GIANT IONIC LATTICES.

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Presentation transcript:

GIANT IONIC LATTICES

Very strong electrostatic attraction Ionic Bonding - the net electrostatic attractions between oppositely charged ions - + Cation Anion Very strong electrostatic attraction

How are ions formed? By atoms losing or gaining electrons More electronegative non-metal atoms GAIN electrons FROM metal atoms CATIONS (+) are formed when atoms (USUALLY METALS) lose electrons to non-metal ANIONS (-) are formed when atoms (USUALLY NON-METALS) gain electrons from metal Example Example Na - 1s22s22p63s1 F - 1s22s22p5 loses its 3s electron to form gains an electron to form Na+ - 1s22s22p63s0 F- - 1s22s22p6 Ions are isoelectronic with nearest noble gas

Na+Cl-(s) IONIC BONDING IN SODIUM CHLORIDE Showing only outer energy levels: Na X 2 , 8 , 1 Cl X 2 , 8 , 7 Na+ 2 , 8 Cl- X 2 , 8 , 8 3D giant lattice with 1:1 ratio of ions to give electrical neutrality Na+Cl-(s)

General Ionic Structure ions arrange in a giant lattice structure cations and anions arranged alternately 3-dimensional array lattice is very strong due to many ionic bonds

Sodium chloride crystal lattice GIANT IONIC CRYSTAL LATTICE Oppositely charged ions held in a regular 3-dimensional lattice by electrostatic attraction The arrangement of ions in a crystal lattice depends on the relative sizes of the ions Sodium chloride crystal lattice Cl- Chloride ion Na+ Sodium ion The Na+ ion is small enough relative to a Cl¯ ion to fit in the spaces so that both ions occur in every plane.

Sodium chloride crystal lattice GIANT IONIC CRYSTAL LATTICE Oppositely charged ions held in a regular 3-dimensional lattice by electrostatic attraction The arrangement of ions in a crystal lattice depends on the relative sizes of the ions Sodium chloride crystal lattice Each Na+ is surrounded by 6 Cl¯ (co-ordination number = 6) and each Cl¯ is surrounded by 6 Na+ (co-ordination number = 6).

Sodium chloride crystal lattice GIANT IONIC CRYSTAL LATTICE Oppositely charged ions held in a regular 3-dimensional lattice by electrostatic attraction The arrangement of ions in a crystal lattice depends on the relative sizes of the ions Sodium chloride crystal lattice Each Na+ is surrounded by 6 Cl¯ (co-ordination number = 6) and each Cl¯ is surrounded by 6 Na+ (co-ordination number = 6).

Summary - The Sodium Chloride Lattice = Na+ = Cl- Each Na+ ion is surrounded by six Cl- ions Each Cl- ion is surrounded by six Na+ ions  6:6 coordination  Na1Cl1 formula Face Centred Cubic Structure

Caesium chloride crystal lattice GIANT IONIC CRYSTAL LATTICE Oppositely charged ions held in a regular 3-dimensional lattice by electrostatic attraction The arrangement of ions in a crystal lattice depends on the relative sizes of the ions Caesium chloride crystal lattice Each Cs+ is surrounded by 8 Cl¯ (co-ordination number = 8) and each Cl¯ is surrounded by 8 Cs+ (co-ordination number = 8).

Caesium chloride crystal lattice GIANT IONIC CRYSTAL LATTICE Oppositely charged ions held in a regular 3-dimensional lattice by electrostatic attraction The arrangement of ions in a crystal lattice depends on the relative sizes of the ions Caesium chloride crystal lattice Each Cs+ is surrounded by 8 Cl¯ (co-ordination number = 8) and each Cl¯ is surrounded by 8 Cs+ (co-ordination number = 8).

Summary - The Caesium Chloride Lattice = Na+ = Cl- Each Cs+ ion is surrounded by eight Cl- ions Each Cl- ion is surrounded by eight Cs+ ions 8 :8 coordination  Cs1Cl1 formula Body Centred Cubic Structure

A comparison of the sodium chloride and caesium chloride lattices Type of structure Face Centred Cubic Body Centred Cubic Coordination number 6:6 8:8 The structures of NaCl and CsCl are different because the Cs+ ion is larger than the Na+ ion, and is therefore able to surround itself with 8Cl-ions, whereas the Na+ ion is smaller and can only fit 6Cl- ions around itself

Physical properties of ionic compounds Melting point very high A large amount of energy must be put in to overcome the strong electrostatic attractions and separate the ions. Strength Very brittle Any dislocation leads to the layers moving and similarly charged ions being next to each other. The repulsion splits the crystal. Electrical do not conduct when solid - ions are held strongly in the lattice. conduct when molten or in aqueous solution - the ions become mobile and conduction takes place. Solubility Insoluble in non-polar solvents but soluble in water Water as it is a polar solvent and stabilises the separated ions. Much energy is needed to overcome the electrostatic attraction and separate the ions stability attained by being surrounded by polar water molecules compensates for this

BRITTLE IONIC LATTICES IONIC BONDING BRITTLE IONIC LATTICES + - IF YOU MOVE A LAYER OF IONS, YOU GET IONS OF THE SAME CHARGE NEXT TO EACH OTHER. THE LAYERS REPEL EACH OTHER AND THE CRYSTAL BREAKS UP.