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MRS. TAYSI’S CHEMISTRY FINAL REVIEW

This review covers various topics in chemistry, including lab safety, experimental vocabulary, chemical equations, element identification, combustion, alloys, separation techniques, and stoichiometry. Study these concepts to prepare for your chemistry final!

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MRS. TAYSI’S CHEMISTRY FINAL REVIEW

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  1. MRS. TAYSI’S CHEMISTRY FINAL REVIEW REVIEW TO SUCCEED! STUDY, STUDY, STUDY. These are meant to help you study—examples are given, but not necessarily all the answers!

  2. 1. What is chemistry? Two things: • Study of matter • How matter changes

  3. 2. What is science? Is it • Predictive? YES • Reproducible? YES • Definitive? NO • Testable? YES • Tentative? YES

  4. 3. Lab safety rules. • What should you do if you spill a base or an acid on the lab bench? Your skin? • How should you heat a test tube? • How should you dispose of broken glass? • How do you use a fire extinguisher?

  5. 4. Lab equipment Be familiar with the following pieces of equipment: • Beaker • Graduated cylinder • Test tube • Eye dropper • Erlenmeyer flask Which of the above is most precise in measuring liquid volume?

  6. 5. Chemical Equations BaCO3(s) + 2HCl(aq)  H2O(l) + CO2(g) + BaCl2(aq) Which represents/means:  • Solid, liquid, gas, dissolved in water • Yields or produces • Formula • Coefficient, subscript • Reactants • Products

  7. 6. Experimental vocabulary Be able to identify the following for an experimental situation: • Independent variable—what you are testing or experimenting with; what YOU change • Dependent variable—what you are measuring about the IV; what you expect to change • Controlled variables—what you keep the same between both the experimental and control groups

  8. 6. Experimental vocabulary • Experimentation—observe, hypothesize, collect, analyze & report data (the whole thing) • Hypothesis—educated guess; what you think will happen & why (If...then…) • Interpretation—an explanation of an observation (It turned blue because…) • Quantitative data—numbers (15 sec, 25 mL) • Qualitative data—word descriptions (blue, red)

  9. 6. Experimental vocabulary • Trials—repetitions of the experiment to be sure of results • Experimental group—group that has the experimental variable applied to it • Control group—group that is left alone; the “normal” situation; done for comparison and not always possible to do for all experiments

  10. 6. Experimental vocabulary • Take the hamburger lab and try to identify the different parts of the experiment.

  11. 7. Potential energy diagrams

  12. 8. Identify as elements, compounds or mixtures: • O2 • H2O • air • water • sodium iodide • tellurium

  13. 9. Element formulas • BrINClHOF—all are diatomic • P4 • S8 • All the rest are monoatomic

  14. 10. Atom or molecule? Element or compound? • Xe • SF6 • PCl3 • Mn

  15. 11. Identify as physical or chemical changes

  16. 12. AIR? • What is in air? • Is it an element, compound or mixture?

  17. 13. Combustion • Combustion—burning of a hydrocarbon compound in the presence of oxygen. • Complete combustion—plenty of oxygen present, so CO2 and H2O are formed. • Incomplete combustion—not enough oxygen is present, so CO instead of CO2 is produced, along with water.

  18. 14. Burner flame—where’s the hottest part, and how did we figure it out?

  19. 15. Alloys • Alloy— mixture of 2 or more metals • Brass? zinc & copper • Steel? iron & carbon(exception—nonmetal!)

  20. 16. Types of steel & crystal size • Annealed heated and then slowly cooled • Hardened heated and then quickly cooled • Tempered heated and cooled slowly several times • What happens to crystal size when cooled quickly? Slowly?

  21. 17. Separation techniques • Electrolysis water was separated into its elements using electricity • Chromatography a pen ink mixture was separated into its component pigments using water

  22. 18. Balancing equations • Practice makes perfect! ___ H2 + ___ O2 ___ H2O ___ S8 + ___ O2  ___ SO2 ___ NaCl + ___ Fe(OH)3  ___ NaOH + ___ FeCl3

  23. 19. Mass  mole conversions • Remember to use the periodic table: • How many moles is 24.0 g of iron? • How many grams is 2.25 moles of nitrogen gas? 24.0g Fe x 1 mole Fe 1 55.8g Fe 2.25 mol N2 x 28.0 g N2 1 1 mol N2

  24. 20. Stoichiometry—mass to mass • Balance this equation: ___ H2 + ___ O2 ___ H2O • How many grams of water will be produced from reacting 32.0 g of oxygen gas with excess hydrogen?

  25. 21. Stoichiometry—mole to mole • Balance this equation: ___ H2 + ___ O2 ___ H2O • How many mol of hydrogen gas is needed to react with 4.00 mol of oxygen gas?

