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Periodic Relationships Among the Elements

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Presentation on theme: "Periodic Relationships Among the Elements"— Presentation transcript:

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

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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

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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

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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

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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


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