(20pts) Q3. Please estimate the length of the cubic unit cell edge and atomic packing factor of CsCl from the ionic radii of Cesium, 0.181 nm, and Chloride, 0.167 nm. (Cs = 123.9 g/mole, Cl = 35.45 g/mole)
Added by Tony C.
Close
Step 1
The CsCl crystal structure is a simple cubic lattice, and the edge length (a) can be calculated using the ionic radii of Cs and Cl. Show more…
Show all steps
Your feedback will help us improve your experience
Sri K and 76 other Physics 101 Mechanics educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Barium has a body-centered cubic structure. If the atomic radius of barium is 222 pm; calculate the edge length and volume of the unit cell
Sri K.
A substance crystallizes into a face centered cubic unit cell like that shown below: If the atomic radius is 140 pm. What is edge length of the unit cell (L)? 560 pm 197 pm 396 pm 280 pm
Madhur L.
Problem 2 (24 pts): The theoretical density p of a ceramic can be calculated by (unit cell mass)/(unit cell volume). Use the following questions to calculate the theoretical density of cesium chloride (CsCl), given the ionic radius Rc=0.169 nm and Re=0.181 nm, and atomic weight Acs (Note: Avogadro's number 6.02 x 10^23 atoms/mole) Cs- 132.9 g/mole and Cl- 35.45 g/mole. a) How many formula units of CsCl are there within each unit cell? (4 pts) b) What is the relationship between unit cell size a and ionic radii (Re and Rei) in this case? (5 pts) c) Calculate the mass of each unit cell (in g). (5 pts) d) Calculate the volume of the unit cell (in cm^3). (5 pts) e) Calculate the theoretical density of this ceramic in g/cm^3 (which is the unit cell mass divided by the unit cell volume). (5 pts)
Hitendra S.
Recommended Textbooks
University Physics with Modern Physics
Physics: Principles with Applications
Fundamentals of Physics
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD