1. Periodicity Periodic Table Trends

2. Describing the Periodic Table periodic law: the properties of elements repeat every so often period: group (family): horizontal row; there are 7 vertical column; there are 18 18 17 16 15 14 13 12 9 10118 7 65 4 1 3 2 1 2 3 4 6 7 5

3. alkaline earth metals halogens noble gases lanthanides alkali metals actinides coinage metals transition elements main block elements metalloids hydrogen more nonmetals more metals

4. Ionization Energy Ionization Energy: The energy required to remove an electron from an atom or ion As you move down a group/family, the energy levels become higher and the electrons are further from the positively charged nucleus, so it is easier for an electron to leave the atom. The ionization energy decreases.

5. Ionization Energy 2 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: too many electrons repel each other away from the nucleus.

6. Ionization Energy 3 Ionization energy increases as you move from left to right across the table. Every element you move across has another proton so the outer electrons become more attracted to the nucleus and harder to remove from the atom.

7. Ionization Energy 4

8. Atomic Radius Bond Radius: ½ the distance from center to center of two like atoms that are bonded together.

9. Atomic Radius 2 Due to increasing number of energy levels as you travel down a group/family, the radius becomes larger As you move across the periodic table, the electrons are more attracted to the nucleus and their radius becomes smaller

10. Atomic Radius 3

11. Electronegativity Electronegativity: a measure of the ability of an atom in a chemical compound to attract electrons As you move down a group/family, energy levels are added and electrons are further from the nucleus. Electron shielding prevents the atom from attracting another electron. As you move across the periodic table, the shielding remains the same, but more protons increases the attraction for more electrons so the electronegativity increases.

12. Electronegativity 2

13. Summary of Periodic Trends Ionic size (cations) Ionic size (anions) decreases Shielding is constant Atomic radius decreases Ionization energy increases Electronegativity increases Nuclear charge increases Shielding increases Atomic radius increases Ionic size increases Ionization energy decreases Electronegativity decreases 1A 2A3A4A 5A 6A7A 0