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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. How many normal boiling points and boiling points are there?

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2. Esterification is...
boiling without losing volatile solvents/reactants
acid + alcohol
Acids; HCOOCH3 is an ester
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

3. bromine
Filtration
Purple
Transition element compounds (except if it has a full or empty d shell)
brown volatile liquid

4. silver compounds
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Insoluble except for nitrate and acetate
Q=It (time in seconds)

5. Name six characteristics of transition elements (or their compounds)
Iodine and CO2 (dry ice)
basic
Pale yellow
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)

6. What is the formula for alkanes?
Acids; HCOOCH3 is an ester
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
CnH2n+2
Cu3(PO4)2

7. What is a dipeptide? polypeptide? protein?
allow for the vapor pressure of water and make sure to level levels
metal oxides and hydrides are ionically bonded and basic
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

8. What do group I/II metal oxides and acids form?
Graduated cylinder
Salt and water
it reacts by substitution NOT addition
Ionic compounds

9. acetates
ClO3?
Soluble
K2
?H-kJ - ?S-J - ?G-kJ

10. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
methyl formate
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Anode - oxygen. Cathode - hydrogen
C2O4²?

11. What are the signs of ?G and E° for spontaneous reactions?
no - they're written undissociated (HAaq)
?G=negative - E° must be positive
bright yellow
ion pairing

12. permanganate
MnO4?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Decant

13. Do anions flow to the cathode or anode?
bases
Anode
CO2 and H2O
Increases.

14. What is the sign of the anode in voltaic cells? in electrolytic cells?
CnH2n
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
NO3?
voltaic: - electrolytic: +

15. chlorite
Ionic compounds
Pour liquids using a funnel or down a glass rod
ClO2?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

16. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
strong acids/bases are written as H+ or OH- ions
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
redox reaction

17. Acid plus base make?
Salt + water.
CO3²?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Only temperature

18. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
Soluble except Ag - Pb - Ca - Sr Ba)
Synthetic condensation polymer (aka a polyamide)
Acidified

19. What is the difference between equivalence point and end point of a titration.
Synthesis - separation and purification of the product and its identification.
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
Greenish-yellow gas
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

20. primary colors
red - green - blue
Insoluble except nitrate and acetate
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Evaporation

21. What do the 'a' and 'b' in Van Der Waal's equation allow for?
T increases exponentially the proportion of molecules with E > Ea
Group I metals (soft metals) are stored under oil
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
a-IMFs - b-molecular volume

22. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
left - ppt will form
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

23. How does half life change for zero-th order - first order - and second order processes?
SO4²?
OH?
Synthetic condensation polymer (aka a polyamide)
zero-th: decreases - first: constant - second: increases

24. Why are i factors (Van't Hoff factors) often less than ideal?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
CnH2n
fractional distillation
ion pairing

25. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
CnH(2n+2)
Ksp = 4s³
zero

26. What shape is carbon dioxide?
O2 needs 4F/mol H2 needs 2F/mol
linear
Insoluble (except group 1 ammonium and Ba)
NO3?

27. What is the general formula for an ester?
RCOOR
Clear
CO2 and H2O
Increases down group 1 decreases down group 17

28. What is H2CO3 (carbonate acid) usually written as?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
K1 x K2
H2O + CO2 (it decomposes readily)
Insoluble (except group 1 ammonium and Ba)

29. How does group 1 metals' density compare to water's?
Salts (ex: CaO + SO2 ? CaSO3)
fractional distillation
Ksp = s²
are less dense than water

30. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
ROH
CnH(2n+2)
Salt and water

31. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
C2O4²?
RCOOR
A) any range. b) 8-10 c) 4-6
H+

32. Why are noble gases stable?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
a-IMFs - b-molecular volume
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
0.10M HCl (more ions)

33. What apparatus do you use to separate 2 immiscible liquids?
It ceases - the circuit is broken.
Synthesis - separation and purification of the product and its identification.
Separating funnel
zero

34. nitrate
0.10M HCl (more ions)
Salt + water
Ions go through the salt bridge - electrons go through metal wires in the external circuit
NO3?

35. How do you get the equation for a net electrolysis reaction?
blue
PO4³?
Combine the equations for the half reactions in the non-spontaneous direction
diamond and graphite

36. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
acid + alcohol
An active metal.
10?8
an oxidized and reduced substance

37. Color (absorbance) is proportional to ________
At half equivalence - pH=pKa
E=q + w (negative is by system - positive is on system)
Concentration
C2O4²?

38. What measuring device would you use for very small volumes of liquids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Pipette (burette if need repetition)
zero
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia

39. 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)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Products - reactants (except for BDE when it's reactants - products)
Most INsoluble except group 1 and ammonium

40. What is precision?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
How grouped results are
Evaporation
Transition element compounds (except if it has a full or empty d shell)

41. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
RX
No - NH3 and HCl gases are extremely soluble
Sulfur
Kc=Kp

42. thiosulfate
bright yellow
small size and high charge
S2O3²?
CnH2n+2

43. When a cell is 'flat' What is its voltage?
zero
red - green - blue
Most INsoluble except group 1 and ammonium
White precipitate

44. What do hydrocarbons form when they burn in air (oxygen)?
CO2 and H2O
An active metal.
same KE - but PEice<PEwater
Disulfur dichloride

45. lead compounds
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Insoluble except nitrate and acetate
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Salt and water

46. Give an example of a dilute strong acid.
Hg²?
Products - reactants (except for BDE when it's reactants - products)
ion pairing
HClO4

47. What is the formula for summation?

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48. group 1 ions/compounds
Soluble
different forms of the same element
ion pairing
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

49. What are the signs for ?G and E° for spontaneous reactions?
P2O5
?G= -ve - E°= +ve
same KE - but PEice<PEwater
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

50. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
it's lower and occurs over less sharp a range
White precipitate

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AP Chemistry 2

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