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

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2. acetate
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
do not change
RCOR
CH3COO?

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

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4. What do ions and electrons travel through in a voltaic/electrolytic cell?
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
CrO4²?
Ions go through the salt bridge - electrons go through metal wires in the external circuit

5. How does group 1 metals' density compare to water's?
are less dense than water
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.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

6. chromate
Insoluble except nitrate and acetate
Graduated cylinder
CrO4²?
ethers

7. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Mono; di; tri; tetra; penta; hexa.
Mn²? - Cr³? - Cr³
bases
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

8. dichromate
H2O + CO2 (it decomposes readily)
Cr2O7²?
blue
Glacial acetic acid

9. What shape is methane?
CH3COO?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Tetrahedral
CrO4²?

10. What process do you use to obtain the precipitate from a solution?
Filtration
An active metal.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
same KE - but PEice<PEwater

11. What process do you use to obtain the solute from a solution?
CH3COO?
Evaporation
metal oxides and hydrides are ionically bonded and basic
Kc=Kp

12. group 1 ions/compounds
Soluble
an oxidized and reduced substance
H3PO4
How close results are to the accepted value

13. If ?S is positive - are the products more or less chaotic than the reactants?
[A?]/[HA] x 100 or [BH?]/[B] x 100
More chaotic (ex: gases made)
The compound with the lowest Ksp value.
It ceases - the circuit is broken.

14. What is the formula for alkynes?
CnH2n-2
lighted splint (positive result=pop)
P2O5
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

15. What process do you use to obtain a solvent from a solution?
it is lower and occurs over less sharp a range
Silvery gray solid - brown - purple
Glowing splint (positive result=relights)
Distillation

16. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Eudiometer
Monomer + monomer = polymer product + a simple molecule such as water or HCl
benzene has a delocalized pi ring structure
basic

17. When a cell is 'flat' What is its voltage?
zero
Soluble
voltaic: - electrolytic: +
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.

18. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
catalyst=conc H2SO4
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Synthetic condensation polymer (aka a polyamide)

19. The definition of acidic basic and neutral aqueous solutions is:
fruit - fish - bases
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
C4H10
Purple

20. dihydrogen phosphate
H2PO4?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
H3PO4
#ligands=charge x2

21. How can metals like iron and zinc be reduced?
CnH(2n+2)
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
benzene is less reactive than alkenes
chemically (ex: with carbon)

22. How do you get Ecell for spontaneous reactions?
Anode
Eudiometer
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

23. Does reactivity increase/decrease going down group 1 and group 17?
proton acceptor.
Increases down group 1 decreases down group 17
Ppt will NOT form (unsaturated)
Pipette (burette if need repetition)

24. What are allotropes?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
blue
different forms of the same element
Ksp = 4s³

25. phosphate
|experimental - accepted|/accepted X 100
PO4³?
Separating funnel
Both electrons come from the same atom (just as good as a regular bond)

26. barium sulfate
Iodine and CO2 (dry ice)
White precipitate
Read the bottom of the meniscus
a-IMFs - b-molecular volume

27. BaSO4
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Most are soluble except Ag - Pb
Ksp = 27s4
Insoluble

28. What is the relationship in strength between sigma and pi bonds?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
basic
CO (poisonous)
Sigma bonds are stronger than pi bonds

29. What two compounds are great oxidizing agents?

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30. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
White precipitate
strong acids/bases are written as H+ or OH- ions
No - it depends on the number of ions produced on dissolving.

31. What do nonmetal oxides plus water form?
Distillation
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
acids
How close results are to the accepted value

32. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Ionic compounds
neutralization: high K - H2O product dissociation: low K - H2O reactant
Acids; HCOOCH3 is an ester
Insoluble except group 1 and ammonium

33. What does saturated mean? Unsaturated?
same KE - but PEice<PEwater
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
CO (poisonous)
an oxidized and reduced substance

34. Do you use J or kJ for ?H - ?S - and ?G?
0.10M HCl (more ions)
do not change
C4H10
?H-kJ - ?S-J - ?G-kJ

35. When driving off water from a hydrate - how do you tell you're done?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
0.10M HCl (more ions)
Ppt will NOT form (unsaturated)
it's lower and occurs over less sharp a range

36. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
blue
The dilution effect when the solutions mix. M1V1 = M2V2
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Pale yellow

37. What do you do to get rid of most of the solution from a precipitate?
PO4³?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
ns² electrons (first in-first out)
Decant

38. What is the formula for alkanes?
Group 1 hydroxides (ex: NaOH)
CnH2n+2
-Ea/R
diamond and graphite

39. How many normal boiling points and boiling points are there?

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40. What type of polymer is nylon?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Molecules with the same molecular formulas - but different structural formulas
Synthetic condensation polymer (aka a polyamide)
RX

41. What is the general formula for an ether?
ROR
NH2?
catalyst=conc H2SO4
water and substances with (s) less dense than

42. hypochlorite
Insoluble except for nitrate and acetate
zero
voltaic: - electrolytic: +
ClO?

43. primary colors
red - green - blue
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
it's lower and occurs over less sharp a range
by electrolysis

44. What is the formula of copper (II) phosphate?
Iodine and CO2 (dry ice)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Cu3(PO4)2
|experimental - accepted|/accepted X 100

45. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
CH3COO?
They stay the same.
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
linear

46. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Identity and purity (impure compounds usually have broad & low melting points)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
H+
Soluble

47. What shape is carbon dioxide?
linear
No - NH3 and HCl gases are extremely soluble
Exothermic
bent

48. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Concentration
Pale yellow

49. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
same KE - but PEice<PEwater
Q=It (time in seconds)
Exothermic

50. Is a graduated cylinder or beaker more accurate?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
H3PO4
At half equivalence - pH=pKa
Graduated cylinder