Solid State
Get insights from 127 questions on Solid State, answered by students, alumni, and experts. You may also ask and answer any question you like about Solid State
- 127
Questions
- 0
Discussions
- 0
Active Users
- 0
Followers
Have a question about Solid State? Ask our experts
Keep it short & simple. Type complete word. Avoid abusive language.
1.34 Calculate the efficiency of packing in case of a metal crystal for (i) Simple cubic (ii) Body-centred cubic (iii) Face-centred cubic (with the assumptions that atoms are touching each other).
1.34 Calculate the efficiency of packing in case of a metal crystal for (i) Simple cubic (ii) Body-centred cubic (iii) Face-centred cubic (with the assumptions that atoms are touching each other).
1.34 (i) The efficiency of packing in case of simple cubic unit cell is given below:
A simple cubic unit cell contains one atom per unit cell.
Also, a=2r, where a is the edge length and r is the radius of atom. Total volume of unit cell = a3
Packing efficiency = Volume of one sphere / Total volum
Upvote 
1.33 Explain (i) The basis of similarities and differences between metallic and ionic crystals. (ii) Ionic solids are hard and brittle.
1.33 Explain (i) The basis of similarities and differences between metallic and ionic crystals. (ii) Ionic solids are hard and brittle.
(i) Both metallic and ionic crystals have strong forces of attraction between their atoms or ions. In metallic crystals there is a strong metallic bond present between electrons and positively charged ions. In ionic crystals there are strong ionic bonds between anions and cations. Both of them cond
Upvote 1.32 How many lattice points are there in one unit cell of each of the following lattice? (i) Face-centred cubic (ii) Face-centred tetragonal (iii) Body-centred
1.32 How many lattice points are there in one unit cell of each of the following lattice? (i) Face-centred cubic (ii) Face-centred tetragonal (iii) Body-centred
1.32 Number of corner atoms per unit cell
= 8 corners atoms ×18 atom per unit cell
=8 × 18 = 1 atom
Number of face face centred atoms per unit cell
= 6 face centred atoms × 12 atom per unit cell
= 6 × 12 = 3 atoms
∴ Total number of atoms (lattice point) = 1 + 3 = 4
(ii) As in (i)
No. of lattice points = 4
(i
Upvote 1.31 How will you distinguish between the following pairs of terms: (i) Hexagonal close-packing and cubic close-packing? (ii) Crystal lattice and unit cell? (iii) Tetrahedral void and octahedral void?
1.31 How will you distinguish between the following pairs of terms: (i) Hexagonal close-packing and cubic close-packing? (ii) Crystal lattice and unit cell? (iii) Tetrahedral void and octahedral void?
1.31 (i) In hexagonal close packing (hcp), the spheres of the third layer are vertically above the spheres of the first layer. It means tetrahedral voids of the second layer are covered by the spheres of the third layer. The AB. type.In cubic close packing (ccp), the spheres of third layer cover the
Upvote 1.30 'Stability of a crystal is reflected in the magnitude of its melting points'. Comment. Collect melting points of solid water, ethyl alcohol, diethyl ether and methane from a data book. What can you say about the intermolecular forces between these molecules?
1.30 'Stability of a crystal is reflected in the magnitude of its melting points'. Comment. Collect melting points of solid water, ethyl alcohol, diethyl ether and methane from a data book. What can you say about the intermolecular forces between these molecules?
1.30 Stability of a crystal is directly proportional to the magnitude of its melting points. Higher is the magnitude of forces holding the constituent particles together, higher will be the melting point and higher will be the stability. Thus ionic crystals (NaCl, KNO3 etc.) have very high melting p
Upvote 1.30 How can you determine the atomic mass of an unknown metal if you know its density and the dimension of its unit cell? Explain
1.30 How can you determine the atomic mass of an unknown metal if you know its density and the dimension of its unit cell? Explain
1.30 Knowing the density of an unknown metal and the dimension of the unit cell, the atomics mass of the metal can be determined.
Let, Atomic mass of element
(M)=d* a3* NA x Z
Where, d = density
- a3= volume of the unit cell
- NA = Avogadro's number
- Z= number of atoms present in one unit cell.
- Density of the
Upvote 1.28 (i) What is meant by the term 'coordination number'? (ii) What is the coordination number of atoms: (a) in a cubic close-packed structure? (b) in a body-centred cubic structure?
1.28 (i) What is meant by the term 'coordination number'? (ii) What is the coordination number of atoms: (a) in a cubic close-packed structure? (b) in a body-centred cubic structure?
1.28 Coordination number is the number of the nearest neighbors with which a given atom is in contact. In an
ionic crystal, the coordination number of an ion refers to the number of oppositely charged ions that
surround that ion.
The coordination number of atoms in a
(a) Cubic close-packed
Upvote 1.27 Classify each of the following solids as ionic, metallic, molecular, network (covalent) or amorphous. (i) Tetra phosphorus decoxide (P4O10) (ii) Ammonium phosphate (NH4) 3PO4 (iii) SiC (iv) I2 (v) P4 (vi) Plastic (vii) Graphite (viii) Brass (ix) Rb (x) LiBr (xi) Si
1.27 Classify each of the following solids as ionic, metallic, molecular, network (covalent) or amorphous. (i) Tetra phosphorus decoxide (P4O10) (ii) Ammonium phosphate (NH4) 3PO4 (iii) SiC (iv) I2 (v) P4 (vi) Plastic (vii) Graphite (viii) Brass (ix) Rb (x) LiBr (xi) Si
1.27 The different solids are classified below:
a) Ionic solids: Ammonium phosphate (NH4)3PO4), LiBr
b) Metallic solid: Brass, Rb
c) Molecular solids: Tetraphosphorous decaoxide (P4O10), Iodine (I2), P4
d) Network (covalent) solids: Graphite, SiC, Si
e) Amorphous solid: Plastics
Upvote 1.26 What makes a glass different from a solid such as quartz? Under what conditions could quartz be converted into glass?
1.26 What makes a glass different from a solid such as quartz? Under what conditions could quartz be converted into glass?
1.26 Quartzis crystalline solid with long range order and glass is amorphous solid (or pseudo solid or super cooled liquid) with short range order and has a tendency to flow. When quartzis heated, it can be converted into glass.
Upvote