P ERIODICITY Unit 4.6-4.7. T ARGETS 6) I can define the following terms: electron shielding, ionization energy, atomic radius, nuclear charge, and electronegativity.

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Presentation transcript:

P ERIODICITY Unit

T ARGETS 6) I can define the following terms: electron shielding, ionization energy, atomic radius, nuclear charge, and electronegativity. 7) I can describe the patterns of the following on the periodic table: atomic number, electron configurations, electron shielding, ionization energy, atomic radius, nuclear charge, and electronegativity.

R EMEMBER ! Going down a group the distance and protons both change. But only the distance between the valance electrons and the nucleus seems to matter. Why doesn’t the number of protons changing change the attraction??? The answer is electron shielding!

W HAT IS ELECTRON SHIELDING ?? Electron shielding: the reduction of the attractive force between a positively charged nucleus and its outermost electrons due to the cancellation of some of the positive charge by the negative charges of the inner electrons. English: extra inside electrons block the extra positive charge of the nucleus The more energy levels there are in between the nucleus and the valance energy level, the less attracted the valance electrons are to the positive nucleus.

E LECTRON SHIELDING TREND - GROUP As you move down a group there are more energy levels. Therefore, there is more electron shielding. For example, lithium only has 2 inner electrons that can block the charge of the nucleus but sodium has 10 and potassium has 18.

E LECTRON SHIELDING TREND - PERIOD As you move across a period, the electron shielding stays the same because all of the elements in a period have the same number of energy levels. For example, Na, Al and Cl all have 10 inner electrons to block the nucleus. The only thing changing is the valance electrons.

S UMMARY OF ALL T RENDS

A CROSS A PERIOD Number of protons increases but the number of energy levels doesn’t. This causes an increased attraction between the valance electrons and the nucleus. The following things can be explained because of the increased attraction: 1) Valance electrons are pulled in closer→ Smaller nucleus 2) It is harder to remove a valance electron → Higher ionization energy 3) The atom will be better at attracting electrons → Higher electronegativity

D OWN A GROUP Number of protons increases but so does the number of energy levels. The electron shielding causes reduced attraction between the nucleus and the valance electrons. The following things can be explained because of the decreased attraction: 1. Valance electrons are not pulled in tightly → larger radius 2. It is easier to remove a valance electron → lower ionization energy. 3. The atom will be worse at attracting electrons → lower electronegativity