KCl has the same crystal structure as NaCl (fcc). a) Calculate the volume of the unit cell for KCl, given that the ionic radii are K+ = 152 pm and Cl- = 167 pm. b) Compute the density of KCl. Show your work. Note: pc: 1 atom/unit cell bcc: 2 atoms/unit cell fcc: 4 atoms/unit cell 1 pm = 1 x 10-10 cm Primitive Cubic (pc): 2 x (atomic radius) = edge Face-Centered Cubic: 4 x (atomic radius) = edge x √2 = face diagonal Body-Centered Cubic: 4 x (atomic radius) = edge x √3 = body diagonal Mass of 1 formula unit (ex. NaCl) x # of formula units per unit cell (ex. 4) = mass of unit cell
KCl has the same crystal structure as NaCl (fcc). a) Calculate the volume of the unit cell for KCl, given that the ionic radii are K+ = 152 pm and Cl- = 167 pm. b) Compute the density of KCl. Show your work. Note: pc: 1 atom/unit cell bcc: 2 atoms/unit cell fcc: 4 atoms/unit cell 1 pm = 1 x 10-10 cm Primitive Cubic (pc): 2 x (atomic radius) = edge Face-Centered Cubic: 4 x (atomic radius) = edge x √2 = face diagonal Body-Centered Cubic: 4 x (atomic radius) = edge x √3 = body diagonal Mass of 1 formula unit (ex. NaCl) x # of formula units per unit cell (ex. 4) = mass of unit cell
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter12: The Solid State
Section12.1: Crystal Lattices And Unit Cells
Problem 12.1CYU: (a) Determining an Atom Radius from Lattice Dimensions: Gold has a face-centered unit cell, and its...
Related questions
Question
KCl has the same crystal structure as NaCl (fcc).
a) Calculate the volume of the unit cell for KCl, given that the ionic radii are K+ = 152 pm and Cl- = 167 pm.
b) Compute the density of KCl. Show your work.
Note:
- pc: 1 atom/unit cell
- bcc: 2 atoms/unit cell
- fcc: 4 atoms/unit cell
1 pm = 1 x 10-10 cm
- Primitive Cubic (pc): 2 x (atomic radius) = edge
- Face-Centered Cubic: 4 x (atomic radius) = edge x √2 = face diagonal
- Body-Centered Cubic: 4 x (atomic radius) = edge x √3 = body diagonal
Mass of 1 formula unit (ex. NaCl) x # of formula units per unit cell (ex. 4) = mass of unit cell
Mass of unit cell ÷ unit cell volume ( ex. = edge3 for NaCl) = density
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
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.Recommended textbooks for you
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
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
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
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
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning