Potassium crystallizes with a body-centered cubic unit cell. The radius of a potassium atom is 227 pm. Part A Calculate the density of solid crystalline potassium in g/cm3.
Added by Tasha T.
Step 1
In a body-centered cubic unit cell, the atoms at the corners and the center of the cell touch each other along the body diagonal. The body diagonal is equal to 4 times the radius of the atom. So, we can write: 4r = ā3a where r is the radius of the atom and a is Show moreā¦
Show all steps
Your feedback will help us improve your experience
Sri K and 88 other Chemistry 101 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
Potassium (atomic mass 39.10 g/mol) crystallizes in a body-centered cubic lattice, and the length of the edge of a unit cell is 532.8 pm. What is the density of K? ______ g/cm^3
Madhur L.
The element potassium has a molar mass of 39.098 grams/mole and crystallizes in a BCC unit cell with a density of 0.856 g/cm3. Calculate the radius in pm of a K atom.
Adi S.
Argon crystallizes in the face-centered cubic arrangement at $40 \mathrm{K}$. Given that the atomic radius of argon is $191 \mathrm{pm},$ calculate the density of solid argon.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD