The document describes various ionic structures and their properties, specifically focusing on different types of crystal lattices such as rock salt, zinc blende, antifluorite, fluorite, and others. It highlights the coordination numbers, types of ions occupying certain sites, and the relationship between crystal structure and lattice energy, including the Born-Haber cycle. Additionally, it covers the significance of silicate structures and how charge interactions affect stability and energy in ionic compounds.

1. STRUCTURE TYPES

2. Rock Salt (NaCl)
• Fcc with respect to anions.
• Cations occupy octahedral voids.
• Octahedral sites are present at edge centres and
body centre.
• There are 4 octahedral sites per unit cell.
• General formula AX.
• CN of anion=8
• CN of cation=8

3. • Each ion and its neighbours can
be
represented
by
apt.
polyhedra.
• Octahedron has 12 edges.
• Each edge shared between two
octahedron.
• Octahedron centred on Na ions.
• Most halides & hydrides of alkali
metals and Ag+ have this
structure.
• Mostly ionic, but TiO metallic.

4. Zinc Blende or Sphalerite (ZnS)
• Fcc w.r.t anions.
• Two types of tetrahedral sites are there : T+ , T_
• Cations occupy tetrahedral sites, either T+ or T_
rest are empty.
• Tetrahedral sites are present at (1/4,1/4,3/4)
position and its equivalent points.
• There are total 8 tetrahedral sites, 4 T+ and 4 T_
• General formula AX.
• CN of anion=4
• CN of cation=4

5. • Contains ZnS4 or SZn4
tetrahedra.
• Each corner shared by
four tetrahedra.
• Bonding is less ionic than
rock salt structure.
• Oxides do not have this
structure
• Exception ZnOdimorphic with zinc
blende and wurtzite.
• Covalent compounds of
Be, Zn, Cd and Hg have
this structure.

6. Antifluorite (Na O)
2
• Fcc w.r.t anions.
• Tetrahedral sites T+ and T_ are occupied by
cations. Octahedral sites are empty.
• General formula A2X
• CN of anion=8
• CN of cation=4
• Structure shown by oxides and chalcogenides of
alkali metals.

7. • For CN of anion displace
unit cell along body
diagonal by ¼, so that
cation becomes new origin
of unit cell.
• It contains cations at
corners, edge centres, face
centres and body centres.
• Centre of smaller cube is
primitive, hence CN 8.

8. Structure can be described in two ways:
1. 3-D network of tetrahedra :
▫
▫
eight NaO4 tetrahedra
Each edge shared between two tetrahedra
2. 3-D network of cubes :
▫
▫
▫
four ONa8 cubes
Each corner common to 4 cubes
Each edge common to 2 cubes

9. Fluorite (CaF2)
• Fcc w.r.t cation.
• Tetrahedral sites T+ and T_ are occupied by
anions. Octahedral sites are empty.
• General formula AX2.
• CN of anion=4
• CN of cation=8
• It includes fluorides of large, divalent cations
and oxides of large tetravalent cations.

10. • Arrangement of cubes shows MF8 coordination
in fluorites.
• Anions at the centre of cube i.e. , in voids.
• Cations at corners and face centres.

11. CsCl Type
•
•
•
•
•
•
Simple cubic w.r.t anion.
Anions present at corners.
Cation present in cubic void i.e., body centre.
General formula AB.
CN of anion=8
CN of cation=8

12. Wurtzite (ZnS)
• HCP w.r.t anion.
• Cations occupy
tetrahedral sites, either
T+ or T_ rest are empty.
• c/a ratio=1.633
(assuming anions are in
contact)
• Tetrahedral site at a
distance 3/8 above anion.
• 12 tetrahedral voids are
present, only 6 are
occupied.

13. Nickel Arsenide (NiAs)
•
•
•
•
HCP w.r.t anion.
Cations occupy octahedral voids.
6 octahedral voids are present.
Ni and As have the same CN but
not the same coordination
environment unlike rock salt
structure.
• AsNi6 trigonal prisms which link
up by sharing edges.
• c/a ratio varies for different
compounds whereas same for
wurtzite.

14. Rutile (TiO2)
• Distorted HCP oxide array or tetragonal packed oxide
array.
• ½ octahedral sites occupied by Ti.
• Alternate rows of octahedral sites are full and empty.
• Oxides of tetravalent metal ions & fluorides of small
divalent ions exhibit this structure.
• M4+ and M2+ are too small to form fluorite structure with
O2- and F- .
In CdI2 layers of octahedral sites are occupied and these
alternate with empty layers.
In CdI2 anions are HCP whereas in CdCl2 they are CCP.

15. Silicate Structures
• Composed of cations and silicate anions.
• Mostly built of SiO4 tetrahedra.
Exception: In SiP2O7 , Si is octahedrally coordinated
to oxygen.
• SiO4 tetrahedra links up by sharing corners. Never
share edges or faces.
• A corner is shared by maximum of 2 tetrahedra.
• To relate formula to structure Si:O ratio is
important.
• Si:O ratio is variable.
• Two types of oxygen atoms: bridged and nonbridged.
• Exact structure cannot be determined.

16. Lattice Energy
• Net potential energy of arrangement of charges.
• Denoted by U.
• Equivalent to sublimation energy.
• U depends on :
▫ Crystal structure
▫ Charge on ions
▫ Inter nuclear separation

17. • Attaractive force given by
F=(Z+ Z- e2 / r2 )
Potential energy V=(- Z+ Z- e2 / r )
• Repulsive energy V=(B/ rn )
B=Born exponent
5<n<12 (for large n V--» 0)
• U is a combination of electrostatic attaraction
and Bohr repulsion.
•U
A is Madelung constant. Depends on geometrical
arrangement of point charges.

18. Born Haber Cycle
• Lattice energy is equivalent to heat of formation
from one mole of its ionic constituents in gaseous
phase. Cannot be measured experimentally.
• ΔHf can be measured. Can be related to U via a
thermodynamic cycle known as Born Haber cycle.
• Stability of compounds can be determined by
finding ΔHf .
• Difference between theoretical & calculated lattice
energies provides evidence for non-ionic bonding.