1. Periodic Relationships Among the Elements
Chapter 6

2. The PeriodicTable
Rows = Periods.
Columns = Families/Groups

3. Need to know... Alkali Metals Alkali Earth Metals Halogens Nobel Gases
Transition Metals
Inner Transition Metals

4. Outermost subshell being filled with electrons
7.8

5. ns2np6 ns1 ns2np1 ns2np2 ns2np3 ns2np4 ns2np5 ns2 d10 d1 d5 4f 5f
Ground State Electron Configurations of the Elements
ns2np6
ns1
ns2np1
ns2np2
ns2np3
ns2np4
ns2np5
ns2
d10 d1 d5 4f 5f

7. Octet Rule
Atoms tend to gain, lose, or share electrons in order to acquire a full set of valence electrons
Atoms on the left of the periodic table lose electrons and form +ions
Atoms on the right side of the periodic table form -ions

8. Trends of the Period Table
All trends depend on one concept:
The force between electrons and protons
Two Factors that Affect this force
Distance
Amount of Charge

11. Atomic Radii

12. Electronegativity: The relative ability of an element to attract electrons to make a chemical bond.

13. Ionization energy is the minimum energy (kJ/mol) required to remove an electron from a gaseous atom in its ground state.
I1 + X (g) X+(g) + e-
I1 first ionization energy
I2 + X+(g) X2+(g) + e-
I2 second ionization energy
I3 + X2+(g) X3+(g) + e-
I3 third ionization energy
I1 < I2 < I3

15. Variation of the First Ionization Energy with Atomic Number
Filled n=1 shell
Filled n=2 shell
Filled n=3 shell
Filled n=4 shell
Filled n=5 shell

16. Electronegativity: The relative ability of an element to attract electrons to make a chemical bond.

17. General Trend in First Ionization Energies
Increasing First Ionization Energy
Increasing First Ionization Energy

19. Copyright McGraw-Hill 2009
Isoelectronic Series
Two or more species having the same electron configuration but different nuclear charges
Size varies significantly
Copyright McGraw-Hill 2009