part b estion FourExplain why the average density of metals is higher than that of ceramics or polymers i.e pmetals >(a)Peramics > Ppolymers.(b) Copper crystallises as FCC (face centred cubic). Given that the atomic radius and mass of a given coppersample are 1.28 x 10:10 m and 64.15 g respectively, calculate the density of the copper sample. TakeAvogadro's number, NA = 6.023 x 1023 atoms/mole.(c) The linear density, LD, of an atom is given by the equation =Natomswhere Natoms is theLdvnumber of atoms and Lav is the unit length of the direction vector, both taken on a particular plane.Calculate the linear density of an aluminium atom with a lattice parameter of 4.05 x 1010 m and in a[110] direction.(d) Using neat sketches, show the difference between a triclinic and hexagonal crystal systems.

Answered: Image /qna-images/answer/97274c1a-6e9b-4d4e-b978-2fb92bc25b1d.jpg

Answered: (b) Copper crystallises as FCC (face…

Elements Of Electromagnetics

7th Edition

ISBN:9780190698614

Author:Sadiku, Matthew N. O.

Publisher:Sadiku, Matthew N. O.

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Vanadium (V) has a BCC crystal structure. The atomic radius is R = 0.132 nm and the atomic mass is M = 50.94 g/mole. What is the density of Vanadium in g/mm3? Given: Avogadro’s Number NA = 0.6023 × 1024 (atoms/mole) Select one: a. 1.5 b. 0.021 c. 0.011 d. 0.0087 e. 0.00597
Sodium chloride (NaCl) has the rock salt crystal structure and a density of 2.17 g/cm³. The atomic weights of sodium and chlorine are 22.99 g/mol and 35.45 g/mol, respectively. (a) Determine the unit cell edge length. nm (b) Determine the unit cell edge length from the radii in the table below assuming that the Nat and Cl- ions just touch each other along the edges. nm Cation Mg2+ Fe2+ Na+ Ionic Radius (nm) 0.072 0.077 0.102 Anion Ionic Radius (nm) CI- 0²- 0.181 0.140
(a) Explain the fotlowing teminologies: i. Crystallinity ii. Allotropy iii. Polymorphism iv. Coordination number 31Page (b) Copper crystallises as FCC (face centred cubic). Given that the atomic radius and density of a given copper sample are 1.28 x 1010 m and 8.98 x 10' kg/m' respectively, carry out the following: Calculate the mass of the copper sample. Take Avogadro's number, NA = 6.023 x 1023 atoms/mole. (i) If the interatomic planar spacing, d, in the sample above is 2.96 x 1010 m, determine the angle at which the first Bragg reflection will occur from the (111) plane if x-radiation of wavelength 1.52 x 1010 m is used for the analysis. (ii) (c) Give two uses of pure copper and two commercial applications of copper alloys.
O h. 0.74 Silver (Ag) has the FCC crystal structure. The atomic radius is R = 0.144 nm and the atomic mass is M = 107.87 g/mole. What is the density of Silver in g/m? Given: Avogadro's Number NA = 0.6023 x 1024 (atoms/mole) Select one: a. 10.6x106 O b. 10.6×105 O c. 10.6×10 O d. 10.60 O e. 10.6x10 Chromium (Cr) has the Boody-Centered Cubic (BCC) crystal structure. The edge length is a= 0.288 nm. What is the linear density in atoms/nm along direction (111P Select one: 9:12 PM O a. 7.48 O O e 4) A ENG 15-Apr-2021
Tungsten (W) has the BCC crystal structure. The atomic radius is R = 0.137 nm and the atomic mass is M = 183.95 g/mole. %3D What is the density of Tungsten in g/cm³? Given: Avogadro's Number NA = 0.6023 × 1024 (atoms/mole) Select one: O a. 5.30 O b. 6.28 Oc. 2.534 Od. 6.77 Oe. 19.28
Vanadium has the Body-Centered Cubic (BCC) crystal structure. The edge length "a" of the unit cell of Vanadium is a 0.3048 nm at room %3D temperature (20°C). Calculate atomic radius "r" of Vanadium? Select one: a. 0.488 b. 0.428 c. 0.304 d. 0.612 e. 0,132
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8- Tungsten W (atomic weight = 183.84 g/mol) forms a body centered cubic (bcc) unit cell. If tungsten has an atomic radius of 147 pm. Calculate the density of the W. %3D * Pm = 10-12 m
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(b) Copper crystallises as FCC (face centred cubic). Given that the atomic radius and mass of a given copper sample are 1.28 x 1010 m and 64.15 g respectively, calculate the density of the copper sample. Take Avogadro's number, NA = 6.023 x 10²3 atoms/mole.