IB Chemistry Topic S2.3.3 Transition Elements and Delocalized D-electrons Revision Notes (HL)

IB Chemistry Topic S2.3.3 Transition Elements and Delocalized D-electrons Revision Notes (HL) | RevisionDojo

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The Role of d-Electrons in Transition Metals and Trends in the d-Block

In most metals, the delocalized electrons come from the s-orbital of the outermost energy level.
However, in transition metals, d-electrons as well as outer s-electrons can contribute to this electron sea.
This additional electron density significantly strengthens metallic bonds, setting transition metals apart.

The Impact of d-Electrons on Properties

The delocalized d-electrons in transition metals give rise to several key properties:

Higher Melting Points

The strength of metallic bonds depends on the density of delocalized electrons and their attraction to the metal cations.
Transition metals, with their additional d-electrons, form stronger metallic bonds than metals like sodium or magnesium.
This explains their generally higher melting points.

Example

Sodium (Na): Melting point = 98°C
Iron (Fe): Melting point = 1538°C

Tip

When comparing melting points, consider both the number of delocalized electrons and the size of the metal cation.
Smaller cations with higher electron density form stronger metallic bonds.

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The Role of d-Electrons in Transition Metals and Trends in the d-Block

In most metals, the delocalized electrons come from the s-orbital of the outermost energy level.
However, in transition metals, d-electrons as well as outer s-electrons can contribute to this electron sea.
This additional electron density significantly strengthens metallic bonds, setting transition metals apart.

The Impact of d-Electrons on Properties

The delocalized d-electrons in transition metals give rise to several key properties:

Higher Melting Points

The strength of metallic bonds depends on the density of delocalized electrons and their attraction to the metal cations.
Transition metals, with their additional d-electrons, form stronger metallic bonds than metals like sodium or magnesium.
This explains their generally higher melting points.

Example

Sodium (Na): Melting point = 98°C
Iron (Fe): Melting point = 1538°C

Tip

When comparing melting points, consider both the number of delocalized electrons and the size of the metal cation.
Smaller cations with higher electron density form stronger metallic bonds.

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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 S2.3.3 Transition Elements and Delocalized D-electrons 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

The Role of d-Electrons in Transition Metals and Trends in the d-Block

The Impact of d-Electrons on Properties

Higher Melting Points

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The Role of d-Electrons in Transition Metals and Trends in the d-Block

The Impact of d-Electrons on Properties

Higher Melting Points

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Duis aute irure dolor in reprehenderit

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