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Entry Task: March 21 st 22 nd Block #2

Entry Task: March 21 st 22 nd Block #2. Question: What is the difference between intramolecular forces and intermolecular forces? You have 5 minutes!. Agenda. Discuss Ch. 13 sec 2-3 reading notes HW: Ch. 13 sec 2-3 ws. I can…. Section -2

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Entry Task: March 21 st 22 nd Block #2

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  1. Entry Task: March 21st 22nd Block #2 Question: What is the difference between intramolecular forces and intermolecular forces? You have 5 minutes!

  2. Agenda • Discuss Ch. 13 sec 2-3 reading notes • HW: Ch. 13 sec 2-3 ws

  3. I can… Section -2 • *Describe and compare Intermolecular and intramolecular forces. • *Distinguish the different types of IMF

  4. I can… Section -3 • *Apply the Kinetic-Molecular theory to liquids and solids • *Properties of liquids and solids

  5. 13.2- Forces of Attraction At room temperature all particles have… The same average kinetic energy

  6. 13.2- Forces of Attraction What are intramolecular forces? The forces within molecules. The force that holds atoms together- ionic, covalent and metallic bonds

  7. 13.2- Forces of Attraction What are intermolecular forces? The forces between other molecules. The force “attractions” among adjacent molecules/compounds

  8. 13.2- Forces of Attraction Define dispersion forces. Dispersion forces are weak forces that result from temporary shifts in the density of electrons in the electron clouds

  9. 13.2- Forces of Attraction Draw a picture of what dispersion forces “look like”. http://www.dlt.ncssm.edu/tiger/Flash/bonding/LondonDispersionForce.html

  10. 13.2- Forces of Attraction What types of molecules have only dispersion forces? Two non-polar molecules become close to each other or collide.

  11. 13.2- Forces of Attraction What types of molecules have dipole-dipole forces? Polar molecules contain permanent dipoles- contain permanent positive end and negative end to their molecules

  12. 13.2- Forces of Attraction Define dipole-dipole forces. Attraction between oppositely charged regions of polar molecules are called dipole-dipole forces

  13. 13.2- Forces of Attraction Draw a couple of molecules showing dipole-dipole attraction. LABEL each molecule with charges!!!

  14. 13.2- Forces of Attraction Define hydrogen bonding. It’s a dipole-dipole attraction that occurs between molecules containing hydrogen and strong EN atoms (FON) with at least 1 lone pair of electrons

  15. 13.2- Forces of Attraction What types of molecules have hydrogen bonding? Molecules that have atoms with strong electronegativity AND lone pairs of electrons like Fluorine, Oxygen, andNitrogen (FON)

  16. 13.2- Forces of Attraction QUESTION: Why are dipole-dipole forces stronger than dispersion forces for molecules of comparable masses? Dipole-dipole have permanent poles. Dispersion forces have temporary poles due to shifting electrons

  17. 13.2- Forces of Attraction Provide the type of intermolecular forces (IMF) that are involved with each of these molecules. EXPLAIN your answer. H2- NH3- HCl- HF- Dispersion- diatomic molecules (non polar) H-bonding- Nitrogen is strong (EN) and lone pairs Dipole-Dipole- Chlorine and hydrogen are polar H-bonding- Fluorine is strong (EN) and lone pairs

  18. 13.2- Forces of Attraction QUESTION: Make a prediction about the relative boiling points of noble gases. Give a reason for your answer. They are gases (low boiling points) because the only IMF holding them together is dispersion forces-very weak thus the low boiling point.

  19. 13.3- Liquids and Solids What must you consider about liquids and solids, besides the kinetic-molecular theory of matter? The forces of attraction between particles as well as the their energy of motion

  20. 13.3- Liquids and Solids Liquids What does the kinetic molecular theory predict about liquid particles? It predicts the constant motion of the liquid particles. They are in motion.

  21. 13.3- Liquids and Solids What about the forces of attraction between these particles? The force of attraction between liquid particles limit their range of motion so that the particles remain closely packed in a fixed volume.