  26. 22. Mass to particles • 56.0 g nitrogen gas has how many particles?

  27. 23. Particles to mass • 1.5 x 1024 particles of hydrogen gas equals how many grams of hydrogen gas?

  28. 24. Reaction types—name these: • 6. A + BC  AC + B ________________ • 7. CH4 + O2 CO2 + H2O _______________ • 8. AB + CD  AD + CB _______________ • 9. A + B  AB ________________ • 10. AB  A + B _________________ • 11. Na + Cl2 NaCl _________________ • 12. C2H6 + O2 CO2 + H2O _____________ • 13. CaF2 + Na3PO4 Ca3(PO4)2 + NaF _____ • 14. CaCO3 Ca + CO2 ______________ • 15. Al + CuSO4  Al2(SO4)3 + Cu __________

  29. 25. Identify the metric unit for each: • Temperature • Volume • Distance • Mass • Density

  30. 26. Density calculation • A graduated cylinder with water in it has a volume of 24.5 mL. When a rock with a mass of 25.0g is placed in the cylinder, the water volume increases to 28.3 mL. What is the density of the rock?

  31. 27. Mass calculation given density • A block with dimensions of 1.0cm by 2.5cm by 4.2cm. If the density of the block is 0.57 g/cm3, what is the mass of the block?

  32. 28. Light phenomena What type of light phenomena is each example/description? • Glow in the dark silly putty • Fireworks • Brightly colored packaging • Light energy is absorbed and then is given off gradually over time • Electrical or heat energy is taken in by electrons and light energy is given off

  33. 29. EM spectrum • Which is higher in energy? gamma rays or UV radio waves or green light • Which is lower in energy? microwaves or radiowaves infrared light or yellow light

  34. 30. Protons, electrons, neutrons & isotopes • What particle determines the isotope of an element? • What particle determines the charge of an ion? • What particle determines the identity of an element? • How is lithium-6 different from lithium-7?

  35. 31. PEN, etc… • What type of atom has 5 protons in its atom? • What is the atomic number of tungsten? • Oxygen-18 has how many neutrons? • A fluoride-19 ion (F-) has how many protons? neutrons? electrons? • What is the charge on a sulfur atom that has 18 electrons?

  36. 32. Alpha, beta & gamma radiation • Rank alpha, beta & gamma in order of ability to penetrate substances, lowest to highest. • Rank alpha, beta & gamma in order of size, smallest to largest.

  37. 33. Groupings on the periodic table • Make sure you have all 15 groups labeled correctly on your periodic table: Metals, nonmetals & metalloids Alkali metals, alkaline earth metals, transition metals, inner transition metals, lanthanides, actinides, B, C, N & O groups, halogens and noble gases

  38. 34. Ion formation using octet rule • What type of ion would sulfur form? • What type of ion would sodium form? • What type of ion would magnesium form? • What type of ion would chlorine form?

  39. 35. The duet rule • Which two elements obey the “duet” rule and why?

  40. 36. Electron configurations Be sure to bring your orbital diagram worksheets to the test!! Know how to use them! • What is the full electron configuration for copper? • Shorthand for copper? • What is the full electron configuration for strontium? • Shorthand for strontium?

  41. 37. Chemical Families • Why do chemical families on the periodic table exhibit similar properties?

  42. 38. Lewis/Electron dot structures • What is the electron dot structure for each of the following elements? (remember the general rule—doesn’t work for transition elements) lithium antimony xenon zirconium

  43. 39. Bond types (metals or nonmetals?) • Covalent bonds involve what types of elements? • Ionic bonds involve what types of elements?

  44. 40. Bonding & electronegativities • Using the electronegativities chart determine the type of bonding for the following formulas: • MgS • N2 • SiO2 • NO2

  45. 41. Bond type using metal/nonmetal rules • Using the metal/nonmetal rules determine the type of bonding for the following formulas: • MgS • N2 • SiO2 • NO2

  46. 42. Molecular Shapes For each formula, determine the shape of the molecule produced: • SiH4 • H2S • BeCl2 • BF3 • NCl3

  47. 43. Solubility and polarity Determine whether or not the following pairs are soluble or insoluble: • H2O and NaI • H2O and CF4 • SiH4 and NCl3

  48. 44. Determining partial charges Draw the bar diagram and label each formula with the proper d+ and d- charges. • CH2F2 • CH4 • H2S

  49. 45. Polarity and chromatography • Why did the Sharpie pen move in ethanol and acetone, but not water? • Be able to use lab results to tell whether an ink is polar or not.

  50. 46. Water and Mickey Mouse • If water is Mickey Mouse, what element represents the face and what represents the ears?

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