Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 12, Problem 49GQ
Interpretation Introduction
Interpretation:
From the picture, picture B is more efficiency than picture A and diagram B is leads to the surface coverage of 78.5% has to be proved.
Concept introduction:
The area of the triangle is calculated by using following formula,
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Chemistry & Chemical Reactivity
Ch. 12.1 - (a) Determining an Atom Radius from Lattice...Ch. 12.2 - If an ionic solid has an fcc lattice of anions (X)...Ch. 12.2 - Potassium chloride has the same unit cell as NaCl....Ch. 12.6 - Prob. 1.1ACPCh. 12.6 - Describe the unit cell of lithium (see Figure).Ch. 12.6 - Prob. 1.3ACPCh. 12.6 - Prob. 1.4ACPCh. 12.6 - Prob. 2.1ACPCh. 12.6 - Prob. 2.2ACPCh. 12.6 - Prob. 2.3ACP
Ch. 12.6 - How many tin atoms are contained in the tetragonal...Ch. 12.6 - Prob. 3.2ACPCh. 12.6 - Prob. 3.3ACPCh. 12.6 - Prob. 3.4ACPCh. 12 - Outline a two-dimensional unit cell for the...Ch. 12 - Outline a two-dimensional unit cell for the...Ch. 12 - A portion of the crystalline lattice for potassium...Ch. 12 - The unit cell of silicon carbide, SiC, is...Ch. 12 - Prob. 5PSCh. 12 - Rutile, TiO2, crystallizes in a structure...Ch. 12 - Cuprite is a semiconductor. Oxide ions are at the...Ch. 12 - The mineral fluorite, which is composed of calcium...Ch. 12 - Calcium metal crystallizes in a face-centered...Ch. 12 - The density of copper metal is 8.95 g/cm3. If the...Ch. 12 - Potassium iodide has a face-centered cubic unit...Ch. 12 - A unit cell of cesium chloride is illustrated in...Ch. 12 - Predict the trend in lattice energy, from least...Ch. 12 - Prob. 14PSCh. 12 - To melt an ionic solid, energy must be supplied to...Ch. 12 - Which compound in each of the following pairs...Ch. 12 - Prob. 17PSCh. 12 - Prob. 18PSCh. 12 - Considering only the molecular orbitals formed by...Ch. 12 - Prob. 20PSCh. 12 - Prob. 21PSCh. 12 - Prob. 22PSCh. 12 - Prob. 23PSCh. 12 - Prob. 24PSCh. 12 - Prob. 25PSCh. 12 - Prob. 26PSCh. 12 - Prob. 27PSCh. 12 - Prob. 28PSCh. 12 - A diamond unit cell is shown here. Unit cell of...Ch. 12 - The structure of graphite is given in Figure...Ch. 12 - We have identified six types of solids (metallic,...Ch. 12 - Prob. 32PSCh. 12 - Classify each of the following materials as...Ch. 12 - Prob. 34PSCh. 12 - Benzene, C6H6, is an organic liquid that freezes...Ch. 12 - The specific heat capacity of silver is 0.235 J/g ...Ch. 12 - Prob. 37PSCh. 12 - Prob. 38PSCh. 12 - Prob. 39PSCh. 12 - If your air conditioner is more than several years...Ch. 12 - Sketch a phase diagram for O2 from the following...Ch. 12 - Tungsten crystallizes in the unit cell shown here....Ch. 12 - Silver crystallizes in a face-centered cubic unit...Ch. 12 - The unit cell shown here is for calcium carbide....Ch. 12 - The very dense metal iridium has a face-centered...Ch. 12 - Vanadium metal has a density of 6.11 g/cm3....Ch. 12 - Prob. 47GQCh. 12 - Prob. 48GQCh. 12 - Prob. 49GQCh. 12 - Consider the three types of cubic units cells. (a)...Ch. 12 - The solid-state structure of silicon is shown...Ch. 12 - The solid-state structure of silicon carbide is...Ch. 12 - Spinels are solids with the general formula AB2O4...Ch. 12 - Using the thermochemical data below and an...Ch. 12 - Prob. 55GQCh. 12 - Prob. 56GQCh. 12 - Prob. 57GQCh. 12 - Prob. 58GQCh. 12 - Prob. 59GQCh. 12 - Prob. 60GQCh. 12 - Like ZnS, lead(II) sulfide, PbS (commonly called...Ch. 12 - CaTiO3, a perovskite, has the structure below. (a)...Ch. 12 - Potassium bromide has the same lattice structure...Ch. 12 - Calculate the lattice energy of CaCl2 using a...Ch. 12 - Why is it not possible for a salt with the formula...Ch. 12 - Prob. 67SCQCh. 12 - Prob. 68SCQCh. 12 - Prob. 69SCQCh. 12 - Phase diagrams for materials that have allotropes...
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- 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?arrow_forwardThe 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.arrow_forwardConsider the three types of cubic units cells. (a) Assuming that the spherical atoms or ions in a primitive cubic unit cell just touch along the cubes edges, calculate the percentage of occupied space within the unit cell. (Recall that the volume of a sphere is (4/3)r3, where r is the radius of the sphere.) (b) Compare the percentage of occupied space in the primitive cell (pc) with the bcc and fcc unit cells. Based on this, will a metal in these three forms have the same or different densities? If different, in which is it most dense? In which is it least dense?arrow_forward
- If 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_forwardA cubic unit cell contains manganese ions at the corners and fluoride ions at the center of each edge. (a) What is the empirical formula of this compound? Explain your answer. (b) What is the coordination number of the Mn3+ ion? (c) Calculate the edge length of the unit cell if the radius of a Mn3+ ion is 0.65 A. (d) Calculate the density of the compound.arrow_forwardThe coordination number of uniformly sized spheres in a cubic closest-packing (FCC) array is 12. Give the coordination number of each atom in (a) a simple cubic lattice. (b) a body-centered cubic lattice.arrow_forward
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