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5 – 3 Electron Configuration and Periodic Properties

5 – 3 Electron Configuration and Periodic Properties. Atomic Radius. As you move down a group it increases The outermost e - are being added to higher energy levels (further from the nucleus. Atomic Radius. As you move across a period, it decreases

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5 – 3 Electron Configuration and Periodic Properties

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  1. 5 – 3 Electron Configuration and Periodic Properties

  2. Atomic Radius • As you move down a group it increases • The outermost e- are being added to higher energy levels (further from the nucleus.

  3. Atomic Radius • As you move across a period, it decreases • Even though e- are being added, they are added to the same energy level (same distance from the nucleus).

  4. Atomic Radius • The charge on the nucleus increases as you move across the period and so it has a “tighter” hold on the e- being added.

  5. Shielding Effect • The reduction of the attractive force between a nucleus and its outer electrons due to the blocking effect of inner electrons.

  6. Ionization Energy • The amount of energy needed to remove an electron from an atom

  7. Ion • An atom that has gained or lost an e- • If it has gained an e-, it will be _____. • If it has lost an e-, it will be _____.

  8. Ionization Energy • As you go down a group, it decreases • Shielding effect and electrons are being added to higher energy levels.

  9. Ionization Energy • As you move across a period, it increases • The charge on the nucleus increases as you move across the period and so it has a “tighter” hold on the e- being added.

  10. Electron Affinity • The attraction of an atom for an additional e- • Metals tend to have low EA • Non-metals tend to have high EA

  11. EA • As you move down a group, EA decreases. • Shielding Effect and electrons are being added to higher energy levels.

  12. EA • It increases as you move across the periodic table. • The charge on the nucleus increases as you move across the period and so it has a “tighter” hold on the e- being added.

  13. Electronegativity • Tendency for an atom to attract e- to itself when combined with another atom. • F is the most EN • EN decreases as you move down a group • EN increases as you move across a period

  14. Electronegativity • Based on the Pauling Scale. • Linus Pauling • 28 Feb 1901 – 19 Aug 1994

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