Titanium metal has a body-centered cubic unit cell. The density of Titanium is 4.50 g/cm^3. Calculate the edge length of the unit cell and a value for the atomic radius of titanium. Ok, I know how to find the density using the atomic …
using data in table 6.5, calculate the densities of (spherical) atoms of potassium and calcium and compare to the listed densitites of these metals K=39.10 amu, .231 nm (atomic radius) Ca= 40.08 amu, .197nm (atomic radius)
KCl crystallizes in a structure like NaCl. The ionic radius of Na+ is 0.525 times the ionic radius of Cl^- and 0.714 times the ionic radius of K+. What is the ratio of the density of NaCl to that of KCl?
Predict the answer to each question according to trends in the periodic table. Justify each answer based on the locations of the elements on the periodic table and/or the shell model. a. Which has a greater atomic radius, Al or Cl?
Difference between K, K+, and K−. The question asks to put them in order from smallest to largest in radius but I don't understand the difference from them in terms of radius since they are the same element