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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. During a titration what is present in the beaker at the equivalence point?
CN?
Experimental mass/theoretical mass X 100
How grouped results are
A salt solution.

2. carbonate
catalyst=conc H2SO4
water and substances with (s) less dense than
CO3²?
Sigma bonds are stronger than pi bonds

3. Do anions flow to the cathode or anode?
Anode
0.10M HCl (more ions)
Selective absorption
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

4. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
10?8
Mono; di; tri; tetra; penta; hexa.
Salt and water

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

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6. What apparatus do you use to separate 2 immiscible liquids?
do not change
Big K=kf/kr
Separating funnel
look for changes in oxidation # - the one that goes up is oxidized and is the RA

7. If Q > Ksp - then system shifts _______ and ppt ______
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
They stay the same.
proton acceptor.
left - ppt will form

8. A Bronsted-Lowry base is...
proton acceptor.
NH4?
CrO4²?
Mn²? - Cr³? - Cr³

9. cyanide
CN?
C2O4²?
Acid rain - dissolves marble buildings/statues and kills trees.
White precipitate

10. What is the general formula for a ketone?
RCOR
methyl formate
q=mc?T q=mL (or n x ?h)
P2O5

11. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
A salt solution.
Mn²? - Cr³? - Cr³
Pour liquids using a funnel or down a glass rod
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

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

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13. What is H2CO3 (carbonate acid) usually written as?
catalyst=conc H2SO4
H2O + CO2 (it decomposes readily)
Only temperature
Decant

14. What do group I/II metal oxides and acids form?
blue
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
CrO4²?
Salt and water

15. What are the units of the first order rate constant?
Cr2O7²?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
K2
Anode - oxygen. Cathode - hydrogen

16. Esterification is...
hydroxides (ex: Ba(OH)2)
An active metal.
acid + alcohol
Saturated - Substitution (which requires more radical conditions)

17. What is the general formula for an ester?
Graduated cylinder
RCOOR
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

18. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
proton donor base
same KE - but PEice<PEwater
10?8
water and substances with (s) less dense than

19. When the salt bridge is removed what happens to the cell reaction?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
yellow
It ceases - the circuit is broken.
Purple

20. What is the catalyst for this reaction Ester + ?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
catalyst=conc H2SO4
boiling without losing volatile solvents/reactants

21. BaSO4
?H formation of an element in standard state=0
Eudiometer
Insoluble
-Ea/R

22. Aromatic compounds contain what?
Unsaturated - addition (ex: decolorize bromine solution)
same KE - but PEice<PEwater
The benzene ring (or more correctly the phenyl group - C6H5)
red - green - blue

23. What is the formula for obtaining charge flowing in a cell?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Q=It (time in seconds)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
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?)

24. If a free element is involved - what type of reaction must be involved?
A salt solution.
S2O3²?
redox reaction
RCOOH

25. How does the melting point of a mixture compare to the MP of a pure substance?

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26. Lattice energy is high for ions with _____ size and _____ charge
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
small size and high charge
are less dense than water
Heat a test tube at an angle at the side of the tube (not bottom)

27. What is the formula for alkanes?
Unsaturated - addition (ex: decolorize bromine solution)
CnH2n+2
Kc=Kp
0 and 14

28. bromothymol
CnH2n-2
blue (BTB)
Combine the equations for the half reactions in the non-spontaneous direction
Salt + water

29. nitrates
CH3COO?
0.10M HCl (more ions)
R=8.31 J/mol/K
Soluble

30. How does the melting point of a mixture compare to the MP of a pure substance?
CrO4²?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
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.
it is lower and occurs over less sharp a range

31. If a weak acid is diluted more - what happens to its % dissociation value?
-Ea/R
Salt + water.
ion pairing
Increases.

32. What do you need to make a polymer?
No - NH3 and HCl gases are extremely soluble
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
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)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

33. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
diamond and graphite
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)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Ksp = 108s5

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

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35. How are more active metals reduced?
by electrolysis
CnH(2n+2)
Clear
E=q + w (negative is by system - positive is on system)

36. sulfate
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
it's lower and occurs over less sharp a range
Orange
SO4²?

37. What is the first law of thermodynamics?
-Ea/R
E=q + w (negative is by system - positive is on system)
Most are soluble except Ag - Pb
Evaporation

38. What type of solutions do small - highly charged cations tend to form?
linear
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Exothermic (?H for ANY sa/sb = -57kJ/mol)

39. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
benzene has a delocalized pi ring structure
water and substances with (s) less dense than
zero
ion pairing

40. Nonmetals are good _____ agents. Metals are good _______ agents.
Tetrahedral
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
A salt solution.
RCHO (carbonyl at end)

41. group 1 ions/compounds
catalyst=conc H2SO4
Products - reactants (except for BDE when it's reactants - products)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Soluble

42. What do nonmetal oxides plus water form?
acids
Iodine and CO2 (dry ice)
O2 needs 4F/mol H2 needs 2F/mol
Increases down group 1 decreases down group 17

43. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
More chaotic (ex: gases made)
Transition element compounds (except if it has a full or empty d shell)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
do not change

44. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
At half equivalence - pH=pKa
Soluble
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
non-metal oxides and hydrides are covalently bonded and are acidic.

45. nitrate
NO3?
Check for air bubbles in the buret and remove the buret funnel from the buret
Glowing splint (positive result=relights)
Ksp = 108s5

46. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
CO (poisonous)
same KE - but PEice<PEwater
water and substances with (s) less dense than
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

47. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
same KE - but PEice<PEwater
S crystal at 0K=0
More chaotic (ex: gases made)

48. What does a short - sharp melting point indicate?
Glacial acetic acid
NH4?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Identity and purity (impure compounds usually have broad & low melting points)

49. What is the conjugate base of NH3?
How close results are to the accepted value
ion pairing
NH2?
R=8.31 J/mol/K

50. carbonates
Cr2O7²?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
same KE - but PEice<PEwater
Insoluble except group 1 and ammonium

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AP Chemistry 2

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