.. _sphx_glr_api_gallery_structure_lewis:

Lewis structures, oxidation states, and electronegativity
----------------------------------------------------------

Lewis's shared electron pair and formal charge, Kossel's ionic limit and
oxidation states, and Pauling's electronegativity scale from bond
energies.


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  <div id='sg-tag-list' class='sphx-glr-tag-list'></div>


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    <div class="sphx-glr-thumbnails">

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    <div class="sphx-glr-thumbcontainer" tooltip="G. N. Lewis (1916) described a covalent bond as a pair of electrons shared by two atoms, and each atom as seeking an octet of eight valence electrons. Often several octet-satisfying structures can be drawn for one molecule. Formal charge ranks them: split every bonding pair evenly, count the electrons each atom then owns, and compare with the free atom,">

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  .. image:: /api/gallery/structure/lewis/images/thumb/sphx_glr_plot_01_lewis_formal_charge_thumb.png
    :alt:

  :doc:`/api/gallery/structure/lewis/plot_01_lewis_formal_charge`

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      <div class="sphx-glr-thumbnail-title">Lewis's shared electron pair: choosing between Lewis structures by formal charge</div>
    </div>


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    <div class="sphx-glr-thumbcontainer" tooltip="Walther Kossel (1916) described bonding as the complete transfer of electrons from one atom to another, leaving ions with noble-gas configurations held together by electrostatic attraction. Oxidation states are the bookkeeping version of that picture: give every bonding pair entirely to the more electronegative atom (sharing only between identical atoms) and compare the electron count with the free atom.">

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  .. image:: /api/gallery/structure/lewis/images/thumb/sphx_glr_plot_02_kossel_oxidation_states_thumb.png
    :alt:

  :doc:`/api/gallery/structure/lewis/plot_02_kossel_oxidation_states`

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      <div class="sphx-glr-thumbnail-title">Kossel's ionic bond: oxidation states as the fully ionic limit</div>
    </div>


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    <div class="sphx-glr-thumbcontainer" tooltip="Linus Pauling (1932) noticed that a bond A-B is usually stronger than the average of the A-A and B-B bonds. He called the excess the extra ionic energy,">

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  .. image:: /api/gallery/structure/lewis/images/thumb/sphx_glr_plot_03_pauling_electronegativity_thumb.png
    :alt:

  :doc:`/api/gallery/structure/lewis/plot_03_pauling_electronegativity`

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      <div class="sphx-glr-thumbnail-title">Pauling's electronegativity scale from bond energies</div>
    </div>


.. thumbnail-parent-div-close

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    </div>


.. toctree::
   :hidden:

   /api/gallery/structure/lewis/plot_01_lewis_formal_charge
   /api/gallery/structure/lewis/plot_02_kossel_oxidation_states
   /api/gallery/structure/lewis/plot_03_pauling_electronegativity