Why does the beryllium 2+ ion have a larger radius than a helium atom?












6












$begingroup$


$ce{Be^2+}$ has an ionic radius of $pu{45 pm}$, while $ce{He}$ has a radius of only $pu{31 pm}$. If they have the same number of electrons (two, in the $mathrm{1p}$ orbital), and $ce{Be}$ has more protons to attract them, why doesn't $ce{Be^2+}$ have a smaller radius?










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$endgroup$








  • 2




    $begingroup$
    He has VDW radisum of 140 pm, what particular radius of He are your referring to? There is more than one.
    $endgroup$
    – permeakra
    20 hours ago








  • 2




    $begingroup$
    It's probably down to different definitions and/or measuring techniques.
    $endgroup$
    – TAR86
    19 hours ago
















6












$begingroup$


$ce{Be^2+}$ has an ionic radius of $pu{45 pm}$, while $ce{He}$ has a radius of only $pu{31 pm}$. If they have the same number of electrons (two, in the $mathrm{1p}$ orbital), and $ce{Be}$ has more protons to attract them, why doesn't $ce{Be^2+}$ have a smaller radius?










share|improve this question











$endgroup$








  • 2




    $begingroup$
    He has VDW radisum of 140 pm, what particular radius of He are your referring to? There is more than one.
    $endgroup$
    – permeakra
    20 hours ago








  • 2




    $begingroup$
    It's probably down to different definitions and/or measuring techniques.
    $endgroup$
    – TAR86
    19 hours ago














6












6








6





$begingroup$


$ce{Be^2+}$ has an ionic radius of $pu{45 pm}$, while $ce{He}$ has a radius of only $pu{31 pm}$. If they have the same number of electrons (two, in the $mathrm{1p}$ orbital), and $ce{Be}$ has more protons to attract them, why doesn't $ce{Be^2+}$ have a smaller radius?










share|improve this question











$endgroup$




$ce{Be^2+}$ has an ionic radius of $pu{45 pm}$, while $ce{He}$ has a radius of only $pu{31 pm}$. If they have the same number of electrons (two, in the $mathrm{1p}$ orbital), and $ce{Be}$ has more protons to attract them, why doesn't $ce{Be^2+}$ have a smaller radius?







atomic-radius






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edited 19 hours ago









andselisk

16.4k653115




16.4k653115










asked 20 hours ago









TrumpetDudeTrumpetDude

415




415








  • 2




    $begingroup$
    He has VDW radisum of 140 pm, what particular radius of He are your referring to? There is more than one.
    $endgroup$
    – permeakra
    20 hours ago








  • 2




    $begingroup$
    It's probably down to different definitions and/or measuring techniques.
    $endgroup$
    – TAR86
    19 hours ago














  • 2




    $begingroup$
    He has VDW radisum of 140 pm, what particular radius of He are your referring to? There is more than one.
    $endgroup$
    – permeakra
    20 hours ago








  • 2




    $begingroup$
    It's probably down to different definitions and/or measuring techniques.
    $endgroup$
    – TAR86
    19 hours ago








2




2




$begingroup$
He has VDW radisum of 140 pm, what particular radius of He are your referring to? There is more than one.
$endgroup$
– permeakra
20 hours ago






$begingroup$
He has VDW radisum of 140 pm, what particular radius of He are your referring to? There is more than one.
$endgroup$
– permeakra
20 hours ago






2




2




$begingroup$
It's probably down to different definitions and/or measuring techniques.
$endgroup$
– TAR86
19 hours ago




$begingroup$
It's probably down to different definitions and/or measuring techniques.
$endgroup$
– TAR86
19 hours ago










1 Answer
1






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oldest

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10












$begingroup$

You are mixing apples and oranges.
Or, to be more precise, an ionic radius for $ce{Be^2+}$ with coordination number (C.N.) 6 and van der Waals radius of $ce{He}$.
To make it clear I compiled data for van der Waals and covalent radii [1, p. 9-58] as well as ionic radii [1, p. 12-13]:



$$
begin{array}{lccccc}
hline
text{Element} & R_mathrm{vdW}/pu{Å} & R_mathrm{cov}/pu{Å} & text{Ion} & text{C.N.} & R_mathrm{i}/pu{Å} \
hline
ce{Be} & 1.52 & 0.99 & ce{Be^2+} & 4 & 0.27 \
& & & & 6 & 0.45 \
ce{He} & 1.40 & 0.37 & & & \
hline
end{array}
$$



Apparently, there is no experimental ionic radii for helium to compare with as helium, well, represents one of the most non-reactive elements.
Also, all radii set are determined using various methods and cannot be directly compared.
From the foreword [1. p. 9-58]:




There are many scales of van der Waals radii, but they are not fully consistent with one another. The van der Waals radii determined by Bondi [...] from x-ray diffraction data, crystal densities, gas kinetic collision cross sections, critical densities, and liquid-
state properties are the most widely used values. [...]



