::::: Official SAT Chemistry 2012 :::::

Archive SAT Subject Test Preparation
61

<p>Ya I got that for the atomic number and concentration.</p>

62

<p>^ magnificent6, what was your timed practice test scores if you don’t mind telling me</p>

63

<p>also for the ionization/solubility constant, which has the smallest concentration? we were given K for 5 choices. I put smallest K value.</p>

64

<p><a href=“46/85”>b</a> :**</p>

<p>Section A :

  1. 80 K to 80 Ar (Nuclear Transformation) *
  2. Iron Oxide produced from iron (Oxidation/Reduction)
  3. One of question set with Iron Oxide (Opposite of Iron oxide answer)
  4. Which has both ionic and covalent bonds? (NH4OH) *
  5. HC2H3O2 pH (pH greater than 1 but less than 7) *
  6. (pH 7) *
  7. (pH greater than 7 but less than 14) *
  8. Lewis Dot structure for some compound CF3 *</p>

<p>**Section B :<a href=“7%20TTCE”>/b</a>
9. Baking powder NaHCO3 neutralizes base BECAUSE NaHCO3 behaves as Bronsted acid (T/T CE) *
10. Something BECAUSE Sugar melting point is higher than water (T/F)
11. Photon emits light BECAUSE electron emits discrete photons when comes to ground state. (T/T CE) *
12. Ideal Condition when high temperature and low pressure BECAUSE intermolecular force is greater so volume of gas particles is insignificant (T/T CE) *
13. 1g of something compared to other 1g of something else BECAUSE 1 mole of something has greater something than something else (F/T) *
14. Adding water to acid BECAUSE It would cause splattering (T/T CE) *
15. HC2H3O2 is strong acid BECAUSE Acetic acid has 4 hydrogen atoms (F/T) *
16. Kw = 1 x 10^-14 when H2O -> H+ + OH- BECAUSE (T/T CE)
17. Proton changes in isotopes BECAUSE they have different atomic mass (F/T) *
18. Na2+ + e- Na+ takes larger energy than Na+ + e- BECAUSE Na+ has larger atomic radius than Na (T/F) *</p>

<p>Section C :
19. Which has multiple bond (CO) *
20. Which does not form solution or something like that (CH4OH w/ NH4 OR CH4OH w/ HF)
21. M = Alkali metal, reaction with Oxygen (2M + O2 -> M2O - Choice A) *
22. (CuSO4 x 5H2O) *
23. (230 KJ = 18 x 13) *
24. This element’s type is good conductor of electricity (Carbon) *
25. C2 (covalent network bonds) *
26. Easiest to be oxidized (1s2 2s2 2p6 3s1) *
27. Highest energy level for the element (3p) *
28. Ba(SO)4 reacted with some 1.0 M X element, white colorless gas, brown gas ()
29. When empirical formula is XO, O mass percent is 64%, find the molar mass of X (9 grams/mole X) *
30. (K = 1 x 10 ^ -5) *
31. Separate Methyl Alcohol and Water (Distillation) *
32. Separate KI, sand, and Iron filing (Water extraction) *
33. Elements combining in different ratio (FeO & Fe2O3) *
34. Which makes a solution weak acid? (CO2)
35. Linear shape (CO2) *
36. As Atomic number increase in halogen (Atomic radius increases)*
37. Order of periodic table (Increase in atomic number) *
38. Highest Rate of Effusion (H2) *
39. explanation of graph where line is straight (Ice melted becomes solidified)
40. (evolves gas)
41. Which is liquid at room temperature (Br2)
42. Which has the highest H grams? (One with 0.6 x 16) *
43. Something about precipitate (Fe)
44. Which is endothermic (CO2 (s) -> CO2 (g))*
45. Ionization constant, so which has smallest concentration? (the one with smallest K)
46. Which of these is not a redox reaction? (H+ + O2- -> H2O) *</p>

65

<p>32, I don’t think it was water extraction, I put filtration.</p>

66

<p>Also, on my practice tests I got 710, 780, 690, 760, 760, 720, 730.</p>

67

<p>Most valence electrons, phosphorus?</p>

68

<p>isn’t sugar melting point higher than waters?</p>

69

<p><a href=“58/85”>b</a> :**</p>

<p>**Section A : **

  1. 40 K to 40 Ar (Nuclear Transformation) *
  2. Iron Oxide produced from iron (Oxidation/Reduction)
  3. One of question set with Iron Oxide (Opposite of Iron oxide answer)
  4. Which has both ionic and covalent bonds? (NH4OH) *
  5. HC2H3O2 pH (pH greater than 1 but less than 7) *
  6. NaCl Salt (pH 7) *
  7. (pH greater than 7 but less than 14) *
  8. Lewis Dot structure for some compound CF3 *
  9. Ozone Destruction (CFCl4) *
  10. Contributes to Acid Rain (SO2) *
  11. Highest Electronegativity (F)
  12. Lowest First Ionization (Na)
  13. Which loses 2 electrons (Mg)</p>

