Chemistry
4th Edition
ISBN: 9780078021527
Author: Julia Burdge
Publisher: McGraw-Hill Education
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Textbook Question
Chapter 11.6, Problem 1PPA
Practice ProblemATTEMPT
Aluminum metal crystallizes in a face-centered cubic unit cell. If the length of the cell edge is 404 pm, what is the density of aluminum in
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An element crystallizes in a face-centered cubic lattice and has a density of 1.456 g/cm³. The edge of its unit cell is 4.52 x
10-8 cm. . What is the mass of a unit cell (in grams)?
(a) 13.40 x 10-19
(b) 3.41 x 10-22
(c) 1.34 x 10-22
(d) 3.49 x 10-19
Gold crystallizes into a face-centered cubic structure (aka closest-packed cubic structure). What is the mass of one unit cell of gold metal in gram? (1 u = 1.6605 x 10–24 g)
(A) 3.271 x 10–22 g
(B) 6.543 x 10–22 g
(C) 9.814 x 10–22 g
(D) 1.308 x 10–21 g
Provide STEP by STEP details correct Explanation.
Question :
iron has a face centered cubic unit cell with a length of 608 pm along an edge. what is the density of iron in kg m-3 .
Chapter 11 Solutions
Chemistry
Ch. 11.1 - Prob. 1PPACh. 11.1 - Prob. 1PPBCh. 11.1 - Prob. 1PPCCh. 11.1 - Prob. 1CPCh. 11.1 - Prob. 2CPCh. 11.2 - Prob. 1PPACh. 11.2 - Prob. 1PPBCh. 11.2 - Prob. 1PPCCh. 11.2 - Prob. 1CPCh. 11.2 - 11.2.2 Given the following information for ...
Ch. 11.2 - 11.2.3 Using the graph, estimate the vapor...Ch. 11.2 - Using the result from question 11.2.3 and another...Ch. 11.3 - Practice ProblemATTEMPT When silver crystallizes,...Ch. 11.3 - Practice Problem BUILD
The density of sodium metal...Ch. 11.3 - Practice Problem CONCEPTUALIZE The diagram shows...Ch. 11.3 - 11.3.1 Nickel has a face-centered cubic unit cell...Ch. 11.3 - A metal crystalizes in a body-centered cubic unit...Ch. 11.4 - Prob. 1PPACh. 11.4 - Prob. 1PPBCh. 11.4 - Prob. 1PPCCh. 11.4 - 11.4.1 The diagram here shows the anions in the...Ch. 11.4 - 11.4.2 At what angle would you expect X rays of...Ch. 11.5 - Practice ProblemATTEMPT LiF has the same unit cell...Ch. 11.5 - Practice ProblemBUILD NiO also adopts the...Ch. 11.5 - Practice ProblemCONCEPTUALIZE Referring to the...Ch. 11.6 - Practice Problem ATTEMPT
Aluminum metal...Ch. 11.6 - Practice Problem BUILD
Copper crystallizes in a...Ch. 11.6 - Prob. 1PPCCh. 11.6 - 11.6.1 How much energy (in kJ) is required to...Ch. 11.6 - 11.6.2 How much energy (in kJ) is given off when...Ch. 11.7 - Practice ProblemATTEMPT Calculate the amount of...Ch. 11.7 - Practice ProblemBUILD Determine the final state...Ch. 11.7 - Prob. 1PPCCh. 11.7 - Prob. 1CPCh. 11.7 - Prob. 2CPCh. 11.8 - Prob. 1PPACh. 11.8 - Practice Problem BUILD
Sketch the phase diagram of...Ch. 11.8 - Prob. 1PPCCh. 11 - Which of the following would you expect to be more...Ch. 11 - 11.2
Which of the following would you expect to be...Ch. 11 - Prob. 3KSPCh. 11 - Prob. 4KSPCh. 11 - Give an example for each type of intermolecular...Ch. 11 - 11.2 Explain the term polarizability. What kind of...Ch. 11 - Prob. 3QPCh. 11 - Prob. 4QPCh. 11 - 11.5 What physical properties are determined by...Ch. 11 - Prob. 6QPCh. 11 - Describe the types of intermolecular forces that...Ch. 11 - Prob. 8QPCh. 11 - Prob. 9QPCh. 11 - The binary hydrogen compounds of the Group 4A...Ch. 11 - 11.11 List the types of intermolecular forces that...Ch. 11 - Prob. 12QPCh. 11 - Prob. 13QPCh. 11 - Arrange the following in order of increasing...Ch. 11 - Diethyl ether has a boiling point of 34 .5°C , and...Ch. 11 - 11.16 Which member of each of the following pairs...Ch. 11 - Prob. 17QPCh. 11 - Explain in terms of intermolecular forces why (a)...Ch. 11 - What kind of attractive forces must be overcome to...Ch. 11 - Prob. 20QPCh. 11 - Prob. 21QPCh. 11 - Explain why liquids, unlike gases, are virtually...Ch. 11 - 11.23 What is surface tension? What is the...Ch. 11 - Prob. 24QPCh. 11 - Prob. 25QPCh. 11 - 11.26 A glass can be filled slightly above the rim...Ch. 11 - 11.27 Draw diagrams showing the capillary action...Ch. 11 - Prob. 28QPCh. 11 - Why does the viscosity of a liquid decrease with...Ch. 11 - Why is ice less dense than water?Ch. 11 - 11.31 Outdoor water pipes have to be drained or...Ch. 11 - Prob. 32QPCh. 11 - Prob. 33QPCh. 11 - Prob. 34QPCh. 11 - Predict the viscosity of ethylene glycol relative...Ch. 11 - 11.36 Vapor pressure measurements at several...Ch. 11 - The vapor pressure of liquid X is lower than that...Ch. 11 - 11.38 Define the following terms: crystalline...Ch. 11 - Describe the geometries of the following cubic...Ch. 11 - Classify the solid states in terms of crystal...Ch. 11 - The melting points of the oxides of the...Ch. 11 - Define X-ray diffraction. What are the typical...Ch. 11 - 11.43 Write the Bragg equation. Define every term...Ch. 11 - 11.44 What is the coordination number of each...Ch. 11 - Calculate the number of spheres that would be...Ch. 11 - Metallic iron crystallizes in a cubic lattice. The...Ch. 11 - Barium metal crystallizes in a body-centered cubic...Ch. 11 - 11.48 Vanadium crystallizes in a body-centered...Ch. 11 - Europium crystallizes in a body-centered cubic...Ch. 11 - 11.50 Crystalline silicon has a cubic structure....Ch. 11 - 11.51 A face-centered cubic cell contains 8 X...Ch. 11 - When X rays of wavelength 0.090 nm are diffracted...Ch. 11 - The distance between layers in an NaCl crystal is...Ch. 11 - Identify the unit cell of molecular iodine ( I 2 )...Ch. 11 - Shown here is a zinc oxide unit cell. What is the...Ch. 11 - Prob. 56QPCh. 11 - Prob. 57QPCh. 11 - A solid is hard, brittle, and electrically...Ch. 11 - A solid is soft and has a low melting point (below...Ch. 11 - Prob. 60QPCh. 11 - 11.61 Which of the following are molecular solids...Ch. 11 - Classify the solid state of the following...Ch. 11 - Prob. 63QPCh. 11 - Prob. 64QPCh. 11 - Define glass. What is the chief component of...Ch. 11 - 11.66 What is a phase change? Name all possible...Ch. 11 - What is the equilibrium vapor pressure of a...Ch. 11 - Use any one of the phase changes to explain what...Ch. 11 - 11.69 Define the following terms: (a) molar heat...Ch. 11 - How is the molar heat of sublimation related to...Ch. 11 - What can we learn about the intermolecular forces...Ch. 11 - The greater the molar heat of vaporization of a...Ch. 11 - Prob. 73QPCh. 11 - As a liquid is heated at constant pressure, its...Ch. 11 - What is critical temperature? What is the...Ch. 11 - Prob. 76QPCh. 11 - 11.77 How do the boiling points and melting points...Ch. 11 - Prob. 78QPCh. 11 - The vapor pressure of a liquid in a closed...Ch. 11 - Wet clothes dry more quickly on a hot, dry day...Ch. 11 - Which of the following phase transitions gives off...Ch. 11 - 11.82 A beaker of water is heated to boiling by a...Ch. 11 - Prob. 83QPCh. 11 - Calculate the amount of heat (in kJ) required to...Ch. 11 - Prob. 85QPCh. 11 - The molar heats of fusion and sublimation of...Ch. 11 - How is the rate of evaporation of a liquid...Ch. 11 - 11.88 The following compounds, listed with their...Ch. 11 - Prob. 89QPCh. 11 - A student hangs wet clothes outdoors on a winter...Ch. 11 - Explain why steam at 100°C causes more serious...Ch. 11 - What is a phase diagram? What useful information...Ch. 11 - 11.93 Explain how water’s phase diagram differs...Ch. 11 - The blades of ice skates are quite thin, so the...Ch. 11 - 11.95 A length of wire is placed on top of a block...Ch. 11 - Prob. 96QPCh. 11 - Prob. 97QPCh. 11 - 11.98 Name the kinds of attractive forces that...Ch. 11 - Prob. 99APCh. 11 - At –35°C , liquid HI has a higher vapor pressure...Ch. 11 - Prob. 101APCh. 11 - Prob. 102APCh. 11 - Prob. 103APCh. 11 - Prob. 104APCh. 11 - Prob. 105APCh. 11 - A CO 2 fire extinguisher is located on the outside...Ch. 11 - Prob. 107APCh. 11 - A flask of water is connected to a powerful vacuum...Ch. 11 - Prob. 109APCh. 11 - The interionic distances of several alkali halide...Ch. 11 - Which has a greater density, crystalline Si O 2 or...Ch. 11 - A student is given four solid samples labeled W,...Ch. 11 - Prob. 113APCh. 11 - Prob. 114APCh. 11 - X rays of wavelength 0.154 nm strike an aluminum...Ch. 11 - 11.116 The properties of gases, liquids, and...Ch. 11 - Prob. 117APCh. 11 - Prob. 118APCh. 11 - Prob. 119APCh. 11 - Prob. 120APCh. 11 - Prob. 121APCh. 11 - 11.122 The distance between and is 257 pm in...Ch. 11 - Prob. 123APCh. 11 - Prob. 124APCh. 11 - 11.125 Calculate the for the following processes...Ch. 11 - 11.126 Which liquid would you expect to have a...Ch. 11 - 11.127 A beaker of water is placed in a closed...Ch. 11 - Prob. 128APCh. 11 - Prob. 129APCh. 11 - Carbon and silicon belong to Group 4A of the...Ch. 11 - Prob. 131APCh. 11 - Prob. 132APCh. 11 - Prob. 133APCh. 11 - Prob. 134APCh. 11 - Prob. 135APCh. 11 - Prob. 136APCh. 11 - Prob. 137APCh. 11 - Prob. 138APCh. 11 - Prob. 139APCh. 11 - 11.140 Sketch the cooling curves of water from...Ch. 11 - Prob. 141APCh. 11 - Prob. 142APCh. 11 - A closed vessel of volume 9.6 L contains 2.0 g of...Ch. 11 - 11.144 The electrical conductance of copper metal...Ch. 11 - 11.145 Assuming ideal behavior, calculate the...Ch. 11 - Prob. 146APCh. 11 - Which of the following compounds is most likely to...Ch. 11 - 11.148 A chemistry instructor performed the...Ch. 11 - Prob. 149APCh. 11 - Prob. 150APCh. 11 - The phase diagram of helium is shown. Helium is...Ch. 11 - 11.152 The phase diagram of sulfur is shown. (a)...Ch. 11 - Prob. 153APCh. 11 - Prob. 154APCh. 11 - Prob. 155APCh. 11 - Prob. 156APCh. 11 - Prob. 157APCh. 11 - Prob. 158APCh. 11 - 11.159 Why do citrus growers spray their trees...Ch. 11 - Prob. 2SEPPCh. 11 - 3. Each cubic unit cell (edge length a = 543 pm)...
