Chemistry - metallic bonding

Metallic bonding

It is an electrostatic attraction between a positively charged ion and its delocalised electrons.

Delocalised

free to move throughout the whole structure

why do metals have high mpt/bpt

???

metallic bonds are very strong meaning a large amount of heat energy is needed to break the bond causing high mpt/bpt

why are metals ductile/ malleable

• The ions are arranged in layers

• these layers can slide over one another

• this allows the metal to be bent or shaped 

why are alloys harder than metals

• the metal ions are different sizes

• this disrupts the lattice structure

• layers of ions cant slide over one another

why are they good conductors of electricity

the delocalised electrons in the metals can carry electrical charge throughout the metal

why are metals good conductors of thermal energy

the delocalised electrons can transfer heat throughout the structure.

name the top five metals on the reactivity scale

• potassium

• sodium

• lithium 

• calcium

• aluminium

name the bottom 5 metals in the reactivity series

• iron

• hydrogen

• copper

• silver

• gold

oxidation

the loss of electrons

reduction

the gain of electrons

redox

oxidation reactions and reduction reactions always happen together, and together are know as redox reactions

oxidising agent

causes another species to be oxidised, itself reduced

reducing agent

causes another species to be reduced, itself oxidised

what means a metal has a stronger metallic bond

• higher charge on the metal

• smaller ion ( protons positive charge is pulling the negative electrons closer since it has less electrons but same strength)

state 3 physical properties of metal

• hard

• malleable

• high mpt/bpt

• conductors

• strong

• ductile

displacement

when a more reactive metal displaces a less reactive metal from its aqueous solution.