Metallic Bonding Flashcards
Give 3 examples
Iron, Copper, Gold…
Describe the structure of a named metal (e.g. iron)
A metal consists of a regular lattice of positive metal ions in a ‘sea’ of delocalised electrons. The giant lattice is held in place by the strong forces of attraction between the positive ions and negative electrons.
Why do metals conduct electricity?
The electrons are free to move (delocalised).
Why do metals generally have high melting and boiling points?
High temperature (energy) needed to overcome the strong forces of attraction between the oppositely charged positive ions and negative electrons.
What is an alloy?
It is a mixture of two or more metals.
Why are metals malleable (bendy)?
The layers of atoms can slide over each other.
Why are alloys stronger (less bendy)?
Different sized atoms stop the layers sliding over each other.
Why is a named alloy (or copper oxide) a poor conductor of electricity
Oxide/other ions disrupt the flow of electrons (there are less delocalised electrons).
