One simple rationalisation for this is Paulings principle of electroneutrality. This simply put says that bonding schemes that reduce charge separation are more stable.
This is not a simple area- many high oxidation states are fluoride compounds- and the very weak F-F bond makes the "elimination" of F2 molecules less likely and hence stabilises the high oxidation state compound. Many high oxidation state compounds are oxides and there are many opportunities for pi bonding interactions in these. The short V=O in vanadyl complexes is a case in point.
The early vs. late transition metals differ in their oxidation states (each metal has different possible oxidation states). Electrons have a stronger attraction to the protons in the late transition metals, so the later transition metals form bonds that are harder to break. You can read more about transition metal properties from the links below.Source(s):
Transition metals
The suffis -ous is added for a lower valence and the suffix -ic for a higher valence.Examples: ferric-ferrous, cupric-cuprous.
transition metals
Roman numerals are used to indicate oxidation states. Apex
transition metals have variable oxidation states
The early vs. late transition metals differ in their oxidation states (each metal has different possible oxidation states). Electrons have a stronger attraction to the protons in the late transition metals, so the later transition metals form bonds that are harder to break. You can read more about transition metal properties from the links below.Source(s):
Transition metals
The suffis -ous is added for a lower valence and the suffix -ic for a higher valence.Examples: ferric-ferrous, cupric-cuprous.
Roman numerals are used to indicate oxidation states.
transition metals
Romann numerals are used: (I), (II)...
Transition metals have multiple oxidation states due to the number of electrons that an atom loses, gains, or uses when joining another atom in compounds. It also determined the ability of an atom to reduce.
Roman numerals are used to indicate oxidation states. Apex
Sc and Zn are not classified as transition metals. They does not have stable different oxidation numbers.
Transition metals can move electrons between the outer shell and the d d orbital. For example, copper can either lose its 2 s electrons or move one of those s electrons into d orbital, which is one electron short of being full.
The transition metals (groups 3-12) can have more than one positive oxidation state. When you write the names of compounds with transition metals, you note their oxidation state with roman numerals, e.g. iron (II) oxide and iron (III) oxide.