Q.Why do the transition elements exhibit higher enthalpies of atomisation?
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Transition Elements: From Intuition to Definition
Imagine you're building a house with bricks. Most bricks are identical — you stack them in neat rows. But some bricks are special: they have extra slots on their sides where you can attach hooks, magnets, or other bricks. These special bricks can change the shape of the wall, conduct electricity, or even change colour when you heat them.
In the periodic table, transition elements are those special bricks. They are the metals that sit in the middle block — groups 3 to 12 — and they have a unique ability: they can use their inner electrons (not just the outermost ones) to form bonds, change oxidation states, and create colourful compounds.
The Intuition: Why "Transition"?
The word "transition" comes from the idea that these elements form a bridge between the highly reactive metals on the left (like sodium, magnesium) and the less reactive metals / non-metals on the right (like aluminium, silicon). Their properties are not extreme — they are in-between.
But the real reason they are special lies in their electron configuration.
The Precise Definition (IUPAC)
A transition element is an element whose atom has an incomplete d sub-shell, or which can give rise to cations with an incomplete d sub-shell.
Let's unpack that.
1. The "d" sub-shell
Electrons are arranged in shells (K, L, M, N...) and sub-shells (s, p, d, f). The d sub-shell can hold a maximum of 10 electrons. In transition elements, the d sub-shell is being filled — but not completely.
For example, consider Iron (Fe):
- Atomic number 26
- Electron configuration: 1s22s22p63s23p64s23d6
- The 3d sub-shell has 6 electrons — it is incomplete (it can hold 10).
So iron is a transition element.
2. The "or" part — cations matter
Some elements have a complete d sub-shell in their neutral atom, but when they lose electrons to form positive ions (cations), the d sub-shell becomes incomplete.
Example: Zinc (Zn)
- Neutral Zn: [Ar]3d104s2 — the 3d sub-shell is full (10 electrons).
- But Zn commonly forms Zn2+: [Ar]3d10 — still full.
- So zinc is NOT a transition element by the IUPAC definition.
Example: Copper (Cu)
- Neutral Cu: [Ar]3d104s1 — 3d is full.
- But Cu2+: [Ar]3d9 — now the 3d sub-shell is incomplete.
- So copper IS a transition element.
A common mistake: thinking that all elements in the d-block (groups 3–12) are transition elements. They are not. Zinc, cadmium, and mercury are d-block elements but NOT transition elements because their common cations have a full d sub-shell.
The "d-block" vs "Transition Elements"
| d-block elements | Transition elements |
|---|---|
| Groups 3 to 12 | Groups 3 to 11 (excluding Zn, Cd, Hg) |
| All have d electrons | Must have incomplete d sub-shell in atom or common cation |
Why this formula?
Transition Element Definition: The "Why" Behind the Definition
The Core Definition
A transition element (IUPAC definition) is an element whose atom has an incomplete d-subshell in its ground state or can form stable ions with an incomplete d-subshell.
Key exam point: This definition covers both the neutral atom and its common ions.
Why This Definition? The Reasoning
1. The d-orbital filling pattern
In the periodic table, transition elements belong to the d-block (Groups 3–12). As we move across a period, electrons fill the (n−1)d orbitals after the ns orbital.
For example, in Period 4:
- Scandium (Sc): [Ar]3d14s2 — has one d-electron → transition element
- Zinc (Zn): [Ar]3d104s2 — d-subshell is full → not a transition element
2. The "incomplete d-subshell" condition
The definition focuses on incompleteness because:
- A full d-subshell (d10) is exceptionally stable (like a noble gas configuration for d-orbitals)
- Elements with d10 configurations do not show the characteristic properties of transition metals (variable oxidation states, coloured compounds, catalytic activity, paramagnetism)
3. Why include ions?
Consider Zinc (Zn):
- Ground state: [Ar]3d104s2 — d-subshell is full → not a transition element
- Common ion: Zn2+: [Ar]3d10 — still full → still not a transition element
Now consider Copper (Cu):
- Ground state: [Ar]3d104s1 — d-subshell is full → by atom definition alone, not a transition element
- But Cu2+: [Ar]3d9 — incomplete d-subshell → is a transition element
Therefore: The definition must include ions to correctly classify elements like Cu, which form stable ions with incomplete d-subshells.
