Ionic and Covalent Bonding

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Ionic and Covalent Bonding

Ionic and covalent bonding is involved when the atoms of an element

chemically combine to make their outer shells full and to make the

atoms stable.

The first type of bonding you can get is ionic bonding. Electrons are

transferred from one atom to another to try and create full outer

shells, this gain and loss of electrons on the atoms results in

positive and negative ions. In these compounds you get electrostatic

force, this is the force/attraction that occurs between the positive

and negative ions that hold the compound together. This type of

bonding takes place between metals and non-metals. The metals lose

electrons and form cations, whereas the non-metals gain electrons and

form anions.

Each energy sub level is made up of orbitals. Every one can hold a

different number of orbitals, these sub-levels are known as S, P, D

and F. when the S and P block elements lose or gain electrons to

become ions they fill their outer shells to get the electronic

structure of a noble gas, however this structure doesn’t apply to most

of the positive ions formed from the transition metals.

Ionic compounds exist as a regular arrangement of ions in a giant

covalent lattice. It is very hard to overcome the strong forces

between them known as the electrostatic force, this means that ionic

compounds are generally solid and they have a very high melting and

boiling points as they need a lot of energy to overcome the

electrostatic force. The bigger the charge on the atom and the smaller

the atom, the bigger the electrostatic force.

In simple ionic compounds the positive ion is often much smaller than

the negati...

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...e larger the strength of the Wan de Waal forces. The

bigger the forces are between the molecules the more energy is needed

to overcome them, giving the substance and higher melting and boiling

point.

There is another type of bonding and this is called metallic bonding,

this type of bonding is the force of attraction between the

delocalised electrons and the positive centres. The atoms of the

elements are packed so closely together that some of their electrons

begin to wander among the nuclei rather than orbiting the nucleus of a

single atom. As the charge on the positive centre and the number of

mobile electrons per atom both increase and the size of the positive

centre decreases the strength of the metallic bond increases. As they

have free electrons they conduct electricity very well in solid and

liquid states.

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