Please correct answer and don't use hand rating A unit cell with titanium (aqua) and oxygen (red) atoms is shown.How many of each atom are in this unit cell?1.oxygen atoms2.titanium atoms3. The titanium atom atoms are intetrahedarl holes.heptagonal holes.octahedral holes.trigonal holes.tetragonal holes.

1. Six oxygen atoms2. Nine titanium atoms3. The titanium atoms are in octahedral holes. An atom…

Answered: A unit cell with titanium (aqua) and…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter11: Liquids And Solids

Section: Chapter Questions

Problem 11.72QE

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Like ZnS, lead(II) sulfide, PbS (commonly called galena), has a 1:1 empirical formula with a 2+ cation combined with the sulfide anion. Unit cell of PbS Sample of galena Does PbS have the same solid structure as ZnS? If different, how are they different? How is the unit cell of PbS related to its formula?
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.
A compound of cadmium, tin, and phosphorus is used in the fabrication of some semiconductors. It crystallizes with cadmium occupying one-fourth of the tetrahedral holes and tin occupying one-fourth of the tetrahedral holes in a closest packed array of phosphide ions. What is the formula of the compound? Explain your answer.
The solid-state structure of silicon is shown below. Unit cell for silicon (a) Describe this crystal as pc, bcc, or fcc. (b) What type of holes are occupied in the lattice? (c) How many Si atoms are there per unit cell? (d) Calculate the density of silicon in g/cm3 (given that the cube edge has a length of 543.1 pm). (e) Estimate the radius of the silicon atom. (Note: The Si atoms on the edges do not touch one another.)
The solid-state structure of silicon carbide is shown below. (a) How many atoms of each type are contained within the unit cell? What is the formulas of silicon carbide? (b) Knowing that the SiC bond length is 188.8 pm (and the SiCSi bond angle is 109.5), calculate the density of SiC. Unit cell of SiC Sample of silicon carbide
Consider 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?
A 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.
CaTiO3, a perovskite, has the structure below. (a) If the density of the solid is 4.10 g/cm3, what is the length of a side of the unit cell? (b) Calculate the radius of the Ti4+ ion in the center of the unit cell. How well does your calculation agree with a literature value of 75 pm? Unit cell of the perovskite CaTiO3 A sample of perovskite, iO3 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.)
A diamond unit cell is shown here. Unit cell of diamond (a) How many carbon atoms are in one unit cell? (b) The unit cell can be considered as a cubic unit cell of C atoms with other C atoms in holes in the lattice. What type of unit cell is this (pc, bcc, fcc)? In what holes are other C atoms located, octahedral or tetrahedral holes?
If one edge of the silicon carbide unit cell is 436.0 pm, what is the calculated density of this compound? (a) 0.803 g/cm3 (b) 0311g/cm3 (c) 321 g/cm3
Phase diagrams for materials that have allotropes can be more complicated than those shown in the chapter. Use the phase diagram for carbon given here to answer the following questions. (a) How many triple points are present and what phases are in equilibrium for each? (b) Is there a single point where all four phases are in equilibrium? (c) Which is more stable at high pressures, diamond or graphite? (d) Which is the stable phase of carbon at room temperature and 1 atmosphere pressure?
Which of the following elements reacts with sulfur to form a solid in which the sulfur atoms form a closest packed array with all of the octahedral holes occupied: Li, Na, Be, Ca, or Al?

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A unit cell with titanium (aqua) and oxygen (red) atoms is shown. How many of each atom are in this unit cell? 1. oxygen atoms 2. titanium atoms 3. The titanium atom atoms are in tetrahedarl holes. heptagonal holes. octahedral holes. trigonal holes. tetragonal holes.