The covalent radii tabulated here are recommendations for single covalent bonds,
and they are based on a comprehensive evaluation of experimental data [...].




Ionic radii are estimated first and foremost from the experimental crystal structure data, averaged and supplemented by empirical and theoretical calculations (extrapolations, e.g. using Zachariasen method).



References




  1. Haynes, W. M.; Lide, D. R.; Bruno, T. J. CRC Handbook of Chemistry and Physics: A Ready-Reference Book of Chemical and Physical Data.; 2017; Vol. 97. ISBN 978-1-4987-5429-3.






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    1 Answer
    1






    active

    oldest

    votes








    1 Answer
    1






    active

    oldest

    votes









    active

    oldest

    votes






    active

    oldest

    votes









    10












    $begingroup$

    You are mixing apples and oranges.
    Or, to be more precise, an ionic radius for $ce{Be^2+}$ with coordination number (C.N.) 6 and van der Waals radius of $ce{He}$.
    To make it clear I compiled data for van der Waals and covalent radii [1, p. 9-58] as well as ionic radii [1, p. 12-13]:



    $$
    begin{array}{lccccc}
    hline
    text{Element} & R_mathrm{vdW}/pu{Å} & R_mathrm{cov}/pu{Å} & text{Ion} & text{C.N.} & R_mathrm{i}/pu{Å} \
    hline
    ce{Be} & 1.52 & 0.99 & ce{Be^2+} & 4 & 0.27 \
    & & & & 6 & 0.45 \
    ce{He} & 1.40 & 0.37 & & & \
    hline
    end{array}
    $$



    Apparently, there is no experimental ionic radii for helium to compare with as helium, well, represents one of the most non-reactive elements.
    Also, all radii set are determined using various methods and cannot be directly compared.
    From the foreword [1. p. 9-58]:




    There are many scales of van der Waals radii, but they are not fully consistent with one another. The van der Waals radii determined by Bondi [...] from x-ray diffraction data, crystal densities, gas kinetic collision cross sections, critical densities, and liquid-
    state properties are the most widely used values. [...]



    The covalent radii tabulated here are recommendations for single covalent bonds,
    and they are based on a comprehensive evaluation of experimental data [...].




    Ionic radii are estimated first and foremost from the experimental crystal structure data, averaged and supplemented by empirical and theoretical calculations (extrapolations, e.g. using Zachariasen method).



    References




    1. Haynes, W. M.; Lide, D. R.; Bruno, T. J. CRC Handbook of Chemistry and Physics: A Ready-Reference Book of Chemical and Physical Data.; 2017; Vol. 97. ISBN 978-1-4987-5429-3.






    share|improve this answer











    $endgroup$


















      10












      $begingroup$

      You are mixing apples and oranges.
      Or, to be more precise, an ionic radius for $ce{Be^2+}$ with coordination number (C.N.) 6 and van der Waals radius of $ce{He}$.
      To make it clear I compiled data for van der Waals and covalent radii [1, p. 9-58] as well as ionic radii [1, p. 12-13]:



      $$
      begin{array}{lccccc}
      hline
      text{Element} & R_mathrm{vdW}/pu{Å} & R_mathrm{cov}/pu{Å} & text{Ion} & text{C.N.} & R_mathrm{i}/pu{Å} \
      hline
      ce{Be} & 1.52 & 0.99 & ce{Be^2+} & 4 & 0.27 \
      & & & & 6 & 0.45 \
      ce{He} & 1.40 & 0.37 & & & \
      hline
      end{array}
      $$



      Apparently, there is no experimental ionic radii for helium to compare with as helium, well, represents one of the most non-reactive elements.
      Also, all radii set are determined using various methods and cannot be directly compared.
      From the foreword [1. p. 9-58]:




      There are many scales of van der Waals radii, but they are not fully consistent with one another. The van der Waals radii determined by Bondi [...] from x-ray diffraction data, crystal densities, gas kinetic collision cross sections, critical densities, and liquid-
      state properties are the most widely used values. [...]



      The covalent radii tabulated here are recommendations for single covalent bonds,
      and they are based on a comprehensive evaluation of experimental data [...].




