Electron Affinity
• Electron affinity - energy required to place an
electron on a gaseous atom, forming an
anion(negativel...
Electron Affinity
Energy change accompanying addition of
electron to gaseous atom:
Cl + e− Cl−
Trends in Electron Affinity
• In general, electron
affinity becomes more
exothermic as you go
from left to right across a
...
4
Electron Affinity
Electron affinities increase (numerical value
becomes more negative) from left to right for a
period a...
Electronegativity and Bond Polarity
• Bonding between the two ends of the bonding
continuum, ionic and covalent bonding, i...
Electronegativity
• Electronegativities increase from left to right across a
period and from bottom to top for a group.
• ...
Electronegativity:
• The ability of atoms in a
molecule to attract
electrons to itself.
• On the periodic
chart, electrone...
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Electron affinity chm11-3

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Electron affinity chm11-3

  1. 1. Electron Affinity • Electron affinity - energy required to place an electron on a gaseous atom, forming an anion(negatively charged) • The attraction of an atom for an electron • Electron affinities may have positive or negative values. • Negative values - energy released • Positive values - energy absorbed
  2. 2. Electron Affinity Energy change accompanying addition of electron to gaseous atom: Cl + e− Cl−
  3. 3. Trends in Electron Affinity • In general, electron affinity becomes more exothermic as you go from left to right across a row. • The greater the attraction between a given atom and an added electron, the more negative the atom’s electron affinity will be.
  4. 4. 4 Electron Affinity Electron affinities increase (numerical value becomes more negative) from left to right for a period and bottom to top for a group. The greater (more negative) the electron affinity, the more stable the anion will be.
  5. 5. Electronegativity and Bond Polarity • Bonding between the two ends of the bonding continuum, ionic and covalent bonding, is described using electronegativity and bond polarity. • Electronegativity is the attraction of an atom for the shared electrons in a covalent bond. – Electronegativities are not measured quantities. – Electronegativities are assigned based on factors such as atomic size, electron affinity, and ionization energy. – The higher the electronegativity value, the more likely an element will attract extra electron density during compound formation.
  6. 6. Electronegativity • Electronegativities increase from left to right across a period and from bottom to top for a group. • Fluorine is the most electronegative element, with an electronegativity of 4.0.
  7. 7. Electronegativity: • The ability of atoms in a molecule to attract electrons to itself. • On the periodic chart, electronegativity increases as you go… – …from left to right across a row. – …from the bottom to the top of a column.
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