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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. carbonate
-Ea/R
CO3²?
Salt and water
it is lower and occurs over less sharp a range

2. What complex ion does ammonia form with silver? copper? cadmium? zinc?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Perform ICE BOX calculation based on K1

3. Colorless doesn't mean ______
Soluble
are less dense than water
Clear
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

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

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5. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
ion pairing
Eudiometer
All single: sp³ - one double: sp² - two doubles: sp - one triple: sp - two single and two lone pairs: sp³ - three single and one lone pair: sp³
CO (poisonous)

6. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
A salt solution.
Nothing
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

7. halides
Time?¹ - (ex. s?¹ - hr?¹ - etc)
zero
?H-kJ - ?S-J - ?G-kJ
Most are soluble except Ag - Pb

8. If a free element is involved - what type of reaction must be involved?
zero
0 and 14
redox reaction
H2PO4?

9. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Pour liquids using a funnel or down a glass rod
do not change
C2O4²?
allow for the vapor pressure of water and make sure to level levels

10. 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
zero
Pale yellow
Iodine and CO2 (dry ice)

11. What does the solubility of organic compounds depend on?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
ion pairing

12. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Suniverse increases for spontaneous processes
Hg²?
Molecules with the same molecular formulas - but different structural formulas
water and substances with (s) less dense than

13. sulfates
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Soluble except Ag - Pb - Ca - Sr Ba)
?G= -ve - E°= +ve
Most are soluble except Ag - Pb

14. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
RX
Increases.
CnH(2n+2)

15. bromine
The compound with the lowest Ksp value.
Big K=kf/kr
brown volatile liquid
Soluble

16. permanganate
MnO4?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Mn²? - Cr³? - Cr³
Filtration

17. How does group 1 metals' density compare to water's?
are less dense than water
H3PO4
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
hydroxides (ex: Ba(OH)2)

18. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Anode
metal oxides and hydrides are ionically bonded and basic
K1 x K2
CO3²?

19. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
ClO3?
Silvery gray solid - brown - purple
Ksp = s²
Most are soluble except Ag - Pb

20. What is an Alkyl group?

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21. What is reflux?
boiling without losing volatile solvents/reactants
H2PO4?
Glacial acetic acid
NH2?

22. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
CnH2n+1 often designated 'R' ex C3H7 is propyl
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Distillation

23. Are weak acids (and bases) written dissociated?

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24. carbonates
voltaic: + electrolytic: -
HClO4
Insoluble except group 1 and ammonium
K2

25. Ca - Sr - Ba
zero
Making sigma bonds and holding lone pairs
The benzene ring (or more correctly the phenyl group - C6H5)
hydroxides (ex: Ba(OH)2)

26. Does reactivity increase/decrease going down group 1 and group 17?
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?)
Sigma bonds are stronger than pi bonds
Group 1 hydroxides (ex: NaOH)
Increases down group 1 decreases down group 17

27. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
O2 needs 4F/mol H2 needs 2F/mol
K1 x K2
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
water and substances with (s) less dense than

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

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29. What are the common strong bases?
linear
Group 1 hydroxides (ex: NaOH)
ns² electrons (first in-first out)
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

30. Color is due to ______ _______ of light.
The dilution effect when the solutions mix. M1V1 = M2V2
fruit - fish - bases
Selective absorption
No - NH3 and HCl gases are extremely soluble

31. ammonium
NH4?
ion pairing
CnH(2n+2)
CO3²?

32. What part of a liquid do you look at to measure its volume?
Soluble
RX
Read the bottom of the meniscus
Soluble

33. What type of compounds do Group 14 form?
voltaic: - electrolytic: +
Clear
+4-covalent - +2-ionic
?H-kJ - ?S-J - ?G-kJ

34. perchlorate
ClO4?
Ksp = 4s³
NH2?
zero

35. Alkanes are _________ and react by _________
Evaporation
Saturated - Substitution (which requires more radical conditions)
Decant
The one with most oxygen atoms (highest oxidation number)

36. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Molecules with the same molecular formulas - but different structural formulas
ClO4?
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
catalyst=conc H2SO4

37. dichromate
boiling without losing volatile solvents/reactants
Cr2O7²?
water and substances with (s) less dense than
Pale purple - (orange)-yellow - red - blue - green.

38. dihydrogen phosphate
CnH(2n+2)
Pale purple - (orange)-yellow - red - blue - green.
H2PO4?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

39. If a weak acid is diluted more - what happens to its % dissociation value?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
CnH2n+2
Increases.
Reduction always takes place at the cathode (RED CAT) In both types of cell!

40. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
hydroxides (ex: Ba(OH)2)
The Faraday or Faraday's constant.
RCOOH

41. If Q < Ksp a ppt ______
proton donor base
Ppt will NOT form (unsaturated)
Q=It (time in seconds)
Add acid to water so that the acid doesn't boil and spit

42. silver compounds
Disulfur dichloride
Insoluble except for nitrate and acetate
They stay the same.
Insoluble (except group 1 ammonium and Ba)

43. copper sulfate
blue
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)
A salt solution.
boiling without losing volatile solvents/reactants

44. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
do not change
redox reaction
Soluble except Ag - Pb - Ca - Sr Ba)

45. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
water and substances with (s) less dense than
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
same KE - but PEice<PEwater

46. What changes Keq?
Silvery gray solid - brown - purple
ROH
Only temperature
Products - reactants (except for BDE when it's reactants - products)

47. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
yellow
Ksp = 27s4
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Mn²? - Cr³? - Cr³

48. chlorate
it is lower and occurs over less sharp a range
Acid rain - dissolves marble buildings/statues and kills trees.
ClO3?
Increases.

49. During a titration what is present in the beaker at the equivalence point?
Identity and purity (impure compounds usually have broad & low melting points)
A salt solution.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

50. What are amphoteric oxides?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
proton donor base
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?)
Salt + water.