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EOC review

EOC review. Data analysis/ experimental design . Pages 2 and 3. Accuracy . How close a measured value is to an accepted value. Precision. Refers to how close a series of measurements are to one another. Independent variable. A variable that is changed by the scientist. Dependent variable .

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EOC review

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  1. EOC review

  2. Data analysis/ experimental design

    Pages 2 and 3
  3. Accuracy How close a measured value is to an accepted value
  4. Precision Refers to how close a series of measurements are to one another
  5. Independent variable A variable that is changed by the scientist
  6. Dependent variable the variable measured in the experiment
  7. Quantitative data Observations based on quantities (numbers)
  8. Qualitative data Observations based on characteristics
  9. Theory An explanation supported by many experiments
  10. Scientific law Describes a relationship in nature
  11. 2.Explain how experimental data can be produced with good precision but poor accuracy All of the measurements can be close to the same value (precision) but not be the correct value (accuracy)
  12. 3. Which student has the highest precision? Student A Which student has the highest accuracy? Student B
  13. 4. Which of the following is most likely to produce data that is not precise A. a balance that is not set to zero B. not reading a graduated cylinder at eye level C. altering the procedure during an experiment D making the same error with each trial
  14. 4. Which of the following is most likely to produce data that is not precise A. a balance that is not set to zero B. not reading a graduated cylinder at eye level C. altering the procedure during an experiment D making the same error with each trial
  15. 5. How many significant figures? A. 304,002 --> 6 significant figures B. 0.00167  3 significant figures C. 0.0030  2 significant figures D. 30,020  4 significant figures E. 6.200x 103  4 significant figures F. 800  1 significant figure
  16. Convert each into scientific notation 5000  5.0x103 123,500  1.235x105 Convert into standard notation: 2.40x 10-3  .00240 2.975 x 105  297500
  17. 7. Answer the following with the appropriate amount of significant figures: a) 5.000 x 2.0000 x 3.000 = 30.00 b) 5.000 x 2.0 x 3.000 = 30. c) 0.0003047 – 4 = -4 d) 3.14 + 6.2 + 1.618 = 11.0
  18. 8. A 7.2 mL sample of liquid has a mass of 6.330 g. What is the density? Show all work and usecorrect sig. figs. D = m v D = 6.330 = .88g/mL 7.2
  19. 9. What is the density of a 2.0 centimeter cube that has a mass of 5.2 grams? Show all work and usecorrect sig. figs. D = m V=LxWxH v 8.0= 2.0 x 2.0 x 2.0 D = 5.2 = .65g/cm3 8.0
  20. 10. Convert 6800cm 1m = 68m 100 cm 2.05 moles 6.02x 1023 = 1.23 x 1024atoms 1 mole 3. 75x 1024 1 mole = 6.23 moles 6.02x 1023

  21. Atomic theory/ periodic table/ isotopes

    Pages 4 and 5
  22. 11. Define ATOM- smallest particle of an element ISOTOPE- same number of protons (same element) but different number or neutrons
  23. 12. Explain how a student would find…. Mass number- Add protons + neutrons Atomic mass- average mass of all the isotopes that occur in nature (periodic table) Atomic number- number of protons
  24. Complete the table 66 30 106 46
  25. 14. Argon has three naturally occurring isotopes with abundances of 0.337 %, 0.063 %, and 99.60 %. If the masses of the isotopes are 35.968 amu, 37.963 amu, and 39.962 amu,respectively, what is the average atomic mass of natural argon? Show all work. (.00337 x 35.968) + (.00063x 37.963) + (.9960 x 39.962) = 39.96 amu b. Why is the average atomic mass of argon closet to the value 39.962 amu? Majority of the isotopes weigh 39.962 amu
  26. 15. Cirlce the atoms that are isotopes: B, C, E The three choices are isotopes because they all have 8 protons.
  27. Daltons 4 postulates 1. Everything is made of atoms 2. Not all atoms are alike. 3. Atoms combine to form compounds in whole number ratios 4. A chemical reactions is the rearranging of atoms.
  28. 17.
  29. 18. Describe relative charge and location relative to the nucleus for each of the following Neutron- neutral charge, relative size of 1, found in the nucleus Proton- positive charge, relative size of 1, found in the nucleus Electron- negative charge, relative size of 1/1840 , found in the electron cloud

