Metals and Metallic bonding Flashcards
what are the properties of metals?
conduct heat and electricitry
malleable
have metallic bonds
solid at room temperature
high melting/boiling points
ductile
dense and strong
magnetic
sonorous
how are the atoms arranged in pure metals?
The atoms are all the same type
they are arranged in layers and form a giant structure
what do the layers in metal allow it to do?
the layers in pure metals are able to slide over eachother so metals can be shaped and bent making them malleable and ductile
what are alloys made from?
alloys are usually made up from two or more different metals
this mean some of the atoms are differently sized
why are alloys harder than pure metals
The different sized atoms of the metals distort the layers in the structure making it more difficult to slide over eachother.
So alloys are harder than metals.
what do metallic bonds occur between?
metallic bonds occur between two metals
what is metalic bonding?
metallic bonding is the strong force of attraction between the sea of delocalized electrons and thew closely packed positive metal ions
how do metallic bonds form?
metals contain positive ions packed closely together.
these form when electrons leave the outer shell of each atom which means these electrons become free to move within the structure of the metal and form a sea of delocalized
this leaves a giant structure of positive metal ion surrounded by electrons
why do metals have high melting and boiling points?
the metallic bonds are very strong so takes a lot of energy to overcome
why can metals conduct electricity?
metals can conduct electricity because there is a seas of delocalized electrons that can carry charge as there free to move
why are metals considered to have a giant metallic structure?
they have a large number of atoms bonded in a large network
