Physical and Chemical Properties of First Transition Series Elements
The Elements Of The First Transition Series are an important set of d-block metals, spanning from scandium to zinc in the periodic table’s fourth period. Known for their diverse oxidation states and intriguing periodic properties, these elements are fundamental to understanding advanced chemistry trends such as ionization energies and colored compound formation. In this article, we break down their key features, electronic structures, periodic trends, and exam-relevant facts with scientific clarity and SEO focus.
Defining Elements Of The First Transition Series
The first transition series includes ten elements, occupying atomic numbers 21 through 30. Situated between the s- and p-blocks, they display remarkable chemical versatility due to their partially filled 3d orbitals.
Members of the First Transition Series
- 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)
Electronic Configuration and Noteworthy Exceptions
- General configuration: $\mathrm{[Ar]\ 3d^{1-10}\ 4s^{0-2}}$.
- Chromium: $\mathrm{[Ar]\ 3d^5\ 4s^1}$ (half-filled d-subshell stability).
- Copper: $\mathrm{[Ar]\ 3d^{10}\ 4s^1}$ (fully filled d-subshell stability).
Periodic Trends and Ionization Enthalpy
Elements Of The First Transition Series reveal distinctive patterns in their ionization energies, linked to electron configurations and nuclear charge.
Ionization Enthalpy Patterns
- Highest First Ionization Enthalpy: Zinc (Zn)
— Its stable $3d^{10}4s^2$ configuration makes electron removal tough. This answers "which element of the first transition series has highest ionization enthalpy" and "which element of the first transition series has highest ionisation enthalpy". - Highest Second Ionization Enthalpy: Scandium (Sc)
— After one electron is lost, Sc forms a stable $3d^1$ ion. This clarifies "which element of the first transition series has highest second ionization enthalpy" and "which element of the first transition series has highest second ionisation enthalpy". - Highest Third Ionization Enthalpy: Manganese (Mn)
— The removal of a third electron yields a half-filled $3d^5$ shell which is highly stable. This addresses "which element of the first transition series has highest third ionization enthalpy" and "which element of the first transition series has highest third ionisation enthalpy". - Lowest Ionization Enthalpy: Vanadium (V)
— Due to its relatively larger atomic radius, it loses electrons most easily among the series.
Other Periodic Trends
- The fifth element of the first transition series is Manganese (Mn) (atomic number 25).
- Some members (like Cu$^{2+}$/Cu) show positive standard electrode potentials (E0), making them less easily oxidized ("elements of first transition series has positive e0").
Key Chemical and Physical Properties
Metals of the first transition series share crucial features, making them essential in both theoretical and applied chemistry.
- Apart from mercury (not in this series), all are solid, lustrous, and metallic.
- Most have high melting/boiling points and good conductivity.
- Multiple oxidation states — Manganese (Mn) exhibits the highest (+7), clarifying "which element of the first transition series shows highest oxidation state".
- Form colored ions/compounds via d-d transition; e.g., CuSO4 (blue), MnO4⁻ (purple).
- Catalyze industrial and biological reactions.
For a refresher on metal behavior, visit the related topic: metal properties and characteristics.
Exam-Relevant Details and Applications
Knowing periodic trends among the Elements Of The First Transition Series is vital for answering competitive exam questions. Key points for quick reference:
- Iron (Fe) — foundation of construction and machinery
- Copper (Cu) — essential for electrical wiring
- Zinc (Zn) — critical for galvanization
- Chromium (Cr) and Manganese (Mn) — important in alloy strengthening
To connect this knowledge with atomic concepts, explore atomic theory basics and review the periodic trends for broader context.
Summary Table: Essential Ionization Facts
| Highest First Ionization Enthalpy | Zinc (Zn) |
| Highest Second Ionization Enthalpy | Scandium (Sc) |
| Highest Third Ionization Enthalpy | Manganese (Mn) |
| Highest Oxidation State | Manganese (Mn, +7) |
| Lowest Ionization Enthalpy | Vanadium (V) |
| Fifth Element | Manganese (Mn) |
The Elements Of The First Transition Series bridge the s- and p-blocks, bringing a wide spectrum of chemical behaviors into one row—from variable oxidation states and colored ions to catalytic potential and diverse ionization energies. Mastering their periodic trends—such as which element has highest second or third ionization enthalpy, or highest oxidation state—not only strengthens your chemistry foundation but also prepares you for advanced learning and competitive exams. For more on foundational chemistry topics, continue to physical science principles.
FAQs on What Are the Elements of the First Transition Series?