The "Formula" — A Decision Tree
The definition can be expressed as a logical condition:
Transition element⟺(Atom has d1−9)∨(Stable ion has d1−9)
Where:
- d1−9 means incomplete d-subshell (1 to 9 electrons)
- d0 or d10 means complete (empty or full) → not a transition element
Common Exam Exceptions …
Enthalpy of atomisation is the energy needed to break a solid metal into free gaseous atoms, so it reflects the strength of the metallic bonding. Transition metals use their many unpaired d-electrons in this bonding, making the interatomic attraction unusually strong. …
More unpaired d-electrons available for metallic bonding means stronger inter-atomic attraction in the solid metal, so more energy is needed to atomise it.
Enthalpy of atomisation is the energy required to convert one mole of a solid metal into gaseous, isolated atoms. In transition metals, both the (n-1)d and ns electrons participate in metallic bonding (unlike s- and p-block metals, where usually only the outer s or s,p electrons are involved). Because the d-orbitals are relatively diffuse, they overlap significantly with orbitals of neighbouring atoms, and unpaired d-electrons contribute strongly to covalent-type metallic bonding in addition to the usual electrostatic metallic bonding. Elements with a large number of unpaired d-electrons (roughly in the middle of a transition series, e.g. Mo, W, Re, Os) therefore show the strongest inter-atomic bonding and hence the highest enthalpies of atomisation, while elements at the two ends of the series (fewer unpaired d-electrons, e.g. Zn, Cd, Hg, which have completel …
Showing the 12 most recent of 37 on this concept.
- CBSE 2026Set 56/1/11 markMCQQ.Which of the following is not a transition metal ? (A) Sc (B) Ag (C) Hg (D) Cu
›Reveal solutionSolution
Transition metals are defined by having partially filled d-orbitals in their common oxidation states. Mercury (Hg) has a full d¹⁰ configuration in both its elemental and common +2 state, so it is not a transition metal. The correct answer is (C).
Why This Definition Matters
The classification of transition metals isn't about being a metal or having d-electrons — it's about partially filled d-orbitals in the atom or in any common ion. This is the IUPAC definition. If an element's d-subshell is completely full (d¹⁰) in all its common forms, it doesn't qualify, even if it sits in the d-block of the periodic table.
Let's check each option against this rule.
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Scandium (Sc, Z=21)
Electronic configuration: [Ar]3d14s2.
Its common ion is Sc³⁺: [Ar] — the 3d orbital is empty.
But the atom has a partially filled d-orbital (3d¹). The definition says "in the atom or in any common oxidation state." Since the atom itself has an incomplete d-subshell, Sc is a transition metal.
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Silver (Ag, Z=47)
Configuration: [Kr]4d105s1.
Common ion: Ag⁺ → [Kr]4d10 — full d-subshell.
However, silver also forms Ag²⁺ (e.g., in AgF₂), which has 4d9 — a partially filled d-orbital. Because at least one common oxidation state (Ag²⁺) has an incomplete d-subshell, Ag qualifies as a transition metal.
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Mercury (Hg, Z=80)
Configuration: [Xe]4f145d106s2.
Common ions: Hg²⁺ → [Xe]4f145d10 (full d¹⁰); Hg₂²⁺ (dimeric) also has each Hg with a full d¹⁰ core.
Mercury does not form any stable ion with a partially filled d-orbital. Its d-subshell is always full. Therefore, Hg is not a transition metal.
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Copper (Cu, Z=29)
Configuration: [Ar]3d104s1. …
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- CBSE 2026Set 56/2/11 markMCQQ.Assertion (A) : Zinc, cadmium and mercury are not considered as transition elements. Reason (R) : These elements have completely filled orbitals in their ground state as well as in their common oxidation states.
›Reveal solutionSolution
The key idea is that transition elements are defined by having partially filled d-orbitals in their ground state or common oxidation states. Since Zn, Cd, and Hg have completely filled d¹⁰ configurations in both, they fail this criterion. Thus, both Assertion (A) and Reason (R) are true, and (R) correctly explains (A).