  30. Electrons- EOC review

    Pages 6 and 7
  31. Ground state- Lowest energy level (closest to the nucleus)
  32. Excited State When an electron gains a quantum of energy it can move up and occupy a higher energy level. The electron in the higher level is in an excited state.
  33. Quantum Minimum amount of energy that can be gained or lost by an atom
  34. Long Wavelength Short Wavelength Low energy High Energy X-Rays Radiowaves Microwaves Ultra-violet GammaRays Infrared. Low Frequency High Frequency Visible Light 700 nm 600 nm 500 nm 400 nm Visible light is only a small part of the larger ELECTROMAGNETIC SPECTRUM
  35. As the frequency of an electromagnetic wave increases, the wavelength DECREASES and the energy of the wave INCREASES.
  36. When an electron moves to a higher energy level it ABSORBS energy. When an electron falls to a lower energy level it EMITS energy which we see as visible light.
  37. Explain what caused the emission of light The emission of light is produced when an electron falls to a lower energy level.
  38. Explain why each element burned a different color Each element requires a different quantum of energy to be released.
  39. What is the equation that relates frequency and wavelength? C= f λ C= 3.00x108 m/s (it is a constant!) λ= (lamda) wavelength (m) F= frequency (Hz)
  40. What is the equation that relates frequency and energy? E=hf E= energy (J) h = plancks constant= 6.63x 10-34JxS F = frequency (hz)

  41. Ionic and Covalent compounds

    Pages 8 and 9
  42. 30. List properties of Ionic and Covalent compounds
  43. 31.List the steps to writing the name of an ionic compound Ionic: Name the cation regularly If the anion is a nonmetal change the ending to –ide If the anion is a polyatomic – use the name of the polyatomic If you have a transition metal – the charge goes in parentheses
  44. 31.List the steps to writing the name of A covalent compound Covalent: Use prefixes before the names (do not use mono before the first element) The second NM should begin with a prefix and end in –ide
  45. 32. Name each of the following compounds: a) BaF2Barium Fluroide b) CuSO4Copper (II) Sulfate c) NH4HCO3Ammonium hydrogen carbonate d) Sn(OH)4 Tin (IV) Hydroxide e) CoCl2Cobalt (II) chloride f) Mn3(PO4)2Manganese (II) Phosphate g) Cd(CO3) Cadmium (II) carbonate h) P2F7Diphosphorousheptafluoride i) SO3Sulfur trioxide j) CCl4Carbon tetrachloride
  46. 33. List the steps to write the chemical formula Ionic- 1. write the symbol for each element 2. write the charges as superscripts on top 3. criss cross the charges 4. reduce as needed
  47. 33. List the steps to write the chemical formula Covalent- 1. use prefixes in the names as subscripts in the formulas
  48. 34. Write the correct ionic compound a) Silver nitrate AgNO3 b) Iron(III) sulfate Fe2(SO4) 2 c) Lead(II) phosphate Pb3(PO4)2 d) Sodium hydroxide NaOH e) Aluminum fluoride AlF3 f) Magnesium oxide MgO g) Copper(II) chloride CuCl2 h) Potassium chromate K2CrO4
  49. 35. Write the compounds for the covalent compounds a) HexanitrogenoctoxideN6O8 b) Sulfur pentoxideSO5 c) DiphosphorusdecachlorideP2Cl10 d) Arsenic nonafluorideAsF9

