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It is said that copper has a higher melting point than zinc because of the d electrons in copper being involved in metallic bonding. However, copper has no unpaired electrons in its d subshell just like zinc. How can we explain this observation ?

wonderingwhy
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  • why was this question closed? just curious – Gaurav Sai Maddipati Feb 07 '24 at 20:28
  • the question seems clear to me, why does copper show a higher melting point than zinc even though both have fully filled d subshells. (not sure about the validity of the premise) – Gaurav Sai Maddipati Feb 07 '24 at 20:30
  • @GauravSaiMaddipati This q. was completely rewritten and might be reopened, but copper does have an unpaired electron. – Mithoron Feb 08 '24 at 16:03
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    https://chemistry.stackexchange.com/questions/4766/melting-and-boiling-points-of-transition-elements/4815#4815 – Mithoron Feb 08 '24 at 16:03
  • @Mithoron Copper does have an unpaired electron, but in its s subshell. The reasoning is given based on the electrons in its d subshell, which makes it confusing. – wonderingwhy Feb 09 '24 at 14:34
  • @wonderingwhy read the link sent by mithoron and your doubt may be clarified. – Gaurav Sai Maddipati Feb 09 '24 at 14:40
  • @GauravSaiMaddipati I did read the link and the other answers. It explains the anomalous behaviours of Cr,Mn and Tc and that is understandable. My doubt is strictly limited to the statement which says that 'the d electrons in copper are involved in metallic bonding due to which it has a higher melting point than zinc'. – wonderingwhy Feb 10 '24 at 03:57
  • Could you give a source for that statement? – Gaurav Sai Maddipati Feb 10 '24 at 06:12
  • There is a multiple choice question going around and that is chosen as the correct answer. For example : https://www.sarthaks.com/2987888/the-melting-point-of-copper-is-higher-than-that-of-zinc-because – wonderingwhy Feb 10 '24 at 14:20

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