1. For the HCP crystal structure, show thata) The volume of the unit cell is given by 6√3R²c.b)The relationship between "a" and "e" is given by 2 √ a = c.c) The atomic packing factor is equal to 0.74. ("a" and "c" represent the short and long unit cell dimensions of the HCP crystal structure,respectively.2. Consids

The HCP crystal lattice is shown as- The hexagonal closed structure has 2 lattice parameters,…

1. For the HCP crystal structure, show that a) The volume of the unit cell is given by 6√3R²c. b) The relationship between "a" and "c" is given by 2 ²√₁₁= LNI c) The atomic packing factor is equal to 0.74. ( "a" and "c" represent the short and long unit cell dimensions of the HCP crystal struc respectively. C. 燙

1. For the HCP crystal structure, show that a) The volume of the unit cell is given by 6√3R²c. b) The relationship between "a" and "c" is given by 2 ²√₁₁= LNI c) The atomic packing factor is equal to 0.74. ( "a" and "c" represent the short and long unit cell dimensions of the HCP crystal struc respectively. C. 燙

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter9: Liquids And Solids

Section: Chapter Questions

Problem 54QAP: Potassium iodide has a unit cell similar to that of sodium chloride (Figure 9.21). The ionic radii...

See similar textbooks

Similar questions

The unit cell of silicon carbide, SiC, is illustrated below. (a) In what type of unit cell are the (dark gray) C atoms arranged? (b) If one edge of the silicon carbide unit cell is 436.0 pm, what is the calculated density of this compound? A portion of the solid-state structure of silicon carbide.
Rutile, TiO2, crystallizes in a structure characteristic of many other ionic compounds How many formula units of TiO2 are in the unit cell illustrated here? (The oxide ions marked by an x are wholly within the cell; the others are in the cell faces.) Unit cell for ruffle
Potassium chloride has the same unit cell as NaCl. Using the ion sizes in Figure 7.11, calculate the density of KCl. FIGURE 7.11 Relative sizes of some common ions. Rodii are given in picometers (1 pm 1 1012 m). (Data taken from J. Emsley, The Elements, Clarendon Press, Oxford, 1998, 3rd edition.)
Silicon carbide, SiC, is a very hard, high-melting solid. What kind of crystal forces account for these properties?
Outline a two-dimensional unit cell for the pattern shown here. If the black squares are labeled A and the white squares are B, what is the simplest formula for a compound based on this pattern?
MnO has either the NaCI type structure or the CsCI type structure (see Exercise 69). The edge length of the MnO unit cell is 4.47 10-8 cm and the density of MnO is 5.28 g/cm3. a. Does MnO crystallize in the NaCl or the CsCl type structure? b. Assuming that the ionic radius of oxygen is 140. pm, estimate the ionic radius of manganese.
Lithium hydride (LiH) has the sodium chloride structure, and the length of the edge of the unit cell is 4.086 108 cm. Calculate the density of this solid.
Potassium iodide has a unit cell similar to that of sodium chloride (Figure 9.21). The ionic radii of K+ and I- are 0.133 nm and 0.216 nm, respectively. How long is (a) one side of the cube? (b) the face diagonal of the cube?
In the LiCl structure shown in Figure 9.21, the chloride ions form a face-centered cubic unit cell 0.513 nm on an edge. The ionic radius of Cl- is 0.181 nm. (a) Along a cell edge, how much space is between the Cl- ions? (b) Would an Na+ ion (r=0.095nm) fit into this space? a K+ ion (r=0.133nm)?
Describe, in general, the structures of ionic solids. Compare and contrast the structure of sodium chloride and zinc sulfide. How many tetrahedral holes and octahedral holes are there per closest packed anion? In zinc sulfide, why are only one-half of the tetrahedral holes filled with cations?
What is a lattice? What is a unit cell? Describe a simple cubic unit cell. How many net atoms are contained in a simple cubic unit cell? How is the radius of the atom related to the cube edge length for a simple cubic unit cell? Answer the same questions for the body-centered cubic unit cell and for the face-centered unit cell.