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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. How do you get Ecell for spontaneous reactions?
Heat a test tube at an angle at the side of the tube (not bottom)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
ion pairing

2. What are amphoteric oxides?
A) any range. b) 8-10 c) 4-6
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
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?)
Soluble except Ag - Pb - Ca - Sr Ba)

3. Which alkali metals float on water?
Ionic compounds
NH2?
?H-kJ - ?S-J - ?G-kJ
All except for lithium

4. carbonates
#ligands=charge x2
OH?
Insoluble except group 1 and ammonium
look for changes in oxidation # - the one that goes up is oxidized and is the RA

5. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
blue (BTB)
Sulfur
No - it depends on the number of ions produced on dissolving.
Pale purple - (orange)-yellow - red - blue - green.

6. potassium permanganate
it is lower and occurs over less sharp a range
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Purple

7. lead iodide
CnH(2n+2)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
bright yellow
CO (poisonous)

8. What is the general formula for an aldehyde?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Current - time and charge on ion (moles of e used in half cell reaction)
RCHO (carbonyl at end)

9. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Decant
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Filtration
Both electrons come from the same atom (just as good as a regular bond)

10. Acidic gases like SO2 in the atmosphere cause what environmental problems?
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?)
K2
Acid rain - dissolves marble buildings/statues and kills trees.
But S° of element is not zero (except at 0K)

11. How do you find the pH for a dibasic acid? (H2A)?
Read the bottom of the meniscus
Perform ICE BOX calculation based on K1
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
CnH2n-2

12. How do you identify which is oxidized or otherwise?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
O2 needs 4F/mol H2 needs 2F/mol
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Soluble

13. The oxidation # for acid base reactions...
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Cu3(PO4)2
do not change
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

14. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
H2PO4?
metal oxides and hydrides are ionically bonded and basic
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

15. 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?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
The compound with the lowest Ksp value.
Hg²?
benzene has a delocalized pi ring structure

16. What device would you use to measure a volume of gas?
Saturated - Substitution (which requires more radical conditions)
Ksp = 27s4
diamond and graphite
Eudiometer

17. Where are group I metals stored?
Group I metals (soft metals) are stored under oil
non-metal oxides and hydrides are covalently bonded and are acidic.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
?G= -ve - E°= +ve

18. silver iodide
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
NH4?
Pale yellow
Pipette (burette if need repetition)

19. What does the solubility of organic compounds depend on?
?H formation of an element in standard state=0
Exothermic (?H for ANY sa/sb = -57kJ/mol)
HClO4
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

20. Alkenes are ________ and react by __________
Sigma bonds are stronger than pi bonds
Exothermic
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
Unsaturated - addition (ex: decolorize bromine solution)

21. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
CnH2n+1 often designated 'R' ex C3H7 is propyl
SO4²?
Combine the equations for the half reactions in the non-spontaneous direction
The dilution effect when the solutions mix. M1V1 = M2V2

22. What does a short - sharp melting point indicate?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
But S° of element is not zero (except at 0K)
Identity and purity (impure compounds usually have broad & low melting points)
Monomer + monomer = polymer product + a simple molecule such as water or HCl

23. perchlorate
Acidified
K1 x K2
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
ClO4?

24. During a titration what is present in the beaker at the equivalence point?
They stay the same.
Q=It (time in seconds)
A salt solution.
benzene is less reactive than alkenes

25. What is precision?
Iodine and CO2 (dry ice)
How grouped results are
Cu3(PO4)2
CrO4²?

26. BaSO4
Add acid to water so that the acid doesn't boil and spit
hydroxides (ex: Ba(OH)2)
voltaic: - electrolytic: +
Insoluble

27. What equipment do you need for a titration?
CnH2n+2
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
|experimental - accepted|/accepted X 100
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

28. If ?S is positive - are the products more or less chaotic than the reactants?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Increases.
More chaotic (ex: gases made)

29. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
A) any range. b) 8-10 c) 4-6
CO (poisonous)
Ksp = 4s³
Sulfur

30. An amphiprotic (amphoteric) species is...
CnH2n
Nothing
Making sigma bonds and holding lone pairs
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

31. Buffer capacity must contain decent amounts of a ________ ________
MnO4?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Conjugate pair (one must be a weak base or acid)
Only temperature

32. If a weak acid is diluted more - what happens to its % dissociation value?
T increases exponentially the proportion of molecules with E > Ea
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Increases.
Iodine and CO2 (dry ice)

33. chlorate
ClO3?
Q=It (time in seconds)
Anode - oxygen. Cathode - hydrogen
Most are soluble except Ag - Pb

34. Does reactivity increase/decrease going down group 1 and group 17?
Combine the equations for the half reactions in the non-spontaneous direction
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Increases down group 1 decreases down group 17

35. chromate ion (soln + most solids)
CnH(2n+2)
yellow
Soluble
Exothermic (?H for ANY sa/sb = -57kJ/mol)

36. group 1 ions/compounds
Initiation energy (NOT Ea)
Soluble
No - it depends on the number of ions produced on dissolving.
ion pairing

37. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
Glacial acetic acid
Ions go through the salt bridge - electrons go through metal wires in the external circuit
benzene has a delocalized pi ring structure

38. mercury (II) ion
atoms
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Hg²?
ClO2?

39. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Tetrahedral
Anode - oxygen. Cathode - hydrogen
zero
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

40. bromine
brown volatile liquid
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)
Silvery gray solid - brown - purple
Insoluble (except group 1 ammonium and Ba)

41. What is the general formula for an acid?
RX
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
ROH
RCOOH

42. How do you dilute an acid?

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43. Ions are not ______.
chemically (ex: with carbon)
Pour liquids using a funnel or down a glass rod
atoms
Iodine and CO2 (dry ice)

44. permanganate
CnH2n+1 often designated 'R' ex C3H7 is propyl
same KE - but PEice<PEwater
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
MnO4?

45. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Trigonal pyramidal
Most are soluble except Ag - Pb
ClO?

46. dichromate
Graduated cylinder
look for changes in oxidation # - the one that goes up is oxidized and is the RA
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Cr2O7²?

47. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Read the bottom of the meniscus
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
water and substances with (s) less dense than
Ksp = s²

48. What is the conjugate acid of H2PO4?
H3PO4
But S° of element is not zero (except at 0K)
yellow
NH4?

49. What is HCOOCH3?
Decant
Concentration
Acids; HCOOCH3 is an ester
RCOR

50. What two compounds are great oxidizing agents?

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