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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 the conjugate base of NH3?
Both electrons come from the same atom (just as good as a regular bond)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
NH2?
Read the bottom of the meniscus

2. What is the formula for obtaining charge flowing in a cell?
redox reaction
a-IMFs - b-molecular volume
Q=It (time in seconds)
NH4?

3. What are amphoteric oxides?
a-IMFs - b-molecular volume
K1 x K2
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?)
allow for the vapor pressure of water and make sure to level levels

4. phosphate
ROH
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Acid rain - dissolves marble buildings/statues and kills trees.
PO4³?

5. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
Tetrahedral
zero
Distillation

6. How do you clean a buret/pipette for a titration?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
O2 needs 4F/mol H2 needs 2F/mol
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Insoluble (except group 1 ammonium and Ba)

7. 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
Synthesis - separation and purification of the product and its identification.
ClO3?
CnH(2n+2)

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

9. What is the general formula for an alcohol?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
#ligands=charge x2
Mn²? - Cr³? - Cr³
ROH

10. What is the difference between equivalence point and end point of a titration.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Equivalence point is the titrant volume when the moles of acid and base are stoichiometrically equal; end point is the titrant volume when the color of the indicator permanently changes. If you choose the correct indicator - they should occur at the
Suniverse increases for spontaneous processes
Salts (ex: CaO + SO2 ? CaSO3)

11. How does half life change for zero-th order - first order - and second order processes?
proton donor base
OH?
zero-th: decreases - first: constant - second: increases
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

12. copper sulfate
blue
Identity and purity (impure compounds usually have broad & low melting points)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
NO3?

13. How many faradays of electric charge do you need to produce one mole of O2? H2?
same KE - but PEice<PEwater
benzene is less reactive than alkenes
Greenish-yellow gas
O2 needs 4F/mol H2 needs 2F/mol

14. What is the general formula for alkyl halides?
CnH2n+2
RX
Current - time and charge on ion (moles of e used in half cell reaction)
Sulfur

15. What is the word equation for condensation polymerisation ?
fractional distillation
Molecules with the same molecular formulas - but different structural formulas
same KE - but PEice<PEwater
Monomer + monomer = polymer product + a simple molecule such as water or HCl

16. Generally - which oxy acid is strongest?
ROH
The one with most oxygen atoms (highest oxidation number)
ClO?
zero

17. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
All single: sp³ - one double: sp² - two doubles: sp - one triple: sp - two single and two lone pairs: sp³ - three single and one lone pair: sp³
brown volatile liquid
White precipitate

18. carbonate
Initiation energy (NOT Ea)
ClO?
CO3²?
basic

19. chlorate
ClO3?
Soluble except Ag - Pb - Ca - Sr Ba)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Concentration

20. When the salt bridge is removed what happens to the cell reaction?
do not change
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Insoluble except group 1 and ammonium
It ceases - the circuit is broken.

21. What are the formulas for q?
Distillation
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
q=mc?T q=mL (or n x ?h)
an oxidized and reduced substance

22. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Evaporation
CO (poisonous)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

23. ammonium
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Unsaturated - addition (ex: decolorize bromine solution)
NH4?
Group I metals (soft metals) are stored under oil

24. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Big K=kf/kr
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
S crystal at 0K=0
Acidified

25. What is the general formula of an alkane?
CnH(2n+2)
RCOOR
Hg²?
The dilution effect when the solutions mix. M1V1 = M2V2

26. Do you use J or kJ for ?H - ?S - and ?G?
water and substances with (s) less dense than
?H-kJ - ?S-J - ?G-kJ
They stay the same.
same KE - but PEice<PEwater

27. bromine
Pale yellow
Unsaturated - addition (ex: decolorize bromine solution)
brown volatile liquid
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

28. What are the common strong bases?
CnH2n
bright yellow
Group 1 hydroxides (ex: NaOH)
Increases.

29. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
ns² electrons (first in-first out)
by electrolysis
brown volatile liquid

30. How are non-metal oxides and hydrides bonded? are they acidic or basic?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
non-metal oxides and hydrides are covalently bonded and are acidic.
a-IMFs - b-molecular volume
Salt + water.

31. Is the freezing of ice endothermic or exothermic?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
S crystal at 0K=0
Exothermic
water and substances with (s) less dense than

32. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Add acid to water so that the acid doesn't boil and spit
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)

33. acetates
E=q + w (negative is by system - positive is on system)
Group 1 hydroxides (ex: NaOH)
an oxidized and reduced substance
Soluble

34. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
same KE - but PEice<PEwater
Making sigma bonds and holding lone pairs
Exothermic

35. Do anions flow to the cathode or anode?
Anode
Pipette (burette if need repetition)
proton acceptor.
voltaic: + electrolytic: -

36. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
Insoluble
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)
it's lower and occurs over less sharp a range

37. Buffer capacity must contain decent amounts of a ________ ________
zero-th: decreases - first: constant - second: increases
Conjugate pair (one must be a weak base or acid)
CnH2n
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.

38. lead iodide
NH2?
OH- and NH3
?H formation of an element in standard state=0
bright yellow

39. dichromate (soln + most solids)
neutralization: high K - H2O product dissociation: low K - H2O reactant
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
More chaotic (ex: gases made)
Orange

40. What are hybrid orbitals used for?
10?8
Ksp = s²
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Making sigma bonds and holding lone pairs

41. What type of polymer is nylon?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Pale purple - (orange)-yellow - red - blue - green.
Synthetic condensation polymer (aka a polyamide)
benzene has a delocalized pi ring structure

42. ________ are Lewis bases - because they can donate a lone pair of electrons.
it is lower and occurs over less sharp a range
ClO4?
CnH2n+2
OH- and NH3

43. What do you do to get rid of most of the solution from a precipitate?
?G=negative - E° must be positive
O2 needs 4F/mol H2 needs 2F/mol
Mono; di; tri; tetra; penta; hexa.
Decant

44. What process do you use to separate two liquids with different boiling points?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
fractional distillation
Eudiometer
ion pairing

45. Give an example of a concentrated weak acid.
White precipitate
The compound with the lowest Ksp value.
Transition element compounds (except if it has a full or empty d shell)
Glacial acetic acid

46. What is the formula for alkenes?
CnH2n
red - green - blue
catalyst=conc H2SO4
Most are soluble except Ag - Pb

47. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
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?)
T increases exponentially the proportion of molecules with E > Ea
Ksp = s²
Increases.

48. chlorite
it is lower and occurs over less sharp a range
proton acceptor.
PO4³?
ClO2?

49. chlorine
Greenish-yellow gas
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Ppt will NOT form (unsaturated)
ROH

50. What is the test for hydrogen?
O2 needs 4F/mol H2 needs 2F/mol
ethers
lighted splint (positive result=pop)
fruit - fish - bases