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Valence Electrons and Electronegativity

JABA Powerpoint company presents. Valence Electrons and Electronegativity. Jason Paik, Alex Swope, brian curless and alex matsiras Period 2 - Kandrick. Valence Electrons - the electrons available to be lost, gained, or shared in the formation of chemical compounds

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Valence Electrons and Electronegativity

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  1. JABA Powerpoint company presents... Valence Electrons and Electronegativity Jason Paik, Alex Swope, brian curless and alex matsiras Period 2 - Kandrick

  2. Valence Electrons - the electrons available to be lost, gained, or shared in the formation of chemical compounds These Valence Electrons are usually located in incompletely filled main-energy levels EX:                 Sodium~Na                    The last piece of the element's electron configuration is "3s"                    The electron in the "3s" energy level is a valence electron Valence Electrons

  3. More about the Valence Electrons • Only the s and p parts of the periodic table contain valence electrons • Groups 1 and 2 have 1 and 2 electrons accordingly • In p, you take the group # -10 to find out the total # of valence electrons EX: Sulfur is a member of group 16 16-10=6 valence electrons

  4. Why are they important? • The number of valence electrons that are present allows you to see how reactive a certain element will be • Less Valence Electrons = Less • Stability = Higher reactivity • More Valence Electrons = More • Stability = Less Reactivity • **The Valence Electrons of Groups 3-12 are not helpful in determining reactivity so they are rarely shown** An atom of helium: how many valence electrons does it contain? stability? reactivity?

  5. Electronegativity Definition: A measure of the ability of an atom in a chemical compound (bonding) to attract electrons. Electronegativities:     - Across a period,electronegativities tend to increase     - Down a group, electronegativities tend to decrease or remain the same

  6. Electronegativity - Increases across a period: the number of charges on the nucleus increases. - Decreases down a group: the bonding pair of electrons is in distant from the attraction of the nucleus.

  7. Electronegativity Pauling Scale: Scale of numerical values reflecting the tendecy of an atom to attract electrons         - Ranges from 0 - 4.0   Fluorine:      - Electronegativity always increases towardsfluorine in the Periodic Table

  8. Sources of Information - http://www.chemguide.co.uk/atoms/bonding/electroneg.html         "Electronegativity" -  http://dl.clackamas.cc.or.us/ch104-06/valence_electrons.htm  -  http://chemed.chem.purdue.edu/genchem/topicreview/bp/c h8/index.php#valence

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