Metallic bonding

Metals have high melting points. This is because metals are in a giant metallic lattice which is held together by very strong electrostatic forces of attraction between delocalised electrons and protons. These forces are strong and therefore hard to overcome. This will therefore require a lot of thermal energy to break the bonds which leads to metals having high melting points.

Metallic bonding is strong electrostatic attraction between negatively charged delocalised electrons and positive metal ions

Malleable Ductile Good conductor of electricity Good conductor of heat High melting and boiling points High density Forms positive ions Shiny

Metals conduct electricity because there is a sea of delocalised electrons that can carry the electrical charge through the metal / free to move around

• metals are in a giant metallic lattice held together by strong electrostatic forces of attraction of a sea of delocalised electrons and protons. • This means that the layers can slide over each other while maintaining this structure and not breaking.

Alkali metlas

Metals in group 1

Low density, Low melting and boiling points(lowers further as you go down the group), soft and very reactive

• more reactive further down the group. • lower down you go, group 1 metals have more shells. • This means that the electrostatic forces of attraction between the electron and the protons in the nucleus are weakened. • This is because the distance between the protons in the nucleus and the electron shell is increased, lowering the attraction. • This means that the group 1 metals further down the group lose their outer electron/valent easier making it more reactive.

Metals lose their electrons to become a stable atom

(metal) hydroxide + hydrogen 2metal + 2H2O –> 2metalOH + H2