Introduction to Transition Elements

What are Transition Elements?

• Transition elements are those that have partially filled (d) or (f) orbitals.
• They have one or more oxidation states.

Role of (d) and (f) Orbitals

• When there are 1 to 9 electrons in the (d) orbital, it is said to be partially filled.
• Similarly, when there are 1 to 13 electrons in the (f) orbital, it is said to be partially filled.

What is Atomic State?

• Atomic state refers to the condition when the symbol of an element is written.
• It represents the atom and electronic configuration of the element.

Possible Oxidation States

• Zinc is always found as (Zn^{2+}).
• Iron is found in both (Fe^{2+}) and (Fe^{3+}).
• Copper is found in (Cu^{+1}) and (Cu^{2+}).

Importance of Transition Elements

• They are called transition elements because they lie between two different types of elements.
• (d)-block elements are called outer transition elements and (f)-block elements are called inner transition elements.

Position of Transition Elements in the Periodic Table

• The (d)-block contains 37 elements.
• The (f)-block contains 28 elements.

Electronic Configuration and Transition Elements

• (d)-block: ((n-1)d^{1-10}ns^{1-2})
• (f)-block: ((n-2)f^{1-14}(n-1)d^{0-1}ns^2)

Specific Properties

• Transition elements form colored compounds.
• They are found in various oxidation states.
• They exhibit diversity in their quantity and chemical properties.
• They have good thermal and electrical conductivity.

Classification of Transition Elements

• General: Those that exhibit all characteristics of transition elements.
• Non-General: Such as zinc, cadmium, and mercury that do not fully follow transition characteristics.

Conclusion

• Transition elements play an important role in chemistry.
• Their properties and various oxidation states make them an important subject of study.

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