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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 are two substances that sublime at 1 atm when heated?
CH3COO?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Salt and water
Iodine and CO2 (dry ice)

2. Generally - which oxy acid is strongest?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Combine the equations for the half reactions in the non-spontaneous direction
Silvery gray solid - brown - purple
The one with most oxygen atoms (highest oxidation number)

3. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Anode - oxygen. Cathode - hydrogen
Hg²?
bases

4. dichromate (soln + most solids)
No - it depends on the number of ions produced on dissolving.
Big K=kf/kr
Orange
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

5. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
it is lower and occurs over less sharp a range
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
hydroxides (ex: Ba(OH)2)

6. What do you use to look at burning magnesium? why?
No - NH3 and HCl gases are extremely soluble
Exothermic (?H for ANY sa/sb = -57kJ/mol)
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?)
blue glass - it filters UV

7. ammonium/ammonium compounds
allow for the vapor pressure of water and make sure to level levels
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Soluble
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

8. What are the formulas for q?
do not change
q=mc?T q=mL (or n x ?h)
No - it depends on the number of ions produced on dissolving.
At half equivalence - pH=pKa

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

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10. How can metals like iron and zinc be reduced?
Initiation energy (NOT Ea)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
chemically (ex: with carbon)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

11. silver compounds
A salt solution.
Insoluble except for nitrate and acetate
H+
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

12. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Kc=Kp
Clear
RCOOH
ClO4?

13. What is the general formula for an ether?
neutralization: high K - H2O product dissociation: low K - H2O reactant
?H-kJ - ?S-J - ?G-kJ
ROR
Group 1 hydroxides (ex: NaOH)

14. Aromatic compounds contain what?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Pour liquids using a funnel or down a glass rod
The benzene ring (or more correctly the phenyl group - C6H5)
Nothing

15. During a titration what is present in the beaker at the equivalence point?
ROH
NO3?
A salt solution.
SO4²?

16. What is the pH of 1.0M HCl? 1M NaOH?
Pour liquids using a funnel or down a glass rod
small size and high charge
Pale yellow
0 and 14

17. mercury (II) ion
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.
Hg²?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
H2PO4?

18. 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
Mono; di; tri; tetra; penta; hexa.
ROH
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

19. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
P2O5
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Eudiometer

20. What is the name of S2Cl2? (Know how to name others like this - too)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Check for air bubbles in the buret and remove the buret funnel from the buret
Disulfur dichloride

21. What process do you use to separate two liquids with different boiling points?
brown volatile liquid
No - it depends on the number of ions produced on dissolving.
fractional distillation
Conjugate pair (one must be a weak base or acid)

22. When is ?G zero?
linear
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
S2O3²?
Hg²?

23. perchlorate
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
ClO4?
bright yellow
Big K=kf/kr

24. What is the formula for percent yield?
Cu3(PO4)2
Experimental mass/theoretical mass X 100
Soluble
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

25. When combining half equations - what do you do to E° values when multiplying coefficients?
Separating funnel
NO3?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Nothing

26. thiosulfate
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
bent
Ppt will NOT form (unsaturated)
S2O3²?

27. lead compounds
Evaporation
Insoluble except nitrate and acetate
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

28. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Identity and purity (impure compounds usually have broad & low melting points)
zero
Glowing splint (positive result=relights)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

29. What is the conjugate base of NH3?
NH2?
Glowing splint (positive result=relights)
Soluble
White precipitate

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
All except for lithium
Ionic compounds
Current - time and charge on ion (moles of e used in half cell reaction)

31. What does a short - sharp melting point indicate?
|experimental - accepted|/accepted X 100
H2PO4?
H3PO4
Identity and purity (impure compounds usually have broad & low melting points)

32. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
basic
Mn²? - Cr³? - Cr³
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

33. What electrons are lost/gained first in transition element ions?
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)
HClO4
ns² electrons (first in-first out)
Graduated cylinder

34. Acid plus base make?
An active metal.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Salt + water.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

35. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Insoluble except for nitrate and acetate
voltaic: + electrolytic: -
All except for lithium

36. At what point during titration do you have the perfect buffer - and what is the pH at this point?
blue (BTB)
At half equivalence - pH=pKa
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
look for changes in oxidation # - the one that goes up is oxidized and is the RA

37. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Only temperature
same KE - but PEice<PEwater
?G= -ve - E°= +ve

38. What do you need to make a polymer?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
How close results are to the accepted value
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
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)

39. What process do you use to obtain a solvent from a solution?
water and substances with (s) less dense than
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Distillation
different forms of the same element

40. carbonates
Insoluble except group 1 and ammonium
Heat a test tube at an angle at the side of the tube (not bottom)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
The Faraday or Faraday's constant.

41. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
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
linear
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
water and substances with (s) less dense than

42. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Trigonal pyramidal
They decrease (or could be the same if the solid has ONLY JUST disappeared)
The Faraday or Faraday's constant.
OH?

43. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
voltaic: + electrolytic: -
CO2 and H2O
Graduated cylinder

44. What is Big K in terms of kf and kr?
Exothermic
Big K=kf/kr
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
OH?

45. What do nonmetal oxides plus water form?
H+
Cr2O7²?
No - NH3 and HCl gases are extremely soluble
acids

46. Can you collect soluble gases over water?
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)
CnH2n
No - NH3 and HCl gases are extremely soluble
Clear

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

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48. What steps do organic labs consist of?
Synthesis - separation and purification of the product and its identification.
0 and 14
Current - time and charge on ion (moles of e used in half cell reaction)
Iodine and CO2 (dry ice)

49. What is the test for oxygen?
Increases down group 1 decreases down group 17
MnO4?
Glowing splint (positive result=relights)
Saturated - Substitution (which requires more radical conditions)

50. ammonium
NH4?
Q=It (time in seconds)
The compound with the lowest Ksp value.
A) any range. b) 8-10 c) 4-6