1. Semester II Review

2. Name the compounds H 2 SO 3 Sulfurous Acid H 2 SHydrosulfuric acid H 3 PO 4 Phosphoric acid HCNHydrocyanic acid H 3 PHydrophosphoric acid HBrHydrobromic acid HClOHypochlorous acid SM II Review

3. Give the formula for the following compounds hydrofluoric acidHF hydroselenic acidH 2 Se carbonic acidH 2 CO 3 nitrous acidHNO 2 sulfuric acidH 2 SO 4 hydrobromic acidHBr Chlorous acidHClO 2 SM II Review

4. Antimony tribromideSbBr 3 Silicon difluorideSiF 2 Tetracarbon octahydrideC 4 H 8 Dinitrogen monoxideN 2 O Pentaphosphorous decoxideP 5 O 10 Sulfur hexachloride SF 6 SM II Review

5. P 2 O 5 Diphosphorous pentoxide SO 2 Sulfur dioxide NO 2 Nitrogen dioxide AsCl 3 Arsenic trichloride P 4 H 8 Tetraphosphorous octahydride SM II Review

6. Semester II Review For the following compound, draw its Lewis structure, give the electron tally, hybridization, name of shape, determine if it is polar or not, and identify the Intermolecular Forces. SO 2 e tally = 2BA 1LP, Hybrid = sp 2, Shape = Bent, Polar, IMF= Dipole

7. Semester II Review For the following compound, draw its Lewis structure, give the electron tally, hybridization, name of shape, determine if it is polar or not, and identify the Intermolecular Forces. NH 3 e tally = 3BA 1LP, Hybrid = sp 3, Shape = Trigonal Pyrmidal, Polar, IMF= H-Bonds

8. Semester II Review For the following compound, draw its Lewis structure, give the electron tally, hybridization, name of shape, determine if it is polar or not, and identify the Intermolecular Forces. SO 4 2- e tally = 4BA 0LP, Hybrid = sp 3, Shape = Tetrahedral, Nonpolar, IMF(Ion)

9. Balance and classify the reactions _2_ C 8 H 18 + _25_ O 2  _16_ CO 2 + _18_ H 2 O ____ FeCl 3 + _3__ NaOH  ____ Fe(OH) 3 + _3__NaCl _4__ P + __5_O 2  _2__P 2 O 5 _2__ Na + _2__ H 2 O  __2_ NaOH +  ____H 2 _2__ Ag 2 O  _4__ Ag + ____O 2 ____ S 8 + _12_ O 2  _8__ SO 3 Semester I Review

10. SM II Review Complete, Balance, and Classify each Rxn 1. 2Al + 3S  Al 2 S 3 Synthesis 2.NaCl + AgNO 3  AgCl + NaNO 3 D.R. 3. C 3 H 8 + 5O 2  3CO 2 + 4H 2 O Combustion 4. 2H 2 O  2 H 2 + O 2 Decomposition 5. 2Li + Na 2 CO 3  2Na + Li 2 CO 3 S.R. In every chemical reaction, what item(s) is/are conserved? Mass and Atoms

11. SM II Review For a given chemical reaction, the theoretical yield is generally more than the actual yield The first step in most stoichiometry problems is to balance the equation.

12. SM II Review Hydrogen gas reacts with nitrogen gas to form ammonia gas. –Write and balance the equation – 3H 2 + N 2  2NH 3 –Determine the Limiting reactant if 3.50 g of hydrogen reacts with 42.0 g of nitrogen. –What is the theoretical yield of the above problem? 39.4 g NH 3 – What is the % yield if the reaction produced 15.3 g of ammonia. 38.8 % –Calculate the amount of grams of excess reactant leftover at the end of the reaction 25.8 g N 2 Leftover

13. What is the empirical formula of a compound that is 32.37 % Na, 22.58 % S, and 45.05 % O. Na 2 SO 4 If the molecular formula molar mass is 284.10, what is the molecular formula of the above compound. Na 4 S 2 O 8 What is the percent composition of FeO? 77.73% Fe and 22.27% O SM II Review

14. Calculate the specific heat of an unknown metal, given that 25.0g of the metal lost 3570 J of energy during a temperature change from 100.0 o C to 25.0 o C c = -3570J / (25.0g)x(-75.0 o C) c = 1.90 J/g o C

15. SM II Review Identify each of the letters on the graph and explain what is occurring. C = solid warming/cooling D = Phase change solid to liquid or vice versa E = liquid warming/cooling F = phase change liquid to gas or vice versa G = gas warming/cooling C D E F G

16. SM II Review Label the solid, liquid, and gas regions on the graph. Label the triple point and critical point At 600 o C and 90 atm, what phase is yummygum in? Liquid solid liquid gas Triple point Critical point

17. SM II Review Calculate the amount of heat released if 25.0g of steam is cooled from 150.0 o C to (-15.0 o C) Phase 1 = -2537.5 J Phase change = -56500 J Phase 2 = -10460 J Phase change = -8350 J Phase 3 = -753.75 J Total Energy = -78600 J

18. SM II Review If the volume of a container holding a gas is reduced, what will happen to the pressure within the container? Increase What happens to the temperature of a gas when it is compressed? Increases What happens to the pressure of a gas inside a container, if the temperature of the gas is lowered? Decreases The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change? Decreases by 2 times

19. SM II Review Boyle’s law states that PV = K, inverse proportion. Charles’ law states that V/T = K, direct proportion. Gay-Lussac’s law states that P/T = K, direct proportion. Avogadro’s law states that V/n = K, direct proportion. Dalton's Law states that sum of all the pressures = the total pressure.

20. Semester II Review How many grams of CO 2 are produced when 34.6 L of CH 4 combusts with oxygen at a pressure of 1.78 atm and a temperature of 28 o C. Balance the equation first. (combustion of hydrocarbon) CH 4 + 2O 2  CO 2 + 2H 2 O 2.49 mol CH 4 will produce 110. g CO 2

21. SM II Review A gas confined in a 305 mL container exerts a pressure of 1.07 atm at 38.6°C. At what Celsius temperature will it exert a pressure of 2.75 atm if it is placed into a 644 mL container? 1506 K - 273 = 1233 °C

22. SM II Review What is the pressure inside a 3.0 L flask if 30.5 g of Carbon Monoxide is held at a temperature of 105.2 o C? 11 atm or 1100 kPa