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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 are the signs for ?G and E° for spontaneous reactions?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
ROR
Anode - oxygen. Cathode - hydrogen
?G= -ve - E°= +ve

2. What is the formula for obtaining charge flowing in a cell?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
do not change
Perform ICE BOX calculation based on K1
Q=It (time in seconds)

3. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Combine the equations for the half reactions in the non-spontaneous direction
Ksp = 27s4
Only temperature
|experimental - accepted|/accepted X 100

4. 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)
Ionic compounds
Anode - oxygen. Cathode - hydrogen
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

5. What steps do organic labs consist of?
Synthesis - separation and purification of the product and its identification.
No - NH3 and HCl gases are extremely soluble
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
zero

6. chlorate
MnO4?
ClO3?
lighted splint (positive result=pop)
Soluble

7. What do ions and electrons travel through in a voltaic/electrolytic cell?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Q=It (time in seconds)
Iodine and CO2 (dry ice)

8. What is the general formula for an aldehyde?
E=q + w (negative is by system - positive is on system)
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?)
RCHO (carbonyl at end)
metal oxides and hydrides are ionically bonded and basic

9. halides
Ksp = 27s4
brown volatile liquid
RCOOR
Most are soluble except Ag - Pb

10. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Insoluble except group 1 and ammonium
benzene is less reactive than alkenes

11. chlorite
Only temperature
ClO2?
a-IMFs - b-molecular volume
zero

12. What effect does increasing the size/surface area of a voltaic cell have on the cell?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
chemically (ex: with carbon)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Pipette (burette if need repetition)

13. Metal hydrides are _____ and form _______ and _______ when added to water
Group I metals (soft metals) are stored under oil
CnH(2n+2)
Hg²?
ionic and form hydrogen and hydroxide

14. What is the pH of 1.0M HCl? 1M NaOH?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
They stay the same.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
0 and 14

15. What are the common strong bases?
ethers
Group 1 hydroxides (ex: NaOH)
T increases exponentially the proportion of molecules with E > Ea
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

16. Can you collect soluble gases over water?
left - ppt will form
The one with most oxygen atoms (highest oxidation number)
No - NH3 and HCl gases are extremely soluble
ROR

17. An amphiprotic (amphoteric) species is...
a-IMFs - b-molecular volume
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
yellow

18. What do metal oxides plus non- metal oxides form?
same KE - but PEice<PEwater
Salts (ex: CaO + SO2 ? CaSO3)
Distillation
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

19. chromate
Nothing
Soluble
same KE - but PEice<PEwater
CrO4²?

20. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
are less dense than water
Disulfur dichloride
Mn²? - Cr³? - Cr³

21. How do you heat a test tube?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
H+
Heat a test tube at an angle at the side of the tube (not bottom)
strong acids/bases are written as H+ or OH- ions

22. What is the second law of thermodynamics?
zero
Suniverse increases for spontaneous processes
No - it depends on the number of ions produced on dissolving.
+4-covalent - +2-ionic

23. What is the formula of copper (II) phosphate?
ClO?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Cu3(PO4)2
Experimental mass/theoretical mass X 100

24. What is the word equation for addition polymerisation?
Identity and purity (impure compounds usually have broad & low melting points)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Ksp = s²
it's lower and occurs over less sharp a range

25. Does Kw increase or decrease with T? Why?
PO4³?
zero
ClO2?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

26. How do you explain trends in atomic properties using Coulomb's Law?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Initiation energy (NOT Ea)
CnH2n-2
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

27. What shape is water?
bent
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
More chaotic (ex: gases made)
ethers

28. What do you use to look at burning magnesium? why?
lighted splint (positive result=pop)
blue glass - it filters UV
ROR
Insoluble except nitrate and acetate

29. nitrate
Sigma bonds are stronger than pi bonds
NO3?
Graduated cylinder
CnH2n+2

30. What are two substances that sublime at 1 atm when heated?
Disulfur dichloride
Iodine and CO2 (dry ice)
Products - reactants (except for BDE when it's reactants - products)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

31. When a cell is 'flat' What is its voltage?
neutralization: high K - H2O product dissociation: low K - H2O reactant
'non-active' metals such as Cu - Ag - Au - Pt - etc.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
zero

32. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
The benzene ring (or more correctly the phenyl group - C6H5)
OH?
Soluble except Ag - Pb - Ca - Sr Ba)

33. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
zero
White precipitate
K1 x K2
Kc=Kp

34. What things should you remember to do when collecting gas over water?
a-IMFs - b-molecular volume
redox reaction
SO4²?
allow for the vapor pressure of water and make sure to level levels

35. What process do you use to obtain the solute from a solution?
Increases down group 1 decreases down group 17
Evaporation
zero
no - they're written undissociated (HAaq)

36. What is the sign of the cathode in voltaic cells? in electrolytic cells?
small size and high charge
voltaic: + electrolytic: -
Most are soluble except Ag - Pb
Transition element compounds (except if it has a full or empty d shell)

37. dichromate
yellow
left - ppt will form
0.10M HCl (more ions)
Cr2O7²?

38. BaSO4
Orange
Insoluble
|experimental - accepted|/accepted X 100
zero

39. What are the signs of ?G and E° for spontaneous reactions?
Identity and purity (impure compounds usually have broad & low melting points)
Trigonal pyramidal
?G=negative - E° must be positive
Ionic compounds

40. silver compounds
Insoluble except for nitrate and acetate
Monomer + monomer = polymer product + a simple molecule such as water or HCl
The dilution effect when the solutions mix. M1V1 = M2V2
Mn²? - Cr³? - Cr³

41. What is the general formula for an amine?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Most are soluble except Ag - Pb
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
RNH2

42. What is the general formula for alkyl halides?
allow for the vapor pressure of water and make sure to level levels
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
chemically (ex: with carbon)
RX

43. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
water and substances with (s) less dense than
ethers
[A?]/[HA] x 100 or [BH?]/[B] x 100

44. What is precision?
chemically (ex: with carbon)
How grouped results are
Current - time and charge on ion (moles of e used in half cell reaction)
zero

45. What is the catalyst for this reaction Ester + ?
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?)
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)
At half equivalence - pH=pKa
catalyst=conc H2SO4

46. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
It ceases - the circuit is broken.
it reacts by substitution NOT addition
[A?]/[HA] x 100 or [BH?]/[B] x 100

47. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Soluble
metal oxides and hydrides are ionically bonded and basic
acid + alcohol

48. What type of compounds do metals/non metals form?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
RCOOH
Ionic compounds
Soluble except Ag - Pb - Ca - Sr Ba)

49. What do you use for an acid spill? base spill?
ion pairing
OH- and NH3
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

50. If a weak acid is diluted more - what happens to its % dissociation value?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
lighted splint (positive result=pop)
Increases.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7