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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
Molecular Polarity
Intermolecular Forces
Intermolecular Forces and Physical Properties
Clausius-Clapeyron Equation
Phase Diagrams
Heating and Cooling Curves
Atomic, Ionic, and Molecular Solids
Crystalline Solids
Simple Cubic Unit Cell
Body Centered Cubic Unit Cell
Face Centered Cubic Unit Cell

Body Centered Cubic Unit Cell contains 2 atoms total.

Body Centered Cubic Unit Cell

Concept #1: The Body-Centered Cubic Unit Cell

Example #1: Iron adopts a body-centered cubic unit cell structure. Illustrate how the number of atoms per unit cell for the iron atom are obtained.

Tungsten possesses a body-centered cubic structure. If its density is 19.28 g/cm3, what is its radius in pm? 

a) 910 pm           b) 316 pm                   c) 137 pm                       d) 3.18 pm

Vanadium has a body-centered cubic structure. If the atomic radius of vanadium is 134 pm, calculate the density of solid vanadium. 

a) 5.33 g/cm3              b) 4.29 g/cm3             c) 5.71 g/cm3            d) 0.52 g/cm3

The edge of a body-centered cubic unit cell of an element Z was found to be 2.88 x 10-8 cm. The density of the element is 7.2 g/cm3. What is the approximate molar mass of Z?