Lithium bromide crystalizes as shown (right) where the lithium ions are represented as white circles and the bromide ions are represented as filled circles. Give all answers to four significant figures. (a) What is the mass of one unit cell in grams? (b) If the density of LiBr is 3.464 g/mL, what is the edge length of the unit cell in pm? (c) Calculate the Li-Br distance in the crystal structure in pm.

Lithium bromide crystalizes as shown (right) where the lithium ions are represented as white circles and the bromide ions are represented as filled circles. Give all answers to four significant figures. (a) What is the mass of one unit cell in grams? (b) If the density of LiBr is 3.464 g/mL, what is the edge length of the unit cell in pm? (c) Calculate the Li-Br distance in the crystal structure in pm.

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 48QAP: Describe the structural units in (a) C (graphite) (b) SiC (c) FeCl2 (d) C2H2

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Describe the structural units in (a) C (graphite) (b) SiC (c) FeCl2 (d) C2H2
4. Lithium bromide crystalizes as shown (right) where the lithium ions are represented as white circles and the bromide ions are represented as filled circles. Give all answers to four significant figures. (a) What is the mass of one unit cell in grams? (b) If the density of LiBr is 3.464 g/mL, what is the edge length of the unit cell in pm? (c) Calculate the Li-Br distance in the crystal structure in pm.
2) Sodium is a bright, white, soft, and wax-like element dissolves in seawater, crystallizes in rock salt. Sodium is common in nature and crystallizes with a body-centered cubic unit cell and its density is 0.971 g/cm'. (Na: 23 g/mol). 3 (a) What is the volume of the unit cell of a sodium atom, in cm'? (b) What is the edge length of the unit cell of a sodium atom, in pm? (c) What is the radius of a sodium atom, in pm?
A metal crystallizes in the face-centered cubic crystal structure with a unit cell edge of 3.52 x 10 -8 cm.The density of the metal is 8.90 g/cc. (a) What is the mass, in grams, of a single atom of this element? (b) What is the atomic weight of the element (g/mol). (c) What is the radius, in cm, of an atom of the element?
At room temperature, the edge length of the cubic unit cell in elemental silicon is 5.431 Å, and the density of silicon at the same temperature is 2.328 g cm-3 . Each cubic unit cell contains eight silicon atoms. Using only these facts, perform the following operations.(a) Calculate the volume (in cubic centimeters) of one unit cell.(b) Calculate the mass (in grams) of silicon present in a unit cell.(c) Calculate the mass (in grams) of an atom of silicon.(d) The mass of an atom of silicon is 28.0855 u. Estimate Avogadro’s number to four significant figures.
1) Palladium (electron configuration is [Kr]4d¹) crystallizes in a face-centered cubic unit cell. its density is 12.0 g/cm³. (NA = 6.02 x 10²³) (a) What is the total mass of palladium atoms contained within one unit cell? (b) Calculate the atomic radius (r) of Pd.
NaH crystallizes with the same crystal structure as NaCl. The edge length of the cubic unit cell of NaH is 4.880 Å.(a) Calculate the ionic radius of H−. (The ionic radius of Li+ is 0.0.95 Å.)(b) Calculate the density of NaH.
6.023 x 1023 Magnesium (Mg) has an HCP crystal structure and a density of 1.740 g/cm³. What is the volume of its unit cell in cubic meters? (Given: Atomic weight of Mg is 24.31 g/mole and N₁ atoms/mole) (a) 9.28 x 10-23 m³. (b) 9.28 x 10-26 m³ (c) 1.39 x 10-25 m³ (d) 1.39 x 10-28 m³ 2.
2) Sodium is a bright and white, soft, wax-like element dissolved in seawater, crystallized in rock salt. Sodium is common in nature and crystallizes with a body-centered cubic unit cell and its density is 0.971 g/cm³. (Na: 23 g/mol) (a) What is the volume of the unit cell, in cm³? (b) What is the edge length of the unit cell, in pm? (c) What is the radius of a sodium atom, in pm?
do (b) What is the relationship between the length of the face diagonal and the radius, r, of the atoms in the cell? (Enter a mathematical expression.) face diagonal = (c) How is the radius of the atoms related to do? (Enter a mathematical expression.) r = (d) Gold metal crystals have an FCC structure. The unit cell edge in gold is 0.4078 nm long. What is the radius (in nm) of a gold atom? nm
1.Indium has a tetragonal unit cell for which the a and c lattice parameters are 0.459 and 0.495 nm, respectively. (a) If the atomic packing factor and atomic radius are 0.693 and 0.1625 nm, respectively, determine the number of atoms in each unit cell. (b) The atomic weight of indium is 114.82 g/mol; compute its theoretical density.
7. Zirconium has an HCP crystal structure and a density of 6.51 g/cm. (a) What is the volume of its unit cell in cubic meters? (b) If the c/a ratio is 1.593, compute the values of c and a. Consider the unit cell volume, V. = 6R?cV3