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Transition metals have multiple oxidation numbers because of their ability to lose different numbers of electrons from their outermost d orbitals. These d orbitals can accommodate varying numbers of electrons, resulting in different oxidation states for transition metals based on how many electrons they gain or lose during chemical reactions.
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What elements tend to have multiple oxidation numbers?
Transition metals such as iron, copper, and chromium often exhibit multiple oxidation states due to the availability of d orbitals in their electron configurations. Nonmetals like sulfur, phosphorus, and chlorine can also have multiple oxidation numbers, with sulfur being able to range from -2 to +6 and chlorine from -1 to +7.
Do all metals have two oxidation numbers?
No, not all metals have two oxidation numbers. Some metals may have multiple oxidation numbers depending on the bonding situation and the compounds they form.
Why transition metals have variable oxidation number?
Transition metals have variable oxidation numbers because they have incompletely filled d orbitals in their outermost electronic shell. These d orbitals can participate in bonding and easily change their oxidation states by gaining or losing electrons. This flexibility allows transition metals to exhibit a wide range of oxidation states in different compounds.
Is it true that Transition Metals can have more than one oxidation charge?
Yes, transition metals can have various oxidation states due to the availability of multiple d orbitals for electron transfer. This allows them to form compounds with different oxidation states depending on their chemical environment.
How do you find the oxidation number using the periodic table of elements?
To find the oxidation number of an element using the periodic table, you need to consider the group number for main group elements and the charge on transition metals. Main group elements typically have oxidation numbers equal to their group number, while transition metals can have multiple oxidation states indicated by Roman numerals in parentheses. Exceptions like oxygen (-2) and hydrogen (+1) exist, and the sum of oxidation numbers in a compound must equal zero.
