IB Chemistry Topic S3.1.8 Properties of Transition Elements Revision Notes (HL)

IB Chemistry Topic S3.1.8 Properties of Transition Elements Revision Notes (HL) | RevisionDojo

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What Makes an Element a Transition Element

Transition elements sit in the d-block of the periodic table.
They are defined by having a partially filled d-sublevel in the atom or in at least one of their stable ions.
Two d-block elements are excluded by this definition: scandium and zinc.
1. Scandium forms only Sc³⁺, which has an empty 3d sublevel (no d electrons).
2. Zinc forms only Zn²⁺, which has a full 3d¹⁰ sublevel.

Electron Configuration and the d-Sublevel

Transition elements lie mainly in groups 3 to 11.
Their configurations follow the pattern $(n-1)d^{1-10}ns^{0-2}$, with the 4s filling before the 3d.

Example

Iron (Fe): $[Ar]\,3d^6\,4s^2$
Copper (Cu): $[Ar]\,3d^{10}\,4s^1$ (an exception, giving a stable full 3d sublevel)

Why Scandium and Zinc Are Excluded

Note

A transition element must have a partially filled d-sublevel in its atom or in one of its ions.
Scandium ($[Ar]\,3d^1\,4s^2$) is excluded because its only ion, Sc³⁺, has an empty 3d sublevel.
Zinc ($[Ar]\,3d^{10}\,4s^2$) is excluded because its 3d sublevel is full in both the atom and the Zn²⁺ ion.

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What Makes an Element a Transition Element

Transition elements sit in the d-block of the periodic table.
They are defined by having a partially filled d-sublevel in the atom or in at least one of their stable ions.
Two d-block elements are excluded by this definition: scandium and zinc.
1. Scandium forms only Sc³⁺, which has an empty 3d sublevel (no d electrons).
2. Zinc forms only Zn²⁺, which has a full 3d¹⁰ sublevel.

Electron Configuration and the d-Sublevel

Transition elements lie mainly in groups 3 to 11.
Their configurations follow the pattern $(n-1)d^{1-10}ns^{0-2}$, with the 4s filling before the 3d.

Example

Iron (Fe): $[Ar]\,3d^6\,4s^2$
Copper (Cu): $[Ar]\,3d^{10}\,4s^1$ (an exception, giving a stable full 3d sublevel)

Why Scandium and Zinc Are Excluded

Note

A transition element must have a partially filled d-sublevel in its atom or in one of its ions.
Scandium ($[Ar]\,3d^1\,4s^2$) is excluded because its only ion, Sc³⁺, has an empty 3d sublevel.
Zinc ($[Ar]\,3d^{10}\,4s^2$) is excluded because its 3d sublevel is full in both the atom and the Zn²⁺ ion.

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Structure 1. Models of the particulate nature of matter5 subtopics

Structure 2. Models of bonding and structure4 subtopics

Structure 3. Classification of matter2 subtopics

Reactivity 1. What drives chemical reactions?4 subtopics

Reactivity 2. How much, how fast and how far?3 subtopics

Reactivity 3. What are the mechanisms of chemical change?4 subtopics

IB Chemistry S3.1.8 Properties of Transition Elements Notes

Structure 1. Models of the particulate nature of matter5 subtopics

Structure 2. Models of bonding and structure4 subtopics

Structure 3. Classification of matter2 subtopics

Reactivity 1. What drives chemical reactions?4 subtopics

Reactivity 2. How much, how fast and how far?3 subtopics

Reactivity 3. What are the mechanisms of chemical change?4 subtopics

What Makes an Element a Transition Element

Electron Configuration and the d-Sublevel

Why Scandium and Zinc Are Excluded

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What Makes an Element a Transition Element

Electron Configuration and the d-Sublevel

Why Scandium and Zinc Are Excluded

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