  50. Moles/percent comp/ empirical and molecular

    Pages 10 and 11
  51. Define a mole 1 mole = 6.02x1023atoms 1 mole = the formula mass
  52. 37. How would a student calculate the molar mass of an element/compound 1. Separate out the elements 2. look up and record atomic mass of each element 3. multiply atomic mass by subscript number 4. add them all together
  53. 38. a) Calculate the molar mass of Ca(NO3)2? Ca: 40.08 x 1 = 40.08 N: 14.007 x 2 = 28.014 O: 15.999x 6 = 95.994 40.08+28.014+95.994 = 164.088g/mol
  54. 38. a) Calculate the molar mass of ammonium chloride Write the formula following ionic rules: NH4Cl N: 14.007 x 1 = 14.007 H: 1.008 x 4 = 4.032 Cl: 35.453 x 1 = 35.453 14.007+4.032+35.453 = 53.492g/mol
  55. 39a) How many moles are there in 19.5 grams of Ca(NO3)2? 19.5 g Ca(NO3)2 1 mole = .119 moles 164. 088g Molar mass of Ca(NO3)2
  56. 39B. How many grams are in 7.45x1020 molecules of Ca(NO3)2? 7.45x1020 atoms 1 mole 164.088g 6.02x1023 1 mole Atoms Answer: .203 grams Avogadros number Molar mass of Ca(NO3)2
  57. 39c. How many Molecules are in 9.85 grams of ammonium oxide? 9.85 grams 1 mole 6.02x1023 molecules 52.077g 1 mole Formula: (NH4)2O Answer: 1.14x1023 Molecules Molar mass of Ca(NO3)2 Avogadros number
  58. 40. Calculate the percent composition of each element in the compound ammonium phosphate. Ionic formula (NH4)3 PO4 N: 14.007 x 3 = 42.021 H: 1.008 x 12 = 12.096 P: 30.974 x 1 = 30. 974 O: 15. 999x 4 = 63. 999 149.087 g/mol N: 42.021 x 100 = 28.19% H:12.096 x 100 = 8.11% 149.087149.087 P: 30.974 x 100= 20.78 O: 63.996 x 100 = 42.93% 149.087 149.087 Molar mass
  59. 41. Label the following formulas as empirical or molecular. If it is molecular, determine the empirical formula. a) C6H12O6 Molecular – empirical : CH2O b) PbO2 Empirical c) Fe2O3 Empirical d) C4H8Cl2 Molecular – empirical C2H4Cl Empirical- all the way reduced Molecular- not reduced
  60. 42. Determine the empirical formula and molecular formula of ibuprofen if the percent composition is75.7% carbon, 8.80% hydrogen, and 15.5% oxygen. The molar mass of the molecular formula is 412g/mol.
  61. Empirical and molecular steps Empirical Percent to grams Grams to moles divide by small Multiply until whole Molecular Molecular weight = Molar mass of empirical weight Multiply the subscripts in the empirical by this answer
  62. Not a whole number. Multiply by 2 to Make it a whole number 42. Empirical C: 75.7g 1 mol = 6.3 mol= 6.5 x2 = 13 12.011 g .969 mol H: 8.80g 1 mol = 8.73 mol = 9 x 2= 18 1.008g .969 mol O: 15.5g 1 mol = .969 mol = 1 x2 =2 15.999g .969 mol Empirical Answer: C13H18O2 Divide by smallest mole
  63. 42. Molecular Empirical Answer: C13H18O2 Find the molar mass of the empirical formula: Molar mass = 206g/mol Molecular mass = 412 = 2 Empirical mass 206 Molecular answer C26H36O4 Multiply the subscripts in the empirical formula by this number!
  64. 43. Determine the empirical and molecular formula of epinephrine if it contains 59.0% carbon, 7.1% hydrogen, 26.2% oxygen, and 7.7% nitrogen by mass. The molar mass of the molecule is 180 g/mol.
  65. 43. Empirical C:59g 1 mol = 4.9 mol= 9 12.011 g .54 mol H: 7.1g 1 mol = 7.04 mol =13 1.008g .54 mol O: 26.2g 1 mol = 1.64mol = 3 15.999g .54 mol N: 7.7g 1 mol = .54 mol = 1 14.007 .54 mol Empirical Answer: C9H13O3N Divide by smallest mole
  66. 43. Molecular Empirical Answer: C9H13O3N Find the molar mass of the empirical formula: Molar mass = 180g/mol Molecular mass = 180 = 1 Empirical mass 180 Molecular answer C9H13O3N *The molecular formula and empirical formula can be the same! Multiply the subscripts in the empirical formula by this number!
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