Respuesta :
The major difference between the number of oxidation states of most transition elements and that of most main-group elements is most of the transition metals have a partially-filled d sublevel.
Why do transition metal have more oxidation states than other elements?
- The d sublevel of the majority of transition metals is only partially occupied.
- Between this and the valence shell, electrons can be transported.
- Every orbital in a particular sublevel tends to have the same number of electrons in the most stable configurations (typically empty or full, but occasionally they're held by unpaired electrons, like the iron).
- Metal-metal bonding has a lot more potential with transition metals.
- The primary distinction between the number of oxidation states of most transition elements and those of most main-group elements is that the bulk of transition metals have a partially-filled d sublevel.
Transition metals are situated between s-block and p-block elements in the periodic table. They go by the name "d-block elements." The term "transition metals" describes a class of metals that exhibit instability and transitional behaviour between s block and p block elements.
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