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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. What changes Keq?
blue
ethers
benzene is less reactive than alkenes
Only temperature

2. What is the formula for alkanes?
Synthesis - separation and purification of the product and its identification.
CnH2n+2
Insoluble
P2O5

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

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4. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
O2 needs 4F/mol H2 needs 2F/mol
The one with most oxygen atoms (highest oxidation number)
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
No - it depends on the number of ions produced on dissolving.

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

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6. What should you check for before you begin titrating?
ClO2?
RNH2
At half equivalence - pH=pKa
Check for air bubbles in the buret and remove the buret funnel from the buret

7. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
Ksp = s²
Heat a test tube at an angle at the side of the tube (not bottom)
NO3?

8. Buffer capacity must contain decent amounts of a ________ ________
Anode - oxygen. Cathode - hydrogen
Conjugate pair (one must be a weak base or acid)
diamond and graphite
CO3²?

9. How are more active metals reduced?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
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.
A salt solution.
by electrolysis

10. If a free element is involved - what type of reaction must be involved?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Group 1 hydroxides (ex: NaOH)
blue
redox reaction

11. How do you identify which is oxidized or otherwise?
H2PO4?
Graduated cylinder
Salt + water.
look for changes in oxidation # - the one that goes up is oxidized and is the RA

12. When driving off water from a hydrate - how do you tell you're done?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
0 and 14

13. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
#ligands=charge x2
Heat a test tube at an angle at the side of the tube (not bottom)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

14. What is the general formula for an ester?
RCOOR
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
At half equivalence - pH=pKa
Increases.

15. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Pour liquids using a funnel or down a glass rod
CH3COO?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

16. What do metal oxides plus non- metal oxides form?
Unsaturated - addition (ex: decolorize bromine solution)
blue
basic
Salts (ex: CaO + SO2 ? CaSO3)

17. What shape is methane?
Tetrahedral
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Synthesis - separation and purification of the product and its identification.

18. How do you get the equation for a net electrolysis reaction?
How grouped results are
RX
Combine the equations for the half reactions in the non-spontaneous direction
non-metal oxides and hydrides are covalently bonded and are acidic.

19. How are metal oxides and hydrides bonded? are they acidic or basic?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
metal oxides and hydrides are ionically bonded and basic
Acids; HCOOCH3 is an ester

20. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
T increases exponentially the proportion of molecules with E > Ea
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)
Decant

21. Color is due to ______ _______ of light.
White precipitate
They stay the same.
Selective absorption
0 and 14

22. What is precision?
How grouped results are
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Distillation

23. Alcohols and _______ are FG isomers
ethers
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
C4H10
neutralization: high K - H2O product dissociation: low K - H2O reactant

24. oxalate
Acids; HCOOCH3 is an ester
C2O4²?
CnH2n+2
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

25. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
CnH2n
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Soluble

26. What is the formula for alkynes?
CnH2n-2
RCOOR
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

27. During a titration what is present in the beaker at the equivalence point?
C4H10
Nothing
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
A salt solution.

28. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
Heptane
Acids; HCOOCH3 is an ester
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

29. What are two substances that sublime at 1 atm when heated?
voltaic: - electrolytic: +
Iodine and CO2 (dry ice)
zero
Distillation

30. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
zero
Pale purple - (orange)-yellow - red - blue - green.
A) any range. b) 8-10 c) 4-6
Ksp = 108s5

31. dichromate
Cr2O7²?
Graduated cylinder
atoms
Exothermic

32. What are amphoteric oxides?
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?)
small size and high charge
H2O + CO2 (it decomposes readily)
acid + alcohol

33. What process do you use to obtain the solute from a solution?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Evaporation
red - green - blue
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

34. Why are i factors (Van't Hoff factors) often less than ideal?
zero-th: decreases - first: constant - second: increases
Purple
ion pairing
Insoluble

35. 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)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Check for air bubbles in the buret and remove the buret funnel from the buret

36. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Ions go through the salt bridge - electrons go through metal wires in the external circuit
a-IMFs - b-molecular volume
The Faraday or Faraday's constant.

37. copper sulfate
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
CN?
blue
Transition element compounds (except if it has a full or empty d shell)

38. If a weak acid is diluted more - what happens to its % dissociation value?
More chaotic (ex: gases made)
Increases.
Soluble except Ag - Pb - Ca - Sr Ba)
No - it depends on the number of ions produced on dissolving.

39. How does the melting point of a mixture compare to the MP of a pure substance?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
0.10M HCl (more ions)
an oxidized and reduced substance
it is lower and occurs over less sharp a range

40. What is the word equation for condensation polymerisation ?
Anode
Monomer + monomer = polymer product + a simple molecule such as water or HCl
NH4?
Unsaturated - addition (ex: decolorize bromine solution)

41. Aromatic compounds contain what?
Products - reactants (except for BDE when it's reactants - products)
Nothing
10?8
The benzene ring (or more correctly the phenyl group - C6H5)

42. ammonium
NH4?
ionic and form hydrogen and hydroxide
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
do not change

43. What is the general formula for a ketone?
Exothermic
RCOR
Group I metals (soft metals) are stored under oil
The dilution effect when the solutions mix. M1V1 = M2V2

44. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
P2O5
Pour liquids using a funnel or down a glass rod
Mono; di; tri; tetra; penta; hexa.

45. carbonates
bases
Group I metals (soft metals) are stored under oil
Insoluble except group 1 and ammonium
CO2 and H2O

46. What is an Alkyl group?

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47. bromothymol
Insoluble except group 1 and ammonium
blue (BTB)
Silvery gray solid - brown - purple
look for changes in oxidation # - the one that goes up is oxidized and is the RA

48. What is Big K in terms of kf and kr?
E=q + w (negative is by system - positive is on system)
NH2?
Big K=kf/kr
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

49. What shape is water?
RCHO (carbonyl at end)
ClO3?
bent
Anode - oxygen. Cathode - hydrogen

50. ammonium/ammonium compounds
Products - reactants (except for BDE when it's reactants - products)
Soluble
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Pour liquids using a funnel or down a glass rod

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AP Chemistry 2

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