METALLIC BONDING
Metals conduct heat and electricity
Metals have theseproperties becauseof the way their atoms are joined together.
METALLIC BONDING
METALLIC BONDING
metal ion
mobile electrons
(de-localised)
Metals consist of ‘Giant structures’.The electrons from outer energy levels are free tomove through the whole structure . These electrons
* hold the atoms together ( + ions attract - electrons)
* allow the atoms to slide over each other (metals bend)* allow the metal to conduct heat and electricity
METALLIC BONDING
The atoms in a metal are closely packed so ……………………………………..
The atoms are in a regular pattern so ……………………………………..
Metallic bonding is strong so ……………………………………...
PHRASE LIST:
metals have high melting points metals are dense
they have a crystal structure
METALLIC BONDING
The atoms in a metal are closely packed so metals are dense.
The atoms are in a regular pattern so they have a crystal structure.
Metallic bonding is strong so metals have high melting points
PHRASE LIST:
metals have high melting points metals are dense
they have a crystal structure
METALLIC BONDING
The crystals on a metal’s surface are called grains.
Crystals join together atgrain boundaries
Galvanised dustbin
If cooled slowly larger crystals grow
giantelectrons outer positive
electrostatic
free
Cool liquid metal slowly to increase crystal sizeSmaller grains give a harder but more brittle metal
The de-localised electrons are like glue because:
they attract the positive metal ions (hold them together)
They are not like glue because: they are able to move through the whole lattice
METALLIC BONDING
http://www.chemguide.co.uk/atoms/structures/metals.html
The crystals on a metal’s surface are called grains.
Crystals join together atgrain boundaries
METALLIC BONDING
METALLIC BONDING
METALLIC BONDING
METALLIC BONDING
Copper ion
Zinc ionBrass
Small grains tend to stop rows of atoms sliding over each other.This makes the metal harder but more brittle.
METALLIC BONDING
Copper ion
Zinc ionBrass
METALLIC BONDING