Other slides in this set

Slide 2

Preview of page 2

Here's a taster:

Ionic compounds form giant ionic lattices in their
solid form.
A lattice describes a regular arrangement of
atoms. The `giant' part refers to the fact that
the same pattern is repeated continually.
Ionic compounds do not conduct electricity as a
solid, but when these are melted or dissolved
they do this is because the compounds can
then move freely and carry charge.
Ionic compounds have high melting points
because the electrostatic forces are strong and
require a high amount of energy to overcome.
Ionic compounds often dissolve in water water
molecules are polar and can pull ions away from
a lattice arrangement.…read more

Slide 3

Preview of page 3

Here's a taster:

Ionic bonding is when ions of opposite charges
bond by electrostatic attraction.
These ions lose or gain electrons to another atom
to achieve full outer shells.
Atoms which lose electrons become +ively
charged ions, called cations.
Atoms which gain electrons become ­ively
charged ions, called anions.
Formed when metals react with non-metals…read more

Slide 4

Preview of page 4

Here's a taster:

Group Charge
1 1+; loses an electron, cation
2 2+; loses 2 electrons, cation
3 3+; loses 3 electrons, cation
4 2+; loses 2 electrons, cation
5 3-; gains 3 electrons, anion
6 2-; gains 2 electrons, anion
7 1-; gains 1 electron, anion
8 Does not form ionic bonds.…read more

Slide 5

Preview of page 5

Here's a taster:

Covalent bonding occurs between non-
metals, when it is not energetically
favourable to form an ionic bond.
Two atoms share a pair/pairs of electrons
(one from each) so that each has a full outer
Electrons involved in bonding are called
bonding pairs, and electrons which do not
form bonds are called lone pairs.
One shared pair of electrons is a single
covalent bond. Two is a double covalent
bond. Three is a triple covalent bond.…read more

Slide 6

Preview of page 6

Here's a taster:

...is when two atoms share an electron pair,
but one atom provides BOTH the shared
electrons, rather than each atom
contributing an electron each.…read more

Slide 7

Preview of page 7
Preview of page 7

Slide 8

Preview of page 8
Preview of page 8

Slide 9

Preview of page 9
Preview of page 9

Slide 10

Preview of page 10
Preview of page 10


No comments have yet been made

Similar Chemistry resources:

See all Chemistry resources »See all resources »