1. The Periodic Table Unit 3/Chapters 3 & 8 Notes Chemistry CPA

2. Periodic Trends Many properties of atoms depend on the strength of attraction between the outer shell electrons and the nucleus This attraction will depend on: 1.The positive charge that attracts the other shell electrons 2.The distance of electrons from the nucleus

3. Four Periodic Trends 1.Atomic Radius 2.Ionization Energy 3.Electronegativity 4.Electron Affinity

4. Atomic Radius What is it? Diameter of atom What happens down a group? Increases since there is an increase in the number of shells. What happens across a period? Decreases since there is an increase in core charge, the outer shell electrons are attracted closer to the nucleus (it’s the same shell but there are more electrons in the shell as you move across the period)

5. Atomic Radius decreases across a period

6. Atomic Radius increases down a family/group

7. Ionization Energy What is it? Amount of energy required to remove the highest energy electron from an atom. (or steal one electron) What happens down a group? Decreases; since the size of the atom is increasing, the attraction is weaker between the outer shell electrons and the nucleus. Therefore electrons are easier to remove. What happens across a period? Increases; since there is an increase in core charge, the attraction is greater between the outer shell electrons and the nucleus. Therefore electrons are harder to remove. ee e e e e

8. Ionization Energy In other words… If its easy to steal a electron, it has low ionization energy If its hard to steal an electron, it has a high ionization energy The smaller the atom, the harder to steal an electron The larger the atom the easier it is to steal an electron

9. Ionization Energy

10. Electronegativity What is it? Measure of the ability of an atom to attract an electron towards itself or love of electrons! What happens down a group? Decreases; since the electrons are further from the nucleus, there is a weaker attraction What happens across a period? Increases; since there is an increase in core charge, there is a greater attraction of the outer shell electrons to the nucleus.

11. Electronegativity

12. Electron Affinity What is it? The energy release when an electron is added to an atom. Most favorable toward NE corner of PT since these atoms have a great affinity (“love and happiness”) for e-. (Think of “Jumping for Joy”!) What happens down a group? Decreases; since the electrons are further from the nucleus, the atom has no desire to hang on to it’s electron, so it won’t release too much “Happiness” (energy) if it gains one. What happens across a period? Increases; the more electrons an atom has in it’s valence shell, the more “happy” it will become when it gets closer to completing it shell.

13. Electron Affinity