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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. thiosulfate
no - they're written undissociated (HAaq)
S2O3²?
CnH2n+2
The compound with the lowest Ksp value.

2. What is the sign of the cathode in voltaic cells? in electrolytic cells?
A) any range. b) 8-10 c) 4-6
Add acid to water so that the acid doesn't boil and spit
voltaic: + electrolytic: -
At half equivalence - pH=pKa

3. What is HCOOCH3?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Most INsoluble except group 1 and ammonium
Acids; HCOOCH3 is an ester
CnH(2n+2)

4. oxalate
ClO?
C2O4²?
|experimental - accepted|/accepted X 100
No - NH3 and HCl gases are extremely soluble

5. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
H+
?H-kJ - ?S-J - ?G-kJ
CnH2n+1 often designated 'R' ex C3H7 is propyl

6. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
CnH2n-2
A) any range. b) 8-10 c) 4-6
voltaic: - electrolytic: +
CO (poisonous)

7. Is the freezing of ice endothermic or exothermic?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Exothermic
ion pairing
Ksp = s²

8. Does Kw increase or decrease with T? Why?
zero
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Sulfur
do not change

9. What is the formula for alkenes?
zero
a-IMFs - b-molecular volume
Greenish-yellow gas
CnH2n

10. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
No - it depends on the number of ions produced on dissolving.
it reacts by substitution NOT addition
The dilution effect when the solutions mix. M1V1 = M2V2
Reduction always takes place at the cathode (RED CAT) In both types of cell!

11. What type of compounds are almost always colored?
zero
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Transition element compounds (except if it has a full or empty d shell)
Concentration

12. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Heat a test tube at an angle at the side of the tube (not bottom)
T increases exponentially the proportion of molecules with E > Ea
same KE - but PEice<PEwater

13. What word is a clue for a redox reaction?
Acidified
Pipette (burette if need repetition)
Anode - oxygen. Cathode - hydrogen
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

14. chromate
Soluble
?H formation of an element in standard state=0
CrO4²?
10?8

15. permanganate
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
a-IMFs - b-molecular volume
MnO4?
strong acids/bases are written as H+ or OH- ions

16. For a dibasic acid (H2A) - [A²?]= ____ ?
Ppt will NOT form (unsaturated)
K2
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
same KE - but PEice<PEwater

17. Name some properties of Group 17
bases
Distillation
CN?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

18. Neutralization is an ________ reaction.
Selective absorption
H3PO4
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Exothermic (?H for ANY sa/sb = -57kJ/mol)

19. Colorless doesn't mean ______
Greenish-yellow gas
Heat a test tube at an angle at the side of the tube (not bottom)
?H-kJ - ?S-J - ?G-kJ
Clear

20. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
ClO3?
The dilution effect when the solutions mix. M1V1 = M2V2
Acids; HCOOCH3 is an ester

21. hydroxide
OH?
Heat a test tube at an angle at the side of the tube (not bottom)
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)
yellow

22. What type of compounds do metals/non metals form?
Ionic compounds
allow for the vapor pressure of water and make sure to level levels
How close results are to the accepted value
-Ea/R

23. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
CnH2n+2
CnH(2n+2)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

24. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
red - green - blue
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.
do not change

25. What is Big K in terms of kf and kr?
Hg²?
Molecules with the same molecular formulas - but different structural formulas
But S° of element is not zero (except at 0K)
Big K=kf/kr

26. How do you get the equation for a net electrolysis reaction?
?G=negative - E° must be positive
Combine the equations for the half reactions in the non-spontaneous direction
voltaic: + electrolytic: -
zero-th: decreases - first: constant - second: increases

27. When is ?G zero?
Pipette (burette if need repetition)
hydroxides (ex: Ba(OH)2)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

28. Does reactivity increase/decrease going down group 1 and group 17?
Insoluble
Perform ICE BOX calculation based on K1
[A?]/[HA] x 100 or [BH?]/[B] x 100
Increases down group 1 decreases down group 17

29. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Concentration
Ksp = 27s4
bright yellow
H+

30. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
a-IMFs - b-molecular volume
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Heptane

31. Esterification is...
allow for the vapor pressure of water and make sure to level levels
linear
Soluble
acid + alcohol

32. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

33. What are amphoteric oxides?
do not change
basic
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?)
voltaic: - electrolytic: +

34. dihydrogen phosphate
Pale purple - (orange)-yellow - red - blue - green.
Pipette (burette if need repetition)
H2PO4?
lighted splint (positive result=pop)

35. What are two substances that sublime at 1 atm when heated?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
voltaic: - electrolytic: +
Iodine and CO2 (dry ice)
Products - reactants (except for BDE when it's reactants - products)

36. During a titration what is present in the beaker at the equivalence point?
do not change
Making sigma bonds and holding lone pairs
HClO4
A salt solution.

37. What element is used to vulcanize rubber?
Sulfur
Kc=Kp
ClO?
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

38. Alkanes are _________ and react by _________
ClO?
ns² electrons (first in-first out)
Saturated - Substitution (which requires more radical conditions)
H2PO4?

39. What do you do to get rid of most of the solution from a precipitate?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
a-IMFs - b-molecular volume
Filtration
Decant

40. What type of solutions do small - highly charged cations tend to form?
ROH
CrO4²?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
?H formation of an element in standard state=0

41. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
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)
Ksp = 108s5
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

42. 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?
blue glass - it filters UV
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
The compound with the lowest Ksp value.
CnH2n

43. A Bronsted-Lowry acid is...
ion pairing
MnO4?
ClO2?
proton donor base

44. Lattice energy is high for ions with _____ size and _____ charge
water and substances with (s) less dense than
small size and high charge
Insoluble except nitrate and acetate
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

45. What is the formula for alkanes?
Glowing splint (positive result=relights)
Silvery gray solid - brown - purple
CnH2n+2
a-IMFs - b-molecular volume

46. group 1 ions/compounds
Soluble
Ksp = 4s³
PO4³?
Experimental mass/theoretical mass X 100

47. lead iodide
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
bright yellow
A salt solution.

48. When combining half equations - what do you do to E° values when multiplying coefficients?
Both electrons come from the same atom (just as good as a regular bond)
Nothing
At half equivalence - pH=pKa
Distillation

49. Is a graduated cylinder or beaker more accurate?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Graduated cylinder
A salt solution.
Distillation

50. The oxidation # for acid base reactions...
do not change
Acidified
benzene has a delocalized pi ring structure
Glacial acetic acid