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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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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. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Pale yellow
Ksp = 4s³
Insoluble (except group 1 ammonium and Ba)
CH3COO?

2. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
different forms of the same element
Insoluble except nitrate and acetate

3. carbonates
Insoluble except group 1 and ammonium
#ligands=charge x2
Current - time and charge on ion (moles of e used in half cell reaction)
same KE - but PEice<PEwater

4. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Anode - oxygen. Cathode - hydrogen
T increases exponentially the proportion of molecules with E > Ea
How close results are to the accepted value
non-metal oxides and hydrides are covalently bonded and are acidic.

5. hypochlorite
ClO?
acids
Kc=Kp
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

6. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Big K=kf/kr
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Concentration
The dilution effect when the solutions mix. M1V1 = M2V2

7. How do you heat a test tube?
T increases exponentially the proportion of molecules with E > Ea
metal oxides and hydrides are ionically bonded and basic
SO4²?
Heat a test tube at an angle at the side of the tube (not bottom)

8. What is the formula for alkanes?
Perform ICE BOX calculation based on K1
catalyst=conc H2SO4
CnH2n+2
blue glass - it filters UV

9. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
benzene is less reactive than alkenes
Purple
Initiation energy (NOT Ea)

10. What measuring device would you use for very small volumes of liquids?
|experimental - accepted|/accepted X 100
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
CnH2n+2
Pipette (burette if need repetition)

11. During a titration what is present in the beaker at the equivalence point?
Sigma bonds are stronger than pi bonds
It ceases - the circuit is broken.
A salt solution.
CnH2n+1 often designated 'R' ex C3H7 is propyl

12. Acid plus base make?
Salt + water.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
water and substances with (s) less dense than
CO3²?

13. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
Heat a test tube at an angle at the side of the tube (not bottom)
water and substances with (s) less dense than
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

14. Does Kw increase or decrease with T? Why?
Group I metals (soft metals) are stored under oil
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
by electrolysis
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

15. ammonium/ammonium compounds
Acid rain - dissolves marble buildings/statues and kills trees.
-Ea/R
#ligands=charge x2
Soluble

16. What is the sign of the anode in voltaic cells? in electrolytic cells?
The dilution effect when the solutions mix. M1V1 = M2V2
Acids; HCOOCH3 is an ester
voltaic: - electrolytic: +
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

17. What is the charge on a chlorine atom?
zero-th: decreases - first: constant - second: increases
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
zero
blue glass - it filters UV

18. What do you need to make a polymer?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
How grouped results are
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)
S crystal at 0K=0

19. thiosulfate
CnH2n
ROR
S2O3²?
voltaic: + electrolytic: -

20. What shape is carbon dioxide?
Mono; di; tri; tetra; penta; hexa.
linear
benzene is less reactive than alkenes
Ksp = 108s5

21. If Q < Ksp a ppt ______
zero
Glacial acetic acid
Ppt will NOT form (unsaturated)
zero

22. What is the catalyst for this reaction Ester + ?
K2
Only temperature
Concentration
catalyst=conc H2SO4

23. A Bronsted-Lowry acid is...
Q=It (time in seconds)
proton donor base
RNH2
CO (poisonous)

24. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Saturated - Substitution (which requires more radical conditions)
H+
catalyst=conc H2SO4
Sigma bonds are stronger than pi bonds

25. Ca - Sr - Ba
hydroxides (ex: Ba(OH)2)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
zero
The Faraday or Faraday's constant.

26. When driving off water from a hydrate - how do you tell you're done?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Ksp = 4s³
How grouped results are
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)

27. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
voltaic: + electrolytic: -
Ksp = 108s5
C2O4²?
Supercooling can occur when cooling a solvent or solution. It occurs when there's a dip and then a rise back up to the melting point on a cooling curve.

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

29. How do you get the equation for a net electrolysis reaction?
10?8
Combine the equations for the half reactions in the non-spontaneous direction
C4H10
water and substances with (s) less dense than

30. At what point during titration do you have the perfect buffer - and what is the pH at this point?
boiling without losing volatile solvents/reactants
Increases down group 1 decreases down group 17
At half equivalence - pH=pKa
Glacial acetic acid

31. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
R=8.31 J/mol/K

32. Give an example of a dilute strong acid.
HClO4
zero-th: decreases - first: constant - second: increases
Insoluble except nitrate and acetate
Unsaturated - addition (ex: decolorize bromine solution)

33. Aromatic compounds contain what?
ionic and form hydrogen and hydroxide
The benzene ring (or more correctly the phenyl group - C6H5)
RCHO (carbonyl at end)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

34. Lattice energy is high for ions with _____ size and _____ charge
acid + alcohol
benzene is less reactive than alkenes
small size and high charge
no - they're written undissociated (HAaq)

35. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
RX
Ksp = 108s5

36. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
More chaotic (ex: gases made)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
non-metal oxides and hydrides are covalently bonded and are acidic.
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

37. BaSO4
The dilution effect when the solutions mix. M1V1 = M2V2
Both electrons come from the same atom (just as good as a regular bond)
Insoluble
redox reaction

38. What changes Keq?
?G= -ve - E°= +ve
OH?
Only temperature
ion pairing

39. When a cell is 'flat' What is its voltage?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
zero
linear
Clear

40. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
voltaic: - electrolytic: +
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
hydroxides (ex: Ba(OH)2)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

41. Nonmetals are good _____ agents. Metals are good _______ agents.
Synthetic condensation polymer (aka a polyamide)
q=mc?T q=mL (or n x ?h)
Transition element compounds (except if it has a full or empty d shell)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

42. nitrate
NO3?
Only temperature
ClO2?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

43. bromothymol
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
blue (BTB)
Insoluble except for nitrate and acetate
Group 1 hydroxides (ex: NaOH)

44. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
10?8
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)
blue

45. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Acid rain - dissolves marble buildings/statues and kills trees.
CO3²?
methyl formate
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

46. dichromate (soln + most solids)
HClO4
Orange
zero
Iodine and CO2 (dry ice)

47. Color is due to ______ _______ of light.
NH4?
Selective absorption
ROH
acids

48. What is the second law of thermodynamics?
Suniverse increases for spontaneous processes
Q=It (time in seconds)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
allow for the vapor pressure of water and make sure to level levels

49. Which would cause the bulb in a conductivity apparatus to be brightest?
OH?
0.10M HCl (more ions)
At half equivalence - pH=pKa
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)

50. Does reactivity increase/decrease going down group 1 and group 17?
?G= -ve - E°= +ve
Increases down group 1 decreases down group 17
non-metal oxides and hydrides are covalently bonded and are acidic.
NH4?