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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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1. When can supercooling occur? What does it look like on a cooling curve?

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2. What is the formula for percent error?
different forms of the same element
|experimental - accepted|/accepted X 100
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

3. lead compounds
Insoluble except nitrate and acetate
ethers
E=q + w (negative is by system - positive is on system)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

4. What process do you use to obtain a solvent from a solution?
Read the bottom of the meniscus
benzene has a delocalized pi ring structure
Cu3(PO4)2
Distillation

5. 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)
C4H10
acid + alcohol
Increases down group 1 decreases down group 17

6. BaSO4
Mono; di; tri; tetra; penta; hexa.
Read the bottom of the meniscus
Insoluble
Q=It (time in seconds)

7. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Salts (ex: CaO + SO2 ? CaSO3)
0.10M HCl (more ions)
Acid rain - dissolves marble buildings/statues and kills trees.
blue (BTB)

8. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
The Faraday or Faraday's constant.
The compound with the lowest Ksp value.

9. What is precision?
How grouped results are
OH- and NH3
The dilution effect when the solutions mix. M1V1 = M2V2
allow for the vapor pressure of water and make sure to level levels

10. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
ClO3?
Sigma bonds are stronger than pi bonds
The compound with the lowest Ksp value.

11. The definition of acidic basic and neutral aqueous solutions is:
linear
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
R=8.31 J/mol/K
Mono; di; tri; tetra; penta; hexa.

12. What electrons are lost/gained first in transition element ions?
NH2?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Pale purple - (orange)-yellow - red - blue - green.
ns² electrons (first in-first out)

13. acetate
same KE - but PEice<PEwater
Ksp = s²
Iodine and CO2 (dry ice)
CH3COO?

14. Does Benzene react by addition or substitution?
zero
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
ClO3?
it reacts by substitution NOT addition

15. What are isotopes?
The benzene ring (or more correctly the phenyl group - C6H5)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
E=q + w (negative is by system - positive is on system)
do not change

16. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
Most are soluble except Ag - Pb
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

17. How do you compute % dissociation?
zero
[A?]/[HA] x 100 or [BH?]/[B] x 100
Perform ICE BOX calculation based on K1
The one with most oxygen atoms (highest oxidation number)

18. What shape is carbon dioxide?
linear
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
CH3COO?
Reduction always takes place at the cathode (RED CAT) In both types of cell!

19. ammonium
Clear
lighted splint (positive result=pop)
NH4?
Orange

20. Do you use J or kJ for ?H - ?S - and ?G?
Synthetic condensation polymer (aka a polyamide)
ns² electrons (first in-first out)
H2PO4?
?H-kJ - ?S-J - ?G-kJ

21. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
|experimental - accepted|/accepted X 100
Graduated cylinder
CnH2n-2

22. hydroxides
Conjugate pair (one must be a weak base or acid)
Insoluble (except group 1 ammonium and Ba)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
by electrolysis

23. What is the conjugate acid of H2PO4?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
H3PO4
Iodine and CO2 (dry ice)
redox reaction

24. What do you use for an acid spill? base spill?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

25. What apparatus do you use to separate 2 immiscible liquids?
basic
Separating funnel
Purple
CrO4²?

26. What are two allotropes of carbon?
diamond and graphite
Evaporation
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
CnH2n-2

27. Name C7H16
OH?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Current - time and charge on ion (moles of e used in half cell reaction)
Heptane

28. acetates
q=mc?T q=mL (or n x ?h)
Exothermic
Soluble
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

29. What is the formula of butane?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
C4H10

30. What are isomers?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Soluble
Transition element compounds (except if it has a full or empty d shell)
Molecules with the same molecular formulas - but different structural formulas

31. nitrate
zero-th: decreases - first: constant - second: increases
CO (poisonous)
NO3?
OH- and NH3

32. What is the general formula for an alcohol?
ClO?
ROH
They stay the same.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

33. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
proton acceptor.
E=q + w (negative is by system - positive is on system)

34. Is a graduated cylinder or beaker more accurate?
Big K=kf/kr
0 and 14
Graduated cylinder
CO (poisonous)

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

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36. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Making sigma bonds and holding lone pairs
Experimental mass/theoretical mass X 100
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Current - time and charge on ion (moles of e used in half cell reaction)

37. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
Disulfur dichloride
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Pipette (burette if need repetition)

38. A Bronsted-Lowry acid is...
Most INsoluble except group 1 and ammonium
proton donor base
Making sigma bonds and holding lone pairs
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.

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

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40. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
They stay the same.
CnH(2n+2)
K2

41. copper sulfate
Disulfur dichloride
ClO?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
blue

42. What is the test for oxygen?
Salt + water
Ppt will NOT form (unsaturated)
Glowing splint (positive result=relights)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

43. For a dibasic acid (H2A) - [A²?]= ____ ?
Combine the equations for the half reactions in the non-spontaneous direction
same KE - but PEice<PEwater
K2
All except for lithium

44. What is the formula for percent yield?
RCOR
RX
Experimental mass/theoretical mass X 100
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

45. Ca - Sr - Ba
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
hydroxides (ex: Ba(OH)2)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Hg²?

46. chromate ion (soln + most solids)
yellow
it is lower and occurs over less sharp a range
Selective absorption
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?)

47. halides
Increases down group 1 decreases down group 17
ns² electrons (first in-first out)
Most are soluble except Ag - Pb
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

48. iodine - iodine solution - iodine vapor
?H-kJ - ?S-J - ?G-kJ
Hg2²?
RCOOH
Silvery gray solid - brown - purple

49. What is the general formula for a ketone?
RCOR
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
H3PO4
an oxidized and reduced substance

50. What do group I/II metal oxides plus water form?
H2O + CO2 (it decomposes readily)
RCOR
bases
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

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AP Chemistry 2

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