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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. Does Benzene react by addition or substitution?
Soluble
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
it reacts by substitution NOT addition
proton donor base

2. oxalate
C2O4²?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Conjugate pair (one must be a weak base or acid)
Pale purple - (orange)-yellow - red - blue - green.

3. Generally - which oxy acid is strongest?
Disulfur dichloride
non-metal oxides and hydrides are covalently bonded and are acidic.
The one with most oxygen atoms (highest oxidation number)
K2

4. Acids + Carbonates (bicarbonates) make?
Glacial acetic acid
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Mn²? - Cr³? - Cr³

5. What do metal oxides plus non- metal oxides form?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Salts (ex: CaO + SO2 ? CaSO3)
CnH2n+1 often designated 'R' ex C3H7 is propyl
Combine the equations for the half reactions in the non-spontaneous direction

6. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
do not change
it's lower and occurs over less sharp a range
water and substances with (s) less dense than
Pour liquids using a funnel or down a glass rod

7. If Q > Ksp - then system shifts _______ and ppt ______
But S° of element is not zero (except at 0K)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
left - ppt will form
Group 1 hydroxides (ex: NaOH)

8. Is the freezing of ice endothermic or exothermic?
A salt solution.
+4-covalent - +2-ionic
different forms of the same element
Exothermic

9. mercury (II) ion
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Ksp = s²
Hg²?

10. Why are i factors (Van't Hoff factors) often less than ideal?
linear
Evaporation
Selective absorption
ion pairing

11. What is the energy you must put into a reaction to make it start called?
ns² electrons (first in-first out)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
It ceases - the circuit is broken.
Initiation energy (NOT Ea)

12. barium sulfate
They decrease (or could be the same if the solid has ONLY JUST disappeared)
allow for the vapor pressure of water and make sure to level levels
White precipitate
Pale purple - (orange)-yellow - red - blue - green.

13. How can metals like iron and zinc be reduced?
CO3²?
chemically (ex: with carbon)
atoms
ClO2?

14. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
an oxidized and reduced substance
Salt and water
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

15. What do you do to get rid of most of the solution from a precipitate?
Decant
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Perform ICE BOX calculation based on K1
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

16. How many normal boiling points and boiling points are there?

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17. Do anions flow to the cathode or anode?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
An active metal.
Anode
Nothing

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

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19. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
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)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Current - time and charge on ion (moles of e used in half cell reaction)
They stay the same.

20. What apparatus do you use to pour liquids?
?H-kJ - ?S-J - ?G-kJ
Pour liquids using a funnel or down a glass rod
The one with most oxygen atoms (highest oxidation number)
lighted splint (positive result=pop)

21. hydroxides
Insoluble (except group 1 ammonium and Ba)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
The compound with the lowest Ksp value.

22. Is a graduated cylinder or beaker more accurate?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
zero-th: decreases - first: constant - second: increases
Graduated cylinder
it's lower and occurs over less sharp a range

23. What is the charge on a chlorine atom?
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
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
zero
Tetrahedral

24. Which value of R do you use for all energy and kinetics calculations?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
R=8.31 J/mol/K
Pale yellow
Glacial acetic acid

25. dihydrogen phosphate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
The compound with the lowest Ksp value.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
H2PO4?

26. When the salt bridge is removed what happens to the cell reaction?
C2O4²?
It ceases - the circuit is broken.
K1 x K2
a-IMFs - b-molecular volume

27. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Eudiometer
The compound with the lowest Ksp value.
RCOOH
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

28. What is the sign of the anode in voltaic cells? in electrolytic cells?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
voltaic: - electrolytic: +
Soluble
proton acceptor.

29. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
An active metal.
zero
E=q + w (negative is by system - positive is on system)

30. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
fruit - fish - bases
Soluble
redox reaction

31. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
Soluble
The compound with the lowest Ksp value.
Current - time and charge on ion (moles of e used in half cell reaction)

32. What is the name of S2Cl2? (Know how to name others like this - too)
Silvery gray solid - brown - purple
Disulfur dichloride
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

33. What electrons are lost/gained first in transition element ions?
blue (BTB)
RCOOR
An active metal.
ns² electrons (first in-first out)

34. Esters smell like _______ and amines smell like _______ and are ______.
Filtration
fruit - fish - bases
Add acid to water so that the acid doesn't boil and spit
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

35. What shape is methane?
Tetrahedral
Identity and purity (impure compounds usually have broad & low melting points)
do not change
Most INsoluble except group 1 and ammonium

36. ammonium
NH4?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
The compound with the lowest Ksp value.
The benzene ring (or more correctly the phenyl group - C6H5)

37. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
ion pairing
The dilution effect when the solutions mix. M1V1 = M2V2

38. What are the signs for ?G and E° for spontaneous reactions?
Acids; HCOOCH3 is an ester
CH3COO?
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
?G= -ve - E°= +ve

39. The definition of acidic basic and neutral aqueous solutions is:
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?)
Pale yellow
H3PO4
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

40. What is the general formula for alkyl halides?
Group I metals (soft metals) are stored under oil
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?)
RX
it reacts by substitution NOT addition

41. What are two substances that sublime at 1 atm when heated?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Iodine and CO2 (dry ice)
Both electrons come from the same atom (just as good as a regular bond)
Clear

42. If ?S is positive - are the products more or less chaotic than the reactants?
Silvery gray solid - brown - purple
More chaotic (ex: gases made)
small size and high charge
|experimental - accepted|/accepted X 100

43. What type of compounds do metals/non metals form?
Salt + water.
Ksp = 108s5
H2PO4?
Ionic compounds

44. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
A) any range. b) 8-10 c) 4-6
More chaotic (ex: gases made)
CnH2n

45. Can you collect soluble gases over water?
Purple
No - NH3 and HCl gases are extremely soluble
voltaic: - electrolytic: +
Soluble except Ag - Pb - Ca - Sr Ba)

46. Why are noble gases stable?
water and substances with (s) less dense than
Mn²? - Cr³? - Cr³
Identity and purity (impure compounds usually have broad & low melting points)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

47. What process do you use to obtain the precipitate from a solution?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Filtration
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

48. 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.
Combine the equations for the half reactions in the non-spontaneous direction
Mn²? - Cr³? - Cr³
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

49. What do the 'a' and 'b' in Van Der Waal's equation allow for?
CnH2n
RCOOH
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
a-IMFs - b-molecular volume

50. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
blue (BTB)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Pale yellow
Ionic compounds