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Copper metal has a face-centred cubic structure with the unit cell length equal to 0.361 nm. Picturing copper ions in contact along the face diagonal. The apparent radius of a copper ion is-
(A). For a face-centred cube, we have.
radius =
A compound alloy of gold and copper crystallizes in a cube lattice in which the gold atoms occupy the lattice points at the corners of a cube and the copper atoms occupy the centres of each of the cube faces. The formula of this compound is-
(C). One-eight of each corner atom (Au) and one-half of each face-centred atom (Cu) are contained with in the unit cell of the compound.
Thus, the number of Au atoms per unit cell = . The formula of the compound is .
Select the correct statement (s) -
(a) The C.N. of cation occupying a tetrahedral hole is 4.
(b) The C.N. of cation occupying a octahedral hole is 6.
(c) In schottky defects, density of the lattice decreases,
(C). Since tetrahedral holes are surrounded by 4 nearest neighbours. So, the C.N. of cation occupying tetrahedral hole is 4. Since octahedral hole is surrounded by six nearest neighbours. So, C.N. of cation occupying octahedral is 6. In schottky a pair of anion and cation leaves the lattice. So, density of lattice decreases.
Among the following types of voids, which one is the largest void-
(D). The vacant spaces between the spheres in closed packed structure is called void. The voids are of two types, tetrahedral voids and octahedral voids. Also radius of tetrahedral voids and octahedral voids are = 0.225 × respectively. Thus, octahedral void is larger than tetrahedral void.
The rank of a cubic unit cell is 4. The type of cell as-
(B). The number of atoms present in sc, fcc and bcc unit cell are 1, 4, 2 respectively.
Close packing is maximum in the crystal which is-
(C). The close packing in the crystal is 0.52, 0.68 and 0.74 for simple cubic, bcc, and fcc respectively i.e. the close packing is maximum is fcc.
Assertion : The stability of a crystal gets reflected in its melting point.
Reason : The stability of a crystal depends upon the strength of the interparticle attractive force. The melting point of a solid depends on the strength of the attractive force acting between the constitutent particles.
(A). The stability of a crystal depends upon the strength of the interparticle attractive force. The melting point of a solid depends on the strength of the attractive force acting between the constitutent particles. Therefore, the stability of a crystal gets reflected in its melting point.
The vapour density of undecomposed N2O4 is 46. When heated, vapour density decreases to 24.5 due to its dissociation to NO2. The percent dissociation of N2O4 at the final temperature is:
(a) normal molar mass/exp. molar mass = 1+ ; (Molar mass = 2 x VD)
M1 =2*46=92
m2=2*24.5=49
92/49 = 1+
... =0.87
At 298 K, 500cm3 H2O dissolved 15.30 cm3 CH4(STP) under a partial pressure of methane of one atm. If Henery's law holds, what pressure is required to cause 0.001 mole methane to dissolve in 300cm3 water ?
The molal depression constant for water=1.85 deg/molal and for benzene is 5.12 deg/molal. If the ratio of the latent heats of fusion of benzene to water is 3:8, calculate the freezing point of benzene.
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