Chemisty

Front 1

1. What is a polar bond? Which bondis most polar H-F, H-S, H-O, O-O, SS?

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1. Electrons pulled toward most enegativeelement. H-F largest enegativitydifference

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2. What do the following instrumentsmeasure: thermometer, barometer,manometer,

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2. T, Atmospheric P, P of enclosedgas

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3. What is happening at the surface ofa liquid that is evaporating?

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3. Some molecules escaping liquidphase- state of equilibrium

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4. Which diatomic element(s) have adouble bond? Triple bond? Singlebond?

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4. Single: halogens + H2, double: O2,triple: N2

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5. Write the generic equations for thefollowing reactions: decomposition,single replacement, doublereplacement, and synthesis.

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5. AB→A+B; A+BC → B+AC;AB+CD → AC + BD; A+B → AB

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6. What does a very high equilibriumconstant signify?

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6. Products are favored

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7. What are ionic bonds?

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7. Between metal and non metals(elements or polyatomic ions).

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8. What is stoichiometry and which lawmust be obeyed?.

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8. Quantitative analysis of chemicalreactions. Law of conservation ofmass.

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9. What is the mass in grams of 4.6 x1024 atoms Zn?

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9. g= 4.6 x 1024 atoms x (1molZn /6.02 x 1023 atoms) x (65.38 g Zn /1mol Zn) = 5 x 102 g Zn

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10. Calculate the approximate volume ofa 0.600 mol sample of gas at 15.0°Cand a pressure of 1.10 atm.

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10.V = (nRT)/P = (0.600mol x 0.0821L.at./mol.K x 288K) / 1.10 atm =12.9 L

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11. What is Avogadro’s number?What quantity has this numberof particles?

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11.The # of particles in one mole of asubstance = 6.02 X 1023 particles

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12. How and why does a gasexpand?

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12.To fill container, expands as T rises, Preduced.

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13. What can be said about 1 molPb and 1 mol Sn?

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13.Same # atoms

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14. What is the difference betweena limiting reactant and areactant that is in excess?

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14.Limiting reactant will run out first – the otherreactant is said to be in excess

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15. How many atoms are in 6.2moles of Sb atoms?

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15.#atoms = 6.2 mole x (6.02 x 1023 atoms /mole) = 3.73 x 1024

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16. What are covalent bonds, andwhy do atoms form bonds??

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16.Bonds between non metallic elements.Electronegativity difference < 1.7. To attainNGC.

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17. What is the Kinetic MolecularTheory?

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17.Describes gases: Atoms in continualrandom motion, elastic collisions,Atomsvery small separated by empty space. Ke =1/2mv2

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18. What type of chemicalsdissolve in water?

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18.Polar molecules, ionic compound whereionic bonds can be pulled apart by polarwater molecules.

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19. What are the units for the molarmass of a substance?

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19.g/mol

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20. Describe the types of IMF.Which are the strongest?Weakest?

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20. Dispersion (or London) forces(weakest,polarity induced between non-polarmolecules)); Dipole-Dipole (between polarmolecules); Strongest are H- bonds(special dipole-dipole where H can bond tounshared e-pair on O, N or F

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21. What symbol is used to showthat a reaction is reversible?

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21. arrows on top of each other, pointing opposite directions

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22. What is an exothermicreaction? Endothermic?

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22.Exo – gives off heat,energy ofproducts < energy ofreactants. Endo, absorbsheat– energy of products >energy of reactants

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23. What is the VSEPR Theory?

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23.Valence Shell Electron PairRepulsion – can predict 3 –dimensional shape ofmolecules

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24. Which phase changes areexothermic? Endothermic?

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24.Exo-condensation, freezing,deposition. Endo – melting,boiling, sublimation.

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25. What does a low equilibriumconstant signify?

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25.Reactants favored

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26. What is the relationshipbetween P and V?

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26.Inverse

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27. What is happening to gasmolecules as a balloon isinflated?

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27.They are pushing against thesides of the balloon. Themore gas molecules the moreV required.

Front 28

28. Which of these changeswould NOT cause anincrease in the pressure of acontained gas?

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28.Higher V, Lower T, fewer mol

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29. How many moles of W atomsare in 3.2 1025 atoms of W?

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29.3.3x1025/6.02x1023=53.2mol

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30. Which are the diatomicelements?

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30.H2O2F2Br2I2N2Cl2

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31. What happens as the temperature ofa gas in a balloon decreases?

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31. V decreases, P constant in flexibleballoon

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32. What causes gas pressure in acontainer?

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32. Molecules colliding with sides ofcontainer

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33. At STP what is the volume of 1.0mole of any gas?

