1. Structure of Solids
Chapter 11
Part III

2. Classification of Solids
Crystalline
Solids with highly regular arrangement of components
Amorphous
Solids with considerable disorder in their structure.

3. X-ray Diffraction
X-ray Diffraction is commonly used to determine the structure of a solid.
X-ray diffraction is explained on page 420.

4. Crystalline Solids
A Lattice represents the regular positioning of the components of a crystal.
A Lattice is the three dimensional system of points designating the positions of the components.
The smallest repeating unit of the lattice is called the Unit Cell.

5. Unit Cell-Simple Cubic, Body centered cubic & Face centered cubic.

6. Types of Crystalline Solid
Ionic Solids: metal and non metal
Molecular solids: non metal and non metal
Atomic solids: single element

7. Ionic Solids: metal and non metal
Ionic substances have ions at the point of the lattice that describe the structure of the compound.
Examples: NaCl, FeSO4, Al2S3

8. Molecular solid: non metal and non metal
Molecular solids have discrete covalently bonded molecules at the end of each of its lattice points.
See ice →

9. Atomic solids: single element
Atomic solids all have atoms at the points of the lattice that describes the structure of the solid.
This example is diamond a network covalent solid.
Other examples include, boron, silicon and all metals.

11. Types of solids

12. Atomic solids: Three types
Metallic Solids
Network Solids
Group VIIIA solids

13. Metallic Solids
These have a type of delocalized non-directional covalent bonding.
Examples are Cs and Au

14. Network Solids
The atoms bond to each other with strong directional covalent bonds that lead to macromolecules or networks of atoms.

15. Group VIIIA solids
Noble gases are attracted to one another at low temperatures with weak London dispersion forces.
The examples are Kr and Xe. Both are cubic close packed.

16. Summary

17. Structure and Bonding in Metals