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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 changes Keq?
E=q + w (negative is by system - positive is on system)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Only temperature
Insoluble (except group 1 ammonium and Ba)

2. barium sulfate
Molecules with the same molecular formulas - but different structural formulas
?G= -ve - E°= +ve
Reduction always takes place at the cathode (RED CAT) In both types of cell!
White precipitate

3. mercury (II) ion
Hg²?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
RCOOR
water and substances with (s) less dense than

4. What is the formula for alkanes?
CnH2n+2
Increases.
Tetrahedral
Insoluble except group 1 and ammonium

5. What is the general formula for alkyl halides?
Insoluble except nitrate and acetate
The Faraday or Faraday's constant.
S crystal at 0K=0
RX

6. What is the catalyst for this reaction Ester + ?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
catalyst=conc H2SO4
No - NH3 and HCl gases are extremely soluble
water and substances with (s) less dense than

7. 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)
no - they're written undissociated (HAaq)
Ksp = 108s5
ns² electrons (first in-first out)

8. An amphiprotic (amphoteric) species is...
NH2?
linear
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
HClO4

9. What are the units of the first order rate constant?
Anode - oxygen. Cathode - hydrogen
CH3COO?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Soluble

10. What process do you use to obtain a solvent from a solution?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Disulfur dichloride
Distillation
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

11. What two compounds are great oxidizing agents?

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12. copper sulfate
proton acceptor.
blue
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Sulfur

13. What are the signs for ?G and E° for spontaneous reactions?
Initiation energy (NOT Ea)
?G= -ve - E°= +ve
small size and high charge
How close results are to the accepted value

14. What is the general formula for an ester?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
RCOOR
small size and high charge

15. What is the general formula for an aldehyde?
OH?
RCHO (carbonyl at end)
ionic and form hydrogen and hydroxide
ion pairing

16. What is the energy you must put into a reaction to make it start called?
It ceases - the circuit is broken.
P2O5
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Initiation energy (NOT Ea)

17. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
blue (BTB)
OH?
E=q + w (negative is by system - positive is on system)
basic

18. What is the sign of the cathode in voltaic cells? in electrolytic cells?
C2O4²?
Silvery gray solid - brown - purple
voltaic: + electrolytic: -
NH4?

19. If Q > Ksp - then system shifts _______ and ppt ______
ion pairing
left - ppt will form
ion pairing
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

20. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Acid rain - dissolves marble buildings/statues and kills trees.
brown volatile liquid
Check for air bubbles in the buret and remove the buret funnel from the buret
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

21. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
The compound with the lowest Ksp value.
Insoluble except nitrate and acetate
Experimental mass/theoretical mass X 100
Increases down group 1 decreases down group 17

22. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
RCOOH
CrO4²?
Perform ICE BOX calculation based on K1
same KE - but PEice<PEwater

23. Alcohols and _______ are FG isomers
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
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)
ethers
HClO4

24. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
metal oxides and hydrides are ionically bonded and basic
same KE - but PEice<PEwater
bases
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

25. carbonate
bent
CO3²?
Insoluble except group 1 and ammonium
water and substances with (s) less dense than

26. Do anions flow to the cathode or anode?
fractional distillation
Acidified
Anode
Soluble

27. What is the formula for percent error?
K1 x K2
Increases down group 1 decreases down group 17
|experimental - accepted|/accepted X 100
ClO4?

28. How do you find the pH for a dibasic acid? (H2A)?
0.10M HCl (more ions)
Perform ICE BOX calculation based on K1
A salt solution.
benzene has a delocalized pi ring structure

29. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Greenish-yellow gas
Mn²? - Cr³? - Cr³
NO3?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

30. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
bent
+4-covalent - +2-ionic
do not change

31. What is the general formula for an acid?
ion pairing
RCOOH
atoms
CN?

32. What do you use for an acid spill? base spill?
do not change
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
blue
The one with most oxygen atoms (highest oxidation number)

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

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34. What type of compounds are almost always colored?
Ksp = 27s4
Insoluble except for nitrate and acetate
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Transition element compounds (except if it has a full or empty d shell)

35. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Decant
NH4?
Acid rain - dissolves marble buildings/statues and kills trees.

36. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Big K=kf/kr
+4-covalent - +2-ionic

37. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Clear
10?8

38. What is the formula of butane?
zero
Glowing splint (positive result=relights)
C4H10
Greenish-yellow gas

39. What electrons are lost/gained first in transition element ions?
Anode - oxygen. Cathode - hydrogen
small size and high charge
ns² electrons (first in-first out)
Eudiometer

40. What is the formula of copper (II) phosphate?
Cu3(PO4)2
Exothermic
Acidified
same KE - but PEice<PEwater

41. What is the first law of thermodynamics?
bases
NH4?
E=q + w (negative is by system - positive is on system)
chemically (ex: with carbon)

42. What is the general formula for an alcohol?
Saturated - Substitution (which requires more radical conditions)
ROH
CO (poisonous)
At half equivalence - pH=pKa

43. What is the formula for alkenes?
CnH2n
Soluble
it is lower and occurs over less sharp a range
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)

44. sulfates
benzene has a delocalized pi ring structure
Pipette (burette if need repetition)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Soluble except Ag - Pb - Ca - Sr Ba)

45. chlorine
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Filtration
All except for lithium
Greenish-yellow gas

46. 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.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Check for air bubbles in the buret and remove the buret funnel from the buret
ROR

47. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
acid + alcohol
Cr2O7²?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

48. What type of compounds do metals/non metals form?
Ionic compounds
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Insoluble except for nitrate and acetate
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)

49. Aromatic compounds contain what?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
A) any range. b) 8-10 c) 4-6
Iodine and CO2 (dry ice)
The benzene ring (or more correctly the phenyl group - C6H5)

50. What is the slope of the graph of lnk vs. 1/T?
0.10M HCl (more ions)
benzene is less reactive than alkenes
Current - time and charge on ion (moles of e used in half cell reaction)
-Ea/R