Mettalic Bonding

Question	Answer
Define metallic bonding	The electrostatic attraction between positive ions and a sea of delocalised electrons
Describe how metallic bonding takes place	The outermost electrons of a metal atom are delocalised. This leaves a positive metal cation (e.g. Na⁺, Mg²⁺, Al³⁺)
Name the structure in which metal elements exist	Giant metallic lattice structures
Describe the properties of giant metallic lattice structures	Malleable and ductile (can be shaped/drawn into a wire) Good thermal and electrical conductor Insoluble (EXCEPT in liquid metals) Number of delocalised electrons per atom affects melting and boiling point
Why are metals malleable and ductile?	No bonds hold specific ions together - metal ions can slide over each other when the structure is pulled
Why are metals good thermal/electrical conductor?	THERMAL Delocalised electrons can pass kinetic energy ELECTRICAL Delocalised electrons can carry a current
What happens to the melting/boiling point as the number of delocalised electrons increase?	The more delocalised electrons there are, the stronger the bonding will be and the higher the melting/boiling point
TRUE OR FALSE: The size of the metal ion and lattice structure affects melting/boiling point	TRUE A smaller ionic radius will hold the delocalised electrons closer to the nuclei

Resource summary

	Created by Yinka F almost 7 years ago