General Properties of Solids

Solid, liquid, gas

Ice is less dense than water because of the hydrogen bonding in water molecules, which creates an open structure in ice, causing it to expand and have a lower density.

True

<p>True</p> Signup and view all the answers

<p>90 degrees</p> Signup and view all the answers

<p>The thickness at the bottom is due to the slow flow of glass as a supercooled liquid, while the milkiness is a result of annealing, which introduces some crystalline character to the glass over time.</p> Signup and view all the answers

<p>A homogeneous part of a solid substance formed by a regular pattern of structural units bonded by planar surfaces making definite angles with each other.</p> Signup and view all the answers

<p>A regular arrangement of constituent particles (atoms, ions, molecules, etc.) in three-dimensional space that represents the repeating unit of a crystal.</p> Signup and view all the answers

<p>A plane surface of the crystal.</p> Signup and view all the answers

<p>The line where two adjacent faces of the crystal intersect.</p> Signup and view all the answers

<p>The angle between the perpendiculars of two intersecting faces of a crystal.</p> Signup and view all the answers

<p>True</p> Signup and view all the answers

<p>Cube</p> Signup and view all the answers

<p>The presence of delocalized electrons.</p> Signup and view all the answers

<p>A solid angle is formed when three or more edges intersect at a point.</p> Signup and view all the answers

<p>Bragg's Law describes the diffraction of X-rays by crystals based on the relationship between the wavelength of X-rays, the distance between crystal planes, and the angle of reflection.</p> Signup and view all the answers

<p>True</p> Signup and view all the answers

<p>Determining the structure and dimensions of ionic crystalline solids, explaining various properties of X-rays, and constructing X-ray spectrometers to analyze crystal structures.</p> Signup and view all the answers

<p>The smallest repeating three-dimensional portion of a crystal lattice that, when repeated in all directions, generates the entire crystal structure.</p> Signup and view all the answers

<p>The edge lengths (a, b, c) and the angles (α, β, γ) between these edges.</p> Signup and view all the answers

<p>True</p> Signup and view all the answers

<p>The four types are simple, face-centered, body-centered, and end-centered unit cells. They differ in the location of lattice points within the cell, with simple having points only at corners, face-centered having points at corners and face centers, body-centered having points at corners and the body center, and end-centered having points at corners and the centers of two opposite faces.</p> Signup and view all the answers

<p>Center of symmetry, axis of symmetry, and plane of symmetry.</p> Signup and view all the answers

<p>Trigonal bipyramidal</p> Signup and view all the answers

<p>True</p> Signup and view all the answers

<p>The seven crystal systems are cubic (a = b = c, α = β = γ = 90°), tetragonal (a = b ≠ c, α = β = γ = 90°), orthorhombic (a ≠ b ≠ c, α = β = γ = 90°), monoclinic (a ≠ b ≠ c, α = β = 90° γ ≠ 90°), triclinic (a ≠ b ≠ c, α ≠ β ≠ γ ≠ 90°), hexagonal (a = b ≠ c, α = β = 90°, γ = 120°), and rhombohedral (a = b = c, α = β = γ ≠ 90°). They differ in their unit cell dimensions, specifically the edge lengths and angles between those edges.</p> Signup and view all the answers

<p>It determines the coordination number of a cation in an ionic crystal, which in turn influences the crystal structure and stability.</p> Signup and view all the answers

<p>Some primary examples include LiX (LiF, LiCl, LiBr, LiI), NaX (NaF, NaCl, NaBr, NaI), KX (KF, KCl, KBr, KI), AgCl, AgBr, and NH4Cl.</p> Signup and view all the answers

<p>The CsCl type structure is a simple cubic arrangement where Cs+ cations occupy the central positions within the unit cell while Cl- anions are arranged at the corners of the unit cell. The coordination number for both Cs+ and Cl- is 8. Some examples of compounds that exhibit this structure include CsX (CsF, CsCl, CsBr, CsI), TiCl, TiBr, NH4Cl, and NH4Br.</p> Signup and view all the answers

<p>In the zinc blend structure, anions (typically S2-) form a face-centered cubic (FCC) lattice, while cations (often Zn2+) reside in alternate tetrahedral voids. The coordination number for both Zn2+ and S2- in this structure is 4. Notable examples of compounds exhibiting this structure include ZnS, CuCl, CuBr, CuI, Agl, and BeO. One prominent characteristic of this structure is its semiconducting nature.</p> Signup and view all the answers

<p>Both structures are based on a face-centered cubic (FCC) lattice, but the roles of cations and anions are reversed. In the fluorite structure, cations occupy FCC positions while anions occupy all tetrahedral voids. Conversely, in the antifluorite structure, anions occupy FCC positions while cations occupy all tetrahedral voids.</p> Signup and view all the answers

<p>AB2O4.</p> Signup and view all the answers