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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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1. If Q < Ksp a ppt ______
Insoluble (except group 1 ammonium and Ba)
by electrolysis
Ppt will NOT form (unsaturated)
voltaic: - electrolytic: +

2. How does group 1 metals' density compare to water's?
methyl formate
are less dense than water
Soluble
Ksp = 27s4

3. How does benzene compare in reactivity to alkenes?
Selective absorption
hydroxides (ex: Ba(OH)2)
benzene is less reactive than alkenes
CnH(2n+2)

4. What do nonmetal oxides plus water form?
Combine the equations for the half reactions in the non-spontaneous direction
acids
CrO4²?
Insoluble (except group 1 ammonium and Ba)

5. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
T increases exponentially the proportion of molecules with E > Ea
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
water and substances with (s) less dense than
OH- and NH3

6. What is the general formula for an aldehyde?
?G= -ve - E°= +ve
How close results are to the accepted value
Silvery gray solid - brown - purple
RCHO (carbonyl at end)

7. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Pale purple - (orange)-yellow - red - blue - green.
ROR
O2 needs 4F/mol H2 needs 2F/mol

8. What are the names and formulas of the 6 strong acids?
|experimental - accepted|/accepted X 100
How grouped results are
Identity and purity (impure compounds usually have broad & low melting points)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

9. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
it reacts by substitution NOT addition
Insoluble except for nitrate and acetate

10. What does a short - sharp melting point indicate?
Initiation energy (NOT Ea)
Identity and purity (impure compounds usually have broad & low melting points)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

11. silver compounds
Silvery gray solid - brown - purple
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Insoluble except for nitrate and acetate
Soluble

12. mercury (II) ion
red - green - blue
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Hg²?
Heat a test tube at an angle at the side of the tube (not bottom)

13. What is the word equation for addition polymerisation?
bright yellow
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
?G= -ve - E°= +ve
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.

14. What is the basic structure of an optical isomer?
Mono; di; tri; tetra; penta; hexa.
Ionic compounds
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Evaporation

15. barium sulfate
OH?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
The Faraday or Faraday's constant.
White precipitate

16. What equipment do you need for a titration?
CnH(2n+2)
Anode - oxygen. Cathode - hydrogen
Disulfur dichloride
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

17. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
RCHO (carbonyl at end)
ionic and form hydrogen and hydroxide
Acids; HCOOCH3 is an ester

18. What are amphoteric oxides?
They stay the same.
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?)
But S° of element is not zero (except at 0K)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

19. nitrates
Soluble
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
CnH2n-2
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

20. What word is a clue for a redox reaction?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
CnH2n-2
Acidified
Pale yellow

21. What shape is methane?
Tetrahedral
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
blue
CnH2n

22. How many ligands attach to a central ion in a complex ion?
allow for the vapor pressure of water and make sure to level levels
#ligands=charge x2
same KE - but PEice<PEwater
PO4³?

23. What process do you use to obtain a solvent from a solution?
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.
Distillation
Anode - oxygen. Cathode - hydrogen
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

24. 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
Eudiometer
proton acceptor.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

25. What two compounds are great oxidizing agents?

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26. What is the formula for percent yield?
zero
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Experimental mass/theoretical mass X 100
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?)

27. An amphiprotic (amphoteric) species is...
Ppt will NOT form (unsaturated)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
?H formation of an element in standard state=0
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

28. If ?S is positive - are the products more or less chaotic than the reactants?
OH?
Insoluble except nitrate and acetate
Hg2²?
More chaotic (ex: gases made)

29. What are two substances that sublime at 1 atm when heated?
benzene has a delocalized pi ring structure
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Iodine and CO2 (dry ice)
RCOOH

30. BaSO4
Kc=Kp
it reacts by substitution NOT addition
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Insoluble

31. What is a coordinate covalent bond?
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.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Both electrons come from the same atom (just as good as a regular bond)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

32. What is the general formula for an acid?
Pale yellow
RCOOH
Mn²? - Cr³? - Cr³
CnH(2n+2)

33. potassium permanganate
a-IMFs - b-molecular volume
Purple
All except for lithium
Making sigma bonds and holding lone pairs

34. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Salts (ex: CaO + SO2 ? CaSO3)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
chemically (ex: with carbon)
Pale purple - (orange)-yellow - red - blue - green.

35. permanganate
redox reaction
CnH2n+1 often designated 'R' ex C3H7 is propyl
it is lower and occurs over less sharp a range
MnO4?

36. Alcohols and _______ are FG isomers
ethers
Clear
?H formation of an element in standard state=0
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

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

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38. iodine - iodine solution - iodine vapor
ns² electrons (first in-first out)
Silvery gray solid - brown - purple
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
NH2?

39. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
left - ppt will form
Trigonal pyramidal
K2

40. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
E=q + w (negative is by system - positive is on system)
|experimental - accepted|/accepted X 100
H2O + CO2 (it decomposes readily)

41. Both Acetic acid and ____________ are also functional isomers.
methyl formate
Sulfur
NH2?
Acids; HCOOCH3 is an ester

42. What is the energy you must put into a reaction to make it start called?
Mn²? - Cr³? - Cr³
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Initiation energy (NOT Ea)

43. What shape is carbon dioxide?
PO4³?
linear
Ksp = 27s4
Salt and water

44. What are two allotropes of carbon?
Ppt will NOT form (unsaturated)
SO4²?
diamond and graphite
Time?¹ - (ex. s?¹ - hr?¹ - etc)

45. What do metal oxides plus non- metal oxides form?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
A) any range. b) 8-10 c) 4-6
Salts (ex: CaO + SO2 ? CaSO3)
Clear

46. Is the freezing of ice endothermic or exothermic?
Experimental mass/theoretical mass X 100
Exothermic
K2
They stay the same.

47. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
same KE - but PEice<PEwater
Salt + water.
Glowing splint (positive result=relights)

48. What is the word equation for condensation polymerisation ?
Group I metals (soft metals) are stored under oil
Acids; HCOOCH3 is an ester
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Hg2²?

49. primary colors
Unsaturated - addition (ex: decolorize bromine solution)
Ksp = s²
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
red - green - blue

50. Color is due to ______ _______ of light.
Ksp = 108s5
ROR
Selective absorption
H2PO4?

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AP Chemistry 2

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