Mercury electron configuration

Zinc, cadmium and mercury are at the end of the transition series and have electron configurations ndw(n + l)s2 with filled d shells. They do not form any compound in which the d shell is other than full (unlike the metals Cu, Ag and Au of the preceding group) these metals therefore do not show the variable valence which is one of the characteristics of the transition metals. In this respect these metals are regarded as non-transition elements. They show, however, some resemblance to the d-metals for instance in their ability to form complexes (with NH3, amines, cyanide, halide ions, etc.). 

Mercury(II)systems For the halides and pseudohaUdes of the acceptor Hg2+ of the electron configuration AH and AHz have much the same value and so have also AHz and AHi. The two latter steps are much less exothermic than the first two. Generally this pattern is strikingly regular. In some cases where deviations have been reported, it seems plausible that these are not real but due to experimental error. This applies to the chloride system at / = 0.5 M where the very narrow range of existence of the third complex 37) makes the separation of AHz and AHi difficult and also to the iodide system where the low solubility of Hgl2 (zz. 10"4-i M Ref. 59)) detracts considerably from the accuracy of measurement. Especially the value of AH2 becomes rather uncertain. 

In this section, we will discuss organometallic derivatives of zinc, cadmium, mercury, and indium. The group IIB and IIIB metals have the d10 electronic configuration in the 2+ and 3+ oxidation states, respectively. Because of the filled d level, the 2+ or 3+ oxidation states are quite stable, and reactions of the organometallics usually do not involve changes in oxidation level. This property makes the reactivity patterns of these organometallics more similar to those of derivatives of the group IA and IIA metals than to those of derivatives of transition metals with vacancies in the d levels. The IIB metals, however, are... 

Mercury has the electronic configuration (Xe)4/145d106s2. The first three ionization potentials are 10.43, 18.65 and 34.4 eV, therefore under chemically significant conditions no more than two electrons are removed from the mercury atom. Only one complex of mercury (III), with d9 configuration and a half-life of 5 s at -78 °C, has been synthesized. The synthesis involved electrochemical oxidation of Hg(l,4,8,ll-tetraazacyclotetradecane)(BF4)2 in propiononitrile solution.11 In contrast to most other metals mercury forms polycations, e.g. Hgf+, Hgf+ or Hg3+. 

How does relativity explain why mercury has a melting point of —39°C while that of neighboring gold is 1064°C The first step in answering this question involves considering the electron configurations of these atoms ... 

You ve probably noticed that in everything we ve said so far about electronic configuration, bonding and formulae we ve missed out a big block of elements altogether. Those are the ones in the centre of the periodic table, starting with scandium in the top left and running to mercury in the bottom right. This block of elements is called the transition metals. What makes them special ... 

The Group 12 metals, zinc, cadmium, and mercury, have valence electron configurations of n - )d Zinc and, to a lesser extent, cadmium resemble beryllium or magnesium in their chemistry. 

It must not be assumed that these two rules exhaust the possi bilities of bond formation. Thus mercuric ion combines with chloride ions to form mercuric chloride in which the mercury atom is bonded to the two chlorine atoms. In this process the mercury atom does not acquire an octet, and the chlorine atoms have the same octets in the chloride ions as in mercuric chloride. The bonds in this case may arise from a specific instability of the electron configuration of the mercuric ion. But the bonds which maintain themselves through the greatest vicissitudes arc those in which the atoms have achieved noble-gas electron configurations. 

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