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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. When a cell is 'flat' What is its voltage?
zero
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Anode - oxygen. Cathode - hydrogen
RCHO (carbonyl at end)

2. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Most are soluble except Ag - Pb
Mono; di; tri; tetra; penta; hexa.
Iodine and CO2 (dry ice)
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

3. What is the conjugate acid of H2PO4?
H3PO4
allow for the vapor pressure of water and make sure to level levels
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
0.10M HCl (more ions)

4. What is the pH of 1.0M HCl? 1M NaOH?
Check for air bubbles in the buret and remove the buret funnel from the buret
Filtration
0 and 14
benzene is less reactive than alkenes

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

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6. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
The dilution effect when the solutions mix. M1V1 = M2V2
Purple
are less dense than water

7. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Most are soluble except Ag - Pb
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

8. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Ksp = s²
Acid rain - dissolves marble buildings/statues and kills trees.
An active metal.
a-IMFs - b-molecular volume

9. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Conjugate pair (one must be a weak base or acid)
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?)
At half equivalence - pH=pKa
it's lower and occurs over less sharp a range

10. How are primary alcohols turned into acids?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
CN?
RX

11. What do you use for an acid spill? base spill?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
+4-covalent - +2-ionic
an oxidized and reduced substance

12. What do group I/II metal oxides plus water form?
bases
10?8
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Insoluble

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

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14. What is the general formula for an acid?
RCOOH
They stay the same.
A salt solution.
CN?

15. nitrates
Initiation energy (NOT Ea)
Soluble
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
More chaotic (ex: gases made)

16. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
HClO4
fractional distillation
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

17. What is an Alkyl group?

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18. What shape is carbon dioxide?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
linear
blue glass - it filters UV
blue

19. What is the formula for summation?

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20. What are the signs of ?G and E° for spontaneous reactions?
?G=negative - E° must be positive
Cu3(PO4)2
Anode - oxygen. Cathode - hydrogen
K2

21. When combining half equations - what do you do to E° values when multiplying coefficients?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
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.
Salt + water
Nothing

22. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
CnH2n-2
K1 x K2
Ksp = 108s5
?H-kJ - ?S-J - ?G-kJ

23. What shape is methane?
Evaporation
A salt solution.
allow for the vapor pressure of water and make sure to level levels
Tetrahedral

24. What do you do to get rid of most of the solution from a precipitate?
Identity and purity (impure compounds usually have broad & low melting points)
blue (BTB)
Decant
Perform ICE BOX calculation based on K1

25. If a free element is involved - what type of reaction must be involved?
water and substances with (s) less dense than
same KE - but PEice<PEwater
redox reaction
Purple

26. How do you find the pH for a dibasic acid? (H2A)?
Group I metals (soft metals) are stored under oil
Perform ICE BOX calculation based on K1
acid + alcohol
lighted splint (positive result=pop)

27. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
ns² electrons (first in-first out)
They stay the same.
are less dense than water
Group I metals (soft metals) are stored under oil

28. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
The dilution effect when the solutions mix. M1V1 = M2V2
0.10M HCl (more ions)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
RCOR

29. Both Acetic acid and ____________ are also functional isomers.
it is lower and occurs over less sharp a range
methyl formate
Glowing splint (positive result=relights)
Silvery gray solid - brown - purple

30. Which value of R do you use for all energy and kinetics calculations?
Sulfur
Ksp = 108s5
R=8.31 J/mol/K
metal oxides and hydrides are ionically bonded and basic

31. What shape is ammonia?
R=8.31 J/mol/K
NH4?
voltaic: + electrolytic: -
Trigonal pyramidal

32. lead compounds
Insoluble except nitrate and acetate
neutralization: high K - H2O product dissociation: low K - H2O reactant
boiling without losing volatile solvents/reactants
Iodine and CO2 (dry ice)

33. Why are i factors (Van't Hoff factors) often less than ideal?
Evaporation
methyl formate
At half equivalence - pH=pKa
ion pairing

34. Give an example of a dilute strong acid.
HClO4
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Increases.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

35. Do you use J or kJ for ?H - ?S - and ?G?
left - ppt will form
zero
?H-kJ - ?S-J - ?G-kJ
More chaotic (ex: gases made)

36. What is the second law of thermodynamics?
Suniverse increases for spontaneous processes
C4H10
The compound with the lowest Ksp value.
Clear

37. Name six characteristics of transition elements (or their compounds)
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)
brown volatile liquid
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
The benzene ring (or more correctly the phenyl group - C6H5)

38. dichromate
NO3?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Cr2O7²?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

39. What does saturated mean? Unsaturated?
Glacial acetic acid
#ligands=charge x2
do not change
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

40. What is the test for oxygen?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
ionic and form hydrogen and hydroxide
Synthetic condensation polymer (aka a polyamide)
Glowing splint (positive result=relights)

41. What do metal oxides plus acids form?
yellow
a-IMFs - b-molecular volume
Salt + water
chemically (ex: with carbon)

42. mercury (II) ion
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Hg²?
ClO3?
CO3²?

43. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Pale purple - (orange)-yellow - red - blue - green.
Both electrons come from the same atom (just as good as a regular bond)
Big K=kf/kr

44. What is the conjugate base of NH3?
NH2?
Clear
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)
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?)

45. What is the general formula for an ether?
bent
ROR
Identity and purity (impure compounds usually have broad & low melting points)
Insoluble except group 1 and ammonium

46. Is a graduated cylinder or beaker more accurate?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
allow for the vapor pressure of water and make sure to level levels
Graduated cylinder
CH3COO?

47. What does a short - sharp melting point indicate?
0.10M HCl (more ions)
C4H10
Identity and purity (impure compounds usually have broad & low melting points)
Cr2O7²?

48. What is HCOOCH3?
Acids; HCOOCH3 is an ester
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Evaporation
Insoluble except group 1 and ammonium

49. The oxidation # for acid base reactions...
do not change
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
bases
ClO3?

50. What is the formula for percent error?
Salt + water
|experimental - accepted|/accepted X 100
CnH(2n+2)
Only temperature