Chemistry: Structure and Properties, Books a la Carte Edition & Modified MasteringChemistry with Pearson eText -- ValuePack Access Card -- for Chemistry: Structure and Properties Package
1st Edition
ISBN: 9780133908695
Author: Nivaldo J. Tro
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 13, Problem 58E
The density of an unknown metal is 12.3 g/cm3 and its atomic radius is 0.314 nm. It is a face-centered cubic lattice. Find the
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
The density of an unknown metal is 2.64 g/cm3 and its atomic radius is 0.215 nm. It has a face-centered cubic lattice. Determine its atomic weight.
2. Lead has a face centered cubic lattice with all atoms at the lattice points and a unit cell edge
length of 495 pm. Its atomic weight is 207.2 g/mol. What is the density of lead in pounds per
cubic feet?
Metallic
chromium
has a body-
centered
cubic
structure
(all atoms at
the lattice
points) and
a density of
3
7.20 g/cm³.
Assume
chromium
atoms to be
spheres. The
spheres in a
body-
centered
array
оcсиру
68.0% of the
total space.
Find the
atomic
radius of
chromium.
The volume
of a sphere
is equal to
4Tr /3.
Radius =
%3|
Chapter 13 Solutions
Chemistry: Structure and Properties, Books a la Carte Edition & Modified MasteringChemistry with Pearson eText -- ValuePack Access Card -- for Chemistry: Structure and Properties Package
Ch. 13 - Determine what state this substance is in at 1 atm...Ch. 13 - Prob. 2SAQCh. 13 - Prob. 3SAQCh. 13 - Prob. 4SAQCh. 13 - Prob. 5SAQCh. 13 - Prob. 6SAQCh. 13 - Prob. 7SAQCh. 13 - Prob. 8SAQCh. 13 - Prob. 9SAQCh. 13 - Prob. 10SAQ
Ch. 13 - What is a phase diagram?Ch. 13 - Draw a generic phase diagram and label its...Ch. 13 - What is the significance of crossing a line in a...Ch. 13 - What is graphene? Why is graphene unique?Ch. 13 - Prob. 5ECh. 13 - What is a crystalline lattice? How is the lattice...Ch. 13 - Prob. 7ECh. 13 - Prob. 8ECh. 13 - What is the difference between hexagonal closest...Ch. 13 - What are the three basic types of solids and the...Ch. 13 - Prob. 11ECh. 13 - What kinds of forces hold each of the three basic...Ch. 13 - Prob. 13ECh. 13 - Prob. 14ECh. 13 - Prob. 15ECh. 13 - Prob. 16ECh. 13 - Prob. 17ECh. 13 - Prob. 18ECh. 13 - Prob. 19ECh. 13 - Consider the phase diagram for iodine shown here....Ch. 13 - Prob. 21ECh. 13 - Prob. 22ECh. 13 - Prob. 23ECh. 13 - Prob. 24ECh. 13 - Prob. 25ECh. 13 - An X-ray beam of unknown wavelength is diffracted...Ch. 13 - Prob. 27ECh. 13 - Determine the coordination number for each...Ch. 13 - Prob. 29ECh. 13 - Molybdenum crystallizes with the body-centred unit...Ch. 13 - Prob. 31ECh. 13 - An atom has a radius of 142 pm and crystallizes in...Ch. 13 - Rhodium has a density of 12.41 g / cm3 and...Ch. 13 - Barium has a density of 3.59 g/cm3 and...Ch. 13 - Prob. 35ECh. 13 - Palladium crystallizes with a face-centered cubic...Ch. 13 - Prob. 37ECh. 13 - Identify each solid as molecular, ionic, or...Ch. 13 - Which solid has the highest melting point? Why?...Ch. 13 - Which solid has the highest melting point? Why?...Ch. 13 - Which solid in each pair has the higher melting...Ch. 13 - Which solid in each pair has the higher melting...Ch. 13 - Prob. 43ECh. 13 - Prob. 44ECh. 13 - Prob. 45ECh. 13 - Prob. 46ECh. 13 - The unit cells for cesium chloride and barium(ll)...Ch. 13 - Prob. 48ECh. 13 - Prob. 49ECh. 13 - Prob. 50ECh. 13 - Prob. 51ECh. 13 - Prob. 52ECh. 13 - Prob. 53ECh. 13 - Prob. 54ECh. 13 - Prob. 55ECh. 13 - Prob. 56ECh. 13 - Prob. 57ECh. 13 - The density of an unknown metal is 12.3 g/cm3 and...Ch. 13 - Prob. 59ECh. 13 - Consider a planet where the pressure of the...Ch. 13 - An unknown metal is found to have a density of...Ch. 13 - Prob. 62ECh. 13 - Potassium chloride crystallizes in the rock salt...Ch. 13 - Calculate the fraction of empty space in cubic...Ch. 13 - Prob. 65ECh. 13 - Prob. 66ECh. 13 - Prob. 67E
