Properties of solid, liquid, & solutions

• Mixture


  A combination of two or more substances that do not combine chemically, but remain the same individual substances; can be separated by physical means
• Types of mixtures

  • Heterogeneous
  • Homogeneous
• Homogeneous mixtures


  • Have a uniform composition throughout the mixture
  • Components are not visible to the naked eye
  • The whole mixture is in the same phase
  • Particle size is often at atomic or molecular level
  • Components cannot be separated easily
• Heterogeneous mixtures


  • Have a mixed composition which may vary from point to point
  • Components can be seen easily
  • Substances can be of two phases and layers may separate
  • Heterogeneous mixtures have large particle sizes
  • Components can be separated easily
• “Hetero” means “different”. Can be separated by filtering
• Examples of Heterogeneous Mixtures

  • Pizza
  • Chocolate chip cookies
  • Sandwich
  • Soda with ice
  • Tossed Salad
• Homogeneous mixtures


  • Have the same uniform appearance and composition throughout; maintain one phase (solid, liquid, gas)
  • Commonly referred to as solutions
• “Homo” means the same. Saltwater is considered a solution
• Solution


  A mixture of two or more substances that is identical throughout (homogeneous) and can be physically separated; composed of solutes and solvents
• Solvent


  The largest part of the solution
• Solute


  The smallest part of the solution
• Soluble (opposite Insoluble) - a substance that dissolves in another substance (general) - solution with water, H2O as a solvent. Aqueous solutions
• Miscible liquids can easily dissolve in one another. Immiscible liquids are not soluble in each other. Miscible vs. Immiscible
• Dissolves


  When a substance dissolves in another substance
• Solution with water

  H2O as a solvent
• Miscible liquids


  Liquids that can easily dissolve in one another
• Immiscible liquids


  Liquids that are not soluble in each other
• Miscible substances


  Substances that fully mix in all proportions
• Immiscible substances


  Substances that never fully mix in any proportions
• Types of solutions

  • Gaseous solutions - air = Oxygen + Nitrogen
  • Liquid solutions - drinks = mix + water
  • Solid solutions - alloys = steel, brass, etc
• Dilute solution


  A solution with a low concentration of solute dissolved
• Concentrated solution


  A solution with a high concentration of solute dissolved
• Concentration


  The amount of solute dissolved in a solvent at a given temperature
• Ways of expressing concentrations of solutions

  • Part per million (PPM)
• Solutions can also be represented as a percentage of solute in a specific mass of solution
• Solid


  Formed when the temperature of a liquid is low and the pressure is sufficiently high causing the particles to come very close to each other. Solids are rigid because their molecules have fixed positions
• Types of Solids

  • Regular arrangement of particles
  • Irregular arrangement of particles
  • Long order in arrangement of particles
  • Short order in arrangement of particles
• True Solids


  • They are called True Solids
  • Long order in arrangement of particles
  • Short order in arrangement of particles
• Pseudo Solids / Super Cooled Liquids


  • No arrangement
  • No long order
  • Inability to flow over time if temperature changes
• Perfect Solids

  • Regular arrangement
  • Long order
• Fake Properties


  • No arrangement
  • No long order
  • Ability to flow over time if temperature changes
• Imperfect Solids


  • No arrangement
  • No long order
• Melting Point

  1. Sharp Melting Point

  2. Ranged Melting Point
• Types of Crystalline Solids

  • NaCl
  • CaCO3
  • MgO
• Crystalline Solids


  • Ordered in well-defined arrangements, have flat surfaces or faces, and sharp angles. They have regular shapes
• Conductors in Molten States

  • Iron
  • Gold
  • Silver
• Metals


  • Iron
  • Gold
  • Silver
• Non-Metal

  • Carbon atoms
  • Atoms
• Molecular Solids


  • CO2
  • H2O
• Types of Solids

  • Crystalline Solids
  • Ionic Solids
  • Metallic Solids
  • Covalent Solids
  • Molecular Solids