<p>Section B : (7 TTCE)

  1. Baking powder NaHCO3 neutralizes base BECAUSE NaHCO3 behaves as Bronsted acid (T/T CE) *
  2. Something BECAUSE Sugar melting point is higher than water (T/F)
  3. Photon emits light BECAUSE electron emits discrete photons when comes to ground state. (T/T CE) *
  4. Ideal Condition when high temperature and low pressure BECAUSE intermolecular force is greater so volume of gas particles is insignificant (T/T CE) *
  5. 1g of something compared to other 1g of something else BECAUSE 1 mole of something has greater something than something else (F/T) *
  6. Adding water to acid BECAUSE It would cause splattering (T/T CE) *
  7. HC2H3O2 is strong acid BECAUSE Acetic acid has 4 hydrogen atoms (F/T) *
  8. Kw = 1 x 10^-14 when H2O -> H+ + OH- BECAUSE (T/T CE)
  9. Proton changes in isotopes BECAUSE they have different atomic mass (F/T) *
  10. Na2+ + e- Na+ takes larger energy than Na+ + e- BECAUSE Na+ has larger atomic radius than Na (T/F) *
  11. Higher temperature increases reaction rate BECAUSE Kinetic Molecular energy exceeds the activation energy (T/T CE)*</p>

<p>Section C :

  1. Which has multiple bond (CO) *
  2. Which does not form solution or something like that (CH4OH w/ NH4 OR CH4OH w/ HF)
  3. M = Alkali metal, reaction with Oxygen (2M + O2 -> M2O - Choice A) *
  4. (CuSO4 x 5H2O) *
  5. (230 KJ = 18 x 13) *
  6. This element’s type is good conductor of electricity (Carbon) *
  7. C2 (covalent network bonds) *
  8. Easiest to be oxidized (1s2 2s2 2p6 3s1) *
  9. Highest energy level for the element (3p) *
  10. Ba(SO)4 reacted with some 1.0 M X element, white colorless gas, brown gas ()
  11. When empirical formula is XO, O mass percent is 64%, find the molar mass of X (9 grams/mole X) *
  12. (K = 1 x 10 ^ -5)
  13. Separate Methyl Alcohol and Water (Distillation) *
  14. Separate KI, sand, and Iron filing (Water extraction) *
  15. Elements combining in different ratio (FeO & Fe2O3) *
  16. Which makes a solution weak acid? (CO2) *
  17. Linear shape (CO2) *
  18. As Atomic number increase in halogen (Atomic radius increases)*
  19. Order of periodic table (Increase in atomic number) *
  20. Highest Rate of Effusion (H2) *
  21. explanation of graph where line is straight (Ice melted becomes solidified)
  22. (evolves gas)
  23. Which is liquid at room temperature (Br2)
  24. Which has the highest H grams? (One with 0.6 x 16) *
  25. Something about precipitate (Fe)
  26. Which is endothermic (CO2 (s) -> CO2 (g))*
  27. Ionization constant, so which has smallest concentration? (one with smallest K)
  28. Which of these is not a redox reaction? (H+ + O2- -> H2O) *
  29. Salt dissolves in water has following properties (D or E, answer was not Higher Vapor Pressure, Higher Freezing point, Lower Melting Point)
  30. Which has the highest pressure in 1L Container? (H2)*
  31. (0.0500 x 6.02 x 10^23)*
  32. (2L x 740/760 x 273/300) *
  33. (0.5 moles H2)
  34. Which has the most Valence electrons? (Phosphorus)*</p>
70

<p>It was Water extraction because they wanted to test you if you know KI is soluble or not. It dissolves in water and you can extract KI from rest of materials.</p>

71

<p>For a balancing equations one, the coefficient for Al(OH2)3 was 2.</p>

72

<p>(59/85) :</p>

<p>Section A :

  1. 40 K to 40 Ar (Nuclear Transformation) *
  2. Iron Oxide produced from iron (Oxidation/Reduction)
  3. One of question set with Iron Oxide (Opposite of Iron oxide answer)
  4. Which has both ionic and covalent bonds? (NH4OH) *
  5. HC2H3O2 pH (pH greater than 1 but less than 7) *
  6. NaCl Salt (pH 7) *
  7. (pH greater than 7 but less than 14) *
  8. Lewis Dot structure for some compound CF3 *
  9. Ozone Destruction (CFCl4) *
  10. Contributes to Acid Rain (SO2) *
  11. Highest Electronegativity (F)
  12. Lowest First Ionization (Na)
  13. Which loses 2 electrons (Mg) *</p>

