

What Are Transition Elements? Definition, List, and Key Properties
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)d1-10 ns0-2. For example, Iron(Fe): [Ar] 3d6 4s2.
Some transition elements show exceptional configurations to increase stability:
Copper (Cu): [Ar] 3d10 4s1
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 equation2. 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 O2–, 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.
FAQs on Transition Elements in Chemistry: Overview, Properties & Uses
1. What are transition elements?
Transition elements are metallic elements found in groups 3 to 12 of the periodic table. They have partially filled d-orbitals and often exhibit properties such as variable oxidation states, formation of colored compounds, and catalytic behavior.
2. List the first 10 transition elements with their symbols.
The first 10 transition elements are:
- Scandium (Sc)
- Titanium (Ti)
- Vanadium (V)
- Chromium (Cr)
- Manganese (Mn)
- Iron (Fe)
- Cobalt (Co)
- Nickel (Ni)
- Copper (Cu)
- Zinc (Zn)
3. What are four main properties of transition elements?
Transition elements have the following key properties:
- They show variable oxidation states
- Form colored compounds
- Demonstrate catalytic activity
- Possess magnetic properties due to unpaired d-electrons
4. Where are transition elements located on the periodic table?
Transition elements occupy the central block (groups 3–12) of the periodic table, also known as the d-block elements, spanning periods 4 to 7.
5. What is the general electronic configuration of transition elements?
The general electronic configuration for transition elements is (n-1)d1–10ns0–2.
For example, Iron (Fe) has [Ar] 3d64s2. Exceptions include Chromium and Copper, where stability favors half-filled or fully filled d-subshells.
6. What is the difference between transition and inner transition elements?
Transition elements are d-block elements (groups 3–12) with partially filled d-orbitals, while inner transition elements are f-block elements (lanthanides and actinides) with partially filled f-orbitals.
7. Why do transition elements form colored compounds?
Transition elements form colored compounds because of electronic transitions between d-orbitals. The absorption of specific wavelengths of visible light results in characteristic colors for different ions.
8. Why are Zn, Cd, and Hg sometimes not considered true transition elements?
Zinc, Cadmium, and Mercury have completely filled d10 configurations in their common oxidation states, so they do not show typical transition element properties like variable oxidation states or colored ions.
9. How do transition elements act as catalysts?
Transition elements can act as catalysts because:
- They provide access to variable oxidation states
- Offer adsorption sites for reactants on their surfaces
- Facilitate the formation of intermediate complexes
10. Give some important uses of transition elements.
Transition elements have vital applications, including:
- Iron: construction (steel manufacture)
- Copper: electrical wiring and coins
- Zinc: galvanizing iron (corrosion protection)
- Chromium: stainless steel production and pigments
11. What are complex ions and how are they related to transition elements?
Complex ions are formed when transition metal ions are surrounded by ligands through coordinate bonds. Transition elements easily form complexes due to small size, high charge, and availability of empty d-orbitals.
12. What are exceptions in the electronic configuration of transition elements?
Chromium (Cr) and Copper (Cu) have unusual configurations for extra stability:
- Cr: [Ar] 3d54s1
- Cu: [Ar] 3d104s1

















