1 / 21

States of Matter

States of Matter. A Matter of Kinetic Energy. Types of States of Matter. Solid Liquid Gas Plasma Beam BEC, or Bose-Einstein Condensate Zero State of Matter Most Dense. Changes of State. Kinetic Energy ( kelvins & paschals ).

luther
Download Presentation

States of Matter

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. States of Matter A Matter of Kinetic Energy

  2. Types of States of Matter • Solid • Liquid • Gas • Plasma • Beam • BEC, or Bose-Einstein Condensate • Zero State of Matter • Most Dense

  3. Changes of State

  4. Kinetic Energy (kelvins & paschals)

  5. chemwiki.ucdavis.edu/Physical_Chemistry/Physical_Properties_of_Matter/Supercritical_Fluidschemwiki.ucdavis.edu/Physical_Chemistry/Physical_Properties_of_Matter/Supercritical_Fluids • Supercritical fluids are useful in science today • extraction of floral fragrance • the process of creating decaffeinated coffee • food science and functional food ingredients • pharmaceuticals, cosmetics, polymers, powders, bio- and functional materials • nano-systems, natural products, biotechnology, fossil & biofuels, microelectronics & environment (Bottini 133).

  6. www.engineeringtoolbox.com/vapor-steam-d_609 • Superheated Vapor • When the temperature is higher than the boiling point @ a given pressure. • Vapor cannot exist in contact with the fluid, nor contain fluid particles. • Increase in pressure or decrease in temperature will not, within limits, condensate out liquid particles in the vapor. • Highly superheated vapors are gases that approximately follow the general gas law.

  7. Critical Temp & Pressure • Critical Temperature • The temperature at which only gas exists, regardless of its pressure • Critical Pressure • The lowest pressure at which liquids exist at critical temperature • Critical Point • The intersection of critical temperature & pressure

  8. Kinetic-Molecular Theory of Gases • Ideal gas = hypothetical gas perfectly aligns with all kinetic-molecular theory assumptions • Five Assumptions • Distance between molecules dwarfs actual size • All collisions are perfectly elastic • Particles are in continuous, rapid, random motion • Particles have NO attraction to each other • Temperature = average kinetic energy of particles

  9. Nature of Gases • Ideal vs. Real • Real approaches ideal @ low pressure/ high temp • Expansion – molecules fill entire space • Fluidity – no intermolecular attractions • Density - ~ 10-3 of liquid or solid state • Compressibility – 100X more molecules • Diffusion & Effusion • Spontaneous mixing via random motion • Passing through tiny opening

  10. C/C Intermolecular Forces

  11. Properties of Liquids • LEAST common state of matter in universe • Fluids (as are gases) • Lower kinetic energy than gases • Interactive forces keep molecules connected • Dipole-dipole forces • Equal but opposite charges separated by short distance • London dispersion forces • Spontaneous creation of dipoles (polar & nonpolar) • Hydrogen bonding (electronegativity)

  12. Hydrogen Bonding

  13. Properties of Liquids, continued • Density: 100x > gases; 10% < solids • Compressibility: @ 103 atm., volume ~ 4% • Diffusion: present, but slower than in gases • Surface tension: high intermolecular attraction • Capillary action: attraction between surfaces of liquid and a solid • Vaporization: evaporation & boiling  gas

  14. Nature of Solids • Interparticle attractions stronger than others • Two types of solids • Crystalline (orderly arrangement) • Amorphous (random arrangement) • supercooled liquids: have liquid properties even if look solid • Shape & Volume: Definite • Melting Point: Definite • Density & Incompressibility: High • Diffusion: Low rate (10-6 less than others)

  15. Dipole-dipole Forces

  16. Covalent Molecular Structures Glucose – C6H12O6 Buckminsterfullerene

  17. Crystalline Solids • Ionic • Alkali & alkaline earth with halogens & Group 16 • Hard, brittle, high melting points, good insulators • Covalent network • Cx (diamonds), (SiO2)x quartz, (SiC)x • Very hard and brittle, high MP, semi- or nonconductors • Covalent molecular (nonpolar & polar) • H2, CH4, C6H6: only weak London dispersion forces • H2O & NH3,: stronger forces but weaker than covalent • Soft, low MP, low BP, good insulators

  18. Crystalline Structures Ionic Structure AgCl

  19. Covalent Network Crystals Diamond Quartz

  20. Covalent Network Carbon Graphite

  21. Covalent Molecular

More Related