Introduction to transition metal Most of the d block elements in the periodic table are transition metal elements. The transition metals are the metallic elements that serve as a bridge, or transition, between the two sides of the table. The number of ligands bound to the transition metal ion is called the coordination number. This is due to the proper numerical position between Groups 2 and 3 of the transition metals. Inner transition metals are usually put at the bottom of the periodic table. Not all the d-block elements are transition metals. INNER TRANSITION METALS The Inner Transition Metals are found in the bottom two rows of the periodic table.The lanthanides and actinides form a group that appears almost disconnected from the rest of the periodic table. Inner transition metals (ITM) are chemical elements on the periodic table.They are normally shown in two rows below all the other elements. Although coordination complexes are particularly important in the chemistry of the transition metals, some main group elements also form complexes. This is the f block of elements, known as the "inner Part of the “inner transition metals” elements # 89 –102 examples: uranium, plutonium, berkelium. Then, for each ion, give the electron configuration: cerium(III) lead(II) Ti 2+ Am 3+ Pd 2+ For the examples that are transition metals, determine to which series they belong. Halogens Group 17 on periodic table “Salt former” –combines with groups 1 and 2 to form salts (ionic bonds) examples: fluorine, bromine, iodine. They can form multiple oxidation states and form different ions. They include elements 57-71 (known as lanthanides) and 89-103 (actinides). The lanthanides are very similar. This is the f block of elements, known as the inner transition series. The following figure shows the d-block elements in periodic table. Moreover, ionization energies increase slowly from one transition element to the next and hardly at all across the inner transition elements. A blank periodic table showing the lanthanide and actinide series : The red highlighted group shows the lanthanide series and the blue highlighted group shows the actinide series. In periodic groups IIIA, IVA, and VA elements near the top of the table have large ionization energies and little metallic character. These elements were sometimes called rare earth elements or rare earth metals due to their extremely low natural occurrence. Recall that for the transition and inner transition metals, it is necessary to remove the s electrons before the d or f electrons. Transition metals are in the d-block and have valence electrons in the d-orbital's. They consist of the Lanthanides and the Actinides. They include elements 57-71, or lanthanides, and 89-103, or actinides.The lanthanides are very similar, and the actinides are all radioactive.. ITMs have three incomplete outermost electron shells and are all metals. Therefore all transition and inner transition elements are metals. Iron, Cobalt and Nickel are ferromagnetic. Transition metals are only those d-block elements which contain unfilled d-orbital even after losing electron to form ion. The inner transition metals (the lanthanoids and actinoids) also form nonstoichiometric hydrides. THE NONMETALS!! Solution For example, lanthanum (La) reacts with hydrogen gas at one atmosphere pressure with little or no heating to produce a black solid that inflames in air and reacts vigorously with water. The actinides are all radioactive. Aluminum, tin, and lead, for example, form complexes such as the AlF 6 3-, SnCl 4 2-and PbI 4 2-ions. Inner transition metals are in the f-block and have valence electrons in the f-orbital's.