Aluminum with a density of 3.37 g/cm³ crystallizes as a face centered The volume V of it's unit cell is: V= 1cm³ 3.37 26.98 I mole Imole 6.022x1023 atoms 4 atoms Unit cell What is the edge length of cell ? Cubic Crystal. .cm (9³ = volume) What is the atomic radius Ст (r = √za) 4 For example, chromium with a density of 7.19 g/cm³ crystallizes as a body centered cubic The volume V of its unit cell is: V = = 1 cm³. 52.0 g. 7.19 g 1 mole 1 mole 6.022x1023 atoms . 2 atoms unit cell = 2.40x10-23 cm³ The edge of the unit cell (a) is the cube root of the volume [V1/3] a= V1/3 = (2.40x10-23 cm³) 1/3 = (24.0x10-24 cm³) 1/3 = 2.89x10-8 cm atomic radius = r = ax 3 1/2/4 ax 31/2/4 = (2.89x10-8 cm)(0.433) = 1.25x10-8 cm crystal tu SU b I
Aluminum with a density of 3.37 g/cm³ crystallizes as a face centered The volume V of it's unit cell is: V= 1cm³ 3.37 26.98 I mole Imole 6.022x1023 atoms 4 atoms Unit cell What is the edge length of cell ? Cubic Crystal. .cm (9³ = volume) What is the atomic radius Ст (r = √za) 4 For example, chromium with a density of 7.19 g/cm³ crystallizes as a body centered cubic The volume V of its unit cell is: V = = 1 cm³. 52.0 g. 7.19 g 1 mole 1 mole 6.022x1023 atoms . 2 atoms unit cell = 2.40x10-23 cm³ The edge of the unit cell (a) is the cube root of the volume [V1/3] a= V1/3 = (2.40x10-23 cm³) 1/3 = (24.0x10-24 cm³) 1/3 = 2.89x10-8 cm atomic radius = r = ax 3 1/2/4 ax 31/2/4 = (2.89x10-8 cm)(0.433) = 1.25x10-8 cm crystal tu SU b I
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter11: Liquids And Solids
Section: Chapter Questions
Problem 11.74QE
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I need help working this problem out step by step, I was trying to use my example from the txt book but all I know how to do is set it up. I need to be shown step by step as I am a visual learner. Please help me.
![Aluminum with a density of 3.37 g/cm³ crystallizes as a face centered
The volume V of it's unit cell is:
V=
1cm³
3.37
26.98
I mole
Imole
6.022x1023
atoms
4 atoms
Unit cell
What is the edge length of cell
?
Cubic
Crystal.
.cm (9³ = volume)
What is the atomic radius
Ст
(r = √za)
4
For example, chromium with a density of 7.19 g/cm³ crystallizes as a body centered cubic
The volume V of its unit cell is:
V =
=
1 cm³. 52.0 g.
7.19 g 1 mole
1 mole
6.022x1023 atoms
.
2 atoms
unit cell
=
2.40x10-23 cm³
The edge of the unit cell (a) is the cube root of the volume [V1/3]
a= V1/3
=
(2.40x10-23 cm³) 1/3 = (24.0x10-24 cm³) 1/3 = 2.89x10-8 cm
atomic radius = r = ax 3 1/2/4
ax 31/2/4 = (2.89x10-8 cm)(0.433)
=
1.25x10-8 cm
crystal
tu
SU
b
I](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F98788fff-5d55-4f08-bd33-832b3c76eea7%2F511fff90-e762-462e-a68d-c29a4b4782c5%2Ftl9qabv_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Aluminum with a density of 3.37 g/cm³ crystallizes as a face centered
The volume V of it's unit cell is:
V=
1cm³
3.37
26.98
I mole
Imole
6.022x1023
atoms
4 atoms
Unit cell
What is the edge length of cell
?
Cubic
Crystal.
.cm (9³ = volume)
What is the atomic radius
Ст
(r = √za)
4
For example, chromium with a density of 7.19 g/cm³ crystallizes as a body centered cubic
The volume V of its unit cell is:
V =
=
1 cm³. 52.0 g.
7.19 g 1 mole
1 mole
6.022x1023 atoms
.
2 atoms
unit cell
=
2.40x10-23 cm³
The edge of the unit cell (a) is the cube root of the volume [V1/3]
a= V1/3
=
(2.40x10-23 cm³) 1/3 = (24.0x10-24 cm³) 1/3 = 2.89x10-8 cm
atomic radius = r = ax 3 1/2/4
ax 31/2/4 = (2.89x10-8 cm)(0.433)
=
1.25x10-8 cm
crystal
tu
SU
b
I
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