form a simple cubic unit cell 1. The anions of CsCl fill the octahedral holes 2. The anions NaCl and ZnS form a body-centered cubic unit cell 3. The cations of CsCI fill the tetrahedral holes 4. The cations of NaCl fill the cubic holes form a face-centered cubic unit cell 5. The cations of ZnS fill every other tetrahedral hole

form a simple cubic unit cell 1. The anions of CsCl fill the octahedral holes 2. The anions NaCl and ZnS form a body-centered cubic unit cell 3. The cations of CsCI fill the tetrahedral holes 4. The cations of NaCl fill the cubic holes form a face-centered cubic unit cell 5. The cations of ZnS fill every other tetrahedral hole

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the unit cell of a face-centred cubic structure of platinum (Pt) atoms, each with radius 139 pm. The unit cell and arrangement of atoms centred on a plane within the unit cell are shown below.
Not all unit cells have a cubic structure. Take for example the below image wherein the unit cell takes the shape of a parallelepiped and has lengths a, b, c and angles α, β, γ. This particular unit cell has an atom arrangement where it has one atom at each corner, one central atom at each of the bases, one atom at the center of the unit cell, and one atom at the center of each of the edge lengths across length c. Given a density of 24.19 g/cm3, calculate the length of edge c in angstroms of a theoretical element Ro given the following unit cell dimensions in angstroms and degrees: a = 9.84A b = 6.4A γ = 43o Atomic Mass: Ro: 50.833 g/mol
1.Using the radius ratio, predict the type of hole where the Mg2+ ion is present in the MgS crystal lattice. The ionic radius of Mg2+ is 0.86 Å and the ionic radius of S2- is 1.70 Å. a.cubic b.trigonal c.octahedral d.tetrahedral2. Which one of the following substances crystallizes as an ionic solid? a.CH3OH b.SiO2 c.K2O d.Sn
A substance is made of elements X, Y and Z. In the unit cell of the compound, X atoms occupy corners of the unit cell, Y atoms occupy center of faces of unit cell and Z atoms occupy edges of the unit cell. Determine the simplest formula of the substance. A. XY3Z4 B. XY3Z C. XY2Z3 D. XY3Z2 E. XY3Z3
Not all unit cells have a cubic structure. Take for example the below image wherein the unit cell takes the shape of a parallelepiped and has lengths a, b, c and angles α, β, γ. This particular unit cell has an atom arrangement where it has one atom at each corner, one central atom at each of the bases, one atom at the center of the unit cell, and one atom at the center of each of the edge lengths across length c. Given a density of 23.93 g/cm3, calculate the length of edge c in angstroms of a theoretical element Ro given the following unit cell dimensions in angstroms and degrees: a = 10.23A b = 6.64A γ = 43o Atomic Mass: Ro: 49.744 g/mol
Not all unit cells have a cubic structure. Take for example the below image wherein the unit cell takes the shape of a parallelepiped and has lengths a, b, c and angles a, B, y. This particular unit cell has an atom arrangement where it has one atom at each corner, one central atom at each of the bases, one atom at the center of the unit cell, and one atom at the center of each of the edge lengths across length c. Given a density of 26.57 g/cm3, calculate the length of edge c in angstroms of a theoretical element Ro given the following unit cell dimensions in angstroms and degrees: a = 10.85A b = 7.56A y = 45° Atomic Mass: Ro: 50.639 g/mol C a + b + c a = ß = 90° ±Y 9. а
9. A binary ionic compound crystallizes in the cubic unit cell shown below. The anions (larger spheres) define the unit cell while four cations (smaller dark spheres) are located in tetrahedral holes within the unit cell. What is the formula for this ionic compound (M = cation, X= anion)? eelo bi biloa bifoa oino biloe ci le of hsk at s sta P. MX b. M2X MX2 d. M2X3 e. MX4 a. с. D. 10. The cubic uniț çell of rhenium trioxide (ReOa) hoo Po
Not all unit cells have a cubic structure. Take for example the below image wherein the unit cell takes the shape of a parallelepiped and has lengths a, b, c and angles α, β, γ. This particular unit cell has an atom arrangement where it has one atom at each corner, one central atom at each of the bases, one atom at the center of the unit cell, and one atom at the center of each of the edge lengths across length c. Given a density of 23.02 g/cm3, calculate the length of edge c in angstroms of a theoretical element Ro given the following unit cell dimensions in angstroms and degrees: a = 9.77A b = 6.68A γ = 44o Atomic Mass: Ro: 54.704 g/mol
Not all unit cells have a cubic structure. Take for example the below image wherein the unit cell takes the shape of a parallelepiped and has lengths a, b, c and angles α, β, γ. This particular unit cell has an atom arrangement where it has one atom at each corner, one central atom at each of the bases, one atom at the center of the unit cell, and one atom at the center of each of the edge lengths across length c. Given a density of 22.82 g/cm3, calculate the length of edge c in angstroms of a theoretical element Ro given the following unit cell dimensions in angstroms and degrees: a = 10.03A b = 6.16A γ = 40o Atomic Mass: Ro: 52.213 g/mol