Periodic Trends
1.
Ionization Energy: the energy required
(necessary) to remove an electron from an atom or ion.
Example: Na by it’s self is very reactive…1s22s22p63s1
Valence
electrons: 1
If you take the
valence electron away…
If the Shell is full it is
stable.
A. The First Ionization Energy: The
amount of energy required to remove the 1st electron
2.
Atomic Radius
3.
Electronegativity
4.
Electron Affinity
Octet:
·
8 electrons in the outer shell = a very stable
atom
·
(full set of electrons in the outer shell)
Explain why
each successive ionization of an electron requires a greater amount of energy… Successive ionization
energies increase in magnitude because the atom from which the electron is
removed becomes progressively more positively charged!!!!!! (THE ELECTRON IS
ATTRACTED TO THE NUCLEUS)
•
The ionization energy of the elements within a period generally increases from left to right.
This is due to valence shell stability.
•
The ionization energy of the elements within a group generally decreases from top to bottom. This is
due to electron shielding.
•
The noble gases possess very high ionization energies because of their
full valence shell as indicated in the graph.
•
Note that Helium has the highest
ionization energy of all the elements.
As
it goes down.. it is easier to remove an electron
If
you move across (to the right) it is harder to remove an electron.
FINISH IN CLASS: YASMINE DO FOR HOMEWORK
Pg
198-199: 43, 44, 45, 64
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