1. What are the elements of the first transition series?
The elements of the first transition series include the ten chemical elements with atomic numbers 21 to 30, spanning the Scandium (Sc) to Zinc (Zn) range in Period 4 of the Periodic Table.
- 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)
2. Why are the elements from Scandium to Zinc called the first transition series?
The elements from Scandium to Zinc are called the first transition series because they are the first set of elements where the d-orbital starts filling after the 4s orbital.
- They belong to Period 4 in the Periodic Table.
- They show gradual filling of 3d orbitals from Sc (3d¹) to Zn (3d¹⁰).
- They display typical transition element properties such as variable oxidation states, formation of coloured compounds, and catalytic activity.
3. What are the general properties of first transition series elements?
The first transition series elements show unique physical and chemical properties due to their electronic structures. Key features include:
- Variable oxidation states
- Formation of coloured ions and compounds
- High melting and boiling points
- Good electrical and thermal conductivity
- Complex formation tendency
- Catalytic activity
- Magnetic properties (paramagnetism or ferromagnetism)
4. What is the electronic configuration of first transition series elements?
The general electronic configuration of first transition series elements is [Ar] 4s² 3d¹-n, where n increases from 1 (Scandium) to 10 (Zinc).
- Sc: [Ar] 4s² 3d¹
- Ti: [Ar] 4s² 3d²
- V: [Ar] 4s² 3d³
- Cr: [Ar] 4s¹ 3d⁵ (exception)
- Mn: [Ar] 4s² 3d⁵
- Fe: [Ar] 4s² 3d⁶
- Co: [Ar] 4s² 3d⁷
- Ni: [Ar] 4s² 3d⁸
- Cu: [Ar] 4s¹ 3d¹⁰ (exception)
- Zn: [Ar] 4s² 3d¹⁰
5. What are transition elements? Give examples from the first transition series.
Transition elements are d-block elements that have partially filled d-orbitals in their ground or common oxidation states.
- Examples from the first transition series include: Scandium (Sc), Titanium (Ti), Vanadium (V), Chromium (Cr), Manganese (Mn), Iron (Fe), Cobalt (Co), Nickel (Ni), Copper (Cu), and Zinc (Zn).
- These elements show typical transition metal properties such as variable valency and formation of coloured ions.
6. Why is Zinc not considered a typical transition element?
Zinc is not considered a typical transition element because its commonly occurring oxidation state (+2) has a fully filled d-subshell (3d¹⁰).
- It does not form coloured ions.
- It does not show variable oxidation states.
- It lacks most typical transition metal characteristics.
7. What are the uses of transition elements from the first transition series?
The transition elements of the first transition series have many applications due to their unique properties:
- Iron: Used to make steel and alloys, tools, and machinery.
- Copper: Used in electrical wiring and electronics.
- Chromium: Used for chrome plating and making stainless steel.
- Titanium: Used in aerospace, medical implants, and strong lightweight alloys.
- Manganese: Used in the steel industry as a hardness enhancer.
8. What are some common oxidation states among the first transition series elements?
The first transition series elements commonly exhibit multiple oxidation states, a key feature in CBSE exams.
- Scandium: +3
- Titanium: +3, +4
- Vanadium: +2, +3, +4, +5
- Chromium: +2, +3, +6
- Manganese: +2, +4, +7
- Iron: +2, +3
- Cobalt: +2, +3
- Nickel: +2, +3
- Copper: +1, +2
- Zinc: +2 (only)
9. Why do transition elements form coloured compounds?
Transition elements form coloured compounds because of the presence of unpaired electrons in their d-orbitals.
- When light passes through these compounds, electrons jump between different d-orbital energy levels, absorbing specific wavelengths and emitting colour.
- The specific colour observed depends on the electronic configuration and the ligands attached to the metal ion.
- This property is characteristic of transition metals and is included in the CBSE syllabus for the first transition series.
10. How does the atomic and ionic radii change across the first transition series?
The atomic and ionic radii of first transition series elements generally decrease from Scandium to Copper due to an increase in nuclear charge, but they remain almost constant or change very little across the series.
- From Sc to Zn, the increase in nuclear charge is counteracted by the increase in electron-electron repulsion in the 3d orbitals.
- This trend is unique among d-block elements and is important for exam preparation.
11. What is the importance of the first transition series in metallurgy?
The first transition series elements play a vital role in metallurgy because they form strong alloys and compounds essential to the industry.
- Iron alloys (like steel) are fundamental to construction.
- Chromium and Nickel are used in stainless steel.
- Titanium is used for lightweight, high-strength materials.
