1 / 33

Chapter 14 and 15 Standard 2 Chemical Bonding

Chapter 14 and 15 Standard 2 Chemical Bonding c. Students know that salt crystals are held together by repeating patterns of positive and negative ions held together by electrostatic attraction.

hinto
Download Presentation

Chapter 14 and 15 Standard 2 Chemical Bonding

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 14 and 15 Standard 2 Chemical Bonding c. Students know that salt crystals are held together by repeating patterns of positive and negative ions held together by electrostatic attraction. d: Students know the atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular forces are too weak to hold the atoms or molecules in a solid form.

  2. I. Physical Properties of the states of matter Yes Slightly No Moderate High Lowest Fills container Definite Definite of container of container own shape Slow-None Rapid Slow Increase Decrease Decrease

  3. Compressibility of gases and liquids

  4. Compressibility of a solid

  5. Ice in water Ice in alcohol

  6. Liquids and Gases take the shape of container

  7. The molecules in a solid, though they vibrate, do not move very far. When they wiggle, they wiggle in place. They fit closely together and keep their position.

  8. Liquids behave this way because in a liquid, the molecules are moving around more than the molecules in a solid. They slide over each other.

  9. The molecules in a gas are moving around like crazy, bouncing everywhere. They do not have to stay close to one another

  10. Gases take the shape of container

  11. What is happening to the volume of a solid when it is heated?

  12. What’s happening to the volume of liquid when heated?

  13. Chapter 14 Terms Please define the following terms, they are found in chapter 14: pages 457-489 • Intramolecular force • Intermolecular force • Viscosity • Surface Tension • Vaporization • Condensation • 7.Sublimation • 8.Deposition • 9.Heat of Fusion • 10.Heating Curve

  14. What would distinguish among H2O (gas)H2O (liquid)H2O( solid)? steam liquid ice

  15. Gas Liquid Solid

  16. The force of attraction between atoms in the same molecule….BONDING The force of attraction between an atom of one molecule and its neighboring molecule. Ionic, Covalent and Metallic Dipole-Dipole, Dispersion & Hydrogen Bonding + + : : Intermolecular Force. The connection between one molecule to another. - : : - - - + : + + - - : Within the same molecule + Very strong Relatively Weak To break this force of attraction it takes 6 kJ of energy (for melting) 40.1kJ of energy (for vaporization) To break H-O bond in a water molecule, it takes 463kJ of energy

  17. III. Compounds ( ) are HELD by Metal and Nonmetal Electrostatic Attraction Ionic Bond Stop Day 1

  18. Review Intra v. Inter Inside Outside Takes much energy to break! Takes little energy to break!

  19. Intramolecular v. Intermolecular Forces “Hand-Holding from one Molecule to another

  20. IV. Types of Intermolecular forces: 1. Dipole-Dipole Attraction between opposite charges of neighboring dipoles. 1. Hydrochloric Acid Draw three molecules of HCl Opposite charges attract!! _ _ _ + + + Covalent Bond (Intramolecuar) Dipole-Dipole (a type of intermolecular force )

  21. Hydrogen Sulfide • Draw 3 molecules of H2S. + + + + : _ : : _ : + + : : _

  22. 2. Dispersion Temporarily creating a dipole by inducing conditions (sufficiently increasing pressure and dereasing the temperature): examples: Noblegases/gases

  23. Helium Electrons are not equally distributed at one instant which gives a small instantaneous dipole and the atom or molecule itself becomes a small dipole.

  24. Neon condensing

  25. • • • • • • • • • • • • • • • • • • • • • • • • O O O O O O - - - - - - H+ H+ H+ H+ H+ H+ H+ H+ H+ H+ H+ H+ 3. HYDROGEN “BONDING”: When Hydrogen is linked to : Fluorine, Oxygen or Nitrogen This stuff is FON!!!! Do you remember how much it takes to melt? Do you remember how much it takes to break? 6kJ to melt 463kJ evaporate? 40.1kJ to evaporate

  26. b. Ammonia : : : Hydrogen bonding H with N

  27. Video on states of matter ..\Streaming Video Files\Gases__Liquids__and_Solids 20 min.asx Start at 8:35

  28. Heating Curve Endothermic Sublimation Gas 100 Evaporation Condensation Liquid Temperature oC Melting Solid Deposition Freezing Exothermic Time 0 sec, min, hr, Melting is also known as Heat of fusion

  29. Some Properties of LIQUIDS • Viscosity: Thickness of a liquid: liquid’s resistance to flow. Due to strong intermolecular forces holding molecules together Viscosity decreases with increasing temperature

  30. A thin membrane made of water molecules on the surface of water. 2.Surface Tension

  31. Water Video

More Related