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
- 8.98 If you know the density of material and the length of the edge of its cubic Iattice, how would you determine if it is face-centered cubic, body-centered cubic, or simple cubic Would you have to look up any information?arrow_forwardAn unidentified elemental solid has a density of 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. Based on its molar mass, what is the atomic symbol for this element? symbol:arrow_forward1)Pure gold has a density of 19.32 g/cm3, and the atoms are packed in a face-centered cubic crystal lattice. What is the radius of a gold atom in pm? 2)The cubic unit cell parameter (a) of polonium (α-Po) is 335 pm. Use the Goldschmidt correction (Table 1) to calculate a metallic radius for this element.arrow_forward
- Lead, Pb, is used in solders as radiation shield. It adopts the face centered cubic unit structure with each of the atom having a diameter of 0.35 nanometer. Find the theoretical density of lead in g/cm^3 if the molecular weight of this metal is 207.2 g/mol.arrow_forwardThe ionic compound, CsI, forms a body centered cubic structure (see below) where the anions occupy the corners of the crystal (red) and the cations the body centered position (green). If the density of the compound is 4.51 g/cm^3 and the ionic radius of Cs + is 169 pm, what is the ionic radius of I − in pm? Key Concept: The atoms are touching the diagonal in the center of the cube. This makes it equal to the sum of 2 times the radius of each atom. Strategy: Determine the length of the diagonal,d, and recall that the length of the side, l, is given by l = d/3 0.5. This is a result of the use of the Pythagorean theorem relating the length of the side to d.With the length of the side you can determine the volume of the unit cell.From the number of atoms in the unit cell determine the mass of the unit cell.Use these to get the density.arrow_forwardA hypotheticàl element, Ny, forms a face-centered cubic lattice with an atomic radius of 156 pm. Calculate the density of the element in g/cm. Atomic Mass: Ny: 114.771 g/mol Round your answer to 2 decimal places.arrow_forward
- A hypothetical element, Ny, forms a face-centered cubic lattice with an atomic radius of 165 pm. Calculate the density of the element in g/cm3. Atomic Mass: Ny: 112.024 g/mol Round to 2 decimal places.arrow_forwardadwa Some hypothetical metal has a simple cubic crystal structure. If its atomic weight is 61.25 g/mol and the atomic radius in atomic radius is 0.174 nm, calculate its theoretical density in g/cm3. NA = 6.022 x 1023 atoms/mo.arrow_forwardA (made-up) metal has a face-centered cubic crystal structure. Its density is 20.5 g/cm 3. Its molar mass is 189 g/mol. What is the radius of an atom of the metal? O 9.39 x 10 7 cm 1.39 x 10 8 cm 8.02 x 10 7 cm 2.60 x 10 -9 cm 1.84 cm x 108 2.69 x 10 8 cm 2.49 x 10 9 cm 1.51 x 10 8 cm O O Oarrow_forward
- A hypothetical element, Ny, forms a face-centered cubic lattice with an atomic radius of 152 pm. Calculate the density of the element in g/cm3.Atomic Mass: Ny: 116.729 g/mol Round your answer to 2 decimal places.arrow_forward11- An unidentified metal crystallizes in a body-centered cubic lattice with an edge length of 351 pm. The density of the metal is found to be 0.533 g/cm³. What is the atomic weight? * Pm = 10-12 marrow_forwardAn element crystallizes in a face-centered cubic lattice and has a density of 1.27 g/cm3. The edge of its unit cell is 4.79×10-8 cm. What are the volume and mass of the unit cell respectively? (Give units). Volume = Mass = Calculate the approximate atomic mass for the element. (Give units as amu).arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
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