1. Periodic Trends by: Katie Green, T’mya Cunningham and Samantha Farley

2. Atomic Radius The distance from the atom to the outer electrons.

3. The atomic radius decreases as you move from left to right across the periodic table. The attractive force between the negatively charged electrons and the positively charged protons in the nucleus.

4. The atomic radius increases as you move from top to bottom on the periodic table By quantum mechanics the number of electron shells increases making the atomic radius larger.quantum mechanics

6. Ionization Energy The energy required to remove an electron from an atom/atoms.

7. Ionization Energy As you move from left to right across the periodic table, the ionization energy gets bigger. Why? It requires more energy to get rid of the outer electrons where there are more valence electrons.

8. Ionization Energy As you move from top to bottom on the periodic table, the ionization energy gets smaller. Why? It takes less energy to get rid of the electrons because the number of electron shells increase making the valence electrons closer to infinity.

10. Electronegativity A chemical property that describes the power of an atom to attract electrons to itself.

11. Electronegativity is helpful in finding if a bond is nonpolar covalent, polar covalent, or ionic.Electronegativity How do you find electronegativity? From the electronegativity chart:

12. Electronegativity cont’d As you move from left to right across the periodic table, the electronegativity gets bigger. As you move from top to bottom on the periodic table the electronegativity gets smaller. Don’t ask why just memorize the thing kay?

13. What kind of bond is it? Nonpolar covalent, polar covalent, or ionic?