An element crystallises in a face-centred cubic (fcc) unit cell with cell edge a. The distance between the centres of two nearest octahedral voids in the crystal lattice is:
An element crystallises in a face-centred cubic (fcc) unit cell with cell edge a. The distance between the centres of two nearest octahedral voids in the crystal lattice is:
In FCC octahedral voids are present at the edge centers and body center
Consider a diagonal projected form edge centre passing through the body centre
Distance between octahedral voids = √2a/2 = a/√2
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ΔG° = –RT * 2.303 log K
–nFE° = +RT * 2.303 log K
2 * 96500 * 0.295 = 8.314 * 298 * 2.303 log10 K
10 = log10 K = 1010
It has chiral centre and differently di substituted double bonded carbon atoms.
For FCC lattice
Packing efficiency = 
CsCl has BCC structure in which Cl– is present at corners of cube and Cs+ at body centre
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Chemistry Ncert Solutions Class 12th 2023
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