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AP Chemistry 2

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. perchlorate
Pale purple - (orange)-yellow - red - blue - green.
Only temperature
ion pairing
ClO4?

2. acetate
Hg2²?
bright yellow
CH3COO?
q=mc?T q=mL (or n x ?h)

3. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Greenish-yellow gas

4. Why are i factors (Van't Hoff factors) often less than ideal?
RX
ion pairing
left - ppt will form
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)

5. What is the general formula for a ketone?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Anode - oxygen. Cathode - hydrogen
RCOR
CO (poisonous)

6. What do the 'a' and 'b' in Van Der Waal's equation allow for?
zero
a-IMFs - b-molecular volume
They stay the same.
Group I metals (soft metals) are stored under oil

7. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
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)
E=q + w (negative is by system - positive is on system)
Disulfur dichloride
They stay the same.

8. What do metal oxides plus non- metal oxides form?
ClO3?
NO3?
Salts (ex: CaO + SO2 ? CaSO3)
Decant

9. lead compounds
Soluble
They stay the same.
It ceases - the circuit is broken.
Insoluble except nitrate and acetate

10. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
K1 x K2
NH4?
Soluble
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

11. What device would you use to measure a volume of gas?
Eudiometer
metal oxides and hydrides are ionically bonded and basic
CnH(2n+2)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

12. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
look for changes in oxidation # - the one that goes up is oxidized and is the RA
boiling without losing volatile solvents/reactants
Big K=kf/kr

13. What effect does increasing the size/surface area of a voltaic cell have on the cell?
zero
strong acids/bases are written as H+ or OH- ions
water and substances with (s) less dense than
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

14. What is Big K in terms of kf and kr?
CrO4²?
Big K=kf/kr
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Nothing

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

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16. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Q=It (time in seconds)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Current - time and charge on ion (moles of e used in half cell reaction)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

17. What reacts with an acid to create hydrogen gas?
An active metal.
basic
same KE - but PEice<PEwater
Anode - oxygen. Cathode - hydrogen

18. permanganate
Conjugate pair (one must be a weak base or acid)
The one with most oxygen atoms (highest oxidation number)
CO2 and H2O
MnO4?

19. Which of the rates changes more when temperature is increased?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
do not change
A) any range. b) 8-10 c) 4-6
look for changes in oxidation # - the one that goes up is oxidized and is the RA

20. If ?S is positive - are the products more or less chaotic than the reactants?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
More chaotic (ex: gases made)
A salt solution.
Sigma bonds are stronger than pi bonds

21. Alkenes are ________ and react by __________
voltaic: + electrolytic: -
Unsaturated - addition (ex: decolorize bromine solution)
Mono; di; tri; tetra; penta; hexa.
K1 x K2

22. What is the formula of copper (II) phosphate?
PO4³?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
CnH(2n+2)
Cu3(PO4)2

23. ammonium/ammonium compounds
RCOOH
Soluble
Cu3(PO4)2
The one with most oxygen atoms (highest oxidation number)

24. What type of solutions do small - highly charged cations tend to form?
Trigonal pyramidal
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
zero

25. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Disulfur dichloride
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
ClO?
A) any range. b) 8-10 c) 4-6

26. What do you need to make a polymer?
Most INsoluble except group 1 and ammonium
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
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)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

27. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
are less dense than water
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
PO4³?

28. dichromate
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Disulfur dichloride
Ionic compounds
Cr2O7²?

29. What is the second law of thermodynamics?
HClO4
They decrease (or could be the same if the solid has ONLY JUST disappeared)
The dilution effect when the solutions mix. M1V1 = M2V2
Suniverse increases for spontaneous processes

30. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
voltaic: - electrolytic: +
Group I metals (soft metals) are stored under oil
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

31. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
|experimental - accepted|/accepted X 100
linear
water and substances with (s) less dense than
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)

32. Are weak acids (and bases) written dissociated?

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33. Where are group I metals stored?
Kc=Kp
Group I metals (soft metals) are stored under oil
Anode
Making sigma bonds and holding lone pairs

34. What do group I/II metal oxides plus water form?
ROH
bases
K1 x K2
Cr2O7²?

35. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
Trigonal pyramidal
Good catalysts - form multiple oxidation states - often paramagnetic - good structural metals - form a host of alloys (similar sized atoms) - have similar I energies (inner filling)
Most INsoluble except group 1 and ammonium

36. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
CO3²?
Acids; HCOOCH3 is an ester
Anode - oxygen. Cathode - hydrogen
Selective absorption

37. What is the relationship in strength between sigma and pi bonds?
Greenish-yellow gas
Synthesis - separation and purification of the product and its identification.
PO4³?
Sigma bonds are stronger than pi bonds

38. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
Heat a test tube at an angle at the side of the tube (not bottom)
NH4?
CO (poisonous)

39. What process do you use to separate two liquids with different boiling points?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
CnH2n-2
fractional distillation
Ksp = 27s4

40. What are two substances that sublime at 1 atm when heated?
Purple
Acids; HCOOCH3 is an ester
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Iodine and CO2 (dry ice)

41. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
C2O4²?
Ksp = 4s³
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Pale purple - (orange)-yellow - red - blue - green.

42. Alkanes are _________ and react by _________
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Saturated - Substitution (which requires more radical conditions)
Insoluble except for nitrate and acetate
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia

43. How do you find the pH for a dibasic acid? (H2A)?
But S° of element is not zero (except at 0K)
Pale purple - (orange)-yellow - red - blue - green.
Soluble
Perform ICE BOX calculation based on K1

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

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45. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
CO3²?
Ksp = 108s5
Salt + water.
CO2 and H2O

46. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
q=mc?T q=mL (or n x ?h)
Ksp = s²
10?8
Ions go through the salt bridge - electrons go through metal wires in the external circuit

47. chromate ion (soln + most solids)
Anode - oxygen. Cathode - hydrogen
water and substances with (s) less dense than
10?8
yellow

48. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Ksp = 27s4
Insoluble (except group 1 ammonium and Ba)
Orange
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

49. What is the third law of thermodynamics?
S crystal at 0K=0
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
A) any range. b) 8-10 c) 4-6
NH4?

50. How does half life change for zero-th order - first order - and second order processes?
Add acid to water so that the acid doesn't boil and spit
Concentration
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
zero-th: decreases - first: constant - second: increases