  22. 13.3- Liquids and Solids Density and Compression Compare the density of gases to liquids? The density (mass per unit of volume) is very low in a gas. Liquids are closer therefore take up less space (volume).

  23. 13.3- Liquids and Solids What does the density of a liquid say about its (IMF)? The higher the density of a liquid, the greater the IMF are between particles

  24. 13.3- Liquids and Solids Fluidity Define Fluidity Fluidity is the ability to flow. Particles can slide passed each other- flow.

  25. 13.3- Liquids and Solids Viscosity Define Viscosity. Viscosity is a measure of the resistance of a liquid to flow. High viscosity = slow flowing Low viscosity = fast flowing

  26. 13.3- Liquids and Solids What is the relationship between viscosity and IMF? The higher the IMF the higher the viscosity the slower the flow.

  27. 13.3- Liquids and Solids How does the size and shape of molecules affect the viscosity? The larger and longer the molecule the higher the viscosity The smaller and shorter the molecule the lower the viscosity

  28. 13.3- Liquids and Solids Viscosity and temperature What is the relationship between viscosity, temperature, kinetic-molecular energy and IMF? High Viscosity Low Viscosity Cooler temperature Lower the KME Higher IMF Hotter temperature Higher the KME Lower IMF

  29. 13.3- Liquids and Solids Surface tension How is surface tension created in a liquid? Particles at the surface of a liquid, there are no attractions from above to balance the attractions from below. Thus, there is a net attractive forces pulling down on the particles at the surface. This creates a “skin” on top of the fluid.

  30. 13.3- Liquids and Solids Define surface tension. Surface tension is a measure of the inward pull by particles in the interior. The higher the IMF the higher the surface tension.

  31. 13.3- Liquids and Solids What are surfactants? Compounds that lower the surface tension of water are surfactants. Soap and detergents are surfactants.

  32. 13.3- Liquids and Solids What is cohesion? The forces of attractions between identical molecules

  33. 13.3- Liquids and Solids What is adhesion? The forces of attractions between different molecules

  34. 13.3- Liquids and Solids What is capillary action? Due adhesion of water to glass molecules and cohesion of water-water molecules allows water to rise up a narrow tube of glass.

  35. 13.3- Liquids and Solids Solids What is the relationship between solid particles, kinetic-molecular energy, IMF, and density? Solid particles have same KME as liquids at same temperature but are solid because they have a higher IMF and therefore have higher density.

  36. 13.3- Liquids and Solids Define crystalline solid. Crystalline solids is a solid whose atoms, ions, or molecules are arranged in an orderly geometric, 3-D structure.

  37. 13.3- Liquids and Solids What are molecular solids? Provide an example. In molecular solids, the molecules are held together by dispersion, dipole-dipole or hydrogen bonding forces. These solids have large molecules with weak IMF like sugar.

  38. 13.3- Liquids and Solids What are covalent network solids? Provide example. Atoms such as carbon and silicon, which can form multiple covalent bonds, able to form a network of bonds. Allotropes of an elemental solid- nonmetals.

  39. 13.3- Liquids and Solids What are ionic solids? Provide example. Created by ionic bonding between oppositely charged particles to create a lattice structure. Salt!

  40. 13.3- Liquids and Solids What are metallic solids? Provide an example. Metal atoms attracted to other metal atoms creating a “sea of electrons”. Copper Iron Most transitional element- metals

  41. 13.3- Liquids and Solids What are amorphous solids? Provide an example. Amorphous solids is one in which the particles are not arranged in a regular, repeating pattern. Glass, rubber, wax and plastics are examples of amorphous solids.

  42. 13.3- Liquids and Solids QUESTIONS: How are unit cells and a crystal lattice related? Unit cells are the building blocks of the crystal lattice

  43. 13.3- Liquids and Solids Explain why solids are not classified as fluids. Solid particles are not able to slide past each other. They only vibrate around a fixed position.

  44. 13.3- Liquids and Solids What is the difference between a molecular solid and a covalent network solid? Molecular solids involve IMF not true covalent bonds like the covalent network solids.

  45. HOMEWORK • Ch. 13 sec 2-3 worksheet

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