Why do metals have different oxidation states?

Because of the orbital split energy and electron pairing energy, transition metal in different complexes would like to “throw” away different numbers of its electrons to achieve the maximum stability. That is why they show different oxidation states in different complexes.

What does varying oxidation states mean?

A variable oxidation state is a value that determines the charge of the atom depending on certain conditions. If one element in the reaction has oxidized, the other must be reduced. To put it more simply, if one element has given up electrons, then another element must accept them.

Which type of metals can have various oxidation states?

Transition metals are the elements in Groups 3 to 12 representing the d block of the periodic table. Due to the relatively low reactivity of unpaired d electrons, these metals typically form several oxidation states and therefore can have several oxidation numbers.

What elements have different oxidation states?

Determining oxidation states

Element	Usual oxidation state	Exceptions
Oxygen	Usually -2	Peroxides and F2O (see below)
Hydrogen	Usually +1	Metal hydrides (-1) (see below)
Fluorine	Always -1
Chlorine	usually -1	Compounds with O or F (see below)

Why do all transition metals have a stable 2+ oxidation state?

Because only two electrons can exist in an S orbital, and removing the electrons from the sub shell below it requires immense amounts of energy, this limits them to a +2 charge most of the time. Although many can from ions with multiple charges, (well known examples in everyday life include iron and copper).

Why is the 2+ oxidation state so common for transition metals?

Transition metals have different electronic states. Since their orbitals have large volume, the energy required to give away electrons is very less. The transition metals have s,p,d and f orbitals. So it is easy to give 2 electrons from S orbital forming common oxidation state in transition metals.

Why do some metals have more than one charge?

Many transition metals cannot lose enough electrons to attain a noble-gas electron configuration. In addition, the majority of transition metals are capable of adopting ions with different charges. Because most transition metals have two valence electrons, the charge of 2+ is a very common one for their ions.

Do all transition metals have multiple oxidation states?

It also determines the ability of an atom to oxidize (to lose electrons) or to reduce (to gain electrons) other atoms or species. Almost all of the transition metals have multiple oxidation states experimentally observed.

Why is oxidation state more stable?

– When chromium loses 3 electrons then the electronic configuration becomes (Ar) 3d3 which is most stable because at the t2g level the dxy, dyz and dxzorbitals are half-filled. – That’s why the oxidation state of +3 is the most stable oxidation state than the +4, +2 and +6 oxidation states.

Do all transition metals have more than one oxidation state?

Why do transition metals have multiple oxidation states?

Transition metals can have multiple oxidation states because of their electrons. The transition metals have several electrons with similar energies, so one or all of them can be removed, depending the circumstances. When they attach to other atoms, some of their electrons change energy levels.

Do all elements have different oxidation states?

Lots of elements do have different oxidation states – the transition metals almost all do, sulphur, nitrogen and chlorine are well known for theirs. In fact, the only elements with fixed oxidation states are the metals in Group 1, Group 2 and Fluorine.

Why do transition metals have variable energy levels?

The transition metals have several electrons with similar energies, so one or all of them can be removed, depending the circumstances. When they attach to other atoms, some of their electrons change energy levels. Keeping this in view, why do transition metals have variable oxidation states?

What happens to the oxidation state when an atom is reduced?

Oxidation results in an increase in the oxidation state. Reduction results in a decrease in the oxidation state. If an atom is reduced, it has a higher number of valence shell electrons, and therefore a higher oxidation state, and is a strong oxidant. For example, oxygen (O) and fluorine (F) are very strong oxidants.