AP Chem: unit 2 quiz

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  1. solute
    the dissolved material
  2. solvent
    dissolving medium
  3. in an aqueous solution, what is the solvent?
    water
  4. water can dissolve ______________ (polar/nonpolar)
    polar
  5. electrolyte
    when dissolved in water, allows solution to conduct electricity
  6. What is the difference between strong and weak electrolytes?
    • strong: all of compound dissociates into ions
    • weak: only a few ions of the compound seperate
  7. does a nonelectroylte dissolve in water, even if it doesnt break into ions?
    yes
  8. Which ionic compounds are generally soluble?
    • NO3
    • C2H3O2
    • Cl
    • Br
    • I
    • SO4
  9. What are the exceptions for Cl?
    Ag, Hg, Pb
  10. What are the exceptions for Br?
    Ag, Hg, Pb
  11. What are the excpetions for I?
    Ag, Hg, Pb
  12. Which compounds are generally insoluble in water?
    • S
    • CO3
    • PO3
    • OH
  13. What are the excpetions for S?
    • NH4
    • alkali metals
    • Ca, Sr, Ba
  14. What are the exceptions for CO3?
    • NH4
    • alkali metals
  15. What are the exceptions for PO4?
    • NH4
    • alkali metals
  16. What are the exceptions for OH?
    • alkali metals
    • Ca, Sr, Ba
  17. What is the molecular equation?
    everything written in standard formulas
  18. What is the complete ionic equation?
    strong ions represented as strong ions
  19. molarity equation?
    moles of solute/liter of solute
  20. definition of acids.
    • produces H+
    • proton donor
  21. define base.
    • produces OH
    • proton acceptor
  22. equivalence point
    known reacts exactly with unknown (no excess)
  23. indicator
    changes color near equivalence point
  24. end point
    point where indicator actually changes color
  25. titration
    measured volume of solution of known concentration reacts with solution of unknown concentration
  26. what are the seven steps to balancing redox reactions in acidic solutions?
    • 1) write half reactions
    • 2) balance all elements except H and O
    • 3) balance O with H2O
    • 4) balance H with H+
    • 5) balance charge with e-
    • 6) multiply both or one reactions to get the same number of e- on both sides
    • 7) add half reactions and cancel
  27. What is the extra step to balancing redox reactions in basic solutions?
    add OH- to both sides of equation to eliminate H+
  28. When does O have an oxidation state that is not -2?
    in peroxides (H2O2)
  29. When does H have an oxidation state that is not +1?
    In metal hydroxides (LiH)

Card Set Information

Author:
 alipeace11
ID:
 108568
Filename:
 AP Chem: unit 2 quiz
Updated:
2011-10-13 02:19:23
Tags:
AP chem
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Description:
note sheets: reaction in aqueous solutions, intro to acid-base reactions, intro to redox reactions
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