The Periodic Table and the Elements What is

The Periodic Table and the Elements

What is the periodic table ? What information is obtained from the table ? How can elemental properties be predicted base on the PT ?

Dmitri Mendeleev (1869) In 1869 Mendeleev and Lothar Meyer (Germany) published nearly identical classification schemes for elements known to date. The periodic table is base on the similarity of properties and reactivities exhibited by certain elements. Later, Henri Moseley ( England, 1887 -1915) established that each elements has a unique atomic number, which is how the current periodic table is organized.

The Periodic Table • A map of the building block of matter.

Periodic Table: The three broad Classes Main, Transition, Rare Earth • Main (Representative), Transition metals, lanthanides and actinides (rare earth)

Periodic Table: Metallic arrangement • Layout of the Periodic Table: Metals vs. nonmetals Metals Nonmetals

Reading the Periodic Table: Classification • Nonmetals, Metalloids, Noble gases

Across the Periodic Table Periods: Are arranged horizontally across the periodic table (rows 1 -7) • These elements have the same number of valence shells. 2 nd Period 6 th Period

Down the Periodic Table • Group or Family: Are arranged vertically down the periodic table (columns or group, 1 - 18 or 1 -8 A, B) • These elements have the same number electrons in the outer most shells, the valence shell. Alkali Family: 1 e- in the valence shell Halogen Family: 7 e- in the valence shell

Infamous Families of the Periodic Table • Notable families of the Periodic Table and some important members: Halogen Alkali Noble Gas Alkaline Chalcogens (earth) Transition Metals

Periodic Table e- configuration from the periodic table H 1 s 1 He 1 s 2 Li Be 2 s 1 2 s 2 Na Mg 3 s 1 3 s 2 K 4 s 1 Sc 3 d 1 Rb 5 s 1 Ca 4 s 2 Sr 5 s 2 Y 4 d 1 V Ti Cr Mn Fe Co 3 d 2 3 d 3 4 s 13 d 5 3 d 6 3 d 7 Zr Nb Mo Tc Ru Rh 4 d 2 4 d 3 5 s 14 d 5 4 d 6 4 d 7 Cs 6 s 1 Ba 6 s 2 La 5 d 1 Hf Ta W Re Os 5 d 2 5 d 3 6 s 15 d 5 5 d 6 Fr 7 s 1 Ra 7 s 2 Ac Rf 6 d 1 6 d 2 Db Sg Bh 6 d 3 7 s 16 d 5 Ni 3 d 8 Ni 4 d 8 Ir Ni 7 5 d 5 d 8 Hs Mt 6 d 6 6 d 7 Cu 4 s 13 d 10 Ag 5 s 14 d 10 Au 6 s 15 d 10 B 2 p 1 • C B N O 1 2 3 • 2 p 2 p 4 F 2 p 5 Ne 2 p 6 Al 3 p 1 Si 3 p 2 S P 3 3 p 3 p 4 Cl 3 p 5 Ar 3 p 6 Zn Ga Ge 3 d 10 4 p 1 4 p 2 Cd In Sn 10 4 d 5 p 1 5 p 2 As Se 4 p 3 4 p 4 Be 4 p 5 Sb Te 5 p 3 5 p 4 I 5 p 5 Kr 4 p 6 Xe 5 p 6 Hg Tl Pb 5 d 10 6 p 1 6 p 2 Bi Po At 6 p 3 6 p 4 6 p 5 Rn 6 p 6

Periodic Table: electron behavior • The periodic table can be classified by the behavior of their electrons

Trend in Atomic Radius • Atomic Radius: • The size of at atomic species as determine by the boundaries of the valence e-. Largest atomic species are those found in the SW corner since these atoms have the largest n, but the smallest Zeff.

Trend in Ionization Energies Ionization energy: The energy required to remove the valence electron from an atomic specie. Largest toward NE corner of PT since these atoms hold on to their valence e- the tightest.

4. Trend in Electron Affinity: The energy release when an electron is added to an atom. Most favorable toward NE corner of PT since these atoms have a great affinity for e-.

Summary of Trend • Periodic Table and Periodic Trends • 1. Electron Configuration 3. Ionization Energy: Largest toward NE of PT 4. Electron Affinity: Most favorable NE of PT 2. Atomic Radius: Largest toward SW corner of PT