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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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1. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
K1 x K2
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Ksp = 108s5
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

2. What is the general formula for an aldehyde?
SO4²?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
RCHO (carbonyl at end)
NH2?

3. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
CO3²?
Insoluble except nitrate and acetate
fractional distillation

4. What reacts with an acid to create hydrogen gas?
neutralization: high K - H2O product dissociation: low K - H2O reactant
An active metal.
?G=negative - E° must be positive
Hg2²?

5. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
by electrolysis
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

6. nitrate
Acid rain - dissolves marble buildings/statues and kills trees.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
NO3?
C2O4²?

7. How do you get Ecell for spontaneous reactions?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
left - ppt will form
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

8. Alcohols and _______ are FG isomers
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)
voltaic: - electrolytic: +
ethers
Both electrons come from the same atom (just as good as a regular bond)

9. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
SO4²?
same KE - but PEice<PEwater
lighted splint (positive result=pop)

10. What are two allotropes of carbon?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
diamond and graphite
Acids; HCOOCH3 is an ester
K1 x K2

11. What is the formula for alkynes?
CnH2n-2
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Clear
Selective absorption

12. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Kc=Kp
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
[A?]/[HA] x 100 or [BH?]/[B] x 100
benzene is less reactive than alkenes

13. What element is used to vulcanize rubber?
Add acid to water so that the acid doesn't boil and spit
Insoluble (except group 1 ammonium and Ba)
Combine the equations for the half reactions in the non-spontaneous direction
Sulfur

14. Does Benzene react by addition or substitution?
Cr2O7²?
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?)
a-IMFs - b-molecular volume
it reacts by substitution NOT addition

15. Is the ?H formation of an element in standard state zero?
H2PO4?
?H formation of an element in standard state=0
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
No - it depends on the number of ions produced on dissolving.

16. Can you collect soluble gases over water?
0 and 14
Salt + water.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
No - NH3 and HCl gases are extremely soluble

17. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
Exothermic
The benzene ring (or more correctly the phenyl group - C6H5)
benzene is less reactive than alkenes

18. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
water and substances with (s) less dense than
[A?]/[HA] x 100 or [BH?]/[B] x 100
Hg2²?

19. What type of metals don't react with water or acids to form H2?

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20. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Eudiometer
non-metal oxides and hydrides are covalently bonded and are acidic.

21. How do you explain trends in atomic properties using Coulomb's Law?
A) any range. b) 8-10 c) 4-6
0.10M HCl (more ions)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
NO3?

22. hydroxides
Insoluble (except group 1 ammonium and Ba)
NH4?
R=8.31 J/mol/K
C2O4²?

23. Nonmetals are good _____ agents. Metals are good _______ agents.
it's lower and occurs over less sharp a range
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
neutralization: high K - H2O product dissociation: low K - H2O reactant
The dilution effect when the solutions mix. M1V1 = M2V2

24. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
ethers
P2O5
MnO4?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

25. If a free element is involved - what type of reaction must be involved?
S2O3²?
Acid rain - dissolves marble buildings/statues and kills trees.
Acidified
redox reaction

26. What changes Keq?
Initiation energy (NOT Ea)
are less dense than water
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Only temperature

27. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
a-IMFs - b-molecular volume
Group I metals (soft metals) are stored under oil
it's lower and occurs over less sharp a range

28. What is the third law of thermodynamics?
S crystal at 0K=0
Increases.
?H formation of an element in standard state=0
ionic and form hydrogen and hydroxide

29. sulfate
SO4²?
hydroxides (ex: Ba(OH)2)
Hg²?
Salts (ex: CaO + SO2 ? CaSO3)

30. Where are group I metals stored?
10?8
Group I metals (soft metals) are stored under oil
acids
ionic and form hydrogen and hydroxide

31. How are primary alcohols turned into acids?
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)
CrO4²?
T increases exponentially the proportion of molecules with E > Ea

32. What does the solubility of organic compounds depend on?
Ionic compounds
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Salt and water
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

33. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
Ionic compounds
Ksp = 27s4
do not change

34. Aromatic compounds contain what?
Both electrons come from the same atom (just as good as a regular bond)
O2 needs 4F/mol H2 needs 2F/mol
The benzene ring (or more correctly the phenyl group - C6H5)
Kc=Kp

35. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
?H formation of an element in standard state=0
benzene is less reactive than alkenes
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Soluble

36. How do you heat a test tube?
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
SO4²?
RCOR
Heat a test tube at an angle at the side of the tube (not bottom)

37. What are the formulas for q?
T increases exponentially the proportion of molecules with E > Ea
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
q=mc?T q=mL (or n x ?h)
Salt and water

38. What do ions and electrons travel through in a voltaic/electrolytic cell?
Greenish-yellow gas
metal oxides and hydrides are ionically bonded and basic
no - they're written undissociated (HAaq)
Ions go through the salt bridge - electrons go through metal wires in the external circuit

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

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40. When driving off water from a hydrate - how do you tell you're done?
Only temperature
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
allow for the vapor pressure of water and make sure to level levels
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

41. How many ligands attach to a central ion in a complex ion?
No - it depends on the number of ions produced on dissolving.
Soluble
#ligands=charge x2
Salt and water

42. Acids + Carbonates (bicarbonates) make?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
a-IMFs - b-molecular volume
?G=negative - E° must be positive

43. Both Acetic acid and ____________ are also functional isomers.
Making sigma bonds and holding lone pairs
Pour liquids using a funnel or down a glass rod
They decrease (or could be the same if the solid has ONLY JUST disappeared)
methyl formate

44. What should you check for before you begin titrating?
CnH2n+1 often designated 'R' ex C3H7 is propyl
HClO4
Check for air bubbles in the buret and remove the buret funnel from the buret
water and substances with (s) less dense than

45. What is the formula for summation?

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46. What do nonmetal oxides plus water form?
CnH2n
P2O5
acids
zero-th: decreases - first: constant - second: increases

47. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
The dilution effect when the solutions mix. M1V1 = M2V2
neutralization: high K - H2O product dissociation: low K - H2O reactant
Mn²? - Cr³? - Cr³
Exothermic

48. What is the difference between equivalence point and end point of a titration.
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
bases
catalyst=conc H2SO4
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

49. cyanide
RCOR
Soluble
CN?
Synthetic condensation polymer (aka a polyamide)

50. silver iodide
Acid rain - dissolves marble buildings/statues and kills trees.
ClO?
Pale yellow
Decant

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AP Chemistry 2

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