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33. 22.4L

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34. Define temperature.

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34. Average Ke of particles in sample

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35. What are the differences betweenionic and covalent bonds?

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35. Ionic stronger, metal to non-metal, enegdifference > 1.7, brittlecompound, when dissolved conductelectricity. High MP and BPCovalent, e-neg diff < 1.7, do notconduct, mostly softer (wax, oil, gas).Low BP and MP. Exception diamond!

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36. What happens to the pressure of agas inside a rigid container if thetemperature of the gas decreases?

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36. P decreases

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37. When would you use the ActivitySeries?

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37. To determine if Single ReplacementRx will take place.

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38. The volume of a sample of helium is4.50 mL at 20.0°C and 203.0 kPa.What will its volume be at 10.0°Cand 203.0 kPa?

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38. V2 = (V1T2) / T1 = 4.3mL

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39. Does the number of moles ofreactants have to equal the numberof moles of products?

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39. No!

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40. Does the mass of the reactants haveto equal the mass of the products?

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40. Yes!

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41. What is the pressure when aliquid is boiling at its normalboiling point?

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41.Vapor pressure of liquid =atmospheric pressure

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42. What is the relationship betweenT and V?

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42.Direct

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43. What is the pH of a solutionwhose hydronium ion

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43.pH = -log 5.03 x 10-1 = 0.300

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44. What is the measured amount ofa product obtained from achemical reaction?

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44.The amount determined byexperimentation in the lab

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45. What is the calculated amount ofa product obtained from achemical reaction?

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45.The amount calculatedstoichiometrically

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46. What is the range of pH valuesfor acids? Bases?

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46.0≤ acid <7: 7 = neutral: 7 < base ≤14

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47. Which gases effuse slowest?

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47.Those that have the largestMolecular Mass

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48. What is a conjugate base?

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48.What an acid becomes after it hasdonated H+ion to base

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49. Why does a liquid evaporatefaster as the temperatureincreases?

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49.Molecules Keincreases until theyhave enough energy to breakbonds of liquid

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50. What are the properties ofacids? Bases?

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50.Acids: sour, sticky. High H+concentration, weak/strong, reactwith metals to produce H2, Bases:slippery, bitter, high OH-,weak/strongconcentration, reactwith oils and grease, BOTH areelectrolyte

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51. What is STP in gas law calculations?

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51.0°C (273 K), 1atm

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52. What are the bond angles in atetrahedral molecule? Linear?Trigonal planar?

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52.109.5°, 180°, 120°

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53. What is the difference between astrong acid (or base) and a weakacid (or base)?

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53.It’s a measure of how much theacid disassociates. Weak acidsdisassociate very little. Strongacids disassociate completely.

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54. How does the molar mass of a liquidaffect its boiling point?

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54.Generally, the heavier a moleculeis the higher its boiling point

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55. How do IMFs affect the boiling pointof a liquid?

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55.The stronger the IMF the higherthe BP.

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56. Find the molar mass of the following:a) H3PO4b) NaHCO3c) FeCl3

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56.MMa) 98 g/molb) 84 g/molc) 162 g/mol

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57. The composition of nicotine is 74.0%C, 8.7% H, and 17.3% N. The molarmass of nicotine is 162 g/mol. Whatis its molecular formula?

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57.C: 74g → 6.166mol H:8.7g →8.630mol, N 17.3g → 1.236 mol.Divide by small: C 5, H 7, N 1. MMempirical formula = 81 g/mol. So,molecular formula is: C10H14N2

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58. What is the % composition ofmagnesium carbonate

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58.MgCO3 MM = 84.3g/mol; Mg =28.8%, C = 14.2%, O = 56.9%

Front 59

59. How many moles are 8.92 x 1023atoms of barium (Ba)

60. What is the mass of this amount ofBa?

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59.Mol = 8.92x1023 / 6.02x1023=1.48mol

60.g = 1.48mol x 137.3g/mol = 203g

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61.Hydrogen is collected over water at 0.975atm and 28C. What is the partialpressure of H2? At this temperature thepartial pressure of water vapor is 3.73x10-2atm.

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61. Ptot - PH2O = PH2.= .975atm –3.73x10-2atm = 0.938 atm

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62.How many moles of chloroform, CHCl3,are required to fill a 253-mL flask at100.0C and 940 torr?

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62. 940 torr =1.24atm; 100 °C =373K; 253 mL = 0.253L: n =PV/RT = (1.24atm x 0.253L) /(0.0821 L.atm/mol.K X 373K)= 1.02 x 10-2 mol

Front 62

63.You want the pressure inside a bottle tobe 75.0 kPa at 23C. At whattemperature in Celsius should you sealthe bottle when the pressure is 1.12 atm?

