Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Lithium crystallizes in a body-centered cubic unit cell. What is the mass of one unit cell in grams?

Solution: Lithium crystallizes in a body-centered cubic unit cell. What is the mass of one unit cell in grams?

Problem

Lithium crystallizes in a body-centered cubic unit cell. What is the mass of one unit cell in grams?

Solution

We’re being asked to calculate the mass of 1 unit cell when lithium (Li) crystallizes in a body-centered cubic unit cell.


A body-centered cubic (BCC) unit cell is composed of a cube with one atom at each of its corners and one atom at the center of the cube


We’re going to calculate the mass of 1 unit cell using the following steps:

Step 1: Determine how many atoms are present in 1 unit cell.
Step 2: Calculate how many moles is present in the unit cell.
Step 3: Calculate the mass using the molar mass of the atom.

View the complete written solution...