What is Metallic Bonding?
Metallic bonding is the strong attraction between metal atoms and a 'sea' of delocalized electrons that move freely throughout the structure. This unique bonding explains why metals are shiny, conduct electricity, and can be bent.
In metallic bonding, valence electrons are not bound to individual atoms but form a mobile electron sea that holds the metal cations together, giving metals their characteristic properties like conductivity and malleability.
- •Delocalized electron sea
- •Metal atoms + free electrons
- •High electrical conductivity
- •Malleable and ductile
- •Localized electron transfer
- •Attraction between ions
- •Variable conductivity
- •Brittle crystals
Step-by-step worked examples
Why is copper a good electrical conductor?
Copper has one valence electron per atom (3d¹⁰ 4s¹). These valence electrons form a delocalized sea. Electrons move freely → high conductivity.
Why can aluminum foil be bent without breaking?
Al atoms in the lattice are held by the electron sea. When bent, cations can slide past each other. Electrons stay between them → no breaking (malleability).
Compare melting points: Na (883 K) vs. Mg (923 K). Why is Mg higher?
Mg has two valence electrons (more charge in electron sea). Stronger metallic bonding → higher melting point. More electrons = stronger electrostatic attraction.
Flashcards
Quick quiz
Q1.In metallic bonding, what are delocalized?
Q2.Why is metal ductile but ionic crystal brittle?
Q3.Melting point of Na vs. Mg: which is higher?
Q4.Can metals conduct electricity in solid state?
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Common mistakes
All electrons in a metal are free to move. — Correct: Only valence electrons form the electron sea; core electrons stay with nuclei.
Metallic bonding is the same as ionic bonding with free electrons. — Correct: Ionic bonding involves fixed electron transfer; metallic has a shared, mobile electron sea.
Metals break easily like ionic crystals because they lack fixed electron positions. — Correct: The opposite: the mobile electron sea allows metals to be bent without breaking.
All metals have the same melting point because they all have metallic bonding. — Correct: Melting points vary — they depend on the number of valence electrons and nuclear charge.
FAQ
What is the electron sea in metallic bonding?
A pool of delocalized valence electrons that move freely among metal cations, holding the structure together.
Why are metals shiny?
Free electrons can absorb and re-emit light easily, reflecting it and creating lustre.
Can nonmetals have metallic bonding?
No, metallic bonding only occurs in metals and some alloys where atoms have low ionization energies.
How does metallic bonding affect properties like melting point?
More valence electrons and higher nuclear charge increase the attraction, raising melting points.