1 / 7

Understanding States of Matter: Gases, Liquids, and Solids

Explore the properties and behaviors of gases, liquids, and solids in this comprehensive guide. Learn about kinetic molecular theory, gas pressure, intermolecular forces, and more. See how diffusion, effusion, and surface tension play roles in different states of matter.

malachi-lindsey
Download Presentation

Understanding States of Matter: Gases, Liquids, and Solids

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/ Gases Pg. 91 Foldable

  2. Gases • Kinetic molecular theory: • Small particles separated by empty space • In constant random motion until they collide elastically (no energy lost) • Can calculate the energy using mass and velocity (KE =1/2mv2) • Behavior of gases • Low density • Can compress and expand • Diffusion and effusion

  3. Diffusion and Effusion • Diffusion- describes movement of one particle through another • Flows from areas of high concentration to low • Rate depends on mass (lighter diffuse more rapidly) • Effusion- when gases escape through tiny openings

  4. Gas pressure • Pressure- force per unit area • Torr = mm Hg • Atmosphere (atm)= 760 Torr = 101.3 kPa • SI- Pascal (Pa) • psi • Use a barometer to measure (height is usually about 760 Torr)

  5. Forces of attraction (intermolecular forces) • Dispersion forces • Weak forces • Occur when molecules that have similar charge are forced together • Dipole-Dipole • Slightly stronger • Occur when there is an unequal balance btw. charges of molecules • Hydrogen bonds • Incredibly strong

  6. Liquids • More dense but less compressibility than gases • Fluidity • Can diffuse • Capillary action • Surface forms a concave miniscus • 2 forces at work cohesion (btw. Same molecules) and adhesion (btw. Molecules that are different • Can be viscous (resistance to flow) • Viscosity decreases with temperature • Surface tension • Measure of the inward pull of particles • Stronger the attraction  greater surface tension • Water has high surface tension • Compounds that lower surface tension are called surfactants

  7. Solids • Closely packed particles • Low KE • Very dense • Crystalline solids- solids arragned in orderly geometric way • Crystal lattice- ions arranged in a orderly fashion. Smallest unit that can be repeated- unit cell • Molecular solids- most liquid at room temp • Covalent network solids- form allotropes (same elements, different covalent bonds) • Metallic solids- wide range of properties • Amorphous solids- particles not arranged in pattern (glass, rubber, plastics)

More Related