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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. The definition of acidic basic and neutral aqueous solutions is:






2. Buffer capacity must contain decent amounts of a ________ ________






3. Name 2 ways in which you can create a buffer?






4. What is the basic structure of an optical isomer?






5. What is the charge on a chlorine atom?






6. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?






7. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base






8. What is the formula for percent yield?






9. What do acids plus active metals form?






10. For a dibasic acid (H2A) - [A?]= ____ ?






11. What apparatus do you use to pour liquids?






12. Do anions flow to the cathode or anode?






13. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?






14. What is the general formula of an alkane?






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






16. What element is used to vulcanize rubber?






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






18. What do group I/II metal oxides plus water form?






19. copper sulfate






20. How many faradays of electric charge do you need to produce one mole of O2? H2?






21. How does the melting point of a mixture compare to the MP of a pure substance?






22. What is the formula for summation?






23. What type of compounds are almost always colored?






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






25. Acidic gases like SO2 in the atmosphere cause what environmental problems?






26. bromothymol






27. What do hydrocarbons form when they burn in air (oxygen)?






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






29. How does benzene compare in reactivity to alkenes?






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






31. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?






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






33. chromate






34. The oxidation numbers of the metals or nonmetals ___________ during such a reaction






35. acetates






36. What do you use for an acid spill? base spill?






37. sulfate






38. Is the freezing of ice endothermic or exothermic?






39. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?






40. hydroxide






41. How many normal boiling points and boiling points are there?






42. Alkenes are ________ and react by __________






43. bromine






44. Give an example of a concentrated weak acid.






45. What are amphoteric oxides?






46. What things should you remember to do when collecting gas over water?






47. During a titration what is present in the beaker at the equivalence point?






48. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?






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






50. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?