Palladium has an atomic weight of 106.42 g/mol and a density of 23.78 g/cm3. Calculateits atomic diameter (in pm) if it forms a face-centered cubic crystalline structure.Express your answer in two decimal places. P:nAVCNAWhere: p density (g/cm³)n = no. of atoms/ unit cellA = atomic weight (g/mol)Importantconversion factors1 cm = 107 nm1 cm = 10¹⁰ pm1 cm = 10⁰ Å1 nm = 10 ÅVc = volume / unit cell (cm³/unit cell) = a³NA = Avogadro's number = 6.022x10²3 atoms/mol

we have to calculate the diameter of unit cell

Palladium has an atomic weight of 106.42 g/mol and a density of 23.78 g/cm3. Calculate its atomic diameter (in pm) if it forms a face-centered cubic crystalline structure. Express your answer in two decimal places.

Palladium has an atomic weight of 106.42 g/mol and a density of 23.78 g/cm3. Calculate its atomic diameter (in pm) if it forms a face-centered cubic crystalline structure. Express your answer in two decimal places.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter8: Molecules And Materials

Section: Chapter Questions

Problem 8.98PAE: 8.98 If you know the density of material and the length of the edge of its cubic Iattice, how would...

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Concept explainers

Crystal Lattices and Unit Cell

Consider a crystal. The regular and repeating pattern of constituent particles is the most distinguishing feature of crystalline solids. A crystal lattice is formed when these particles are replaced with representative points. The three-dimensional arrangement of constituent particles is known as a crystal lattice. Unit cell is that the smallest portion of a space lattice which when repeated in several directions, generate the whole lattice. Unit cell is a building block of a lattice. It is the smallest unit of cell.

Question

Palladium has an atomic weight of 106.42 g/mol and a density of 23.78 g/cm3. Calculate
its atomic diameter (in pm) if it forms a face-centered cubic crystalline structure.
Express your answer in two decimal places.

P:
nA
VCNA
Where: p density (g/cm³)
n = no. of atoms/ unit cell
A = atomic weight (g/mol)
Important
conversion factors
1 cm = 107 nm
1 cm = 10¹⁰ pm
1 cm = 10⁰ Å
1 nm = 10 Å
Vc = volume / unit cell (cm³/unit cell) = a³
NA = Avogadro's number = 6.022x10²3 atoms/mol

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