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INTRODUCTION
Transition metals are the elements that are present in groups 3 to 12 of the periodic table. The transition metals cover up to about 60 percent of all known elements in the periodic table. Along with copper (Cu), common examples of transition metals include iron (Fe), zinc (Zn), silver (Ag), gold (Au), etc.
Transition metals have the characteristics that define the metals class except for some metals. They are very good conductors of electricity, and they also are lustrous, malleable, and ductile.
Transition metals are higher conductors of both heat as well as electricity. They are malleable, which refers to the feature that they can be beaten into sheets, and ductility means they can be turned into wires. They have high melting and boiling points, and all are hard at room temperature, except for mercury (Hg), which at room temperature is a liquid. Transition metals also have high density and are very solid. They are usually white or silvery in color, and they are generally shiny. The compounds that are formed by transition metals with other elements are generally very colorful.
ELECTRONIC CONFIGURATION OF TRANSITION ELEMENTS
There are four principle orbitals namely, s, p, d, and f which are completed according to the level of energy and valence electrons of the element. All four orbitals can accommodate different numbers of electrons. The s-orbital can hold 2 electrons, and the other three orbitals can hold up to 6, 10, and 14 electrons, respectively. The s-orbital mainly represents group 1 or group 2 elements, the p-orbital represents group 13, 14, 15, 16, 17, or 18 elements, and the f-orbital represents the Lanthanides and Actinides group. The electron configuration of transition metals is found in the d-orbitals or d-block.
The electron configuration of transition metals is unique in the language that they can occur in multiple states of oxidation. Although the elements can show many different oxidation states, they generally show a common oxidation state based on what elements are considered most stable.
FIRST ROW TRANSITION ELEMENTS
Ten elements are found in the first row of the transition elements, which are Scandium (Sc), Titanium (Ti), Vanadium (V), Chromium (Cr), Manganese (Mn), Iron (Fe), Cobalt (Co), Nickel (Ni), Copper (Cu), and Zinc (Zn).
Scandium: Scandium is a chemical element represented with the symbol Sc and with atomic number 21. It is a silvery-white metallic d-block transition element. Anciently, it has been classified as a rare-earth element along with yttrium and the lanthanides. It was discovered in 1879 by spectral analysis of the mineral euxenite and gadolinite from Scandinavia.
Titanium: Titanium (Ti) is a chemical element that is a silvery-gray metal of Group 4 (IVB) of the periodic table. Titanium is light in mass, with high strength, low-corrosion structural metal, and is used in form of alloys for the production of various parts in high-speed aircraft. A compound of titanium and oxygen was discovered in 1791 by the English chemist and mineralogist William Gregor and it was rediscovered in 1795 individually and got its name from the German chemist Martin Heinrich Klaproth.
Vanadium: Vanadium is a chemical element represented with the symbol V and has an atomic number 23. It is a solid, silvery-grey, malleable transition metal. This metal is hardly found in nature in a free state, but once it is artificially isolated, the formation of a layer of oxygen, simply called passivation somewhat regulates the free metal against further oxidation.
Chromium: Chromium is a chemical element represented with the symbol Cr and with atomic number 24. It is the first element in Group 6. It is a steely-grey, lustrous, solid, and brittle transition metal. Chromium metal is marked valuable for its high resistance to corrosion and hardness. Major growth in steel production was the invention that steel could be made strongly resistant to corrosion and discoloration by the addition of metallic chromium to form stainless steel.
Manganese: Manganese is a chemical element represented with the symbol Mn and with the atomic number 25. It is a hard-brittle and silvery metal, usually found in combination with iron in minerals. Manganese is a transition metal with a complicated collection of alloy uses in industries, especially in the stainless-steel industry. It enhances strength, workability, and resistance to wear.
Iron: Iron is a chemical element represented with the symbol Fe. In Latin called Ferrum and has an atomic number 26. It is a metal that has its place in the first transition series and Group 8 of the periodic table. It is, by weight, the most common element on Earth. It is the fourth most abundant element in the crust of the Earth.
Cobalt: Cobalt is a hard-magnetic metal, which is a silvery-white, solid, lustrous, and brittle element. It is a member of group 8 of the periodic table. Like iron, cobalt can also be magnetized. It is familiar to iron and nickel in their physical properties. The element is chemically active and forms many compounds. Cobalt is constant in air and does not get affected by water but is gradually attacked by dilute acids.
Nickel: Nickel is a chemical element represented with the symbol Ni and with atomic number 28. It is a silvery-white lustrous metal with a light golden touch. Nickel fits in the group of transition metals and is solid and ductile. It is among the four elements along with iron, cobalt, and gadolinium that are magnetic at or near room temperature.
Copper: Copper is a chemical element represented with the symbol Cu. In Latin, known as cuprum, it has an atomic number 29. It is a non-solid, malleable, and ductile metal with very high heat and electrical conductivity. Pure copper has a pinkish-orange color when exposed to fresh surfaces.
Zinc: Zinc is a chemical element represented with the symbol Zn and with atomic number 30. Zinc is a little brittle metal at room temperature and has a silvery-greyish color when oxidation is removed. In Group 12 (IIB) of the periodic table, it is the first element.
METALLIC CHARACTER OF TRANSITION METALS
Transition elements exhibit the character of metals as they have low energies of ionization and have various vacant orbitals in their extreme most shell. This property supports the creation of metallic bonds in the transition metals, and so they attain proper metallic properties. These metals are solid in their form which reflects the existence of covalent bonds. This occurs as the transition metals have non-paired d-electrons. The d-orbital which has the non-paired electrons may intersect and form covalent bonds in the chemical reaction. The greater the number of unpaired electrons in the transition metals, the larger is the count of covalent bonds formed by them. This later increases the strength of the metal and also makes it more solid in form.
CONCLUSION
Learning from this article, we can conclude that the transition metals are the elements that are present in groups 3 to 12 of the periodic table. The transition metals cover up to about 60 percent of all known elements in the periodic table. Along with copper, common examples of transition metals include iron, zinc, silver, gold, etc. Ten elements are found in the first row of the transition elements, which are Scandium, Titanium, Vanadium, Chromium, Manganese, Iron, Cobalt, Nickel, Copper, and Zinc. Transition elements exhibit the character of metals as they have low energies of ionization and have various vacant orbitals in their most extreme shell. This property supports the creation of metallic bonds in the transition metals, and so they attain proper metallic properties.
