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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. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
zero
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Kc=Kp

2. chromate ion (soln + most solids)
Mono; di; tri; tetra; penta; hexa.
yellow
White precipitate
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

3. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
CO (poisonous)
same KE - but PEice<PEwater
H2O + CO2 (it decomposes readily)

4. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Ksp = 27s4
yellow
More chaotic (ex: gases made)

5. How do you compute % dissociation?
Group 1 hydroxides (ex: NaOH)
Sulfur
Trigonal pyramidal
[A?]/[HA] x 100 or [BH?]/[B] x 100

6. What is HCOOCH3?
Ksp = 108s5
Acids; HCOOCH3 is an ester
left - ppt will form
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

7. What do you do to get rid of most of the solution from a precipitate?
H+
chemically (ex: with carbon)
same KE - but PEice<PEwater
Decant

8. Metal hydrides are _____ and form _______ and _______ when added to water
Filtration
?G= -ve - E°= +ve
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)
ionic and form hydrogen and hydroxide

9. What is the general formula for an amine?
RNH2
Identity and purity (impure compounds usually have broad & low melting points)
left - ppt will form
Evaporation

10. What type of metals don't react with water or acids to form H2?

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11. Name C7H16
Add acid to water so that the acid doesn't boil and spit
The dilution effect when the solutions mix. M1V1 = M2V2
OH?
Heptane

12. Does Benzene react by addition or substitution?
Soluble
#ligands=charge x2
Kc=Kp
it reacts by substitution NOT addition

13. What are isomers?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
RX
Molecules with the same molecular formulas - but different structural formulas
it's lower and occurs over less sharp a range

14. What measuring device would you use for very small volumes of liquids?
Graduated cylinder
ion pairing
Pipette (burette if need repetition)
Glacial acetic acid

15. What part of a liquid do you look at to measure its volume?
All except for lithium
CnH(2n+2)
Read the bottom of the meniscus
T increases exponentially the proportion of molecules with E > Ea

16. mercury (II) ion
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Insoluble except for nitrate and acetate
Hg²?

17. What is the formula for alkanes?
CnH2n+2
benzene has a delocalized pi ring structure
acids
red - green - blue

18. hydroxide
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?)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
S2O3²?
OH?

19. Ions are not ______.
An active metal.
Pipette (burette if need repetition)
atoms
Current - time and charge on ion (moles of e used in half cell reaction)

20. Do you use J or kJ for ?H - ?S - and ?G?
Concentration
?H-kJ - ?S-J - ?G-kJ
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 are soluble except Ag - Pb

21. If a weak acid is diluted more - what happens to its % dissociation value?
Orange
catalyst=conc H2SO4
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Increases.

22. What are the prefixes for the naming of binary molecular compound formulas (up to six)
?G= -ve - E°= +ve
Mono; di; tri; tetra; penta; hexa.
Big K=kf/kr
?G=negative - E° must be positive

23. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Nothing
Ions go through the salt bridge - electrons go through metal wires in the external circuit
No - it depends on the number of ions produced on dissolving.
Combine the equations for the half reactions in the non-spontaneous direction

24. What is the formula of copper (II) phosphate?
Cu3(PO4)2
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)
ion pairing
H+

25. What should you check for before you begin titrating?
linear
Iodine and CO2 (dry ice)
Check for air bubbles in the buret and remove the buret funnel from the buret
neutralization: high K - H2O product dissociation: low K - H2O reactant

26. Why are i factors (Van't Hoff factors) often less than ideal?
More chaotic (ex: gases made)
ion pairing
H+
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

27. How many faradays of electric charge do you need to produce one mole of O2? H2?
Ksp = 27s4
Acid rain - dissolves marble buildings/statues and kills trees.
Synthetic condensation polymer (aka a polyamide)
O2 needs 4F/mol H2 needs 2F/mol

28. lead compounds
The Faraday or Faraday's constant.
Insoluble except nitrate and acetate
Both electrons come from the same atom (just as good as a regular bond)
acid + alcohol

29. Neutralization is an ________ reaction.
brown volatile liquid
Synthesis - separation and purification of the product and its identification.
10?8
Exothermic (?H for ANY sa/sb = -57kJ/mol)

30. What is the third law of thermodynamics?
The benzene ring (or more correctly the phenyl group - C6H5)
bases
S crystal at 0K=0
Transition element compounds (except if it has a full or empty d shell)

31. group 1 ions/compounds
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Insoluble except for nitrate and acetate
Soluble
q=mc?T q=mL (or n x ?h)

32. What process do you use to separate two liquids with different boiling points?
Pale yellow
fractional distillation
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
A) any range. b) 8-10 c) 4-6

33. perchlorate
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Only temperature
ClO4?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

34. Acid plus base make?
Salt + water.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Glacial acetic acid
zero-th: decreases - first: constant - second: increases

35. acetates
Synthetic condensation polymer (aka a polyamide)
K2
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Soluble

36. How are strong ones written?
Iodine and CO2 (dry ice)
strong acids/bases are written as H+ or OH- ions
Insoluble
Ksp = 108s5

37. If ?S is positive - are the products more or less chaotic than the reactants?
fractional distillation
it is lower and occurs over less sharp a range
More chaotic (ex: gases made)
allow for the vapor pressure of water and make sure to level levels

38. What word is a clue for a redox reaction?
Heptane
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)
All except for lithium
Acidified

39. What reacts with an acid to create hydrogen gas?
More chaotic (ex: gases made)
Separating funnel
An active metal.
Trigonal pyramidal

40. carbonates
acid + alcohol
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Insoluble except group 1 and ammonium
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

41. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
No - NH3 and HCl gases are extremely soluble
Insoluble (except group 1 ammonium and Ba)

42. barium sulfate
ethers
Increases.
White precipitate
Ionic compounds

43. silver iodide
Pale yellow
Evaporation
bent
It ceases - the circuit is broken.

44. How does half life change for zero-th order - first order - and second order processes?
allow for the vapor pressure of water and make sure to level levels
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
zero-th: decreases - first: constant - second: increases
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

45. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
by electrolysis
NH2?
proton donor base

46. Is a graduated cylinder or beaker more accurate?
H2O + CO2 (it decomposes readily)
H3PO4
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Graduated cylinder

47. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Q=It (time in seconds)
Mono; di; tri; tetra; penta; hexa.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
catalyst=conc H2SO4

48. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
bases
ClO2?
Transition element compounds (except if it has a full or empty d shell)
Anode - oxygen. Cathode - hydrogen

49. What is the formula of butane?
hydroxides (ex: Ba(OH)2)
C4H10
ns² electrons (first in-first out)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

50. What are the products of the reaction between group 1 metals and water?

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