Why this approach works
The definition of a transition element is not arbitrary — it stems from the unique chemistry of d-block elements. The IUPAC defines a transition element as an element whose atom has a partially filled d-subshell, or which can give rise to cations with an incomplete d-subshell. This means we must check two things: the ground state electron configuration of the neutral atom, and the configurations of its common oxidation states. If either has a partially filled d-orbital, the element qualifies. If both are completely filled, it does not.
Zinc, cadmium, and mercury sit at the end of their respective d-block series (Group 12). Their neutral atoms have the configuration (n−1)d10ns2 — the d-subshell is full. Their common oxidation state is +2, formed by losing the two s-electrons, leaving (n−1)d10 — still full. No partially filled d-orbital appears anywhere. Hence, they are not transition elements.
Let’s walk through the reasoning step by step.
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Recall the defining criterion for transition elements.
A transition element must have an atom or a common ion with an incomplete d-subshell. This is the official IUPAC definition. Elements that have completely filled d-orbitals in both the ground state and all common oxidation states are excluded.
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Examine the ground state configurations of Zn, Cd, and Hg.
- Zinc (Z=30): [Ar]3d104s2
- Cadmium (Z=48): [Kr]4d105s2
- Mercury (Z=80): [Xe]4f145d106s2 In each case, the d-subshell is completely filled (d10). No partially filled d-orbital exists in the neutral atom.
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Check their common oxidation states.
The most stable and common oxidation state for all three is +2. For example:
- Zn loses its two 4s electrons to form Zn2+: [Ar]3d10
- Cd loses its two 5s electrons to form Cd2+: [Kr]4d10
- Hg loses its two 6s electrons to form Hg2+: [Xe]4f145d10 In every case, the d-subshell remains completely filled. No partially filled d-orbital appears in any common oxidation state. …
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- CBSE 2026Set DZ1 markMCQQ.Which of the following is not a transition metal?(a) Cu(b) Cr(c) Fe(d) Na
›Reveal solutionSolution
A transition metal has a partially filled d-subshell (in the atom or a common ion). Cu, Cr and Fe qualify; Na does not — so option (d).
A transition element is defined as one whose atom or one of its stable ions has an incompletely filled d-orbital.
- Cu ([Ar]3d104s1): forms Cu2+ (3d9) — partially filled d → transition metal.
- Cr ([Ar]3d54s1) — partially filled d → transition metal. …
- CBSE 2026Set ANNUAL1 markMCQQ.Transition element among the following is(a) Zinc(b) Cadmium(c) Cerium(d) Rutherfordium
›Reveal solutionSolution
A transition element is defined as one having a partially (incompletely) filled d-subshell in the ground state or in any of its common oxidation states.
- Zinc (3d10 4s2) and Cadmium (4d10 5s2) have a completely filled d-subshell in the atom AND in their only common +2 ion, so they are NOT classified as transition elements (they are 'post-transition'/group 12 metals).
- Cerium is an f-block (lanthanide) element, not d-block. …
- CBSE 2026Set ANNUAL1 markQ.Why is Zn not considered as transition element? (Z = 30)
›Reveal solutionSolution
Transition elements must have partly filled d-orbitals in the elemental or common ionic state; zinc's d-subshell is always completely full, so it does not qualify.
Zinc (Z = 30) has the electronic configuration [Ar] 3d10 4s2. When it forms its common oxidation state, Zn2+, it loses the two 4s electrons, giving [Ar] 3d10 - the d-subshell remains completely filled (all 10 electrons present) in both the metal and its ion.
…
- CBSE 2026Set ANNUAL1 markMCQQ.Chromium belongs to which block?(a) s-block(b) p-block(c) d-block(d) f-block
›Reveal solutionSolution
Chromium (Z=24) has the configuration [Ar] 3d⁵ 4s¹, placing it in the d-block.
