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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 is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Disulfur dichloride
lighted splint (positive result=pop)
Distillation
Ksp = 27s4

2. What is the general formula for an ester?
Synthetic condensation polymer (aka a polyamide)
fractional distillation
RCOOR
Glowing splint (positive result=relights)

3. Acid plus base make?
Pipette (burette if need repetition)
Cu3(PO4)2
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Salt + water.

4. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
P2O5
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
boiling without losing volatile solvents/reactants

5. dichromate
Increases.
Cr2O7²?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
?H formation of an element in standard state=0

6. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
0 and 14
More chaotic (ex: gases made)
Insoluble except for nitrate and acetate
same KE - but PEice<PEwater

7. What is the relationship in strength between sigma and pi bonds?
ROR
Selective absorption
Sigma bonds are stronger than pi bonds
Salt + water.

8. chlorite
Experimental mass/theoretical mass X 100
OH- and NH3
ClO2?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

9. Alcohols and _______ are FG isomers
Sigma bonds are stronger than pi bonds
blue
ethers
Evaporation

10. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Pour liquids using a funnel or down a glass rod
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
ROR
by electrolysis

11. What do hydrocarbons form when they burn in air (oxygen)?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
CO2 and H2O
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Add acid to water so that the acid doesn't boil and spit

12. What type of compounds do metals/non metals form?
Ionic compounds
The compound with the lowest Ksp value.
Eudiometer
Increases down group 1 decreases down group 17

13. How many ligands attach to a central ion in a complex ion?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
C2O4²?
Selective absorption
#ligands=charge x2

14. What word is a clue for a redox reaction?
Acidified
bent
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
No - it depends on the number of ions produced on dissolving.

15. Is the ?H formation of an element in standard state zero?
zero
?H formation of an element in standard state=0
Increases.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

16. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
blue (BTB)
?G=negative - E° must be positive
Ksp = 108s5
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

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

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18. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
The dilution effect when the solutions mix. M1V1 = M2V2
do not change

19. sulfates
RNH2
Soluble except Ag - Pb - Ca - Sr Ba)
a-IMFs - b-molecular volume
ROH

20. 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.
OH?
Molecules with the same molecular formulas - but different structural formulas
A) any range. b) 8-10 c) 4-6
Insoluble except for nitrate and acetate

21. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
ClO?
Exothermic
Read the bottom of the meniscus

22. Where are group I metals stored?
Group I metals (soft metals) are stored under oil
Insoluble except for nitrate and acetate
CnH2n+2
blue glass - it filters UV

23. Which of the rates changes more when temperature is increased?
voltaic: - electrolytic: +
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
RCOR
ion pairing

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

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25. permanganate
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Experimental mass/theoretical mass X 100
MnO4?
-Ea/R

26. What are the prefixes for the naming of binary molecular compound formulas (up to six)
?H formation of an element in standard state=0
Mono; di; tri; tetra; penta; hexa.
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
by electrolysis

27. chromate ion (soln + most solids)
0.10M HCl (more ions)
yellow
RNH2
Nothing

28. What is HCOOCH3?
NH4?
Acids; HCOOCH3 is an ester
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
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

29. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Graduated cylinder
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
non-metal oxides and hydrides are covalently bonded and are acidic.

30. How do you compute % dissociation?
Glowing splint (positive result=relights)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
[A?]/[HA] x 100 or [BH?]/[B] x 100
CO3²?

31. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Ksp = 27s4
Reduction always takes place at the cathode (RED CAT) In both types of cell!
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
E=q + w (negative is by system - positive is on system)

32. What is the general formula for alkyl halides?
CnH(2n+2)
RX
H+
Group I metals (soft metals) are stored under oil

33. carbonate
CO3²?
Iodine and CO2 (dry ice)
RCOR
Combine the equations for the half reactions in the non-spontaneous direction

34. What is the first law of thermodynamics?
left - ppt will form
E=q + w (negative is by system - positive is on system)
bases
Experimental mass/theoretical mass X 100

35. What is Big K in terms of kf and kr?
Increases.
voltaic: - electrolytic: +
NH4?
Big K=kf/kr

36. What are two allotropes of carbon?
Anode
SO4²?
diamond and graphite
CnH2n

37. What things should you remember to do when collecting gas over water?
PO4³?
allow for the vapor pressure of water and make sure to level levels
No - it depends on the number of ions produced on dissolving.
Ions go through the salt bridge - electrons go through metal wires in the external circuit

38. What is the formula for alkynes?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Anode - oxygen. Cathode - hydrogen
The compound with the lowest Ksp value.
CnH2n-2

39. What measuring device would you use for very small volumes of liquids?
The dilution effect when the solutions mix. M1V1 = M2V2
Pipette (burette if need repetition)
voltaic: + electrolytic: -
left - ppt will form

40. A Bronsted-Lowry acid is...
proton donor base
voltaic: - electrolytic: +
The Faraday or Faraday's constant.
benzene is less reactive than alkenes

41. dihydrogen phosphate
same KE - but PEice<PEwater
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
small size and high charge
H2PO4?

42. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
ionic and form hydrogen and hydroxide
R=8.31 J/mol/K
CO (poisonous)

43. When the salt bridge is removed what happens to the cell reaction?
RX
It ceases - the circuit is broken.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
acids

44. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Synthetic condensation polymer (aka a polyamide)
Ksp = 108s5

45. halides
Synthetic condensation polymer (aka a polyamide)
Most are soluble except Ag - Pb
H+
K1 x K2

46. mercury (I) ion
Hg2²?
A) any range. b) 8-10 c) 4-6
Eudiometer
acids

47. What is the formula of copper (II) phosphate?
OH- and NH3
Cu3(PO4)2
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Acids; HCOOCH3 is an ester

48. hydroxides
Anode
Identity and purity (impure compounds usually have broad & low melting points)
Ksp = s²
Insoluble (except group 1 ammonium and Ba)

49. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
CnH2n
K1 x K2
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

50. silver iodide
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Pale yellow
Transition element compounds (except if it has a full or empty d shell)
Eudiometer