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Periodicity

How are the electron configurations related to the atomic radius, ionization energy, and all the other “facts” about atoms?. Periodicity. Atomic radius – half the distance between the nuclei of two adjacent atoms. Periodicity- rEpeating properties.

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Periodicity

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  1. How are the electron configurations related to the atomic radius, ionization energy, and all the other “facts” about atoms? Periodicity

  2. Atomic radius – half the distance between the nuclei of two adjacent atoms. Periodicity- rEpeating properties As you go across a period, no new layers are added. Each atom has progressively more protons to attract the electrons. As you go across a period the atomic size decreases. Shielding is constant. Nuclear charge increases. H = 1s Li = 1s 2s Mg = 1s2s 3s Na = 1s2s 3s Al = 1s2s 3s As you go down a period, you add layers. Each layer increases shielding, and increases the size of the atom.

  3. Ionization energy– The amount of energy required to remove an electron from a gaseous element. Periodicity- rEpeating properties As you go across a period, no new layers are added. Each atom has progressively more protons to attract the electrons. As you go across a period the ionization energy increases. Shielding is constant. Nuclear charge increases. H = 1s Li = 1s 2s Mg = 1s2s 3s Na = 1s2s 3s Al = 1s2s 3s As you go down a period, you add layers. Each layer increases shielding, and decreases the ionization energy.

  4. Tightly held electrons are difficult to remove – high energy. The more nuclear charge, and/or the smaller the atom, the more tightly held the electrons will be. General Trends in electronegativity • The greater nuclear charge and the smaller the atom, the more likely an electron will be accepted into an atom.

  5. Summary

  6. Which is larger (higher atomic radius? Same sheilding, greater nuclear charge.

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