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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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1. What are the prefixes for the naming of binary molecular compound formulas (up to six)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
diamond and graphite
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Mono; di; tri; tetra; penta; hexa.

2. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
Salt and water
Big K=kf/kr
C4H10

3. Alkanes are _________ and react by _________
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)
Saturated - Substitution (which requires more radical conditions)
P2O5
CO2 and H2O

4. Neutralization is an ________ reaction.
H+
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Conjugate pair (one must be a weak base or acid)

5. What apparatus do you use to pour liquids?
Ksp = 108s5
Soluble
proton donor base
Pour liquids using a funnel or down a glass rod

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

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7. How does group 1 metals' density compare to water's?
The one with most oxygen atoms (highest oxidation number)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
are less dense than water
Increases.

8. Nonmetals are good _____ agents. Metals are good _______ agents.
Iodine and CO2 (dry ice)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
ns² electrons (first in-first out)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

9. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Initiation energy (NOT Ea)
voltaic: + electrolytic: -
Disulfur dichloride
redox reaction

10. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
Filtration
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
ethers

11. Is the freezing of ice endothermic or exothermic?
proton acceptor.
K2
More chaotic (ex: gases made)
Exothermic

12. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
allow for the vapor pressure of water and make sure to level levels
A) any range. b) 8-10 c) 4-6
Initiation energy (NOT Ea)
MnO4?

13. How many faradays of electric charge do you need to produce one mole of O2? H2?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Cr2O7²?
linear
O2 needs 4F/mol H2 needs 2F/mol

14. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
The Faraday or Faraday's constant.
Current - time and charge on ion (moles of e used in half cell reaction)

15. oxalate
?G=negative - E° must be positive
C2O4²?
boiling without losing volatile solvents/reactants
MnO4?

16. What is the general formula for an ester?
Salt + water
ionic and form hydrogen and hydroxide
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
RCOOR

17. How do you clean a buret/pipette for a titration?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
small size and high charge
allow for the vapor pressure of water and make sure to level levels
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

18. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Soluble
ClO3?
basic

19. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Insoluble except nitrate and acetate
Experimental mass/theoretical mass X 100
Distillation
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

20. What do ions and electrons travel through in a voltaic/electrolytic cell?
zero
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Ionic compounds

21. What shape is ammonia?
Trigonal pyramidal
'non-active' metals such as Cu - Ag - Au - Pt - etc.
PO4³?
Big K=kf/kr

22. What are two substances that sublime at 1 atm when heated?
Experimental mass/theoretical mass X 100
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
do not change
Iodine and CO2 (dry ice)

23. What do metal oxides plus acids form?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
different forms of the same element
Salt + water
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

24. What process do you use to separate two liquids with different boiling points?
fractional distillation
P2O5
Purple
by electrolysis

25. A Bronsted-Lowry base is...
Read the bottom of the meniscus
do not change
proton acceptor.
a-IMFs - b-molecular volume

26. If a weak acid is diluted more - what happens to its % dissociation value?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Check for air bubbles in the buret and remove the buret funnel from the buret
Increases.

27. The oxidation # for acid base reactions...
Q=It (time in seconds)
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?)
NO3?
do not change

28. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
acid + alcohol
Distillation
different forms of the same element

29. What is the conjugate acid of H2PO4?
zero
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
How grouped results are
H3PO4

30. How do you compute % dissociation?
Big K=kf/kr
CnH(2n+2)
Concentration
[A?]/[HA] x 100 or [BH?]/[B] x 100

31. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
?G= -ve - E°= +ve
non-metal oxides and hydrides are covalently bonded and are acidic.
Making sigma bonds and holding lone pairs
Kc=Kp

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

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33. What is the first law of thermodynamics?
0.10M HCl (more ions)
H+
E=q + w (negative is by system - positive is on system)
ion pairing

34. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Mono; di; tri; tetra; penta; hexa.
Mn²? - Cr³? - Cr³
OH?

35. Do you use J or kJ for ?H - ?S - and ?G?
?H-kJ - ?S-J - ?G-kJ
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
acid + alcohol
MnO4?

36. What process do you use to obtain a solvent from a solution?
Salts (ex: CaO + SO2 ? CaSO3)
Distillation
yellow
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

37. What equipment do you need for a titration?
ClO?
RX
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
strong acids/bases are written as H+ or OH- ions

38. Ca - Sr - Ba
hydroxides (ex: Ba(OH)2)
small size and high charge
S crystal at 0K=0
Salt + water.

39. How does benzene compare in reactivity to alkenes?
Heat a test tube at an angle at the side of the tube (not bottom)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
acids
benzene is less reactive than alkenes

40. What is the formula of butane?
Transition element compounds (except if it has a full or empty d shell)
C4H10
Insoluble except group 1 and ammonium
NO3?

41. chlorine
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Greenish-yellow gas
Soluble
Iodine and CO2 (dry ice)

42. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
chemically (ex: with carbon)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
#ligands=charge x2
RX

43. What is HCOOCH3?
Acids; HCOOCH3 is an ester
Ksp = s²
OH?
chemically (ex: with carbon)

44. What do the 'a' and 'b' in Van Der Waal's equation allow for?
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
a-IMFs - b-molecular volume
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Salt and water

45. Is a graduated cylinder or beaker more accurate?
Heptane
Graduated cylinder
Reduction always takes place at the cathode (RED CAT) In both types of cell!
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

46. What is the general formula for alkyl halides?
Sigma bonds are stronger than pi bonds
Soluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
RX

47. What is the general formula for an ether?
Products - reactants (except for BDE when it's reactants - products)
Soluble
H2PO4?
ROR

48. What is the conjugate base of NH3?
NH2?
Insoluble
ClO3?
K1 x K2

49. silver compounds
ClO?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Insoluble except for nitrate and acetate
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

50. Does reactivity increase/decrease going down group 1 and group 17?
blue glass - it filters UV
Increases down group 1 decreases down group 17
ethers
voltaic: - electrolytic: +

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AP Chemistry 2

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