Periodic Trends: 3. Ionization Energy 4. Electronegativity

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Presentation transcript:

Periodic Trends: 3. Ionization Energy 4. Electronegativity What is ionization energy? What is electronegativity?

IONIZATION ENERGY Ionization Energy is energy needed to remove an outer valence electron. 1st IE energy required to remove 1st e- 2nd IE energy required to remove 2 e- 3rd IE energy required to remove 3 e-

Ionization Energy Before: Neutral Na Atom After: 1st valence e- is removed 11p+ 11 e- Overall Net Charge = 0 Result: 11p+ 10e- Overall Net Charge = +1

What is the trend and why? In groups = as you go down WHY? Increased shielding effect,  distance between e- and nucleus In rows = as you move across WHY? Increased positive nuclear charge, as nucleus becomes more +,  nuclear charge, holds e- closer More difficult to remove e- as they are located closer to nucleus.

What is the shielding effect? Shielding of outer electrons by inner electrons Prevents outer electrons from “feeling” effective nuclear charge

What is the shielding effect?

What is electronegativity? Electronegativity is the ability of an atom to attract electrons Used as a prediction of the type of bond that will form FLOURINE is the MOST ELECTRONEGATIVE CESIUM is the LEAST ELECTRONEGATIVE

What is the trend?

What is the periodic trend? In groups = as you go down WHY? Atom has higher number of energy levels, more inner electrons, less ability to attract e- In rows = as you move across WHY? Increased valence e- on outer energy level

TREND SUMMARY