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- Gold crystallizes into a face-centered cubic structure (aka closest-packed cubic structure). If the density of gold is 19.3 g/cm3, what is the atomic radius of gold in picometers (pm)? (A) 177 pm (B) 155 pm (C) 144 pm (D) 134 pmarrow_forwardGold crystallizes into a face-centered cubic structure (aka closest-packed cubic structure), and the density of gold is 19.3 g/cm3. Calculate the atomic radius of gold in picometer (pm). (A) 177 pm (B) 155 pm (C) 144 pm (D) 134 pmarrow_forwardAn element crystallizes in a face-centered cubic lattice and has a density of 1.456 g/cm³. The edge of its unit cell is 4.52 x 10-8 cm. What is the volume of a unit cell (in cm³)? (a) 9.23 x 10-23 (b) 92.3 x 10-20 (c) 82.3 x 10-23 (d) 8.23 x 10-23arrow_forward
- Consider an unknown metal M. If the density of M is 19.3 g/cm3 and radius is 137 pm, find out the crystal lattice of M. Answer Choices: (A) FCC (В) ВСС (С) НСР (D) Simple cubicarrow_forwardA metal crystallises in face centred cubic structure with metallic radius √2 Å. The volume of the unit cell (in m³) is (a) 6.4 × 10-29 (b) 4 x 10 -29 (c) 6.4 × 10-30 (d) 4 × 10-10 xarrow_forwardIridium (Ir) has a face-centered cubic unit cell with an edge length of 383.3 pm. What is the atomic radius of iridium? The atomic mass of iridium is 192.2 g/mol. (Avogadro’s #, NA = 6.022 x 1023/mol; 1 pm = 10–10 cm) (A) 135.5 pm (B) 166.0 pm (C) 191.6 pm (D) 271.0 pmarrow_forward
- 2) Sodium is a bright and white, soft, wax-like element dissolved in seawater, crystallized in rock salt. Sodium is common in nature and crystallizes with a body-centered cubic unit cell and its density is 0.971 g/cm³. (Na: 23 g/mol) (a) What is the volume of the unit cell, in cm³? (b) What is the edge length of the unit cell, in pm? (c) What is the radius of a sodium atom, in pm?arrow_forwardSilver is a metal commonly used in jewelry and photography. It crystallizes with a face-centered cubic (FCC) unit cell 0.507 nm on an edge. What is the volume of Ag atom? (A) 3.42 х 10-22 ст3 5.4 x 10-25 cm3 5.499 ст3 2.41 x 10-23 cm3 E 1.79 х1о-8 ст3arrow_forwardCr crystallizes in a body-centered cubic lattice. The atomic radius of Cr is 128 pm. Calculate the unit cell edge length in angstrom (Å). (Conversion factors: 1 m = 1x 1012 pm; 1 m = 1 x 1010 A A 2.54 A B 2.96 Å (c) 3.62 A D 1.28 Åarrow_forward
- Iridium (Ir) has a face-centered cubic unit cell with an edge length of 383.3 pm. What is the density of iridium? The atomic mass of iridium is 192.2 g/mol. (Avogadro’s #, NA = 6.022 x 1023/mol; 1 pm = 10–10 cm) (A) 5.668 g/cm3 (B) 16.49 g/cm3 (C) 17.00 g/cm3 (D) 21.79 g/cm3arrow_forwardGold crystallizes into a face-centered cubic structure (aka closest-packed cubic structure). If the density of gold is 19.3 g/cm3, what is the edge length of the unit cell of gold in picometers? (Atomic mass of gold = 197.0 u; 1 u = 1.6605 x 10–24 g; 1 pm = 10–10 cm) (A) 324 pm (B) 371 pm (C) 408 pm (D) 439 pmarrow_forwardDiamond has a face-centered cubic unit cell, with fourmore C atoms in tetrahedral holes within the cell. Densities of diamonds vary from 3.01 g/cm³ to 3.52 g/ cm³ C atoms are missing from some holes. (a) Calculate the unit-cell edge length of the densest diamond. (b) Assuming the cell dimensions are fixed, how many C atoms are in the unit cell of the diamond the lowest density?arrow_forward
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