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S.O.L. Review

S.O.L. Review. Down to the wire!. What do you need to do now?. Eat a good dinner, go to bed at a decent hour. Be on time for school tomorrow. Eat a good breakfast and avoid excess caffeine. I will be serving snacks in my room from 8:15-8:50 Your SOL is in the library at 9:05.

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S.O.L. Review

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  1. S.O.L. Review Down to the wire!

  2. What do you need to do now? • Eat a good dinner, go to bed at a decent hour. • Be on time for school tomorrow. • Eat a good breakfast and avoid excess caffeine. • I will be serving snacks in my room from 8:15-8:50 • Your SOL is in the library at 9:05

  3. What do I need to study? • Review with your flashcards, but remember they do not cover everything • Review the chapter summaries in your textbook • Look over your notes and old tests • Look at the ppt on my website • USA Test Preps & J-Labs ARE NOT ENOUGH!!!!!

  4. Gas Laws • P, V? • P, T? • V, T? • What law does this graph represent?

  5. Chemical or Physical Change? • A banana turns brown • Water boils • Licking a lollipop • Baking bread • Soda explodes when you shake it up

  6. Safety • What do you do with waste chemicals? • Where do you find information on a chemical? • What equipment protects you from toxic vapors? • Where does broken glass go? • What do you do when you get splashed with a chemical?

  7. NaF sodium fluoride K2CO3 potassium carbonate MgCl2 magnesium chloride Be(OH)2 beryllium hydroxide Ca3(PO4)2 calcium phosphate (NH4)2SO4 ammonium sulfate Mn(NO3)3 manganese (III) nitrate FePO4 iron (III) phosphate Name these chemicals!

  8. potassium fluoride KF ammonium nitrate NH4NO3 magnesium iodide MgI2 copper (II) sulfate CuSO4 aluminum phosphate AlPO4 lead (II) nitrate Pb(NO3)2 cobalt (II) selenide CoSe silver cyanide AgCN copper (II) carbonate CuCO3 iron (II) oxide FeO Write these formulas!

  9. These are covalent, why? • SiF4 • silicon tetrafluoride • N2S3 • dinitrogen trisulfide • HBr • hydrogen bromide (or hydrobromic acid) • Br2 • bromine

  10. Write these covalent compounds? • diboron hexahydride • B2H6 • nitrogen tribromide • NBr3 • sulfur hexafluoride • SF6 • diphosphorus pentoxide • P2O5

  11. What is the empirical formula? • C2H4O2 • CH2O • methane • CH4 • C6H12O6 • CH2O

  12. What do these look like? • carbon disulfide • CS2 is linear and non-polar • boron trifluoride • BF3 is trigonal planar and non-polar • difluoromethane • CH2F2 is tetrahedral and polar

  13. Conversions . . . YEA! • 30 grams of H3PO4 • 0.31 moles • 25 grams of HF • 1.25 moles • 110 grams of NaHCO3 • 1.31 moles • 1.1 grams of FeCl3 • 0.0068 moles

  14. Moles to mass . . . • 4 moles of Cu(CN)2 • 462 grams • 5.6 moles of C6H6 • 436.8 grams • 21.3 moles of BaCO3 • 4202.5 grams • 1.2 moles of (NH4)3PO3 • 159.6 grams

  15. Moles  gas volume . . . • 25 Liters of O2 • 1.12 moles • 10 moles of N2 • 224 L • 1.0 x 105 Liters NH3 • 4460 moles • 2.35 x 10-2 moles H2O(g) • 0.527 L

  16. Percent Error • If you measured 23 out of 90 • 74.4% error • If you measured 78 out of 85 • 8.23% error • If you start with 100g but only recover 43%. • 57% error

  17. Balancing Equations • Balance equations because of the Law of Conservation of Matter: the mass of the reactants = mass of products __N2 + __H2 __NH3 __C6H12O6 + __O2 __H2O + __CO2 __Ca3(PO4)2 + __ZnCl2  __CaCl2 + __Zn3(PO4)2

  18. Percent Yield • My theoretical yield is 500g but actual recovery was only 327g • 65.4% recovery • If the recipe is written to yield 24 muffins, but you only got 21 out of them, • 87.5% recovery

  19. Molarity!!!!!!!!!!!!!!!!!!!!!!!! • What is the formula for molarity? • Molarity = moles solute/L of solution • How do you find moles if you are given mass? • Moles = mass / molar mass (periodic chart) • What is the formula for a dilution? • M1V1 = M2V2

  20. Calculate it • You have 4.5L of a solution that you added 3.15 moles of NaCl to. • 0.7M • How many moles of CuBr do you need to make 10.0L of a 3M solution? • 30 moles • What is the volume of a 6.3M solution made from 3.22moles of AgNO3 • 0.511 L or 511 mL

  21. What are these? • Isotopes? • Atomic Number? • Ions? • Trend in electronegativity? • Trend in ionization energy? • Trend in atomic mass?

  22. Random • Formula for density? • D = m/V • Kelvin conversion? • K = C + 273 • Ideal Gas Law? • PV = nRT • Specific Heat? • cp= q / m x T • pH • -log10[H3O+]

  23. What is . . . • Standard temperature and pressure? • Oxidation? • Reduction? • Arrhenius Acid/Base? • Bronsted-Lowry Acid/Base?

