Periodic Relationships Among the Elements Chapter 6

The PeriodicTable Rows = Periods. Columns = Families/Groups

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

Outermost subshell being filled with electrons 7.8

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

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

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

Atomic Radii

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

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

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

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

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

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