Solid State

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1. Crystalline solids: Regular, periodic arrangement of particles; sharp melting points; anisotropic properties (except cubic); examples: NaCl, diamond, metals 2. Amorphous solids: Random arrangement

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Isomorphism: Two or more substances having the same crystal structure and same atomic ratios. Examples: NaF and MgO (1:1 ratio), NaNO₃ and CaCO₃ (1:1:3 ratio) Polymorphism: A single substance existin

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Ionic: Ions held by electrostatic forces; hard, brittle; high melting points; conduct when melted (NaCl) Covalent network: Atoms in 3D covalent network; very hard; high melting points; poor conductors

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Unit cell: The smallest repeating structural unit of a crystalline solid that generates the entire crystal when repeated in three dimensions. Four types: 1. Primitive/Simple: particles only at corner

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Simple Cubic (sc): 8 corner particles × 1/8 = 1 particle per unit cell Body-Centered Cubic (bcc): 8 corner particles × 1/8 + 1 center particle = 2 particles per unit cell Face-Centered Cubic (fcc):

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ρ = (n × M)/(a³ × Nₐ) Where: ρ = density of substance n = number of particles per unit cell M = molar mass a = edge length of unit cell Nₐ = Avogadro's number This equation allows calculation of any

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Coordination number: The number of neighboring atoms/ions that directly touch a given atom/ion in a crystal structure. Simple Cubic (sc): 6 (4 in same layer + 1 above + 1 below) Body-Centered Cubic (

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Both start with hexagonal close-packed layers (ABAB... pattern in 2D): HCP: Third layer aligns with first layer → ABAB... pattern CCP: Third layer covers octahedral voids → ABCABC... pattern (same as