<p>Section B : (7 TTCE)

  1. Baking powder NaHCO3 neutralizes base BECAUSE NaHCO3 behaves as Bronsted acid (T/T CE) +
  2. Something BECAUSE Sugar melting point is higher than water (T/F)
  3. Photon emits light BECAUSE electron emits discrete photons when comes to ground state. (T/T CE) +
  4. Ideal Condition when high temperature and low pressure BECAUSE intermolecular force is greater so volume of gas particles is insignificant (T/T CE) +
  5. 1g of something compared to other 1g of something else BECAUSE 1 mole of something has greater something than something else (F/T) +
  6. Adding water to acid BECAUSE It would cause splattering (T/T CE) +
  7. HC2H3O2 is strong acid BECAUSE Acetic acid has 4 hydrogen atoms (F/T) +
  8. Kw = 1 x 10^-14 when H2O -> H+ + OH- BECAUSE (T/T CE) +
  9. Proton changes in isotopes BECAUSE they have different atomic mass (F/T) +
  10. Na2+ + e- Na+ takes larger energy than Na+ + e- BECAUSE Na+ has larger atomic radius than Na (T/F) +
  11. Higher temperature increases reaction rate BECAUSE Kinetic Molecular energy exceeds the activation energy (T/T CE) +</p>

<p>Section C :

  1. Which has multiple bond (CO) *
  2. Which does not form solution or something like that (CH4OH w/ NH4 OR CH4OH w/ HF)
  3. M = Alkali metal, reaction with Oxygen (2M + O2 -> M2O - Choice A) *
  4. (CuSO4 x 5H2O) *
  5. (230 KJ = 18 x 13) *
  6. This element’s type is good conductor of electricity (Carbon) *
  7. C2 (covalent network bonds) *
  8. Easiest to be oxidized (1s2 2s2 2p6 3s1) *
  9. Highest energy level for the element (3p) *
  10. Ba(SO)4 reacted with some 1.0 M X element, white colorless gas, brown gas ()
  11. When empirical formula is XO, O mass percent is 64%, find the molar mass of X (9 grams/mole X) *
  12. (K = 1 x 10 ^ -5)
  13. Separate Methyl Alcohol and Water (Distillation) *
  14. Separate KI, sand, and Iron filing (Water extraction) *
  15. Elements combining in different ratio (FeO & Fe2O3) *
  16. Which makes a solution weak acid? (CO2) *
  17. Linear shape (CO2) *
  18. As Atomic number increase in halogen (Atomic radius increases)*
  19. Order of periodic table (Increase in atomic number) *
  20. Highest Rate of Effusion (H2) *
  21. explanation of graph where line is straight (Ice melted becomes solidified)
  22. (evolves gas)
  23. Which is liquid at room temperature (Br2)
  24. Which has the highest H grams? (One with 0.6 x 16) *
  25. Something about precipitate (Fe)
  26. Which is endothermic (CO2 (s) -> CO2 (g))*
  27. Ionization constant, so which has smallest concentration? (one with smallest K)
  28. Which of these is not a redox reaction? (H+ + O2- -> H2O) *
  29. Salt dissolves in water has following properties (D or E, answer was not Higher Vapor Pressure, Higher Freezing point, Lower Melting Point)
  30. Which has the highest pressure in 1L Container? (H2)*
  31. (0.0500 x 6.02 x 10^23)*
  32. (2L x 740/760 x 273/300) *
  33. (0.5 moles H2)
  34. Which has the most Valence electrons? (Phosphorus)*
  35. Balancing Al(OH)2 (2)</p>
73

<p>Are you sure the elements combining in different ratios is FeO2 and Fe2O3 and not NO2 and N2O4?</p>

74

<p>^ yeah, i am pretty sure it’s FeO and Fe2O3. NO2 and N2O4 has same Ratio, which was tricky. </p>

<p>People, Nuclear Transformation and Nuclear Fusion choices were on the same Question Set??</p>

75

<p>Guys how much is a -10? :frowning: I think I have more than 10 wrong now…</p>

76

<p>-10 is around 740 according to Sparknotes, which isn’t saying much. The actual curve varies. Chances are, if you found it hard, everybody else did too and the curve will be more generous as a result.</p>

77

<p>People, Nuclear Transformation and Nuclear Fusion choices were on the same Question Set??</p>

78

<p>Nuclear Transformation and Fission were on same question set.</p>

<p>and again, what was the sugar vs water melting point question exactly? Because sugar melts at 150+ celsius…</p>

79

<p>I also got NO2 and N2O4 (it was the only one that was different) the iron one, there was other answers like it. And I remember I put nuclear fission for that Argon one</p>

80

<p>answer is FeO & Fe2O3,</p>