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Periodicity Topic #12

Periodicity Topic #12. Hypothesize (Face Partners). How do valence electrons change as you go: Across a period - (increases, decreases, stays the same) Down a group - (increases, decreases, stays the same) How does ionization energy change as you go:

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Periodicity Topic #12

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  1. PeriodicityTopic #12

  2. Hypothesize (Face Partners) • How do valence electrons change as you go: • Across a period - (increases, decreases, stays the same) • Down a group - (increases, decreases, stays the same) • How does ionization energy change as you go: • Across a period - (increases, decreases, stays the same) • Down a group - (increases, decreases, stays the same) • How does atomic radius change as you go: • Across a period - (increases, decreases, stays the same) • Down a group - (increases, decreases, stays the same)

  3. Periodicity • Atomic radius • Ionization energy • Electronegativity • Metallic character

  4. Atomic radius • One half the distance between the nuclei of identical atoms that are bonded together. • Atoms shrink as you advance across a period because added protons in the nucleus pull the added electrons more tightly in the absence of effective shielding. • Atoms in the same column increase in size as you go down the family since electrons are being added on successively higher energy levels and are well shielded by the previous completed electron energy levels.

  5. Atomic radius • Radius (or size): • Decreases from left to right (across periods) • Increases from top to bottom (within a family)

  6. Ionization Energy • Amount of energy required to remove an electron from an atom. • The outer-most electron becomes increasingly more difficult to remove as you advance across a period since shielding is very poor and the added protons continue to exert a stronger attraction. • The outer-most electron is easier to remove as you move down a column since each time you are one energy level farther from the nucleus, benefiting from that much more shielding.

  7. Electronegativity • The tendency of a bonded atom to attract the electrons in that bond. • The ability to attract additional electrons increases as you advance across a period, since shielding is largely ineffective and the pull of the increased protons in the nucleus is sufficient to influence electrons which approach the outer limits of the atom from other sources. • Any attractive force of the nucleus is so diminished by effective shielding of electrons in lower levels that additional electrons become more difficult to hold onto as you move down a column.

  8. Metallic character Metallic properties are related to the freedom of the outer electrons to move in a macroscopic sample and thus these properties are most pronounced at the left side of the table where shielding is at a maximum. • This means that metallic properties will also increase as you move down a family since shielding improves.

  9. Metallic character Fr (Francium) is the most reactive metal. F (Fluorine) is the most reactive non-metal. The noble gases are very un-reactive.

  10. Summary of Periodic Trends

  11. Conclusions • Valence electrons: • Across a period - (increases) • Down a group - (stays the same) • Ionization energy: • Across a period - (increases) • Down a group - (decreases) • Atomic radius: • Across a period - (decreases) • Down a group - (increases)

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