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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. oxalate
C2O4²?
Identity and purity (impure compounds usually have broad & low melting points)
NH4?
different forms of the same element

2. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
zero
Concentration

3. How many faradays of electric charge do you need to produce one mole of O2? H2?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
O2 needs 4F/mol H2 needs 2F/mol
CO3²?
Insoluble except group 1 and ammonium

4. When driving off water from a hydrate - how do you tell you're done?
basic
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
ClO2?
Soluble

5. Acid plus base make?
Salt + water.
Trigonal pyramidal
Most INsoluble except group 1 and ammonium
Reduction always takes place at the cathode (RED CAT) In both types of cell!

6. group 1 ions/compounds
Filtration
0 and 14
Soluble
it's lower and occurs over less sharp a range

7. What are the names and formulas of the 6 strong acids?
No - it depends on the number of ions produced on dissolving.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Pale yellow
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

8. The oxidation # for acid base reactions...
No - NH3 and HCl gases are extremely soluble
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
allow for the vapor pressure of water and make sure to level levels
do not change

9. Where are group I metals stored?
NH2?
No - NH3 and HCl gases are extremely soluble
Iodine and CO2 (dry ice)
Group I metals (soft metals) are stored under oil

10. acetate
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Selective absorption
CH3COO?

11. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
zero
Ksp = 108s5
Disulfur dichloride
an oxidized and reduced substance

12. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Anode
H3PO4

13. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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14. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Insoluble except nitrate and acetate
basic
Reduction always takes place at the cathode (RED CAT) In both types of cell!

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

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16. What do you use to look at burning magnesium? why?
Evaporation
White precipitate
blue glass - it filters UV
fractional distillation

17. What is the third law of thermodynamics?
S crystal at 0K=0
White precipitate
allow for the vapor pressure of water and make sure to level levels
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

18. If Q < Ksp a ppt ______
T increases exponentially the proportion of molecules with E > Ea
Add acid to water so that the acid doesn't boil and spit
ion pairing
Ppt will NOT form (unsaturated)

19. What is the name of S2Cl2? (Know how to name others like this - too)
-Ea/R
Disulfur dichloride
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Mono; di; tri; tetra; penta; hexa.

20. What are amphoteric oxides?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
are less dense than water
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?)
Most INsoluble except group 1 and ammonium

21. How do you identify which is oxidized or otherwise?
OH- and NH3
A salt solution.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

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

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23. Why are noble gases stable?
fruit - fish - bases
a-IMFs - b-molecular volume
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Selective absorption

24. How do you clean a buret/pipette for a titration?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Mn²? - Cr³? - Cr³
Heat a test tube at an angle at the side of the tube (not bottom)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

25. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
basic
water and substances with (s) less dense than
[A?]/[HA] x 100 or [BH?]/[B] x 100

26. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
ion pairing
The benzene ring (or more correctly the phenyl group - C6H5)
hydroxides (ex: Ba(OH)2)

27. Which of the rates changes more when temperature is increased?
Heptane
Soluble
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

28. What is Big K in terms of kf and kr?
redox reaction
Big K=kf/kr
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Iodine and CO2 (dry ice)

29. Do anions flow to the cathode or anode?
red - green - blue
Time?¹ - (ex. s?¹ - hr?¹ - etc)
blue glass - it filters UV
Anode

30. When combining half equations - what do you do to E° values when multiplying coefficients?
Separating funnel
Nothing
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
do not change

31. What device would you use to measure a volume of gas?
Insoluble (except group 1 ammonium and Ba)
Eudiometer
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

32. What is the test for oxygen?
Perform ICE BOX calculation based on K1
Glowing splint (positive result=relights)
P2O5
same KE - but PEice<PEwater

33. hypochlorite
0 and 14
same KE - but PEice<PEwater
ClO?
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.

34. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
Sigma bonds are stronger than pi bonds
blue
strong acids/bases are written as H+ or OH- ions

35. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
bright yellow
CnH2n+1 often designated 'R' ex C3H7 is propyl

36. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Insoluble
Salt + water.

37. What apparatus do you use to pour liquids?
Most are soluble except Ag - Pb
Pour liquids using a funnel or down a glass rod
fractional distillation
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

38. How are strong ones written?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
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
Soluble
strong acids/bases are written as H+ or OH- ions

39. Can you collect soluble gases over water?
Sulfur
no - they're written undissociated (HAaq)
No - NH3 and HCl gases are extremely soluble
OH- and NH3

40. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
Nothing
benzene is less reactive than alkenes
P2O5
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

41. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
RCOOH
H2PO4?
Filtration

42. What process do you use to obtain a solvent from a solution?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
0 and 14
Distillation
diamond and graphite

43. What is the general formula for alkyl halides?
Iodine and CO2 (dry ice)
RX
metal oxides and hydrides are ionically bonded and basic
Insoluble

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

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45. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Cr2O7²?
RX

46. What type of compounds do Group 14 form?
+4-covalent - +2-ionic
ethers
same KE - but PEice<PEwater
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

47. hydroxide
OH?
Ksp = 108s5
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)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

48. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
RCOR
H2O + CO2 (it decomposes readily)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

49. How does the melting point of a mixture compare to the MP of a pure substance?
More chaotic (ex: gases made)
bent
no - they're written undissociated (HAaq)
it is lower and occurs over less sharp a range

50. If a weak acid is diluted more - what happens to its % dissociation value?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Read the bottom of the meniscus
OH- and NH3
Increases.