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Crystalline Solid
Solid with a regular atomic arrangement.
Unit Cell
Simplest repeating unit in a crystalline structure.
Coordination Number
Number of nearest neighbors around an atom.
Simple Cubic Structure
Atoms arranged in layers directly above each other.
Body-Centered Cubic
Unit cell with an atom at the center.
Face-Centered Cubic
Unit cell with atoms at each face center.
Atomic Radius
Half the distance between two adjacent atoms.
Density Calculation
Mass of unit cell divided by volume.
X-ray Diffraction
Technique to determine crystalline structures.
Lattice Points
Positions representing atoms in a unit cell.
Polonium
Only metal crystallizing in simple cubic structure.
Edge Length
Distance between corners of a unit cell.
Volume of Unit Cell
Calculated as edge length cubed.
Intermolecular Energy
Total energy due to interactions between particles.
Metallic Properties
Malleability and ductility due to atomic arrangement.
Cubic Lattice Types
Includes simple, body-centered, and face-centered.
Mass of Unit Cell
Total mass of atoms within the unit cell.
Crystalline Structure
Regular arrangement of atoms in solids.
Packing Efficiency
Percentage of volume occupied by atoms.
Atomic Diameter
Twice the atomic radius.
Nickel Density
Actual density of nickel is 8.90 g/cm³.
Polonium Density Calculation
Density derived from unit cell mass and volume.
Lattice Structure
Arrangement of atoms in a crystalline solid.
Crystalline Arrangement
Maximizes attractive interactions between particles.
Metal Crystal Geometries
Common types include simple, body-centered, face-centered.
Eight Corners
Each corner atom contributes one-eighth to unit cell.
Layer Arrangement
Spheres in layers directly above or below.
Volume Units
Converted from pm to cm for density.
Density of Polonium
Calculated using unit cell dimensions and mass.
Crystalline Solids
Over 90% of naturally occurring solids.
Body-Centered Cubic (BCC)
Cubic unit cell with atoms at corners and center.
BCC Atom Count
Contains two atoms per unit cell.
BCC Packing Efficiency
Atoms occupy about 68% of total volume.
Isomorphous Metals
Metals crystallizing in the same structure.
Face-Centered Cubic (FCC)
Cubic unit cell with atoms at corners and faces.
FCC Atom Count
Contains four atoms per unit cell.
FCC Packing Efficiency
Atoms occupy about 74% of total volume.
Cubic Closest Packing (CCP)
Another name for face-centered cubic arrangement.
Coordination Number in FCC
Each atom contacts 12 nearest neighbors.
Hexagonal Closest Packing (HCP)
Consists of two alternating layers of atoms.
Layer Arrangement in HCP
Stacking follows ABABAB pattern.
Layer Arrangement in CCP
Stacking follows ABCABC pattern.
Atomic Radius Calculation (FCC)
Diagonal equals four atomic radii.
Calcium Unit Cell Edge Length
558.8 pm for face-centered cubic structure.
Silver Unit Cell Edge Length
409 pm for face-centered cubic structure.
Total Atoms in FCC Unit Cell
Includes 1 from corners and 3 from faces.
Density of Calcium
Density calculated from unit cell mass and volume.
Density of Silver
Density calculated from unit cell mass and volume.
Face Diagonal in FCC
Connects atoms at corners and face centers.
Hexagonal Layer Contact
Atoms in second layer touch three in first.
Metallic Crystallization
Most metals crystallize in closest-packed arrays.
Examples of Isomorphous Metals
K, Ba, Cr, Mo, W, Fe in BCC.
Examples of HCP Metals
Cd, Co, Li, Mg, Na, Zn.
Examples of CCP Metals
Ag, Al, Ca, Cu, Ni, Pb, Pt.
Axes of Unit Cell
Lengths a, b, and c define unit cell dimensions.
Angles of Unit Cell
Angles α, β, and γ between unit cell axes.
Lattice Systems
Seven distinct arrangements of crystal lattices.
Ionic Crystals
Crystals formed from different sized ions.
Monatomic Ions
Single charged ions behaving as spheres.
Stable Ionic Structures
Formed by surrounding opposite charge ions.
Cations
Positively charged ions in ionic compounds.
Anions
Negatively charged ions in ionic compounds.
Tetrahedral Hole
Space surrounded by four anions in tetrahedron.
Octahedral Hole
Space surrounded by six anions in octahedron.
Closest-Packed Array
Maximized packing of ions in crystal structure.
Cation:Anion Ratio
Proportion of cations to anions in compounds.
Zinc Sulfide
ZnS, zinc occupies half tetrahedral holes.
Lithium Selenide
Li3Se, lithium occupies all tetrahedral holes.
Stoichiometry
Ratio of elements in a compound.
Aluminum Oxide
Al2O3, aluminum occupies two-thirds octahedral holes.
Titanium Oxide
TiO2, titanium occupies half octahedral holes.
Simple Cubic Array
One cubic hole per anion in structure.
Cubic Holes
Spaces in cubic arrays for cation occupancy.
Ionic Compound Structure
Determined by ion sizes and stoichiometry.
HCP Structure
Hexagonal close-packed arrangement of ions.
CCP Structure
Cubic close-packed arrangement of ions.
Vacant Tetrahedral Holes
Unoccupied spaces in tetrahedral arrangements.
Octahedral Hole Ratio
1:1 ratio of octahedral holes to anions.
Cation Size Influence
Cation size determines hole type occupancy.
Ionic Compound Examples
Li2O, Na2O, Li2S, Na2S in tetrahedral holes.
Cation Occupancy
Cations occupy holes based on size.
Ionic Compound
A compound formed by cations and anions.
Cation
Positively charged ion, e.g., Cs+.
Anion
Negatively charged ion, e.g., Cl−.
Cesium Chloride (CsCl)
Example of ionic compound with simple cubic structure.
Body Diagonal
Diagonal line connecting opposite corners of a cube.
1:1 Stoichiometry
Equal ratio of cations to anions in a compound.
FCC Structure
Face-centered cubic arrangement of ions.
Sodium Chloride (NaCl)
Example of ionic compound with FCC structure.
Octahedral Holes
Spaces in FCC structure occupied by smaller cations.
Zinc Sulfide (ZnS)
Ionic compound with FCC structure and tetrahedral holes.
Tetrahedral Holes
Spaces in FCC structure occupied by smaller ions.
Calcium Fluoride (CaF2)
Ionic compound with FCC structure and 1:2 ratio.
Ionic Radii
Size of ions in an ionic compound.
Pythagorean Theorem
Mathematical relation used for calculating distances.
X-ray Crystallography
Technique to determine crystal structure using X-rays.
Diffraction
Change in direction of waves encountering barriers.
Constructive Interference
Waves combine to increase amplitude.
Interatomic Distance
Distance between atoms in a crystal.
Wavelength (λ)
Distance between successive peaks of a wave.
