Metallic Bonding Flashcards
What structure do metal elements exist as?
Metals form giant metallic structures in which electrons in the outer shells of the metal atoms are free to move.
What is metallic bonding?
Metallic bonding is the type of bonding found in metallic elements.
This is the electrostatic force of attraction between positively charged ions and delocalised outer electrons.
What 4 things about metals are explained by metallic bonding?
Melting and boiling points.
Ability to be shaped.
Conductivity.
Solubility.
How does metallic bonding explain melting and boiling points of metals?
The number of delocalised electrons per atom affects the melting and boiling points- more = the stronger the bonding and the higher the mp/bp.
The size of the metal ion and the lattice structure also affect the melting and boiling points.
How does metallic bonding explain metals ability to be shaped?
As there are no bonds holding specific ions together, the metal ions can slide over each other when the structure is pulled.
So metals are malleable and ductile.
How does metallic bonding explain conductivity?
The delocalised electrons can pass kinetic energy to each other, making metals good thermal conductors.
Metals are good electrical conductors because the delocalised electrons can carry a current.
How does metallic bonding explain solubility?
Metals are insoluble, except in liquid metals, because of the strength of the metallic bonds.
Describe the structure of magnesium.
Magnesium exists as a giant mettallic lattice structure.
The outermost shell of electrons of a magnesium atom is delocalised- the electrons are free to move about the metal.
This leaves positive metal ions, Mg2+, which are attracted to the delocalised negative electrons.
They form a lattice of closely packed positive ions in a sea of delocalised electrons.
What type of bonding can be found in magnesium?
Metallic bonding.
Explain why a solution of copper(II) nitrate conducts electricity.
Ions are mobile
