Transition Elements in Chemistry: Overview, Properties & Uses

Transition elements are essential in chemistry and help students understand various practical and theoretical applications related to this topic. They explain the unique behavior of metals found in the middle of the periodic table and reveal how these elements impact everything from the color of gemstones to the speed of chemical reactions.

What is Transition Element in Chemistry?

A transition element refers to a metallic element whose atom or ion has a partially filled d-subshell. These elements are placed in groups 3 to 12 (d-block) of the modern periodic table. Transition elements appear in chapters related to periodic classification, electronic structure, and coordination compounds, making them a foundational part of your chemistry syllabus.

Transition Elements List and Series

Transition elements are arranged in four main transition series depending on which d-subshell is being filled by electrons. The most commonly studied are the first 10 transition elements of the 3d series. See their names and atomic numbers below:

Element	Symbol	Atomic Number
Scandium	Sc	21
Titanium	Ti	22
Vanadium	V	23
Chromium	Cr	24
Manganese	Mn	25
Iron	Fe	26
Cobalt	Co	27
Nickel	Ni	28
Copper	Cu	29
Zinc	Zn	30

Other transition element series include the 4d (Y to Cd), 5d (Hf to Hg), and 6d (elements beyond Rf) series. These elements are also called d-block elements.

General Properties of Transition Elements

• They display variable oxidation states (for example, Fe²⁺ and Fe³⁺).
• Most form colored compounds and ions due to d-d electronic transitions.
• Many are good catalysts in both natural and industrial reactions.
• Transition elements often show magnetic properties (paramagnetism) due to unpaired electrons.
• They have high melting and boiling points, and are all metals with high density and hardness.
• They can form complex ions with molecules like water, ammonia, and cyanide.

Electronic Configuration of Transition Elements

The electronic configuration of transition elements typically follows the pattern (n-1)d^1-10 ns^0-2. For example, Iron(Fe): [Ar] 3d⁶ 4s².

Some transition elements show exceptional configurations to increase stability:

These configurations give extra stability due to half-filled (d⁵) or fully-filled (d¹⁰) d-subshells. Many transition elements can lose variable numbers of d and s electrons, leading to multiple oxidation states.

Transition vs. Inner Transition Elements

Property	Transition Elements	Inner Transition Elements
Periodic Table Location	Groups 3-12 (d-block)	f-block (Lanthanides & Actinides; separate rows at bottom)
Differentiating Electron	(n-1)d electrons	(n-2)f electrons
Examples	Fe, Cu, Zn, Cr	La, Ce, U, Th
Main Use	Catalysis, metallurgy, alloys	Nuclear fuel, strong magnets

Uses of Transition Elements in Real Life

Transition elements play important roles in everyday life and industry:

• Iron (Fe): Used in construction (steel), tools, and our blood (hemoglobin).
• Copper (Cu): Electrical wiring, important in alloys like bronze.
• Nickel (Ni) and Chromium (Cr): Making stainless steel (corrosion resistance).
• Palladium (Pd) and Platinum (Pt): Automobile catalytic converters, jewelry.
• Manganese (Mn): Used in dry cell batteries.
• Many colored gemstones (like ruby, emerald) get color from traces of transition elements (Cr, Fe, Co).

Relation with Other Chemistry Concepts

Transition elements are closely related to d-block elements and coordination compounds. Understanding these topics helps connect how their electronic structure results in colored ions and how they act as catalysts or form stable complex ions. You can also compare their properties with main-group elements and explore different blocks of the periodic table for a complete understanding.

Step-by-Step Reaction Example

Let’s look at the oxidation of iron (Fe) to form iron (III) oxide (rust):

1. Write the balanced equation

2. Iron starts as Fe⁰ (metal). Each Fe atom loses electrons to become Fe³⁺ (oxidation state increases; a typical property of transition metals).
3. Oxygen molecules accept these electrons and convert into O^2–, making the ionic oxide.
4. Final Answer: Rust formation involves a change in oxidation states—showing variable oxidation states—a key property of transition elements.

Lab or Experimental Tips

Remember transition elements by looking for elements in the “d-block” (groups 3–12). Most are metals showing color in their compounds or ions. Vedantu educators often use color charts of transition compounds to help students visualize these properties during live classes.

Try This Yourself

• Write the full electronic configuration for chromium (atomic number 24).
• List any two colored compounds of transition metals found in daily life.
• What is the main difference between d-block and f-block elements?
• Name one industrial use each of iron and platinum.

Final Wrap-Up

We explored transition elements—their definition, properties, series, electronic structure, and practical importance. They are vital to our lives, from construction to medicine and technological advances. For easy-to-follow notes and in-depth guidance, explore live classes and expert solutions on Vedantu.