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Turn in Missing Work on Time and Avoid Credit Loss

Don't be that person who loses credit at the end of the semester. Submit your missing work by 5/26/19 or make prior arrangements.

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Turn in Missing Work on Time and Avoid Credit Loss

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  1. Note – All Missing and Late Workis due by 5/26/19 unless previous arrangements have been made with me. Thank You

  2. Don’t be that person at the end of the semester who’s getting no credit. Turn in that missing work.Don’t even ask!

  3. Bellringer A sample of argon has a volume of 5.0 cm3 and the pressure is 1.92 atm. If the intial temperature is 30.° K, the final volume is 51 L, and the final pressure is 837. mm Hg, what was the final temperature of the argon in Celsius?

  4. Ch. 13 - Liquids & Solids I. Bonding Review Types: Chart on 3 types of bonds -

  5. A. Inter… and Intra… • Intermolecular Forces • Intramolecular Forces

  6. A. Inter… and Intra… • Attractive forces between molecules. • Chemical bonds within molecules.

  7. B. Types of Chemical Bonds IONIC “COVALENT” e- are transferred from metal to nonmetal e- are shared between two nonmetals Bond Formation Type of Structure Both intra- and inter- “true Molecules crystal lattice Physical State liquid or gas solid Melting Point Low (Intermolecular force breaks) high Solubility in Water yes usually not yes (solution or liquid) Electrical Conductivity no Other Properties Weak bonds Strong bonds

  8. Don’t be that person at the end of the semester who’s getting no credit. Turn in that missing work.Don’t even ask!

  9. B. Types of Chemical Bonds METALLIC e- are delocalized among metal atoms Bond Formation Type of Structure “electron sea” Physical State solid Melting Point very high Solubility in Water no yes (any form) Electrical Conductivity malleable, ductile, lustrous Other Properties

  10. B. Types of Chemical Bonds • Difference in the elements’ e-negs determines bond type: > 2.0 Ionic 0.4 – 2.0 Polar C < 0.4 Nonpolar C

  11. Types of IMF(InterMF)

  12. C. Types of IMF • London Dispersion Forces

  13. Note – All Missing and Late Workis due by 5/26/19 unless previous arrangements have been made with me. Thank You

  14. + - C. Types of IMF • Dipole-Dipole Forces

  15. C. Types of IMF • Hydrogen Bonding

  16. B. Types of Chemical Bonds Ionic Bonding - Crystal Lattice RETURN

  17. B. Types of Chemical Bonds Covalent Bonding - True Molecules Diatomic Molecule -7 RETURN

  18. B. Types of Chemical Bonds Metallic Bonding - “Electron Sea” RETURN

  19. Molecular Formula: The actual formula for a molecule. • Problem: • A compound has an empirical formula of ClCH2 and a molecular weight of 98.96 g/mol. What is its molecular formula? • Strategy: • Find the mass of the empirical unit. • Figure out how many empirical units are in a molecular unit. • Write the molecular formula.

  20. Note – All Missing and Late Workis due by 5/26/19 unless previous arrangements have been made with me. Thank You

  21. Strategy: • Find the mass of the empirical unit.Mass of empirical unit = mass Cl + mass C + 2(mass H) Mass of empirical unit = 35.45 + 12.00 + 2(1.008) = 49.47 g/mol • Figure out how many empirical units are in a molecular unit.# of empirical units = (mass of molecular unit/ mass of empirical unit) (98.96 g/mol) / (49.47 g/mol) = 2.000 empirical units per molecular unit • Write the molecular formula.It takes two empirical units to make a molecular unit, so, the molecular formula is: Dichloro Ethane Cl2C2H4

  22. The percent composition (percentage composition) of a compound is a relative measure of the mass of each different element present in the compound. To calculate the percent composition (percentage composition) of a compound • Calculate the molecular mass(molecular weight, formula mass, formula weight), MM, of the compound • Calculate the total mass of each element present in the formula of the compound • Calculate the percent composition (percentage composition): % by weight (mass) of element     = (total mass of element present ÷ molecular mass) x 100

  23. Examples • Calculate the percent by weight of sodium (Na) and chlorine (Cl) in sodium chloride (NaCl) • Calculate the molecular mass (MM):MM = 22.99 + 35.45 = 58.44 • Calculate the total mass of Na present:1 Na is present in the formula, mass = 22.99 • Calculate the percent by weight of Na in NaCl:%Na = (mass Na ÷ MM) x 100 = (22.99 ÷ 58.44) x 100 = 39.34% • Calculate the total mass of Cl present:1 Cl is present in the formula, mass = 35.45 • Calculate the percent by weight of Cl in NaCl:%Cl = (mass Cl ÷ MM) x 100 = (35.45 ÷ 58.44) x 100 = 60.66% •     The answers above are probably correct if %Na + %Cl = 100, that is,     39.34 + 60.66 = 100.

  24. Calculate the percent by weight of each element present in sodium sulfate (Na2SO4). • Calculate the molecular mass (MM):MM = (2 x 22.99) + 32.06 + (4 x 16.00) = 142.04 • Calculate the total mass of Na present:2 Na are present in the formula, mass = 2 x 22.99 = 45.98 • Calculate the percent by weight of Na in Na2SO4:%Na = (mass Na ÷ MM) x 100 = (45.98 ÷ 142.04) x 100 = 32.37% • Calculate the total mass of S present in Na2SO4:1 S is present in the formula, mass = 32.06 • Calculate the percent by weight of S present:%S = (mass S ÷ MM) x 100 = (32.06 ÷ 142.04) x 100 = 22.57% • Calculate the total mass of O present in Na2SO4:4 O are present in the formula, mass = 4 x 16.00 = 64.00 • Calculate the percent by weight of O in Na2SO4:%O = (mass O ÷ MM) x 100 = (64.00 ÷ 142.04) x 100 = 45.06% •     The answers above are probably correct if %Na + %S + %O = 100, that is,     32.37 + 22.57 + 45.06 = 100

  25. Melting / Freezing : Vaporization / Condensation: Sublimation / Deposition

  26. Don’t be that person at the end of the semester who’s getting no credit. Turn in that missing work.Don’t even ask!

  27. Questions: 1. What is the most likely state of matter when particles are moving slow or fast? 2. How do Intermolecular forces determine the state of matter? 3. What type of IMF do gas particles have? Name the other two and strength of force. Draw and label the heating curve of water 4. What does the heating curve graph show us? 5. What does each plateau indicate? 6. What temp is the heat of fusion of ice? The heat of vaporization of water? 7. Why is there NOT a temp change during the phase changes?

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