Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 9, Problem 57QAP
Consider the sodium chloride unit cell shown in Figure 9.21. Looking only at the front face (five large Cl- ions, four small Na+ ions),
(a) how many cubes share each of the Na+ ions in this face?
(b) how many cubes share each of the Cl- ions in this face?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
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.
6. A compound consists of A-atoms and B-atoms, and its solid crystal forms a cubic unit cell structure, as shown below.
A-atoms occupy corners and faces of the cube. B-atoms are inside the cube and are not shared by adjacent cubic unit
cells. Based on the information here, we can conclude that
(a) A-atoms form an FCC structure; the empirical formula of the compound is A,B2.
(b) A-atoms form an FCC structure; the empirical formula of the compound is AB.
(c) A-atoms form a BCC structure; the empirical formula of the compound is A¬B2.
(d) A-atoms form a BCC structure; the empirical formula of the compound is AB.
(e) None of the above.
A-atoms
(corners and faces)
B-atoms
(inside, not
shared)
a m n T OF THE FL EMENTS
Which of the following statements is/are CORRECT? If an ionic compound with the formula MX forms a face-centered cubic unit cell with the anions (Xn–) at the lattice points, the cations (Mn+) may occupy
1.
one fourth of the tetrahedral holes in each unit cell.
2.
all of the octahedral holes in each unit cell.
3.
the center of each face in each unit cell.
(a) 1 only
(b)2 only
(c)3 only
(d)1 and 2
(e)1, 2, and 3
Chapter 9 Solutions
Chemistry: Principles and Reactions
Ch. 9 - Prob. 1QAPCh. 9 - Prob. 2QAPCh. 9 - The vapor pressure of I2(s) at 30C is 0.466 mm Hg....Ch. 9 - Prob. 4QAPCh. 9 - Trichloroethane, C2H3Cl3 is used as a degreaser...Ch. 9 - p-Dichlorobenzene, C6H4Cl2, can be one of the...Ch. 9 - Prob. 7QAPCh. 9 - Dichloromethane, CH2Cl2,is widely used as a...Ch. 9 - Prob. 9QAPCh. 9 - Prob. 10QAP
Ch. 9 - At a resort in Sante Fe, New Mexico, the...Ch. 9 - Prob. 12QAPCh. 9 - Prob. 13QAPCh. 9 - Consider the following data for the vapor pressure...Ch. 9 - Referring to Figure 9.7, state what phase(s)...Ch. 9 - Referring to Figure 9.7, state what phase(s) is...Ch. 9 - Prob. 17QAPCh. 9 - Consider the phase diagram of the compound in...Ch. 9 - Prob. 19QAPCh. 9 - Prob. 20QAPCh. 9 - Given the following data about xenon,...Ch. 9 - Given the following data about CO2: • triple...Ch. 9 - A pure substance X has the following properties:...Ch. 9 - Prob. 24QAPCh. 9 - Prob. 25QAPCh. 9 - Arrange the following compounds in order of...Ch. 9 - Which of the following would you expect to show...Ch. 9 - Which of the following compounds would you expect...Ch. 9 - Prob. 29QAPCh. 9 - Prob. 30QAPCh. 9 - Explain in terms of forces between structural...Ch. 9 - Prob. 32QAPCh. 9 - Prob. 33QAPCh. 9 - In which of the following processes is it...Ch. 9 - For each of the following pairs, choose the member...Ch. 9 - Follow the directions for Question 35 for the...Ch. 9 - What are the strongest attractive forces that must...Ch. 9 - What are the strongest attractive forces that must...Ch. 9 - Prob. 39QAPCh. 9 - Prob. 40QAPCh. 9 - Of the four general types of solids, which one(s)...Ch. 9 - Of the four general types of solids, which one(s)...Ch. 9 - Prob. 43QAPCh. 9 - Prob. 44QAPCh. 9 - Give the formula of a solid containing Si that is...Ch. 9 - Prob. 46QAPCh. 9 - Prob. 47QAPCh. 9 - Describe the structural units in (a) C (graphite)...Ch. 9 - Molybdenum has an atomic radius of 0.145 nm. The...Ch. 9 - Nickel has an atomic radius of 0.162 nm. The edge...Ch. 9 - Lead (atomicradius=0.181nm) crystallizes with a...Ch. 9 - Iridium crystallizes in a face-centered unit cell....Ch. 9 - In the LiCl structure shown in Figure 9.21, the...Ch. 9 - Potassium iodide has a unit cell similar to that...Ch. 9 - Prob. 55QAPCh. 9 - Consider the CsCl cell (Figure 9.21). The ionic...Ch. 9 - Consider the sodium chloride unit cell shown in...Ch. 9 - Consider the CsCl unit shown in Figure 9.21. How...Ch. 9 - A 1.25-L clean and dry flask is sealed. The air in...Ch. 9 - Aluminum metal crystallizes with a face-centered...Ch. 9 - Consider a sealed flask with a movable piston that...Ch. 9 - Prob. 62QAPCh. 9 - Prob. 63QAPCh. 9 - Prob. 64QAPCh. 9 - Chloroform, CHCl3, has a normal boiling point of...Ch. 9 - Prob. 66QAPCh. 9 - Prob. 67QAPCh. 9 - In the blanks provided, answer the questions...Ch. 9 - Answer the questions below, by filling in the...Ch. 9 - Prob. 70QAPCh. 9 - Prob. 71QAPCh. 9 - What is the difference between (a) a covalent bond...Ch. 9 - Four shiny solids are labeled A, B, C, and D....Ch. 9 - Prob. 74QAPCh. 9 - The following data are given for CC14:...Ch. 9 - Iron crystallizes in a body-centered unit cell....Ch. 9 - Prob. 77QAPCh. 9 - Trichloroethane, C2H3Cl3, is the active ingredient...Ch. 9 - Prob. 79QAPCh. 9 - Prob. 80QAPCh. 9 - Prob. 81QAP
