Metallic Bonding Flashcards
Why are metals good at conducting electricity and heat?
They have delocalised electrons that are free to move throughout the structure, so can transfer charge and heat energy
What does malleable mean?
a structure can be hammered into shape.
Why are metals malleable?
The layers can slide over each other which allows the structure to bend
What is an alloy?
a mixture of 2 or more metals
What is the disadvantage of pure metals?
Too soft (alloys make them stronger )
Why do metals have high melting and boiling points?
There are strong electrostatic forces of attraction between metal atoms and the sea of delocalised electrons which require a lot of energy to break.
Describe the structure and bonding of metals
metals have a giant structure
The metal atom gives up their outer electron shell, which becomes delocalised
The metal ions are arranged in a regular lattice structure
There are strong electrostatic forces of attraction between the positive metal ions and the negative delocalised electrons
These forces are metallic bonds.
Why are alloys harder than pure metals
The different elements have different sized atoms
This disrupts the regular layered structure
Meaning the layers cannot slide over each other anymore
This makes them less malleable, so harder
