First Row Transition Elements

Introduction:

There are four principle orbitals (s, p, d, and f) in each element, which are filled in accordance with the element’s energy level and valence electron configuration. Each of the four orbitals has a different capacity for holding electrons. The s-orbital has a capacity of two electrons, while the other three orbitals have capacities of six, ten, and fourteen electrons, respectively. The s-orbital is used to denote elements in groups 1 or 2, the p-orbital is used to denote elements in groups 13, 14, 15, 16, 17, or 18, and the f-orbital is used to denote elements in the Lanthanides and Actinides groups. But the main focus of this module will be on the electron configuration of transition metals, which can be found in the d-orbitals of atoms and molecules (d-block).

As a result of their ability to be found in numerous oxidation states, transition metals’ electron configurations are particularly interesting. Despite the fact that the elements can exhibit a wide range of oxidation states, they typically exhibit a common oxidation state depending on what makes that element the most stable in the environment. We will only be working with the first row of transition metals in this module; however, the other rows of transition metals generally follow the same patterns as the first row.

Transition Metals

Scandium (Sc), Titanium (Ti), Vanadium (V), Chromium (Cr), Manganese (Mn), Iron (Fe), Cobalt (Co), Nickel (Ni), Copper (Cu), and Zinc (Zn) are the ten elements that can be found in the first row of transition metals.

Filling Transition Metal Orbitals

An argon (noble gas) core is used as the electron configuration for the first row transition metals, which consists of 4s and 3d subshells. Because this is only applicable to the transition metals in the first row, modifications will be required when writing the electron configuration for the transition metals in the other rows. The noble gas preceding the first row of transition metals would be the core, which would be written with brackets around the element symbol (for example, [Ar] would be used for the first row of transition metals), and the electron configuration would follow a [Ar] nsxndx format. In the case of transition metals from the first row, the electron configuration would simply be [Ar] 4sx3dxOn the periodic table, the energy level, “n,” of an element can be determined by simply looking at the row number in which the element is located. Except for the d-block and the f-block, there is an exception in which the energy level “n” for the d block is “n-1” (“n” minus 1) and for the f block is “n-2.”  In this case, the “x” in nsx and ndx is the number of electrons in a specific orbital (i.e. s-orbitals can hold up to a maximum of 2 electrons, p-orbitals can hold up to 6 electrons, d-orbitals can hold up to 10 electrons, and f-orbitals can hold up to 14 electrons). When attempting to determine the electron configuration of an element, count the number of boxes you come across before reaching the element for which you are attempting to determine the electron configuration.

Characteristics Of Transition Metal

Iron, cobalt, copper, and zinc are among the first-row transition metals that are essential to human health. Manganese and iron are among the first-row transition metals that are essential to human health. Three more first-row transition elements, including chromium, vanadium, and nickel, have demonstrated some beneficial biological effects in animal studies. Most of the time, these metals are consumed as part of a varied diet or as nutritional additives, and in the human body, they perform both structural and functional functions, including the maintenance of cellular functions that are involved in a wide range of biological activities, such as reproduction. Normal function, on the other hand, necessitates that the levels of metal ions be maintained within an acceptable range; lower concentrations may result in nutritional deficiency, while higher concentrations may result in toxicity. The physical properties of first-row elements, particularly titanium and nickel, are also important for the preparation of new materials and alloys, which results in technological advantages that improve the overall quality of life. According to some definitions, nine out of the ten first-row transition metals have densities greater than 5.0 g/cm3, indicating that they are considered to be “heavy metals.” However, despite the fact that this definition is commonly used by some, chemists do not agree with it. This is primarily because this definition is based on the density of the metal rather than the chemical properties of the metal. Furthermore, the negative connotation associated with the term “heavy metal,” as well as the toxicity of metals such as cadmium and mercury, stands in stark contrast to the fact that five of the first-row transition elements are required for the survival of all living things. Based on chemical properties, a more concise definition of the ambiguous term “heavy metal” could be developed, and it would include the block of metals in Groups 3 to 16 that are in periods 4 and greater. This definition of “heavy metals” does not include first-row elements, but rather only transition metals from the second and third rows of the periodic table. Even this definition, however, is up for debate. All five of the most important first-row transition metals, however, are not toxic “heavy metals,” as has been suggested in the literature.

Conclusion:

All first-row transition metals have extremely sensitive chemistry to their surrounding environments. Because water is present, each metal ion transforms into an equal number of hydrated ions, which undergo pH and concentration-dependent chemistry that is dictated by the presence of metabolites, proteins and other biological components. It is critical to understand that in cells, redox active metal ions do not exist as free ions, as is commonly assumed. This causes these metals to go through a process known as speciation chemistry, which is controlled by the oxidation state of the metal ion, pH of the surrounding environment, ionic strength, and the stability of metal complexes with biological molecules. According to the specific conditions, several metal ions form multinuclear species in aqueous solution, and as a result, many activities and functions will not be linear but will be extremely sensitive to concentrations and interactions with biomolecules. When it becomes clear that the identification of components in the system demystifies poorly understood processes in biology, the appreciation for classical speciation chemistry grows exponentially.