List of Elements in the First Transition Series
Elements of the First Transition Series is essential in chemistry and helps students understand various practical and theoretical applications related to this topic. This group of elements, often called the 3d transition metals, forms a critical foundation for understanding the behavior of d-block elements, their oxidation states, magnetic properties, and practical relevance in fields ranging from industry to biology.
What is Elements of the First Transition Series in Chemistry?
A First Transition Series element refers to any of the ten d-block elements from Scandium (Sc, atomic number 21) to Zinc (Zn, atomic number 30) in the fourth period of the modern periodic table. This concept appears in chapters related to transition elements, electronic configuration of d-block elements, and oxidation states of elements, making it a foundational part of your chemistry syllabus.
Molecular Formula and Composition
There is no single molecular formula for the entire first transition series since it represents a set of chemical elements, not a compound. The series includes: Scandium (Sc), Titanium (Ti), Vanadium (V), Chromium (Cr), Manganese (Mn), Iron (Fe), Cobalt (Co), Nickel (Ni), Copper (Cu), and Zinc (Zn). All are categorized under transition metals, and each displays unique chemical and physical characteristics due to their electronic configuration.
Preparation and Synthesis Methods
Elements of the first transition series are primarily found in the Earth's crust as ores and minerals. Their extraction involves processes like reduction of oxides, electrolytic reduction, and purification through methods such as zone refining. For example, iron is commonly extracted using blast furnace reduction, while copper is purified by electrolysis. These processes are covered in more detail within Vedantu’s metallurgy and extraction of elements page.
Physical Properties of Elements of the First Transition Series
The first transition series elements are typically hard, have high melting and boiling points, shiny metallic luster, and high density (except Sc and Zn). They are generally good conductors of heat and electricity. Many form beautifully colored compounds due to d-d electronic transitions. For instance, copper compounds appear blue or green, and manganese compounds are often pink to purple. Most are found as solid metals at room temperature, with different crystal structures.
Chemical Properties and Reactions
These elements show variable oxidation states, form stable complexes, and have a high tendency to act as catalysts. For example, iron forms Fe2+ and Fe3+ ions; manganese can go from +2 to +7. They often form colored ionic compounds and can participate in redox, acid-base, and salt formation reactions. Chromium can exist as Cr2+, Cr3+, or Cr6+, each with distinct chemistry. Many of these metals also readily alloy with one another.
Frequent Related Errors
- Confusing the first transition series with inner transition elements (lanthanides/actinides).
- Ignoring the special stability of half-filled (Cr) and fully-filled (Cu, Zn) d-orbitals when writing electronic configurations.
- Forgetting exceptions in electron filling—especially in Chromium and Copper.
- Assuming all transition metals are magnetic, while Zn and Cu are not due to paired electrons.
Uses of Elements of the First Transition Series in Real Life
Elements of the first transition series are widely used in our daily lives and industries. Iron (Fe) is essential for making steel and machinery parts. Copper (Cu) is used for electrical wiring and plumbing due to its high conductivity. Zinc (Zn) is applied in galvanization to prevent rusting. Manganese improves the hardness of steel. Chromium is key in stainless steel and as pigments.
Relevance in Competitive Exams
Students preparing for NEET, JEE, and Olympiads should be familiar with elements of the first transition series, as these elements often feature in questions related to periodic trends, exceptions, colored compounds, variable oxidation states, and practical extraction methods. Understanding these properties can also help solve conceptual and calculation-based problems in board exams.
Relation with Other Chemistry Concepts
Elements of the first transition series are closely related to topics such as magnetic properties of transition elements and catalysis, helping students build a bridge between periodicity, bonding, and practical application chapters. Connections and variable oxidation states also deepen understanding of chemical reactivity and complex formation.
Step-by-Step Reaction Example
- Oxidation of Iron (Formation of Rust):
4Fe(s) + 3O2(g) + 6H2O(l) → 4Fe(OH)3(s) - Explaination:
Iron reacts with oxygen and water in the air to form hydrated iron(III) oxide (rust). The process is catalyzed by the presence of moisture and can be further accelerated by salt.
Lab or Experimental Tips
Remember the order of elements in the first transition series using the mnemonic: "Scary Tigers Vanish Craving Many Fish Coated Nicely Covered with Zinc." Vedantu educators often suggest such memory aids to help you recall the 10 elements and their atomic numbers effectively.
Try This Yourself
- List the electronic configuration of Chromium (Cr) and explain its exception.
- Which element in the first transition series shows the highest oxidation state?
- Give two examples of industrial uses for Copper and Zinc.
- Arrange these metals in order of increasing atomic number: Fe, Cu, Ti, V.
Final Wrap-Up
We explored elements of the first transition series—their order, unique properties, exceptions in electron configuration, chemical reactivity, and their widespread use in real life. A strong grasp of these concepts boosts your confidence and performance in chemistry exams. For more in-depth learning, revision notes, and live problem-solving with experts, visit Vedantu’s topic pages and live sessions.
