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The Electronegativity of Ions?

  1. Sep 6, 2012 #1
    1. The problem statement, all variables and given/known data

    "Rank the following in the order of increasing absolute electronegativity: F, Li, Ti4+, P, H, C, Mg2+, Li+."


    2. Relevant equations



    3. The attempt at a solution

    - I can rank neutral species no problem. Periodic table has that covered, and Pauling values are easy to find. Ions don't have this.

    - I know these ions have an electron configuration of the noble gases: [He], [Ne], and [Ar] which are not electronegative, but due to the increases effective nuclear charge on the valence shell of these ions, I'm not sure if the same trend applies.

    - I've looked into ionization energies, atomic radii, electron affinities, etc., but I'm really stumped. I can rank the ions on their own, and the neutral atoms on their own, but I'm not sure how to integrate them.

    - As for the ions, I believe that it makes sense for Li+ to have the greatest EN of the three ions due to it being the harder specie. Harder species tend to have an increases EN, while softer ones have lower EN.

    - My Inorganic textbook mentioned the following: "Li has a low electronegativity, the Li+ ion has a relatively high EN resulting from the extremely high second ionization potential." I looked up, and compared all the ionization energies pertaining to the valence electrons of each species, and the ranking came up as follows:

    Li < P < H < C < Ti4+ < F < Mg2+ < Li+

    I'm not sure how I feel about Mg2+ and Li+ being above F in electronegativity though, so I feel like I may be missing a factor. Please help!
     
  2. jcsd
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