Atomic Structure - Types Of Bonding

No. of protons

No. Of protons + neutrons

1 1 and 1/1840

+1 0 -1

Nucleus , nucleus, shell

JJ Thompson - 1897

Rutherford - 1911

Chadwick- 1932

Charged particles Positive ions formed when atoms lose electrons Negative ions formed when atoms gain electrons

Atoms have a radius of 0.1 nanometres (nm) or 1 x 10 to the power of -10m

Atoms of the same element which have the same number of protons but different numbers of neutrons

R.A.M = (Mass Number 1 x abundance) + ( Mass number 2 x abundance) / total abundance

Giant ionic lattice Occurs in metal ions when reacting with non-metal ions. The positive metal ion transfers one or more electrons to the negative non-metal ion that both end up with full outer shells. They are attracted by electrostatic attractions.

Strong and lots of heat energy needed to break

Lose electrons- cations Gains electrons- anions

A shared pair of electrons. A molecule is 2 or more atoms covalently bonded together. Two non metals Molecular covalent bonding is 2 molecules sharing electrons Giant covalent lattice bonding is 2 atoms sharing electrons

High melting and boiling point as strong ionic bonds requires a lot of heat energy to break Conducts electricity when molten as free electrons to move and carry a charge Soluble in water Brittle

When 2 of the same atom are covalently bonded together e.g chlorine

There are weak forces of attraction - van der waals Do not conduct electricity as they have no free electrons Have low solubility in water Have low melting and boiling points

Different forms of the same element in the same physical state e.g diamond, graphite and graphene

Metallic Lattice The electrostatic attraction between the positive metal ions and delocalised electrons Only between metals

Look in book

High melting and boiling points- strong attraction Conducts heat and electricity- delocalised electrons Strong malleable and ductile - layers of metal ions can Slide Over each other

Crimson red orange lilac brick red green-blue