  24. Who is? • Thomsson? • Rutherford? • Bohr? • Mendeleev? • Moseley?

  25. What type of reaction is this? • Na + Cl = NaCl • Synthesis • H2O = H2 + O2 • Decomposition • CxHyOz + O2 = H2O + CO2 • Combustion • A + BX = AX + B • Single Replacement • AX + BY = AY + BX • Double Replacement

  26. What are these rules? • Aufbau • Hund’s Rule • Heisenberg Uncertainty Principle • Periodic Law • Pauli’s Exclusion Principle

  27. Which forces hold these atoms and molecules together? • H2O • Intramolecular: Covalent Bond • Intermolecular: Hydrogen Bonding • NaCl • Intramolecular: Ionic • Intermolecular: Ionic • NH3 • Intramolecular: Covalent • Intermolecular: Dipole-dipole

  28. Organic Compounds • Men Meth- • Eat Eth- • Popcorn & Prop- • Butter But- • Single is –ane • Double is –ene • Triple is -yne

  29. SOL Review Speed Round

  30. Read each question carefully and choose the best answer. • 1. The average kinetic energy of a sample of water molecules is • Increased as the temperature is increased • Increased as the temperature is decreased • Unaffected by temperature changes • Always equal to zero

  31. 2. The element chlorine exists as two naturally occurring isotopes. Cl-35 occurs 75% of the time and Cl-37 occurs 25% of the time. Which of the following calculations should be used to calculate the correct average atomic mass of chlorine? • A. (35 amu x .75) + (37 amu x .25) • B. (35 amu x 3) + 37 amu • 2 • (35 amu x 3) + 37 amu • 3 • 35 amu + 37 amu • 2

  32. 3. The mass of an object was recorded as 9.93 g, 9.90 g, and 10.02 g, using an electronic analytical balance. What is the average of these three masses expressed to the correct number of significant figures? • 9.9 g B. 9.95 g C. 10.0 g D. 10.00 g

  33. 4. Which of these shows a volume of 1.25 liters expressed in milliliters? A. 125 mL B. 12.5 x 101 mL C. 1.25 x 102 mL D. 1.25 x 103 mL

  34. 5. How does the radioactive isotope C-14 differ from its • stable counterpart C-12? • It has a different number of protons and two less neutrons than C-12 • It has the same number of protons and two more electrons than C-12 • It has the same number of protons but two more neutrons than C-12 • It has a different number of protons and two more neutrons than C-12

  35. 6. What is the first step that should be taken when a caustic chemical gets into a person’s eyes? • Identify the chemical • Call for an ambulance • Flush the affected area with water • Apply a neutralizing agent

  36. 7. Which of these conclusions can be drawn from Rutherford’s experiment? • Each atom contains electrons. • The nucleus of an atom can be split. • Each atom contains protons. • Atoms are mostly empty space.

  37. 8. According to the above data, which of the following represents the average density for sample X using the correct number of significant figures? A. 1 g/mL B. 0.8 g/mL C. 0.81 g/mL D. 0.821 g/mL

  38. 1. Which is the correct formula for iron (III) sulfate? • Fe3(SO4)2 B. FeSO4 • C. Fe2(SO4)3 D. Fe2(SO3)3

  39. 2. Which of these represents the empirical formula and the molecular formula, respectively, for a given organic compound? • CH and C2H2 • CH and CH4 • CH2 and C2H2 • CH3 and C3H12

  40. 3. Which of these describes a tendency for atomic radii as displayed on the periodic chart? • Atomic radii decrease left to right across a period. • Atomic radii increase left to right across a period. • Atomic radii decrease top to bottom down a group. • Atomic radii increase, then decrease from top to bottom down a group.

  41. 4. Chlorine forms a 1- ion. How many electrons does a chloride ion have? A. 1 B. 16 C. 17 D. 18

  42. ? • 5. Which of the groups below has the electron dot structure shown above? • Noble gases • Halogens • Alkali metals • Transition elements

  43. 6. An element has an electron configuration of • 1s22s22p63s2. Which of these will be in the same group as this element? • 1s22s22p6 • 1s22s22p63s23p64s2 • 1s22s22p63s1 • 1s22s22p63s23p6

  44. 7. Which of these elements is the most chemically active? A. F B. Cl C. Br D. I

  45. 1. What is the percentage of aluminum in aluminum oxide (Al2O3)? A. 47% B. 48% C. 53% D. 54%

  46. 2. A student wanted to calculate the formula for hydrated copper sulfate. After careful massing, she heated the compound to remove the water. She calculated the formula to be CuSO4 .4H2O. The actual formula was CuSO4 .5H2O. What is the most likely source of analytical error in the student’s experiment? • The water was not completely evaporated from the compound. • The actual mass of the anhydrous CuSO4 was less than the measurement. • The CuSO4 reacted with elemental copper. • The atmospheric pressure prevented complete reaction.

  47. 5. Which is an example of a synthesis reaction? • HCl + KOH  KCl + H2O • Pb(NO3)2 + 2HBr  PbBr2 + 2HNO3 • Mg + H2SO4  MgSO4 + H2 • C + O2  CO2

  48. 3MgO + 2Al  ? • 6. What would be the product(s) of this reaction? • 2Mg3Al2O3 • Mg3Al2 + 3O2 • 6Mg + Al3O2 • 3Mg + Al2O3

  49. 7. Using the chart above, which of these combinations will probably form a precipitate? A. Ammonium chloride B. Barium bromide C. Calcium chromate D. Copper (II) carbonate

  50. 8. • Very Active Metal + Water  Metal hydroxide + ? • Which of these completes this reaction? • Oxygen • Hydrogen • Metal oxide • Air

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