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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.
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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 variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Current - time and charge on ion (moles of e used in half cell reaction)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
|experimental - accepted|/accepted X 100
Iodine and CO2 (dry ice)

2. What do metal oxides plus non- metal oxides form?
No - it depends on the number of ions produced on dissolving.
Salts (ex: CaO + SO2 ? CaSO3)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Cu3(PO4)2

3. 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.
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)
boiling without losing volatile solvents/reactants
[A?]/[HA] x 100 or [BH?]/[B] x 100

4. When is ?G zero?
water and substances with (s) less dense than
a-IMFs - b-molecular volume
The one with most oxygen atoms (highest oxidation number)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

5. What type of compounds do metals/non metals form?
ns² electrons (first in-first out)
Ionic compounds
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
S crystal at 0K=0

6. What is Big K in terms of kf and kr?
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
Big K=kf/kr
More chaotic (ex: gases made)

7. What are amphoteric oxides?
Pale purple - (orange)-yellow - red - blue - green.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
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?)
P2O5

8. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Insoluble (except group 1 ammonium and Ba)
Most INsoluble except group 1 and ammonium
Mn²? - Cr³? - Cr³
bright yellow

9. dihydrogen phosphate
CnH2n+2
Acid rain - dissolves marble buildings/statues and kills trees.
CN?
H2PO4?

10. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
diamond and graphite
benzene has a delocalized pi ring structure
Insoluble except group 1 and ammonium

11. If a free element is involved - what type of reaction must be involved?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
same KE - but PEice<PEwater
redox reaction
Increases.

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

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13. 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
lighted splint (positive result=pop)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
bright yellow

14. What are the signs of ?G and E° for spontaneous reactions?
Soluble
?G=negative - E° must be positive
same KE - but PEice<PEwater
White precipitate

15. What is the general formula for an ether?
fruit - fish - bases
ROR
same KE - but PEice<PEwater
RNH2

16. hypochlorite
CrO4²?
ClO?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
zero-th: decreases - first: constant - second: increases

17. chromate
Salts (ex: CaO + SO2 ? CaSO3)
CrO4²?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

18. Does Benzene react by addition or substitution?
Sulfur
it reacts by substitution NOT addition
zero
The Faraday or Faraday's constant.

19. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
0.10M HCl (more ions)
At half equivalence - pH=pKa
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
neutralization: high K - H2O product dissociation: low K - H2O reactant

20. What electrons are lost/gained first in transition element ions?
Acids; HCOOCH3 is an ester
Only temperature
boiling without losing volatile solvents/reactants
ns² electrons (first in-first out)

21. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
are less dense than water
?G= -ve - E°= +ve
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)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

22. What do hydrocarbons form when they burn in air (oxygen)?
zero
All except for lithium
CO2 and H2O
Silvery gray solid - brown - purple

23. sulfates
PO4³?
Soluble except Ag - Pb - Ca - Sr Ba)
bases
are less dense than water

24. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
A) any range. b) 8-10 c) 4-6
Ksp = 27s4
ClO?

25. hydroxide
Cu3(PO4)2
OH?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
At half equivalence - pH=pKa

26. Is the ?H formation of an element in standard state zero?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
?H formation of an element in standard state=0
|experimental - accepted|/accepted X 100
voltaic: + electrolytic: -

27. If Q < Ksp a ppt ______
Sulfur
P2O5
Ppt will NOT form (unsaturated)
|experimental - accepted|/accepted X 100

28. What is the word equation for condensation polymerisation ?
fruit - fish - bases
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Monomer + monomer = polymer product + a simple molecule such as water or HCl
proton donor base

29. Do anions flow to the cathode or anode?
Acid rain - dissolves marble buildings/statues and kills trees.
Anode
Insoluble
HClO4

30. When the salt bridge is removed what happens to the cell reaction?
methyl formate
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Experimental mass/theoretical mass X 100
It ceases - the circuit is broken.

31. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
?H formation of an element in standard state=0
Ksp = 27s4
it reacts by substitution NOT addition
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

32. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
strong acids/bases are written as H+ or OH- ions
Filtration
neutralization: high K - H2O product dissociation: low K - H2O reactant
lighted splint (positive result=pop)

33. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Tetrahedral
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
NH2?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

34. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Group I metals (soft metals) are stored under oil
Acid rain - dissolves marble buildings/statues and kills trees.
PO4³?
E=q + w (negative is by system - positive is on system)

35. When combining half equations - what do you do to E° values when multiplying coefficients?
Selective absorption
Synthetic condensation polymer (aka a polyamide)
Insoluble except nitrate and acetate
Nothing

36. What do the 'a' and 'b' in Van Der Waal's equation allow for?
RX
Ksp = 27s4
Pale yellow
a-IMFs - b-molecular volume

37. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
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
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Pale yellow

38. One mole of electrons carries 96500Coulombs - what is this quantity called?

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39. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
do not change
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Group 1 hydroxides (ex: NaOH)
CnH2n+1 often designated 'R' ex C3H7 is propyl

40. What is the general formula for an ester?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
RCOOR
MnO4?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

41. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
water and substances with (s) less dense than
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

42. At what point during titration do you have the perfect buffer - and what is the pH at this point?
a-IMFs - b-molecular volume
At half equivalence - pH=pKa
RX
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

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

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44. What is the difference between equivalence point and end point of a titration.
Read the bottom of the meniscus
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
brown volatile liquid
Most are soluble except Ag - Pb

45. During a titration what is present in the beaker at the equivalence point?
Nothing
A salt solution.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Soluble

46. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
?G=negative - E° must be positive
a-IMFs - b-molecular volume
+4-covalent - +2-ionic

47. What is the catalyst for this reaction Ester + ?
The Faraday or Faraday's constant.
CnH2n+1 often designated 'R' ex C3H7 is propyl
catalyst=conc H2SO4
no - they're written undissociated (HAaq)

48. Give an example of a dilute strong acid.
bent
ion pairing
H2O + CO2 (it decomposes readily)
HClO4

49. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
O2 needs 4F/mol H2 needs 2F/mol
More chaotic (ex: gases made)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Experimental mass/theoretical mass X 100

50. What is the charge on a chlorine atom?
Pale purple - (orange)-yellow - red - blue - green.
zero
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Q=It (time in seconds)