Question

What are the two important oxidation states of Group 6 elements of the periodic table?

Answer 1

A group (also known as a family) in chemistry is a column of chemical elements in the periodic table. The topmost member of a group may either be used to identify it, or it can be given a name. Group 16 is known as the "oxygen group" and the "chalcogens," for example.

Complete answer:
The periodic table's Group 6 is a group of elements numbered according to IUPAC form. Chromium (Cr), molybdenum (Mo), tungsten (W), and seaborgium are among its members (Sg). Many of these elements are transition metals, with the exception of chromium, molybdenum, and tungsten, which are refractory metals. Though the outermost shells do correspond with patterns in chemical activity, the electron structure of these elements does not follow a coherent pattern.

ATOMIC NUMBER	ELEMENT	ELECTRONIC CONFIGURATION
24	chromium	2, 8, 13, 1
42	molybdenum	2, 8, 18, 13, 1
74	tungsten	2, 8, 18, 32, 12, 2
106	seaborgium	2, 8, 18, 32, 32, 12, 2

When an atom joins with another atom in a complex, its oxidation state is related to the amount of electrons it loses, gains, or appears to use. It also affects an atom's tendency to oxidise (lose electrons) or minimise (gain electrons) other atoms or species. Almost all transition metals can exist in several oxidation states.
Since transition metals are comparatively quick to lose electrons compared to alkali metals and alkaline earth metals, most of them have several oxidation states. The valence s-orbital of alkali metals has one electron, and their ions nearly all have oxidation states of +1. (from losing a single electron). Alkaline earth metals, on the other hand, have two electrons in their valence s-orbitals, resulting in ions with a +2 oxidation state (from losing both). Transition metals, on the other hand, are more complex, with a wide variety of visible oxidation states owing to the loss of d-orbital electrons.
Group 6 has two significant oxidation states: +3 and +6.
Suppose you consider Cr $[{\text{Ar}}]3\;{{\text{d}}^5}4\;{{\text{s}}^1}$
Cr has 24 electrons. It can either lose 3 or 6 electrons to become stable.

Note:
Transition metal oxidation states are similar to those of most other ions, with the exception that the d orbital is degenerate with the s orbital of the higher quantum number. Transition metals gain equilibrium by arranging their electrons in the correct order and then being oxidised or losing electrons to other atoms and ions. These cations either go on to form coordination complexes or contribute to the synthesis of other compounds.