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AP Chemistry 2

Subjects : science, ap, chemistry
Instructions:
  • Answer 50 questions in 15 minutes.
  • If you are not ready to take this test, you can study here.
  • Match each statement with the correct term.
  • Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.
1. phosphate






2. Which of the rates changes more when temperature is increased?






3. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?






4. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?






5. Esterification is...






6. How are metal oxides and hydrides bonded? are they acidic or basic?






7. thiosulfate






8. If Q < Ksp a ppt ______






9. How are strong ones written?






10. When can supercooling occur? What does it look like on a cooling curve?

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11. How do you identify which is oxidized or otherwise?






12. What do metal oxides plus acids form?






13. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?






14. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?






15. What effect does increasing the size/surface area of a voltaic cell have on the cell?






16. Is the freezing of ice endothermic or exothermic?






17. What are the prefixes for the naming of binary molecular compound formulas (up to six)






18. How does benzene compare in reactivity to alkenes?






19. Lattice energy is high for ions with _____ size and _____ charge






20. What do the 'a' and 'b' in Van Der Waal's equation allow for?






21. ammonium






22. When combining half equations - what do you do to E° values when multiplying coefficients?






23. What is the general formula for an acid?






24. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?






25. What do group I/II metal oxides and acids form?






26. What type of compounds do metals/non metals form?






27. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?






28. What is the sign of the cathode in voltaic cells? in electrolytic cells?






29. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium






30. What are the signs for ?G and E° for spontaneous reactions?






31. How do you dilute an acid?

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32. How do you clean a buret/pipette for a titration?






33. How many ligands attach to a central ion in a complex ion?






34. What steps do organic labs consist of?






35. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)






36. What process do you use to obtain the precipitate from a solution?






37. What do metal oxides plus non- metal oxides form?






38. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?






39. Name C7H16






40. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?






41. copper sulfate






42. Generally - which oxy acid is strongest?






43. What is the energy you must put into a reaction to make it start called?






44. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?






45. iodine - iodine solution - iodine vapor






46. ________ are Lewis bases - because they can donate a lone pair of electrons.






47. What shape is methane?






48. chromate ion (soln + most solids)






49. Name some properties of Group 17






50. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?