3. metallic bonding

Bonding

metal elements exist as…

…giant metallic lattice structures

the outermost shell of electrons for metal atoms is delocalised…

leaving a positive metal ion like Na+ which are attracted to the negative delocalised electrons

metallic bonding is when

the positive ions and sea of delocalised electrons form a lattice

metallic bonding properties

• high melting point

• ability to be shaped

• conductivity

• solubility

metals have a high melting point

because of strong electrostatic attraction between the positive metal ions and sea of delocalised electrons.

the more delocalised electrons per atom the stronger the bonding will be

therefore the higher the melting point that’s why Mg²⁺ has a higher melting point that Na⁺

there are no bonds holding specific ions together

so the metal ions can slide over each other when the structure is pulled making metals malleable and ductile (can be drawn into wires)

metals are good thermal and electrical conductors

sea of delocalised electrons can pass kinetic energy to each other AND they are free to carry the flow of charge

metals are insoluble apart from liquid metals

due to the strength of the metallic bonds

solids

high density which makes them incompressible. solid particles vibrate in a fixed position and cant move freely

liquids

similar density to solids and virtually incompressible. particles flow freely and randomly

gases

particles have loads of energy and are much further apart, density is generally low and its very compressible

in simple covalent substances the covalent bonds DONT break during melting/ boiling

you only have to overcome the weak intermolecular forces that hold the molecule together

in giant covalent substances you DO need to break the covalent bonds holding the atoms together

that’s why giant covalent compounds have very high melting and boiling points

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