Question

A metal crystallizes in the face-centered cubic crystal structure with a unit cell edge of 3.89 x 10^-8 cm. The density of the metal is 12.0 g/cc. (a) What is the mass, in grams, of a single atom of this element? (b) What is the atomic weight of the element (g/mol). (c) What is the radius, in cm, of an atom of the element?

Name: A metal crystallizes in the face-centered cubic crystal structure with a unit cell edge of 3.89 x 10^-8 cm. The density of the metal is 12.0 g/cc. (a) What is the mass, in grams, of a single atom of this element? (b) What is the atomic weight of the element (g/mol). (c) What is the radius, in cm, of an atom of the element?
Uploaded: 2022-01-22T22:30:30-08:00
Duration: 6 min 17 s
Channel: Ivan Kochetkov
Description: A metal crystallizes in the face-centered cubic crystal structure with a unit cell edge of 3.89 x 10^-8 cm. The density of the metal is 12.0 g/cc. (a) What is the mass, in grams, of a single atom of this element? (b) What is the atomic weight of the element (g/mol). (c) What is the radius, in cm, of an atom of the element?

          A metal crystallizes in the face-centered cubic crystal structure with a unit cell edge of 3.89 x 10^-8 cm. The density of the metal is 12.0 g/cc. (a) What is the mass, in grams, of a single atom of this element? (b) What is the atomic weight of the element (g/mol). (c) What is the radius, in cm, of an atom of the element?

A metal crystallizes in the face-centered cubic crystal structure with a unit cell edge of 3.89 x 10^-8 cm. The density of the metal is 12.0 g/cc. (a) What is the mass, in grams, of a single atom of this element? (b) What is the atomic weight of the element (g/mol). (c) What is the radius, in cm, of an atom of the element?

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Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ivan Kochetkov

01/22/2022

Step 1

Given: Density of the metal (ρ) = 12.0 g/cm^3 Unit cell edge (a) = 3.89 x 10^(-8) cm The volume of the unit cell (V) = a^3 = (3.89 x 10^(-8) cm)^3 The mass of a single atom (m) can be calculated using the formula: ρ = m/V m = ρ x V Substitute the values: m = Show more…

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A metal crystallizes in the face-centered cubic crystal structure with a unit cell edge of 3.89 x 10^-8 cm. The density of the metal is 12.0 g/cc. (a) What is the mass, in grams, of a single atom of this element? (b) What is the atomic weight of the element (g/mol). (c) What is the radius, in cm, of an atom of the element?