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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 should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
K1 x K2
H2PO4?

2. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
yellow
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)
RCOR

3. How do you compute % dissociation?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
bases
RCHO (carbonyl at end)
[A?]/[HA] x 100 or [BH?]/[B] x 100

4. mercury (I) ion
RCHO (carbonyl at end)
Hg2²?
NH4?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

5. What apparatus do you use to separate 2 immiscible liquids?
H+
Ksp = 27s4
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Separating funnel

6. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Pour liquids using a funnel or down a glass rod
Ksp = 4s³
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

7. thiosulfate
proton acceptor.
Nothing
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
S2O3²?

8. cyanide
CnH(2n+2)
atoms
MnO4?
CN?

9. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Suniverse increases for spontaneous processes
RCOOR
C4H10
Ksp = 108s5

10. What is the general formula for a ketone?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Orange
RCOR
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

11. What type of compounds do Group 14 form?
+4-covalent - +2-ionic
CH3COO?
PO4³?
Making sigma bonds and holding lone pairs

12. What are hybrid orbitals used for?
Silvery gray solid - brown - purple
Clear
Making sigma bonds and holding lone pairs
it is lower and occurs over less sharp a range

13. What measuring device would you use for very small volumes of liquids?
benzene has a delocalized pi ring structure
proton acceptor.
Ksp = 108s5
Pipette (burette if need repetition)

14. What is the test for hydrogen?
redox reaction
same KE - but PEice<PEwater
lighted splint (positive result=pop)
S crystal at 0K=0

15. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
P2O5
Greenish-yellow gas
chemically (ex: with carbon)
Most are soluble except Ag - Pb

16. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
[A?]/[HA] x 100 or [BH?]/[B] x 100
bright yellow
?G=negative - E° must be positive
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

17. sulfate
do not change
SO4²?
Decant
a-IMFs - b-molecular volume

18. What is the general formula for an acid?
RCOOH
q=mc?T q=mL (or n x ?h)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
yellow

19. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
it is lower and occurs over less sharp a range
zero

20. What effect does increasing the size/surface area of a voltaic cell have on the cell?
H3PO4
Ksp = s²
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
More chaotic (ex: gases made)

21. What type of compounds are almost always colored?
do not change
CH3COO?
Distillation
Transition element compounds (except if it has a full or empty d shell)

22. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
CN?
basic
it is lower and occurs over less sharp a range
P2O5

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

24. What is the energy you must put into a reaction to make it start called?
Decant
different forms of the same element
Increases.
Initiation energy (NOT Ea)

25. carbonate
CO3²?
voltaic: - electrolytic: +
Soluble
?H-kJ - ?S-J - ?G-kJ

26. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
do not change
CO (poisonous)
Glacial acetic acid
K1 x K2

27. What do hydrocarbons form when they burn in air (oxygen)?
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)
Heat a test tube at an angle at the side of the tube (not bottom)
proton acceptor.
CO2 and H2O

28. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
different forms of the same element
ROR
Cr2O7²?

29. phosphates
Most INsoluble except group 1 and ammonium
Anode - oxygen. Cathode - hydrogen
blue (BTB)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

30. Can you collect soluble gases over water?
voltaic: + electrolytic: -
Perform ICE BOX calculation based on K1
metal oxides and hydrides are ionically bonded and basic
No - NH3 and HCl gases are extremely soluble

31. What process do you use to separate two liquids with different boiling points?
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
fractional distillation
How close results are to the accepted value
Glowing splint (positive result=relights)

32. What do group I/II metal oxides and acids form?
Experimental mass/theoretical mass X 100
Ksp = s²
More chaotic (ex: gases made)
Salt and water

33. How does benzene compare in reactivity to alkenes?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
benzene is less reactive than alkenes
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Evaporation

34. An amphiprotic (amphoteric) species is...
+4-covalent - +2-ionic
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Identity and purity (impure compounds usually have broad & low melting points)
[A?]/[HA] x 100 or [BH?]/[B] x 100

35. What device would you use to measure a volume of gas?
Exothermic
ClO?
Eudiometer
Combine the equations for the half reactions in the non-spontaneous direction

36. A geometric (or cis-trans) isomer exists due to.....
voltaic: + electrolytic: -
PO4³?
C2O4²?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

37. What apparatus do you use to pour liquids?
Pale yellow
Insoluble except for nitrate and acetate
Pour liquids using a funnel or down a glass rod
Check for air bubbles in the buret and remove the buret funnel from the buret

38. A Bronsted-Lowry base is...
proton acceptor.
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Decant
S crystal at 0K=0

39. What does saturated mean? Unsaturated?
CnH2n-2
by electrolysis
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

40. When a cell is 'flat' What is its voltage?
Heptane
How close results are to the accepted value
zero
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

41. What causes the dramatic effect of T on rate?
atoms
it's lower and occurs over less sharp a range
Heat a test tube at an angle at the side of the tube (not bottom)
T increases exponentially the proportion of molecules with E > Ea

42. What is precision?
do not change
The dilution effect when the solutions mix. M1V1 = M2V2
Acidified
How grouped results are

43. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
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?)
do not change
Pale purple - (orange)-yellow - red - blue - green.
Making sigma bonds and holding lone pairs

44. What is the pH of 1.0M HCl? 1M NaOH?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
0 and 14
NO3?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

45. What is the formula of copper (II) phosphate?
Cu3(PO4)2
Sulfur
K1 x K2
#ligands=charge x2

46. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
bent
do not change
0 and 14

47. Do you use J or kJ for ?H - ?S - and ?G?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
NH4?
?H-kJ - ?S-J - ?G-kJ
ClO2?

48. What is Big K in terms of kf and kr?
a-IMFs - b-molecular volume
Synthetic condensation polymer (aka a polyamide)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Big K=kf/kr

49. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
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
H+
Increases down group 1 decreases down group 17
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

50. Name some properties of Group 17
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Distillation
bent
water and substances with (s) less dense than