1 / 23

Chapter 13

Chapter 13. States of Matter Liquids and Solids Changes of State. Objectives. Liquid (13.2) How the atoms are arranged Basic properties Solids (13.3) How the atoms are arranged Basic properties Changes of State (13.4) What does equilibrium mean?

camilla-todd
Download Presentation

Chapter 13

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. Chapter 13 States of Matter Liquids and Solids Changes of State

  2. Objectives • Liquid (13.2) • How the atoms are arranged • Basic properties • Solids (13.3) • How the atoms are arranged • Basic properties • Changes of State (13.4) • What does equilibrium mean? • Le Chatelier’s Principle (We will talk more in another unit) • The six basic phase changes • Be able to describe the parts of a heating and cooling curve • Understand a phase diagram

  3. The Four States of Matter Solid Gas Liquid Plasma

  4. What determines which state of matter you are in? • Particle arrangement • Energy of the particles • Distance between particles

  5. STATES OF MATTERSOLIDS • Particles of solids are tightly packed, vibrating about a fixed position. • Solids have a definite shape and a definite volume.

  6. STATES OF MATTERLIQUID • Particles of liquids are tightly packed, but are far enough apart to slide over one another. • Liquids have an indefinite shape and a definite volume.

  7. STATES OF MATTERGAS • Particles of gases are very far apart and move freely. • Gases have an indefinite shape and an indefinite volume.

  8. Compression of Gases, Liquids and Solids • Gases are compressible fluids. Their molecules are widely separated. • Liquids are relatively incompressible fluids. Their molecules are more tightly packed. • Solids are nearly incompressible and rigid. Their molecules or ions are in close contact and do not move.

  9. Properties of Liquids • Relative High Density • Relative Incompressibility • Ability to diffuse • Surface Tension • Viscosity • Capillary Action • Vaporization (Evaporation and Boiling) • Freezing

  10. Properties of Solids • High Density • High Incompressibility • Definite Melting Point • Low Rate Of Diffusion • Amorphous versus Crystalline

  11. Equilibrium A condition in which two opposing changes occur at equal rates in a closed system

  12. PHASE CHANGES

  13. PHASE CHANGES

  14. But what happens if you raise the temperature to super-high levels…between 1000°C and 1,000,000,000°C ? Will everything just be a gas?

  15. STATES OF MATTERPLASMA • A plasma is an ionized gas. • A plasma is a very good conductor of electricity and is affected by magnetic fields. • Plasmas, like gases have an indefinite shape and an indefinite volume. • Plasma is the • common state • of matter

  16. STATES OF MATTER LIQUID PLASMA SOLID GAS Tightly packed, in a regular pattern Vibrate, but do not move from place to place Close together with no regular arrangement. Vibrate, move about, and slide past each other Well separated with no regular arrangement. Vibrate and move freely at high speeds Has no definite volume or shape and is composed of electrical charged particles

  17. The Six Basic Phase Changes

  18. Phase Changes: Where Does the Heat Go?

  19. Heating/Cooling Curve

  20. Heating/Cooling Curve

  21. Heating/Cooling Curve

  22. Phase Diagrams • Graph of pressure-temperature relationship: Show were each of the phases are • Lines indicate equilibrium state two phases. • Triple point- Temp. and Pressure where all three phases co-exist in equilibrium. • Critical temp.- Temp. where substance must always be gas, no matter what pressure. • Critical pressure- vapor pressure at critical temp. • Critical point- point where system is at its critical pressure and temp.

  23. Phase Diagram of H2O Water <---Melting Freezing---> <---Condensation Vaporization ---> Ice Triple Point Water Vapor <---Deposition Sublimation--->

More Related