7. I) LOCATION OF IONS:
In NaCl, Na+ ions are so located that there
are six Cl- ions around it and vice versa.
The size of Na+ ion is smaller than Cl- ion.
8. II) CO-ORDINATION NUMBER:
The no. Of anions which contact a unit cation
is called it’s co-ordination number.
In NaCl, co-ordination number is 6.
9. III) NO. OF NaCl IN EACH UNIT:
In NaCl there are 8 Cl- ions at each
corner of the cube.
Each corner ion is shared
between eight unit cells, each face shares
with two unit cells.
10. Cl- Ions (Green)
8 at corners = 8/8 = 1
6 at face centers = 6/2 = 3
Total = 1+3 = 4
Na+ Ions (Violet)
12 at edge centers = 12/4 = 3
1 at body center = 1
Total = 3+1= 4
4Na+ + 4Cl- 4 NaCl
17. 1. IONIC CRYSTALS
An ionic solid is a solid that
consists of cations and anions
held together by electrical
attraction of opposite charges
(ionic bond).
Example: NaCl (Rock Salt)
18. IONIC CRYSTALS
High melting points
Hard and brittle
Conduct electricity
only in their molten
state (or solution)
Thermally stable
19. 2. COVALENT CRYSTALS
A covalent network solid is
a solid that consists of atoms
held together in large
networks or chains by
covalent bonds.
20. COVALENT CRYSTALS
High Melting points
Hard & Rigid
Giant covalent
network structure
Bad conductors of
electricity (Except
Graphite)
High latent heat of
fusion
Low coefficient of
expansion
21. 3.METALLIC CRYSTALS
A metallic solid is a solid
that consists of positive
cores of atoms held
together by a surrounding
“sea” of electrons (metallic
bonding).