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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 general formula for alkyl halides?
RX
Evaporation
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
CO2 and H2O

2. What do you use for an acid spill? base spill?
redox reaction
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Group I metals (soft metals) are stored under oil
allow for the vapor pressure of water and make sure to level levels

3. What are the signs of ?G and E° for spontaneous reactions?
linear
?G=negative - E° must be positive
are less dense than water
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

4. Nonmetals are good _____ agents. Metals are good _______ agents.
?G= -ve - E°= +ve
Cr2O7²?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

5. Alkanes are _________ and react by _________
An active metal.
CO (poisonous)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Saturated - Substitution (which requires more radical conditions)

6. copper sulfate
Evaporation
ionic and form hydrogen and hydroxide
blue
Increases.

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

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8. acetate
CH3COO?
Insoluble (except group 1 ammonium and Ba)
zero
Greenish-yellow gas

9. Do you use J or kJ for ?H - ?S - and ?G?
Transition element compounds (except if it has a full or empty d shell)
T increases exponentially the proportion of molecules with E > Ea
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
?H-kJ - ?S-J - ?G-kJ

10. Why are i factors (Van't Hoff factors) often less than ideal?
Heptane
Clear
ion pairing
ionic and form hydrogen and hydroxide

11. Color (absorbance) is proportional to ________
Orange
No - it depends on the number of ions produced on dissolving.
Concentration
diamond and graphite

12. During a titration what is present in the beaker at the equivalence point?
They stay the same.
How grouped results are
Pale purple - (orange)-yellow - red - blue - green.
A salt solution.

13. lead iodide
bright yellow
water and substances with (s) less dense than
Trigonal pyramidal
Perform ICE BOX calculation based on K1

14. potassium permanganate
Purple
It ceases - the circuit is broken.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
left - ppt will form

15. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
?H formation of an element in standard state=0
zero
it is lower and occurs over less sharp a range
water and substances with (s) less dense than

16. How do you explain trends in atomic properties using Coulomb's Law?
Cr2O7²?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

17. What element is used to vulcanize rubber?
bent
ROR
Sulfur
Trigonal pyramidal

18. What is the general formula for an amine?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
RNH2
ns² electrons (first in-first out)

19. What do you do to get rid of most of the solution from a precipitate?
Decant
Filtration
same KE - but PEice<PEwater
zero-th: decreases - first: constant - second: increases

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

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21. carbonate
CO3²?
Heat a test tube at an angle at the side of the tube (not bottom)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Sigma bonds are stronger than pi bonds

22. What do group I/II metal oxides plus water form?
Glowing splint (positive result=relights)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
different forms of the same element
bases

23. What are two substances that sublime at 1 atm when heated?
MnO4?
No - NH3 and HCl gases are extremely soluble
CO3²?
Iodine and CO2 (dry ice)

24. What are the common strong bases?
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?)
Greenish-yellow gas
Group 1 hydroxides (ex: NaOH)
non-metal oxides and hydrides are covalently bonded and are acidic.

25. Do anions flow to the cathode or anode?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Anode
ClO?

26. What are hybrid orbitals used for?
Insoluble (except group 1 ammonium and Ba)
lighted splint (positive result=pop)
?H formation of an element in standard state=0
Making sigma bonds and holding lone pairs

27. hydroxide
fractional distillation
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
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.
OH?

28. What is the formula for percent yield?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
RCOOR
Experimental mass/theoretical mass X 100
Heptane

29. What process do you use to obtain the solute from a solution?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Greenish-yellow gas
Evaporation
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

30. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
fruit - fish - bases
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

31. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
The compound with the lowest Ksp value.
Kc=Kp
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

32. What is the conjugate acid of H2PO4?
?H formation of an element in standard state=0
H3PO4
Tetrahedral
The compound with the lowest Ksp value.

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

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34. phosphate
small size and high charge
PO4³?
are less dense than water
Group 1 hydroxides (ex: NaOH)

35. How does the melting point of a mixture compare to the MP of a pure substance?

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36. Does reactivity increase/decrease going down group 1 and group 17?
non-metal oxides and hydrides are covalently bonded and are acidic.
Most are soluble except Ag - Pb
S2O3²?
Increases down group 1 decreases down group 17

37. What do the 'a' and 'b' in Van Der Waal's equation allow for?
H2O + CO2 (it decomposes readily)
catalyst=conc H2SO4
a-IMFs - b-molecular volume
fractional distillation

38. What is the general formula for an alcohol?
0.10M HCl (more ions)
Tetrahedral
Q=It (time in seconds)
ROH

39. Esters smell like _______ and amines smell like _______ and are ______.
Unsaturated - addition (ex: decolorize bromine solution)
Silvery gray solid - brown - purple
fruit - fish - bases
Group I metals (soft metals) are stored under oil

40. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
basic
allow for the vapor pressure of water and make sure to level levels

41. phosphates
Most INsoluble except group 1 and ammonium
H3PO4
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
CnH2n

42. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
Check for air bubbles in the buret and remove the buret funnel from the buret
no - they're written undissociated (HAaq)
H+

43. What process do you use to obtain a solvent from a solution?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
RX
Distillation
Saturated - Substitution (which requires more radical conditions)

44. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
benzene has a delocalized pi ring structure
SO4²?
a-IMFs - b-molecular volume

45. When combining half equations - what do you do to E° values when multiplying coefficients?
Nothing
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
SO4²?

46. chromate
bases
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
CrO4²?
red - green - blue

47. nitrate
NO3?
diamond and graphite
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
CrO4²?

48. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Most INsoluble except group 1 and ammonium
Current - time and charge on ion (moles of e used in half cell reaction)
Insoluble
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.

49. What kind of bonding structure does benzene have?
Clear
benzene has a delocalized pi ring structure
Graduated cylinder
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

50. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
An active metal.
Exothermic
H3PO4