effective nuclear charge
Why are cesium atoms so big? Cesium has a large valence shell and a relatively low effective nuclear charge. The valence shell (the outer 'peel' of the atom) is largest in atoms at the bottom of the periodic table. A low nuclear charge means that electrons can wander further, on average, from the nucleus. Nuclear charge increases going left to right across table rows, so the largest atoms should be found on the left edge of the table.
Does having such large atoms make any difference in cesium's properties? Yes. Cesium is one of the most reactive elements known, partially because its atoms are so large. Cesium's lone valence electron is so far away from the nucleus on average that it is very easily removed. The electron is taken from cesium by other substances in violent chemical reactions. Cesium bursts into flames on contact with oxygen in air. Water and even ice reacts more violently with cesium than any of the other common metals:
2 Cs(s) + 2 H2O() 2 CsOH(aq) + H2(g)
Why aren't francium atoms the biggest? The usual periodic trend for atomic size places larger atoms at the left of a row and towards the bottom of a column on the periodic table. It's no surprise that cesium is large. But shouldn't francium, in the next period with an even larger valence shell, be even larger?
The answer is "possibly, but we just don't know yet." Francium isn't easy to study. It's the least stable of the first 103 elements; the most stable Fr isotope has a half-life of just 22 minutes . The distance between atoms in metallic francium has not yet been measured.
How can we predict the atomic radius of francium? We can try to predict unknown properties by extrapolating the properties of its 'brothers and sisters' in the same family. The simple extrapolation of the atomic radius trend for the alkali metals in the graph at left suggests that francium is definitely a contender for largest atom. However, as a period 7 element, francium is subject to a phenomena called the "lanthanide contraction". Elements with filled 4f subshells are smaller than might otherwise expected. The intervention of the lanthanides increases the effective nuclear charge, which offsets the size increase expected from filling the n=6 valence shell. As a consequence, sixth period transition metals are about the same size as their fifth period counterparts. The lanthanide contraction may make francium's atoms only slightly larger than those of cesium. In fact, they may even be slightly smaller.
|Current research and facts about francium, the most unstable element of the first 103.|
Author: Fred Senese email@example.com
Copyright © 1997-2010 by Fred Senese
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Last Revised 08/17/15.URL: http://antoine.frostburg.edu/chem/senese/101/periodic/faq/print-what-atom-is-largest.shtml