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Published on: 21/06/2021
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Questions + Answers key
Take MCQ Chemistry Test1.
A compound forms hexagonal dosed packed structure. What is the total number of voids in 0.5 mol of it? How many of these are tetrahedral voids?
2.
What is F centre?
3.
Distinguish between cubic and hexagonal unit cells.
4.
In CaF2 crystal, Ca2+ ions are present in arrangement. Calculate the number of F- ions in the unit cell.
5.
Name the seven primitive crystal systems.
1.
1 Mole of hexagonal packed structure contains 1 mole of octahedral voids and two moles of tetrahedral voids. Therefore, 0.5 moles of hexagonal packed structure contains 0.5 moles of octahedral voids and 1 mole of tetrahedral voids.
No. of tetrahedral voids = 6.022 x 1023
No. of octahedral voids\(\frac{1}{2}\) x no. of tetrahedral voids
No. of octahedral voids = \(\frac{1}{2}\) x 6.022 x 1023
= 3.011 x 1023
Total No. of voids = (6.022+3.011) x 1023
= 9.033 x 1023.
2.
Anionic vacancies which are occupied by: unpaired electrons are called F centers. Hence, the formula of NaCI which contains excess Na+ ions can be written as Na1+x Cl.
3.
| Cubic | Hexagonal |
| a=b=c | a=b≠c |
| ∝=β=૪=90o | ∝=β=90o, ૪=120o |
4.
No. of Ca2+ ions per unit cell
= 8 x \(\frac{1}{8}+6\times \frac{1}{2}\)
= 1 + 3 = 4
Hence No. of F- ions per unit cell = 2 x 4 = 8
5.
There are seven primitive crystal systems; cubic, tetragonal, orthorhombic, hexagonal, monoclinic, triclinic and rhombohedral.
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