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Chapter 20: Problem 3

Explain why atomic radii decrease very gradually from scandium to copper.

Short Answer

Expert verified
Atomic radii decrease gradually from scandium to copper due to the increase in nuclear charge which pulls the electrons closer to the nucleus, contracting the atomic radius. However, this decrease is gradual because electron-electron repulsion within the 3d and 4s shells slightly counteracts the greater nuclear pull, preventing a dramatic decrease in atomic radius.

Step by step solution

01

Understand Atomic Radius

Atomic radius describes the size of an atom. It is typically measured from the center of the nucleus to the boundary of the surrounding electron cloud. Across a period in the periodic table, atomic radii usually decrease because electrons are added to the same energy level while the nucleus becomes more positively charged due to the addition of protons. The increased positive charge attracts the electrons more strongly, pulling them closer to the nucleus, which decreases the atomic radius.
02

Analyze the Electron Configuration from Scandium to Copper

Beginning with Scandium (Sc), which has the electron configuration [Ar] 3d1 4s2, we move across the period to Copper (Cu), which has the electron configuration [Ar] 3d10 4s1. The number of protons increases from 21 in Sc to 29 in Cu. These additional protons cause an increase in the nuclear charge, pulling the shell electrons towards the nucleus and slightly decreasing the atomic radius.
03

Explain the Gradual Decrease

The decrease is gradual because electron-electron repulsion in the same energy level (3d and 4s shells) counteracts the increased pull of the nucleus. This repulsion prevents the atomic radius from decreasing dramatically. The additional 3d electrons do not completely shield the increased nuclear charge, allowing the atomic radius to decrease, but at a slow rate.

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Most popular questions from this chapter

Chromium exhibits several oxidation states in its compounds, whereas aluminum exhibits only the +3 oxidation state. Explain.

How many geometric isomers are in these species: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{4}\right]^{-},(\mathrm{b})\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3}\right] ?\)

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?

A student in 1895 prepared three chromium coordination compounds having the same formulas of \(\mathrm{CrCl}_{3}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\) with these properties: Write modern formulas for these compounds and suggest a method for confirming the number of \(\mathrm{Cl}^{-}\) ions present in solution in each case. (Hint: Some of the compounds may exist as hydrates, which are compounds that have a specific number of water molecules attached to them. The \(\mathrm{Cr}\) has a coordination number of 6 in all three compounds.)

A concentrated aqueous copper(II) chloride solution is bright green in color. When diluted with water, the solution becomes light blue. Explain.
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