Transition Metal Compounds




The IUPAC definition, defines a transition metal like an element whose atom posseses an incomplete d sub-shell or which can give increase to cations with an unfinished d sub-shell.

Many scientists explain a transition metal as an element in the d-block of the periodic table (all are metals), which contains groups 3 to 12 on the periodic table. In actual practice, the f-block actinide and lanthanide series are also regarded as transition metals and are referred to as inner transition metals. 

You can find a number of properties shared by the transition components that are not seen in other elements, which results from the partially loaded d shell. Such as

the development of compounds in numerous oxidation states, because of the relatively low reactivity of unpaired d electrons.

the formation of compounds whose colour is due to dĖd electronic transitions

the formation of numerous paramagnetic compounds due to the existence of unpaired d electrons. Several compounds of principal group elements are also paramagnetic (e.g. oxygen and nitric oxide)

Naming Compounds with Transition Metals

Numerous transition metals exist as greater than one kind of cation. For instance, iron exists as Fe3+ and Fe2+. Therefore, whenever you are naming compounds with transition metals that contains iron, it is essential to indicate which oxidation number the metal has.

For metals, the oxidation number is the identical as the charge. Fe2+ in a compound with chloride would be named iron(II) chloride and would have a formula FeCl2. (The oxidation number looks like a Roman numeral in parenthesis following the cation.) The cation Fe3+ paired with oxygen would have the name iron(III) oxide and would have the formula Fe2O3. 

Example 1: Write a proper chemical formula for every of the following ionic compounds: a. Aluminum oxide; b. Copper(II) chloride; c. Iron(III) oxide.

Solution 1: a. Aluminum is 3+, oxide is 2-; Al2O3. b. From the oxidation state that is provided, copper is 2+, chloride is 1-; CuCl2. c. From the oxidation state, iron is 3+, oxide is 2-; Fe2O3.

Example 2: Write the appropriate chemical name for all of the following ionic compounds: a. Li2S; b. NiCl2; c. FeO.

Solution 2: a. We do not utilize multipliers, so this is just lithium sulfide. b. We do not need to specify an oxidation state for nickel, so this is nickel chloride. c. We should specify that iron is 2+ in this compound, so this is iron(II) oxide.

Transition Metal Ionic Compounds

Ionic compounds are created when a metal gives up its electrons to some nonmetal. Basically if the compound includes a metal, it is ionic. But you can find different sets of rules with regard to transition metal ionic compounds. A transition metal is a component having an atomic number of 57 to 80 or 21 to 30, 39 to 48.

a. So for any compound with any other metal, utilize these rules:

The metal ion's name does not change no matter charge

The non-metal's name finishes in ide.

For instance:

AlCl3 = aluminum chloride

Na2S = sodium sulfide

K2O = potassium oxide

MgH2 = magnesium hydride






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