Exploring the impact of crystal structures on the physical properties of matter, this overview delves into how different types of bonding and atomic arrangements affect characteristics like melting point, hardness, and electrical conductivity. It highlights the unique properties of molecular, network covalent, metallic, and ionic crystals, as well as the anomalous behaviors of water due to hydrogen bonding.
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Physical properties are characteristics of matter that can be observed or measured without changing its chemical composition
Physical properties are different from chemical properties, which describe a substance's potential to undergo chemical changes
Examples of physical properties include state of matter, melting and boiling points, density, color, and solubility
Crystal structures can be simple molecular, network covalent, ionic, or metallic, each with unique physical properties
Molecular crystals have weaker intermolecular forces and tend to have lower melting and boiling points, as well as being soft or brittle
Network covalent crystals have a continuous network of covalent bonds, resulting in high hardness and melting points
Metallic crystals have a lattice of metal cations surrounded by delocalized electrons, leading to high conductivity, malleability, and ductility
Ionic crystals have a regular arrangement of alternating positive and negative ions held together by ionic bonds, resulting in high hardness and brittleness
Water exhibits unique physical properties due to its hydrogen bonding, including expansion upon freezing and high melting and boiling points
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Examples of Physical Properties
State of matter, melting/boiling points, density, color, solubility.
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Physical vs Chemical Change
Physical change: matter's form alters, not composition (e.g., water to ice). Chemical change: substance's composition changes (e.g., rusting iron).
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Significance of Melting/Boiling Points
Indicate temperatures at which a substance transitions between solid/liquid/gas states; characteristic for pure substances.