FAQs on Elements of the First Transition Series
1. What are the elements of the first transition series as per the NCERT syllabus?
The first transition series, also known as the 3d series, consists of the ten elements in the fourth period of the periodic table where the 3d orbitals are progressively filled. These elements begin with Scandium (Sc), atomic number 21, and end with Zinc (Zn), atomic number 30. The elements are: Scandium (Sc), Titanium (Ti), Vanadium (V), Chromium (Cr), Manganese (Mn), Iron (Fe), Cobalt (Co), Nickel (Ni), Copper (Cu), and Zinc (Zn).
2. How is the electronic configuration of the first transition series elements written?
The general electronic configuration for the first transition series (3d series) is [Ar] 3d1-10 4s1-2. Electrons first fill the 4s orbital before filling the 3d orbital, but there are notable exceptions. For example, the configuration of Chromium is [Ar] 3d5 4s1, not 3d4 4s2, due to the extra stability of a half-filled d-orbital. Similarly, Copper has the configuration [Ar] 3d10 4s1 instead of [Ar] 3d9 4s2 due to the stability of a completely filled d-orbital.
3. Why are there anomalies in the electronic configurations of Chromium (Cr) and Copper (Cu)?
The anomalies in the electronic configurations of Chromium and Copper are due to the enhanced stability associated with half-filled and completely filled d-orbitals. A half-filled d-orbital (d5) and a completely filled d-orbital (d10) exhibit greater stability due to symmetrical electron distribution and higher exchange energy.
4. Why do the elements of the first transition series exhibit variable oxidation states?
The first transition series elements show variable oxidation states because the energy difference between the (n-1)d orbitals (i.e., 3d) and the ns orbital (i.e., 4s) is very small. This allows electrons from both the 3d and 4s orbitals to participate in chemical bonding. For example, Manganese (Mn) can show oxidation states from +2 to +7, the highest in the series.
5. What is the general trend in atomic radii across the first transition series?
Across the first transition series (from Sc to Zn), the atomic radius initially decreases, then remains nearly constant, and finally increases slightly. The initial decrease (Sc to Cr) is due to the increasing nuclear charge. The nearly constant radius (Mn to Ni) results from the balance between increasing nuclear charge and increased shielding by d-electrons. The slight increase (Cu to Zn) is caused by increased electron-electron repulsion in the filled d-orbital of Zinc.
6. Why are most compounds of the first transition series elements coloured?
Most compounds of the first transition series are coloured due to the presence of incompletely filled d-orbitals in their ions. This allows for a phenomenon called d-d transition. When visible light falls on these compounds, an electron from a lower energy d-orbital absorbs a specific wavelength of light to get excited to a higher energy d-orbital. The colour we see is the complementary colour of the light absorbed.
7. How do the magnetic properties of the first transition series elements relate to their electronic configuration?
The magnetic properties are directly linked to the number of unpaired electrons in the d-orbitals. Elements with unpaired d-electrons exhibit paramagnetism (weak attraction to a magnetic field), while those with no unpaired d-electrons are diamagnetic (weak repulsion by a magnetic field).
8. What types of oxides are formed by the first transition series elements?
The elements of the first transition series form different types of oxides depending on their oxidation state. The character of the oxide changes from basic to amphoteric and finally to acidic as the oxidation state of the metal increases. Examples include: basic oxides (Sc2O3, TiO, FeO), amphoteric oxides (TiO2, Cr2O3, ZnO), and acidic oxides (V2O5, CrO3, Mn2O7).
9. Why do elements of the first transition series have high melting and boiling points?
The high melting and boiling points of these elements are attributed to the strength of their metallic bonds. These bonds involve not only the ns electrons but also the unpaired (n-1)d electrons. The greater the number of unpaired d-electrons available for bonding, the stronger the interatomic attraction, leading to high melting and boiling points. Zinc is an exception due to its filled d-orbital, resulting in weaker metallic bonds.
10. Why are the first transition series elements good catalysts?
First transition series elements and their compounds are excellent catalysts primarily due to their variable oxidation states and ability to form complexes. Their variable oxidation states provide alternative reaction pathways with lower activation energies. Their ability to form complexes allows them to bind to reactants, facilitating the reaction. For example, Iron is a crucial catalyst in the Haber process for ammonia synthesis.
11. What are some important applications of the first transition series elements?
Elements of the first transition series have numerous applications. Iron is vital in steel production, Titanium is used in aerospace alloys due to its high strength-to-weight ratio, Chromium enhances the corrosion resistance of steel (stainless steel), Manganese is used in steelmaking to increase hardness, and Copper is extensively used in electrical wiring due to its high conductivity. Many elements also serve as essential components in catalysts, pigments, and various industrial processes.
12. Explain the difference between paramagnetism and diamagnetism in the context of the first transition series.
Paramagnetism arises from the presence of unpaired electrons, resulting in a net magnetic moment and a weak attraction to an external magnetic field. Many transition metal ions exhibit paramagnetism. Diamagnetism, conversely, is observed in substances with all paired electrons; it's characterized by a weak repulsion from an external magnetic field. Ions with completely filled d-orbitals, like Zn2+, are diamagnetic.
