IB Chemistry Topic S2.3.2 Strength of Metallic Bonds Revision Notes (SL/HL)

IB Chemistry Topic S2.3.2 Strength of Metallic Bonds Revision Notes (SL/HL) | RevisionDojo

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Cation Charge and Radius Determine Metallic Bond Strength and Melting Points

Definition

Alloy

An alloy is a mixture of a metal with one or more other elements, which can be either metals or non-metals

Factors Affecting Bond Strength in Metals

The strength of metallic bonds arises from the electrostatic attraction between positively charged metal cations and the "sea" of delocalized electrons surrounding them.
Two key factors influence this attraction: the charge of the cations and the radius of the cations.

Charge of Cations

The charge of a metal cation directly affects the strength of the metallic bond.
Cations with higher charges exert a stronger pull on the delocalized electrons, increasing the bond strength.

Example

Sodium (Na) forms cations with a charge of $+1$.
Magnesium (Mg) forms cations with a charge of $+2$.
Aluminium (Al) forms cations with a charge of $+3$.
As the charge increases from $+1$ to $+3$, the metallic bond becomes stronger.
This explains why aluminium has a higher melting point than magnesium or sodium.

Radius of Cations

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Cation Charge and Radius Determine Metallic Bond Strength and Melting Points

Definition

Alloy

An alloy is a mixture of a metal with one or more other elements, which can be either metals or non-metals

Factors Affecting Bond Strength in Metals

The strength of metallic bonds arises from the electrostatic attraction between positively charged metal cations and the "sea" of delocalized electrons surrounding them.
Two key factors influence this attraction: the charge of the cations and the radius of the cations.

Charge of Cations

The charge of a metal cation directly affects the strength of the metallic bond.
Cations with higher charges exert a stronger pull on the delocalized electrons, increasing the bond strength.

Example

Sodium (Na) forms cations with a charge of $+1$.
Magnesium (Mg) forms cations with a charge of $+2$.
Aluminium (Al) forms cations with a charge of $+3$.
As the charge increases from $+1$ to $+3$, the metallic bond becomes stronger.
This explains why aluminium has a higher melting point than magnesium or sodium.

Radius of Cations

Definition

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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 S2.3.2 Strength of Metallic Bonds 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

Cation Charge and Radius Determine Metallic Bond Strength and Melting Points

Factors Affecting Bond Strength in Metals

Charge of Cations

Radius of Cations

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Duis aute irure dolor in reprehenderit

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Cation Charge and Radius Determine Metallic Bond Strength and Melting Points

Factors Affecting Bond Strength in Metals

Charge of Cations

Radius of Cations

anim nostrud sit dolore minim proident quis fugiat velit et eiusmod nulla quis nulla mollit dolor sunt culpa aliqua

Duis aute irure dolor in reprehenderit

Excepteur sint occaecat cupidatat non proident

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