Concept explainers
Interpretation:
The interionic distance of Barium sulfide has to be calculated and a comparison of this value with the sum of ionic radii has to be done.
Concept Introduction:
Fcc unit cell:
Eight atoms occupy the corner position of a cube each contributing
Density:
It is the ration of mass and volume of a substance. Mathematically, it can be represented as given below.
Where,
Volume of a cubic unit cell:
Volume of cubic unit cell
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Chapter 9 Solutions
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
- Which substance has the greatest electrical conductivity? The smallest electrical conductivity? Explain your choices briefly. (a) RbCl() (b) NaBr(s) (c) Rb (d) Diamondarrow_forwardWhat is the relationship between the structures of buckminsterfullerene and carbon nanotubes?arrow_forwardIf an ionic solid has an fcc lattice of anions (X) and all of the tetrahedral holes are occupied by metal cations (M), is the formula of the compound MX, MX2, or M2X?arrow_forward
- How could you tell experimentally if TiO2 is an ionic solid or a network solid?arrow_forwardLithium 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.arrow_forwardThe ionic compound, CsCl, forms a body centered cubic structure (see below) where the anions occupy the corners of the crystal (red) and the cations the body centered position (green). If the density of the compound is 3.99 g/cm3 and the ionic radius of Cs+ is 169 pm, what is the ionic radius of Cl− in pm?arrow_forward
- BaTiO3 has the perovskite structure shown below. The ionic size of Ba2+, Ti4*, and O2- are 0.161 nm, 0.061 nm, and 0.141 nm. The atomic mass of Ba, Ti, and O are 137 g/mol, 48 g/mol, and 16 g/mol. Bal Explain why Ti occupies the B site (cube center). • Using the density of BaTiO3 of 5.89 g/mol, calculate the unit cell length for the structure. If a Fe3+ substitutes for Tit* ion, what point defects might occur in BaTiO3?arrow_forwardThe density of a metal is 8.92 g/cm3. The metal crystalizes into FCC structure. If the atomic radius of the metal is 173 pm, determine the molar mass of the metal (3 significant figures).arrow_forwardWhich of the following set of compounds form an ionic solid, a molecular solid, and a covalent network solid, in that order? (A) Na2O, Na2O2, SiO2; (B) Na2O, MgO, Al2O3; (C) BaO, BaO2, CO2; (D) CaO, SO2, SiO2;arrow_forward
- Crystal structure represents the manner in which atoms or ions are arrayed in space. It is defined in terms of the unit celI (1) and the atom (2) within the unit cell. (1) = direction, (2) = sizes. (1) = plane, (2) = positions. (1) = geometry, (2) = positions. (1) = geometry, (2) = sizes.arrow_forwardA certain compound, whose density is 4.56 g/cm³, crystallizes in the tetragonal system with unit lattice dimensions of a = b = 6.58 Å and c = 5.93 Ả. If the unit lattice contains four molecules, calculate the molar mass of the compound in g mol"arrow_forwardQ1/A B) Describe the Bohr model of hydrogen atom. What are the shortcomings of the Bohr model? Prove that the atomic packing factor (APF) for the BCC crystal structure is 0.68.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningPhysical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,
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