      Ionic radii are estimated first and foremost from the experimental crystal structure data, averaged and supplemented by empirical and theoretical calculations (extrapolations, e.g. using Zachariasen method).



      References




      1. Haynes, W. M.; Lide, D. R.; Bruno, T. J. CRC Handbook of Chemistry and Physics: A Ready-Reference Book of Chemical and Physical Data.; 2017; Vol. 97. ISBN 978-1-4987-5429-3.






      share|improve this answer











      $endgroup$
















        10












        10








        10





        $begingroup$

        You are mixing apples and oranges.
        Or, to be more precise, an ionic radius for $ce{Be^2+}$ with coordination number (C.N.) 6 and van der Waals radius of $ce{He}$.
        To make it clear I compiled data for van der Waals and covalent radii [1, p. 9-58] as well as ionic radii [1, p. 12-13]:



        $$
        begin{array}{lccccc}
        hline
        text{Element} & R_mathrm{vdW}/pu{Å} & R_mathrm{cov}/pu{Å} & text{Ion} & text{C.N.} & R_mathrm{i}/pu{Å} \
        hline
        ce{Be} & 1.52 & 0.99 & ce{Be^2+} & 4 & 0.27 \
        & & & & 6 & 0.45 \
        ce{He} & 1.40 & 0.37 & & & \
        hline
        end{array}
        $$



        Apparently, there is no experimental ionic radii for helium to compare with as helium, well, represents one of the most non-reactive elements.
        Also, all radii set are determined using various methods and cannot be directly compared.
        From the foreword [1. p. 9-58]:




        There are many scales of van der Waals radii, but they are not fully consistent with one another. The van der Waals radii determined by Bondi [...] from x-ray diffraction data, crystal densities, gas kinetic collision cross sections, critical densities, and liquid-
        state properties are the most widely used values. [...]



        The covalent radii tabulated here are recommendations for single covalent bonds,
        and they are based on a comprehensive evaluation of experimental data [...].




        Ionic radii are estimated first and foremost from the experimental crystal structure data, averaged and supplemented by empirical and theoretical calculations (extrapolations, e.g. using Zachariasen method).



        References




        1. Haynes, W. M.; Lide, D. R.; Bruno, T. J. CRC Handbook of Chemistry and Physics: A Ready-Reference Book of Chemical and Physical Data.; 2017; Vol. 97. ISBN 978-1-4987-5429-3.






        share|improve this answer











        $endgroup$



        You are mixing apples and oranges.
        Or, to be more precise, an ionic radius for $ce{Be^2+}$ with coordination number (C.N.) 6 and van der Waals radius of $ce{He}$.
        To make it clear I compiled data for van der Waals and covalent radii [1, p. 9-58] as well as ionic radii [1, p. 12-13]:



        $$
        begin{array}{lccccc}
        hline
        text{Element} & R_mathrm{vdW}/pu{Å} & R_mathrm{cov}/pu{Å} & text{Ion} & text{C.N.} & R_mathrm{i}/pu{Å} \
        hline
        ce{Be} & 1.52 & 0.99 & ce{Be^2+} & 4 & 0.27 \
        & & & & 6 & 0.45 \
        ce{He} & 1.40 & 0.37 & & & \
        hline
        end{array}
        $$



        Apparently, there is no experimental ionic radii for helium to compare with as helium, well, represents one of the most non-reactive elements.
        Also, all radii set are determined using various methods and cannot be directly compared.
        From the foreword [1. p. 9-58]:




        There are many scales of van der Waals radii, but they are not fully consistent with one another. The van der Waals radii determined by Bondi [...] from x-ray diffraction data, crystal densities, gas kinetic collision cross sections, critical densities, and liquid-
        state properties are the most widely used values. [...]



        The covalent radii tabulated here are recommendations for single covalent bonds,
        and they are based on a comprehensive evaluation of experimental data [...].




        Ionic radii are estimated first and foremost from the experimental crystal structure data, averaged and supplemented by empirical and theoretical calculations (extrapolations, e.g. using Zachariasen method).



        References




        1. Haynes, W. M.; Lide, D. R.; Bruno, T. J. CRC Handbook of Chemistry and Physics: A Ready-Reference Book of Chemical and Physical Data.; 2017; Vol. 97. ISBN 978-1-4987-5429-3.







        share|improve this answer














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        edited 14 hours ago

























        answered 19 hours ago









        andseliskandselisk

        16.4k653115




        16.4k653115






























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