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Rutile, TiO2, crystallizes in a structure characteristic of many other ionic compounds How many formula units of TiO2 are in the unit cell illustrated here? (The oxide ions marked by an x are wholly within the cell; the others are in the cell faces.) Unit cell for rufflearrow_forwardA metal has a body-centered cubic lattice with a unit cell edge length of 2.866 Å (1 Å = 10⁻¹⁰ m). The density of the metal is 7.87 g/cm³. What is the mass of an atom of this metal? (1 m = 10¹² pm).arrow_forwardThe radius of a gold atom is 1.44A. What is the length of the cell edge for gold crystals whose atoms are packed according to a face-centered lattice? What is the density of gold if the atomic weight of gold is 196.967?(Avogadro constant=6.02x10^-23)arrow_forward
- An unidentified elemental solid has a density of 5.36 g/cm3. 5.36 g/cm3. As a solid this element adopts a cubic unit cell with eight atoms per unit cell and an edge length of 565 pm. 565 pm. Based on its molar mass, what is the atomic symbol for this element?arrow_forward1. Simple Cubic Unit Cell a. Consider one unit cell and assume the length of the side of the cube is "a". Remember that “a" is the distance between the centers of two adjacent atoms. How long is “a", the edge of a unit cell, in terms of radius, r, of an atom? b. A simple cubic cell has the equivalent of only 1 atom. Recall the volume of sphere with radius, r, is expressed as V = 4/3 r. With this information, find the total volume of all the spheres in this unit cell, expressed in terms of r. To do this, take the total number of atoms and multiply it by the volume of one atom, with radius, r) c. Find the volume of the entire unit cell including the empty space in terms of r. Remember for a cube the volume, V=1 xw xh. You already know the edge length of the side in terms of "r" based in the earlier questions. d. Find the fraction of the total volume of the cube (which is the unit cell's volume) is occupied by the atoms. Express this as percent and write your answer in the summary table.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
- Sample Exercise 6: Empirical Formula and Density: Ionic Solid The unit cell of a binary compound of copper and oxygen is shown here. Given this image and the ionic radii rcut = 0.74 Å and ro² = 1.26 Å, (a) determine the empirical formula of this compound, (b) determine the coordination numbers of copper and oxygen, (c) estimate the length of the edge of the cubic unit cell, and (d) estimate the density of the compound. Solution (a) To determine the empirical formula we need to determine how many of each type of ion there are per unit cell. O: 8(1/8) + 1 = 2 0²-ions in the unit cell. Cu: 4(1) = 4 Cut ions in the unit cell. Empirical Formula: Cu₂O (b) If we can visually determine the coordination number of one of the ions, we can use Equation 12.1 to determine the coordination number of the other ion. Number of cations per formula unit Number of anions per formula unit anion coordination number cation coordination number Cation coordination number = anion coordination number Copper…arrow_forwarddo (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? nmarrow_forward11. The unit cell of a compound containing strontium, iron, and oxygen is shown here. (a)What type of lattice does this crystal possess (all three lattice vectors are mutually perpendicular)? (b)What is the empirical formula? –3.98 Å 3.98 Å Sr Fe - 3.47 Åarrow_forward
- 9 - Choose the correct alternative that NaCl presents. (a) the total number of atoms in the unit cell and (b) the density. Data (Na)=22.99 g/mol, (Cl)=36.54 g/mol, and (NaCl)=5.64 Å and NA=6.02*10²³ mol-1. A) 8 (a) and (b) 2.20*10⁶ g/m3 D) 4 (a) and (b) 2.14*10⁶ g/cm3 B) 2 (a) and (b) 2.20*10⁶ g/m3 E) 8 (a) and (b) 2.16*10⁶ g/mL C) 4 (a) and (b) 2.16 g/mL F) 2 (a) and (b) 2.20*10⁶ g/m3arrow_forwardAt 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.arrow_forwardIn a simple cubic lattice (based on a single element) with atoms at each point in the lattice and with a lattice constant a, what is the density of atoms (number per unit area) on a surface (100) .arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Unit Cell Chemistry Simple Cubic, Body Centered Cubic, Face Centered Cubic Crystal Lattice Structu; Author: The Organic Chemistry Tutor;https://www.youtube.com/watch?v=HCWwRh5CXYU;License: Standard YouTube License, CC-BY