Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?
Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only? Answer: Both fluorine and oxygen have small size, high electronegativity and also high negative electron gain enthalpy. Thus, the highest oxidation states are shown in the oxides and fluorides of transition metals.
Why is the highest oxidation state stable with F and O?
For example, oxygen (O) and fluorine (F) are very strong oxidants. Both oxide and fluoride ions are highly electronegative and have a very small size. Due to these properties, they are able to oxidize the metal to its highest oxidation state.
Why are higher oxidation states of transition metals unstable?
In group of d-block elements the oxidation state for heavier elements is more stable as the core (after removing valence electrons the remainder is called core) of these elements is unstable and hence can lose one or more electrons from the unstable core gives higher oxidation states, due to which their covalent …
Why lower oxidation states are more stable than higher oxidation states?
Lower oxidation states are favoured by the heavier members of the p-block. The elements of group 13-18 have 3 to 8 electrons in their valence shell (ns2npl-6) and, therefore, exhibit, oxidation state of + 3, +2, so on. Hence, there is high stability of lower oxidation states for the heavier elements of p-block.
Why is the highest oxidation state of a transition metal exhibited?
Oxygen and fluorine behave as strong oxidising agents because of their high electronegativities and small sizes. Hence, they bring out the highest oxidation states from the transition metals. In other words, a transition metal shows higher oxidation states in oxides and fluorides.
Why is the highest oxidation state of a metal exhibited?
– Therefore, the highest oxidation state of metals is exhibited by oxides and fluorides due to their high oxidizing power. Note: Remember due to high electronegativity, oxygen and fluorine have high oxidizing power and hence, highest oxidation state of metals is achieved in their oxide or fluoride form.
How does the stability of higher oxidation states vary down the groups of transition elements explain with an example?
On moving down the group in the transition elements the stability of higher oxidation states increases. This is due to the similarity of the energy of the d orbitals with the outer s orbitals. Hence the d orbitals are more available towards the bond formation.
What is the highest oxidation state exhibited by transition metals?
If we consider all the transition metals the highest oxidation state is eight and the element which shows +8 oxidation state are Ruthenium (Ru) and Os(Osmium).
Are higher oxidation states more stable?
stability of higher oxidation states of transition metal halides. 2.In higher oxidation states covalent bonds are formed because of that the compounds of higher oxidation state of d-block elements are stable.
Why does oxidation state stability decrease?
The stability of group oxidation state decreases down the group due to inert pair effect. Inert pair effect is simply the non participation of s orbitals in bond formation .
What can high oxidation states be Stabilised by?
Stabilization of high oxidation states by strong electron-donating ligands.
Why are most transition metal compounds highly colored?
The reason why transition metal in particular are colorful is because they have unfilled or either half filled d orbitals. There is Crystal field theory which explains the splitting of the d orbital, which splits the d orbital to a higher and lower orbital. Now, the electrons of the transition metal can “jump”.