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63. P2 = 75.0 kPa = 0.740 atm; T2= 23 °C = 296K; P1 = 1.12 atm:T1=(T2P1)/P2 = 448K = 175 °C

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64.A diver’s lungs hold about 20.0 L of airunderwater at a pressure of 875 mm Hg.Assuming he holds his breath and hislungs don’t burst, what will be the volumeof air in his lungs at standard pressure onthe water’s surface.

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64. Standard P = 760 mmHgV2=P1V1 / P2 =23L

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65.A soccer ball containing 12.0 dm3 of gasat 21C is left outside on a cold, winterday. What is the temperature outside inCelsius if the ball shrunk to 10,500 cm3?

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65. 1 dm3 = 1L; 21C = 294K;10,500cm3=10.5L; T2=T1V2/V1= 257 K = -16C

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66. What pressure is required to compress agas that occupies 6500 L at 25C and 1.0atm to a volume of 40.0 L at 18C?

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66. P2=P1V1T2/ T1V2 = (1atm x 6500Lx 291K) / (298K x 40.0L) = 1.59 x102 atm

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67. Balance the following equations and statewhat type of reaction they represent:a) C2H2 + O2 → CO2 + H2Ob) K2O + H2O → KOHc) H2O2 → H2O + O2d) Fe2(SO4)3 + KOH → K2SO4 + Fe(OH)3e) Cu + AgNO3 → Ag + CuNO3

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67. Balanceda) 2,5,4,2b) 1,1,2c) 2,2,1d) 1,6,3,2e) 1,1,1,1

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68. How many moles of CO are in a 2.0Lcontainer at STP?

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68. 2L x (1mol/22.4L) = 8.9 x 10-2mol

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69. For each of the following molecules:• Determine which are polar or non-polar.• What type of intermolecular force(s)(IMF) you think hold them together as aliquid?• Which do you expect to have the lowestboiling point?

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69. All polar except hexane which isnon-polar. Hexane: Londondispersion forces (v. weak). Therest have dipole – dipole IMF.Strong H bonds in H2O & NH3.

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70. For the balanced equation shown below, ifthe reaction of 50.3 grams ofH3BO3 produces 8.97 grams of H2O, whatis the percent yield?6H3BO3→H4B6O11+7H2O

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70. % yield = (actual/theoretical)x100Actual yield = 8.97g H2O.Theoretical g H2O = 50.3g H3BO3x(1molH3BO3/ 61.81g)x(7 molH2O/6mol H3BO3) x (18.0gH2O/1mol H2O) = 17.1g H20. %yield = 52.4%

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71. If you have 0.800 moles ofpotassium phosphate (excessaluminum nitrate), what is themass of aluminum phosphatethat is produced? K3PO4 +Al(NO3)3 → 3KNO3 + AlPO4

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71.gAlPO4= 0.8000mol K3PO4 x(1mol AlPO4/1 mol K3PO4) x(121.98g AlPO4/ 1 mol AlPO4) =97.6g AlPO4

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72. If you have 18.5g of potassiumphosphate (excess aluminumphosphate), how many mol ofaluminum phosphate isproduced?K3PO4 + Al(NO3)3 →3KNO3 + AlPO4

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72.Mol AlPO4 = 18.5 g K3PO4 x (1mol K3PO4/ 212.3g K3PO4) x(1mol AlPO4/ 1mol K3PO4) =8.7x10 -2 mol AlPO4

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73. A 10.00 L sample of a gas has amass of 19.2 g at STP. What isthe molar mass of the gas?

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73.MM=(19.2g/10L) x (22.4L/1mol) =43.01 g/mol

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74. How do you write equilibriumconstant?

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74.Keq = ([products]/[reactants]

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75. What is LeChatelier’s Principle?

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75.How system at equilibriumresponds to stress

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76. How do you write the acidionization constant, Ka?

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76.Ka = [H+][A-]/ [HA] whereA-is conjugate base,and HA is acid

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77. What is the pH of a solutionwith [H] = 0.003M?

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77.pH= - log 0.003 = 2.5

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78. What is the [H] of a solutionwith a pH 2.3?

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78.[H+] = 10 -2.3= 5.0x10-3M

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79. Ammonia (NH3) has a___________ geometry and___________ shape

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79.Tetrahedral, trigonalpyramidal

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80. What is true at chemicalequilibrium?

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80.Rate of forward rx = rateof reverse rx. Basicallyseems that rx hasceased bot it has NOT! Ithas reached equilibrium.

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