Types of bonding

A brief explanation and the properties of ionic, metallic, simple covalent and giant covalent bonding.

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  • Created by: R_Hall
  • Created on: 25-06-11 15:12
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Type of bonding Between How held together Boiling/Melting pointConducting Other properties Examples
Ionic Metals and Transfer electrons to form High. Only when molten of Soluble in water. Sodium Chloride
Nonmetals ions (charged particles with a Strong electrostatic aqueous as the ions (NaCl)
full outer shell). attraction between are free to move. Calcium
Strong bonds between ions ions, so lots of Carbonate
because of electrostatic energy needed to (CaCO3)
attraction. break the bonds.
Regular lattice structure.
Metallic Metals (1 Made up of positive ions and High. Yes, can conduct Malleable The layers Aluminium (Al)
metal or an a sea of free (delocalised) Strong electrostatic
heat and electricity of ions can slide over Copper (Cu)
alloy) electrons. There is strong attraction between
when solid and each other. Iron (Fe)
electrostatic attraction ions, so lots of liquid. Sea of High density the atoms Silver (Ag)
between the 2 particles. energy needed to delocalised electrons are closely packed Steel
break the bonds. can move carry the together in a regular Bronze
charge. structure
Simple Covalent 2 Electrons are shared between Low. No. Low density weak Oxygen (O2)
nonmetals. atoms to gain a full outer shell.Weak bonds Never any free ions intermolecular forces Chlorine (Cl2)
Strong covalent bonds within between molecules or electrons to carry (often gases). Carbon Dioxide
molecule, but weak between so less energy a charge in any (CO2)
molecules. needed to separate state. Water (H2O)
Giant covalent 2 nonmetals Electrons are shared between High. No. Very hard Diamond (C)
atoms. Very strong covalent Never any free ions Sand (SiO2)
bonds hold structure of electrons to carry Graphite (C)
a charge. Quartz (SiO2)

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Apart from
high temperatures. graphite, which has
free electrons).…read more


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