Chromium has atomic number 24 and electronic configuration [Ar] 3d⁵ 4s¹ (an exception to the expected 3d⁴4s², arising from the extra stability of a half-filled d-subshell). Since its last-entering electron occupies a …
- CBSE 2026Set ANNUAL1 markQ.______ block elements are called transition elements.
›Reveal solutionSolution
d-block elements are called transition elements.
The periodic table is divided into four blocks (s, p, d, f) based on which subshell receives the last (differentiating) electron. Elements in which the last electron enters a d-orbital form the d-block, spanning groups 3 to 12. These are called transition elements because most of them have partially filled d-orbitals in their elemental or common ionic states, giving them properties 'transitional' between the highly reactive s-b …
- CBSE 2026Set ANNUAL1 markMCQQ.Transition metals have incomplete(a) s-orbital(b) p-orbital(c) d-orbital(d) f-orbital
›Reveal solutionSolution
Transition metals have incomplete d-orbitals.
Transition elements are defined as those whose atoms or stable ions have partially filled (incomplete) d-orbitals. This partly filled d-subshell is responsible for their characteristic properties: var …
- CBSE 2026Set ANNUAL1 markMCQQ.Total number of elements are in d-block is ______(a) 39(b) 40(c) 38(d) 36
›Reveal solutionSolution
Four transition series of 10 elements each -> 40 d-block elements.
The d-block (transition elements) consists of elements in which the last electron enters a d-subshell. There are four such series:
- 3d series (Sc to Zn),
- 4d series (Y to Cd),
- 5d series (La/Hf to Hg),
- 6d series (Ac/Rf onward). …
- CBSE 2026Set ANNUAL1 markQ.Fill in the blank: Zn, Cd and Hg generally do not considered as a ______ elements.
›Reveal solutionSolution
Zn, Cd and Hg are not true transition elements because their d-orbitals are completely filled.
A transition element is defined as one that has a partially filled d-subshell in its atomic state or in one of its common oxidation (ionic) states. Zinc, cadmium and mercury have the configuration (n-1)d10 ns2, and even in their common +2 ions they are (n-1)d10 - the d-subshell is completely filled. Since they …
- CBSE 2026Set ANNUAL1 markMCQQ.Choose the correct order of atomic and ionic radii of chlorine atom and chloride (Cl-) ion (in pm) is(a) a) 136 and 90(b) b) 167 and 99(c) c) 99 and 181(d) d) 186 and 90
›Reveal solutionSolution
[!TLDR]
c) 99 and 181
Why
The covalent/atomic radius of Cl is about 99 pm, while the Cl- ion is larger (extra electron, same n …
- CBSE 2025Set 56/6/11 markMCQQ.Which of the following is the softest metal ? (A) Zn (B) Sc (C) Cu (D) Fe
›Reveal solutionSolution
Softness in metals is determined by how easily their atoms slide past one another; among the transition elements listed, scandium (Sc) has the weakest metallic bonding due to having only one d-electron available for bonding, making it the softest. The answer is (B).
Understanding Metallic Softness
Hardness in metals arises from the strength of metallic bonding—the electrostatic attraction between the "sea" of delocalized electrons and the positive metal ions. The more electrons available for delocalization (especially from d-orbitals in transition metals), and the smaller the atomic radius, the stronger the bonding and the harder the metal.
Conversely, a soft metal has weaker metallic bonds. Its atoms can slide past one another more easily under stress, making it malleable and easy to deform.
Comparing the Four Metals
Let's examine each candidate by looking at their electronic configurations and the number of electrons contributing to metallic bonding:
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Zinc (Zn): Electronic configuration [Ar]3d104s2
All ten d-electrons are paired in filled orbitals. While the two 4s electrons participate in bonding, the filled d10 subshell contributes relatively little to directional bonding. Zinc is moderately soft but not the softest here.
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Scandium (Sc): Electronic configuration [Ar]3d14s2
Only one d-electron is available. This is the first transition metal in the series, with minimal d-orbital participation in bonding. The metallic bond is weak because there are fewer electrons to delocalize and the d-orbitals are only just beginning to fill. Scandium is notably soft and can be cut with a knife.
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Copper (Cu): Electronic configuration [Ar]3d104s1 …
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