1. Periodic Trends

2. Atomic Radius
Total distance from an atoms nucleus to the outermost orbital of an electron (similar to the radius of a circle where the center is the nucleus)
Measured by half of the distance between two bonding atoms nuclei
affected by both the number of protons and distance of which its valance electrons

3. Atomic Radius Trend
Increases
Increases

4. Ionic Radius radius of an atoms ion
Trend compares ions to their neutral counterparts

5. Ions Variation in the number of electrons; results in an atom becoming charged
Anion
Cation
gain of electrons
overall charge is negative
lose of electrons
overall charge is positive
11 protons
12 neutrons
11electrons
10 electrons
Sodium atom
Sodium ion 1+ Na 1− F

6. Cations and Anions Of Representative Elements+1 +2 +3 -3 -2 -1

7. Cation vs Atom

8. Anion vs Atom

9. Cation is always smaller than atom from which it is formed.
Anion is always larger than atom from which it is formed.

10. Ionization Energy
Minimum energy required to remove an electron from a gaseous atom in its ground state
Indication of how strongly an atom’s nucleus holds onto its valence electron (columbic attraction)

11. What do you notice between successive ionization energies
What do you notice between successive ionization energies? What is the trend across and down?

12. General Trends in First Ionization Energies
Increasing First Ionization Energy
Increasing First Ionization Energy

13. Electronegativity
Chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself
An atoms electronegativity is affected by both its atomic number and the distance at which its valance electrons reside from the charged nucleus (columbic attraction)