becomes more stable in comparison with the +3 state. Why is this so?
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