CH3 - Metallic Bonding

What are the properties of metals?

• High melting and boiling point

  • Bonds between particles are very strong

• Conducts electricity well

  • Charged particles are able to move around

• Conducts heat well

  • Particles can transfer energy through easily

• High density

  • Particles must be packed closely

• Malleable and ductile

  • The bonding between particles remains when force is applied

• Lustrous

  • Free electrons must be present to reflect light

How does metallic bonding occur?

1. Metal atoms lose their valence electrons to become cations

2. These cations are then arranged into a tightly packed lattice

3. Freed valence electrons move in between the cations. These electrons are ‘delocalised’ and are shared amongst the whole lattice

   • Within the structure, the attraction between the delocalised electrons and the cations is very strong

What are the properties of metallic bonds?

• High melting and boiling points

  • The attraction between the cations and the delocalised electrons is very strong and needs a lot of energy to be able to overcome

• Conduct heat and electricity well

  • Delocalised electrons can carry charge through metals. In doing so, they are also able to bump into each other and the cations to transfer heat energy across the lattice

• Malleable and ductile

  • When a force is applied, the cations slide over each other, but due to the delocalised electrons, the lattice continues to be able to sustain its shape

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