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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. How do you find the pH for a dibasic acid? (H2A)?
atoms
Perform ICE BOX calculation based on K1
Saturated - Substitution (which requires more radical conditions)
No - NH3 and HCl gases are extremely soluble

2. halides
#ligands=charge x2
How grouped results are
Most are soluble except Ag - Pb
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

3. What process do you use to separate two liquids with different boiling points?
fractional distillation
H3PO4
blue
Ions go through the salt bridge - electrons go through metal wires in the external circuit

4. What is the pH of 1.0M HCl? 1M NaOH?
The one with most oxygen atoms (highest oxidation number)
blue (BTB)
Making sigma bonds and holding lone pairs
0 and 14

5. Name six characteristics of transition elements (or their compounds)
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)
Insoluble
C2O4²?
Big K=kf/kr

6. What is the third law of thermodynamics?
ROR
redox reaction
methyl formate
S crystal at 0K=0

7. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
do not change
Anode - oxygen. Cathode - hydrogen
Kc=Kp
Eudiometer

8. Acids + Carbonates (bicarbonates) make?
ethers
Only temperature
?G= -ve - E°= +ve
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

9. What is Big K in terms of kf and kr?
P2O5
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.
Cu3(PO4)2
Big K=kf/kr

10. Which alkali metals float on water?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Synthetic condensation polymer (aka a polyamide)
All except for lithium
bright yellow

11. Nonmetals are good _____ agents. Metals are good _______ agents.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
SO4²?
0.10M HCl (more ions)

12. What type of compounds do metals/non metals form?
Ionic compounds
RCOOR
OH?
atoms

13. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
RX
q=mc?T q=mL (or n x ?h)

14. A Bronsted-Lowry acid is...
CO2 and H2O
Saturated - Substitution (which requires more radical conditions)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
proton donor base

15. What do metal oxides plus acids form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Salt + water
Pale purple - (orange)-yellow - red - blue - green.
Transition element compounds (except if it has a full or empty d shell)

16. BaSO4
Products - reactants (except for BDE when it's reactants - products)
Insoluble
Iodine and CO2 (dry ice)
proton donor base

17. What part of a liquid do you look at to measure its volume?
K1 x K2
Read the bottom of the meniscus
an oxidized and reduced substance
by electrolysis

18. ________ are Lewis bases - because they can donate a lone pair of electrons.
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
OH- and NH3
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
bright yellow

19. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
it's lower and occurs over less sharp a range
Anode - oxygen. Cathode - hydrogen
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

20. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
White precipitate
Silvery gray solid - brown - purple
Increases down group 1 decreases down group 17

21. bromothymol
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
ClO3?
Combine the equations for the half reactions in the non-spontaneous direction
blue (BTB)

22. How can metals like iron and zinc be reduced?
small size and high charge
chemically (ex: with carbon)
allow for the vapor pressure of water and make sure to level levels
Experimental mass/theoretical mass X 100

23. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
H3PO4
?H formation of an element in standard state=0
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)

24. What does the solubility of organic compounds depend on?
NH2?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

25. copper sulfate
Group I metals (soft metals) are stored under oil
blue
C4H10
OH?

26. What process do you use to obtain a solvent from a solution?
Distillation
#ligands=charge x2
boiling without losing volatile solvents/reactants
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

27. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
CN?
water and substances with (s) less dense than
Evaporation
ROH

28. Does reactivity increase/decrease going down group 1 and group 17?
Suniverse increases for spontaneous processes
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?)
Increases down group 1 decreases down group 17
lighted splint (positive result=pop)

29. cyanide
CN?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Trigonal pyramidal
blue

30. potassium permanganate
CO2 and H2O
it is lower and occurs over less sharp a range
Purple
fractional distillation

31. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Salt and water
Glacial acetic acid
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
No - it depends on the number of ions produced on dissolving.

32. If Q < Ksp a ppt ______
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Ppt will NOT form (unsaturated)

33. thiosulfate
water and substances with (s) less dense than
S2O3²?
ROH
Molecules with the same molecular formulas - but different structural formulas

34. How do you compute % dissociation?
q=mc?T q=mL (or n x ?h)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Soluble

35. Generally - which oxy acid is strongest?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Insoluble except for nitrate and acetate
The one with most oxygen atoms (highest oxidation number)
same KE - but PEice<PEwater

36. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
H2PO4?
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.

37. sulfate
bases
Silvery gray solid - brown - purple
CN?
SO4²?

38. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
H2PO4?
ion pairing
same KE - but PEice<PEwater
Concentration

39. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
an oxidized and reduced substance
a-IMFs - b-molecular volume
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

40. What are isotopes?
C4H10
|experimental - accepted|/accepted X 100
They stay the same.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

41. ammonium/ammonium compounds
Insoluble except group 1 and ammonium
CnH2n+1 often designated 'R' ex C3H7 is propyl
Insoluble
Soluble

42. What is H2CO3 (carbonate acid) usually written as?
|experimental - accepted|/accepted X 100
Pale purple - (orange)-yellow - red - blue - green.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
H2O + CO2 (it decomposes readily)

43. How do you heat a test tube?
Products - reactants (except for BDE when it's reactants - products)
Heat a test tube at an angle at the side of the tube (not bottom)
allow for the vapor pressure of water and make sure to level levels
different forms of the same element

44. Alkanes are _________ and react by _________
Saturated - Substitution (which requires more radical conditions)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Decant

45. chlorite
fractional distillation
Perform ICE BOX calculation based on K1
redox reaction
ClO2?

46. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
Increases.
boiling without losing volatile solvents/reactants
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

47. How does group 1 metals' density compare to water's?
Synthetic condensation polymer (aka a polyamide)
RCOOR
are less dense than water
ClO3?

48. What is the difference between equivalence point and end point of a titration.
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.
Making sigma bonds and holding lone pairs
ClO4?
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

49. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
a-IMFs - b-molecular volume
They stay the same.

50. What type of compounds do Group 14 form?
+4-covalent - +2-ionic
PO4³?
acids
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant