ChemistryAluminum has an atomic mass of 26.97 g/moland a density of 2699 kg/m3.calculatea) mass of an atomb) number of atoms in 1 mgc) volume and edge of the unit celld) number of atoms and moles per m3e) mass of a unit cellf) number of cells in a 1g of metalg) atomic radiush) packing factori) linear atomic density in the 110 and 111directionsj) surface atomic density in planes (1 1 0) and (111)

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Chemistry Aluminum has an atomic mass of 26.97 g/mol and a density of 2699 kg/m3. calculate a) mass of an atom b) number of atoms in 1 mg c) volume and edge of the unit cell

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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

Chemistry
Aluminum has an atomic mass of 26.97 g/mol
and a density of 2699 kg/m3.
calculate
a) mass of an atom
b) number of atoms in 1 mg
c) volume and edge of the unit cell
d) number of atoms and moles per m3
e) mass of a unit cell
f) number of cells in a 1g of metal
g) atomic radius
h) packing factor
i) linear atomic density in the 110 and 111
directions
j) surface atomic density in planes (1 1 0) and (11
1)

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