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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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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 the formula for alkenes?
Pale yellow
CnH2n
Add acid to water so that the acid doesn't boil and spit
acid + alcohol

2. What two compounds are great oxidizing agents?

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3. What are the signs of ?G and E° for spontaneous reactions?
zero
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Insoluble except for nitrate and acetate
?G=negative - E° must be positive

4. What steps do organic labs consist of?
brown volatile liquid
Both electrons come from the same atom (just as good as a regular bond)
Synthesis - separation and purification of the product and its identification.
acids

5. sulfate
How close results are to the accepted value
?G=negative - E° must be positive
But S° of element is not zero (except at 0K)
SO4²?

6. Does Kw increase or decrease with T? Why?
0 and 14
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Soluble

7. Color (absorbance) is proportional to ________
CO3²?
Concentration
Filtration
R=8.31 J/mol/K

8. A Bronsted-Lowry base is...
Soluble
A salt solution.
proton acceptor.
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)

9. How does group 1 metals' density compare to water's?
Greenish-yellow gas
Group I metals (soft metals) are stored under oil
hydroxides (ex: Ba(OH)2)
are less dense than water

10. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
CrO4²?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
water and substances with (s) less dense than

11. What type of solutions do small - highly charged cations tend to form?
Ksp = s²
neutralization: high K - H2O product dissociation: low K - H2O reactant
0.10M HCl (more ions)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

12. Why are i factors (Van't Hoff factors) often less than ideal?
boiling without losing volatile solvents/reactants
ion pairing
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Insoluble except nitrate and acetate

13. What shape is water?
Decant
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
C4H10
bent

14. What element is used to vulcanize rubber?
Ksp = s²
Sulfur
NH2?
blue (BTB)

15. What is the general formula for alkyl halides?
|experimental - accepted|/accepted X 100
Insoluble except for nitrate and acetate
RX
different forms of the same element

16. oxalate
The Faraday or Faraday's constant.
Ksp = 4s³
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
C2O4²?

17. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
H2O + CO2 (it decomposes readily)
yellow
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CO (poisonous)

18. The oxidation # for acid base reactions...
Insoluble except for nitrate and acetate
different forms of the same element
R=8.31 J/mol/K
do not change

19. BaSO4
Insoluble
Insoluble (except group 1 ammonium and Ba)
Most INsoluble except group 1 and ammonium
small size and high charge

20. Give an example of a concentrated weak acid.
Glacial acetic acid
it is lower and occurs over less sharp a range
Selective absorption
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

21. An amphiprotic (amphoteric) species is...
Insoluble (except group 1 ammonium and Ba)
Q=It (time in seconds)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

22. What are two substances that sublime at 1 atm when heated?
S crystal at 0K=0
a-IMFs - b-molecular volume
Glowing splint (positive result=relights)
Iodine and CO2 (dry ice)

23. What word is a clue for a redox reaction?
Pale purple - (orange)-yellow - red - blue - green.
blue
CH3COO?
Acidified

24. What are the units of the first order rate constant?
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)
ClO3?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
OH- and NH3

25. During a titration what is present in the beaker at the equivalence point?
-Ea/R
A salt solution.
?G=negative - E° must be positive
water and substances with (s) less dense than

26. cyanide
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
voltaic: + electrolytic: -
CN?
The compound with the lowest Ksp value.

27. What is the formula for alkanes?
left - ppt will form
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
CnH2n+2

28. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
Unsaturated - addition (ex: decolorize bromine solution)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

29. Both Acetic acid and ____________ are also functional isomers.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Anode - oxygen. Cathode - hydrogen
How grouped results are
methyl formate

30. What are allotropes?
CnH2n
different forms of the same element
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Kc=Kp

31. What is accuracy?
The Faraday or Faraday's constant.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
How close results are to the accepted value
P2O5

32. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
0 and 14
Glacial acetic acid
Salt and water

33. What do the 'a' and 'b' in Van Der Waal's equation allow for?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
a-IMFs - b-molecular volume
Experimental mass/theoretical mass X 100
ethers

34. What do you need to make a polymer?
CO2 and H2O
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)
Increases down group 1 decreases down group 17
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

35. How many faradays of electric charge do you need to produce one mole of O2? H2?
Group 1 hydroxides (ex: NaOH)
Kc=Kp
Check for air bubbles in the buret and remove the buret funnel from the buret
O2 needs 4F/mol H2 needs 2F/mol

36. What is the slope of the graph of lnk vs. 1/T?
Iodine and CO2 (dry ice)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
-Ea/R
Synthetic condensation polymer (aka a polyamide)

37. What is the formula for obtaining charge flowing in a cell?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Q=It (time in seconds)
NH2?
fruit - fish - bases

38. chlorine
ROR
[A?]/[HA] x 100 or [BH?]/[B] x 100
Greenish-yellow gas
Glowing splint (positive result=relights)

39. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Glowing splint (positive result=relights)
zero

40. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
zero
same KE - but PEice<PEwater
How close results are to the accepted value
Identity and purity (impure compounds usually have broad & low melting points)

41. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
Saturated - Substitution (which requires more radical conditions)
are less dense than water
Acids; HCOOCH3 is an ester

42. What do ions and electrons travel through in a voltaic/electrolytic cell?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Graduated cylinder
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

43. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Tetrahedral
Ppt will NOT form (unsaturated)
They stay the same.

44. Color is due to ______ _______ of light.
Selective absorption
An active metal.
ROH
The benzene ring (or more correctly the phenyl group - C6H5)

45. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
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.
Soluble
it reacts by substitution NOT addition
water and substances with (s) less dense than

46. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
Synthesis - separation and purification of the product and its identification.
H2PO4?
Filtration

47. Why are noble gases stable?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
P2O5
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
NH2?

48. What apparatus do you use to separate 2 immiscible liquids?
CO (poisonous)
Separating funnel
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

49. What apparatus do you use to pour liquids?
Pour liquids using a funnel or down a glass rod
Soluble
Mono; di; tri; tetra; penta; hexa.
CN?

50. Alkenes are ________ and react by __________
Pipette (burette if need repetition)
Unsaturated - addition (ex: decolorize bromine solution)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Synthesis - separation and purification of the product and its identification.