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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. lead compounds






2. How are non-metal oxides and hydrides bonded? are they acidic or basic?






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






4. What is the word equation for condensation polymerisation ?






5. What do you use to look at burning magnesium? why?






6. How are more active metals reduced?






7. What is the first law of thermodynamics?






8. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?






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






10. acetate






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

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12. What is the test for hydrogen?






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






14. When a cell is 'flat' What is its voltage?






15. What is the difference between equivalence point and end point of a titration.






16. What do you do to get rid of most of the solution from a precipitate?






17. dichromate






18. What is the pH of 1.0M HCl? 1M NaOH?






19. chromate






20. At what point during titration do you have the perfect buffer - and what is the pH at this point?






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






22. cyanide






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






24. phosphate






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

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26. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?






27. A Bronsted-Lowry base is...






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






29. What is the formula for alkynes?






30. chlorine






31. mercury (I) ion






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






33. What do acids plus active metals form?






34. What is the general formula for an aldehyde?






35. lead iodide






36. silver iodide






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






38. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?






39. What device would you use to measure a volume of gas?






40. copper sulfate






41. nitrate






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






43. What is the general formula for an ester?






44. What is a dipeptide? polypeptide? protein?






45. Is the freezing of ice endothermic or exothermic?






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






47. What are amphoteric oxides?






48. One mole of electrons carries 96500Coulombs - what is this quantity called?

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49. The oxidation # for acid base reactions...






50. carbonate