SC5 - Ionic Bonding ✓

• Cation: A positively charged ion (A metal which has lost an electron) • Anion is a negatively charged ion (A non-metal which has gained an electron)

• A charged particle formed by the transfer of electrons

Electrostatic forces of attraction

• Metals loose an electron(s) as they are closer to 0/8 electrons in their outermost shell and so its easier to loose electrons • Non-metals are closer to 8/8 electrons in theri outermost shell and so it is easier for them to gain electrons

• Ammonium, NH4+ • Hydroxide, OH- • Nitrate, NO3- • Carbonate, CO32- • Sulfate, SO42-

• An atom’s ionic formula will depend on the number of electrons in its outer shell. • If it has to lose electrons to gain a full outer shell, it will be positive by that much. • If it has to gain electrons it will be negative by that much. • In a compound, the charges of the ionic compound of an element need to cancel out. • e.g Mg 2+ and O 2- will form MgO while Na+ and S2- will form Na2S

When billons of ions are packed together in a regular structure.

For a substance to be conductive it must contain particles that are: • Charged • Free to move So Ionic compounds can conduct electricity when they are aqueous or molten.

• Mg2+ and O2- have more than one charge - this means they will attract other ions more strongly than ions with one charge. • More neergy is required to overcome these stronger electrostatic forces of attraction so melting point is higher

They are high as they have strong electrostatic forces of attraction which require a lot of energy to overcome and break

The negative ions flow to the anode(+) and the positive ions flow to the cathode(-). electrons do not flow.