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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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This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.

1. What is the formula for alkenes?
Cu3(PO4)2
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Anode - oxygen. Cathode - hydrogen
CnH2n

2. phosphates
Synthetic condensation polymer (aka a polyamide)
Pipette (burette if need repetition)
chemically (ex: with carbon)
Most INsoluble except group 1 and ammonium

3. What is the formula of copper (II) phosphate?
CnH2n-2
Salts (ex: CaO + SO2 ? CaSO3)
Transition element compounds (except if it has a full or empty d shell)
Cu3(PO4)2

4. 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.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
blue glass - it filters UV
NH2?
A) any range. b) 8-10 c) 4-6

5. What shape is methane?
water and substances with (s) less dense than
Tetrahedral
Exothermic (?H for ANY sa/sb = -57kJ/mol)
same KE - but PEice<PEwater

6. What do you do to get rid of most of the solution from a precipitate?
Decant
blue (BTB)
MnO4?
HClO4

7. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Cr2O7²?
zero-th: decreases - first: constant - second: increases
T increases exponentially the proportion of molecules with E > Ea

8. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
CN?
K1 x K2
CO3²?

9. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
MnO4?
Cr2O7²?
by electrolysis

10. How can metals like iron and zinc be reduced?
neutralization: high K - H2O product dissociation: low K - H2O reactant
boiling without losing volatile solvents/reactants
blue (BTB)
chemically (ex: with carbon)

11. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
Suniverse increases for spontaneous processes
Salt and water
Separating funnel

12. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
a-IMFs - b-molecular volume
Mono; di; tri; tetra; penta; hexa.
Transition element compounds (except if it has a full or empty d shell)

13. copper sulfate
No - NH3 and HCl gases are extremely soluble
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
blue
RCHO (carbonyl at end)

14. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
HClO4
Ksp = 4s³
small size and high charge
0 and 14

15. What shape is water?
Mono; di; tri; tetra; penta; hexa.
bent
E=q + w (negative is by system - positive is on system)
zero

16. Why are i factors (Van't Hoff factors) often less than ideal?
Glowing splint (positive result=relights)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
same KE - but PEice<PEwater
ion pairing

17. silver compounds
The dilution effect when the solutions mix. M1V1 = M2V2
Insoluble except for nitrate and acetate
PO4³?
redox reaction

18. Which of the rates changes more when temperature is increased?
Sulfur
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Molecules with the same molecular formulas - but different structural formulas
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

19. Name C7H16
Heptane
Greenish-yellow gas
blue (BTB)
An active metal.

20. sulfate
Ions go through the salt bridge - electrons go through metal wires in the external circuit
+4-covalent - +2-ionic
0 and 14
SO4²?

21. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
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)
allow for the vapor pressure of water and make sure to level levels
#ligands=charge x2

22. Esterification is...
Eudiometer
Glowing splint (positive result=relights)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
acid + alcohol

23. 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)
PO4³?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
ion pairing

24. What is the general formula of an alkane?
CnH(2n+2)
Soluble
Combine the equations for the half reactions in the non-spontaneous direction
A) any range. b) 8-10 c) 4-6

25. How are non-metal oxides and hydrides bonded? are they acidic or basic?
|experimental - accepted|/accepted X 100
left - ppt will form
non-metal oxides and hydrides are covalently bonded and are acidic.
no - they're written undissociated (HAaq)

26. What is precision?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
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
Most INsoluble except group 1 and ammonium
How grouped results are

27. What is accuracy?
How close results are to the accepted value
All except for lithium
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

28. How do you get the equation for a net electrolysis reaction?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
by electrolysis
Soluble
Combine the equations for the half reactions in the non-spontaneous direction

29. What effect does increasing the size/surface area of a voltaic cell have on the cell?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
yellow
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

30. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Anode
strong acids/bases are written as H+ or OH- ions
They stay the same.
ROR

31. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
ethers
Selective absorption
Ksp = 27s4

32. What device would you use to measure a volume of gas?
Eudiometer
Add acid to water so that the acid doesn't boil and spit
Group 1 hydroxides (ex: NaOH)
ion pairing

33. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Clear
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
-Ea/R
Distillation

34. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
brown volatile liquid
How close results are to the accepted value
Salt + water
same KE - but PEice<PEwater

35. How does group 1 metals' density compare to water's?
are less dense than water
Monomer + monomer = polymer product + a simple molecule such as water or HCl
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
brown volatile liquid

36. What are isotopes?
T increases exponentially the proportion of molecules with E > Ea
10?8
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Making sigma bonds and holding lone pairs

37. sulfates
RCOR
Soluble except Ag - Pb - Ca - Sr Ba)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Read the bottom of the meniscus

38. What process do you use to obtain the precipitate from a solution?
Filtration
Soluble
diamond and graphite
R=8.31 J/mol/K

39. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
water and substances with (s) less dense than
no - they're written undissociated (HAaq)
water and substances with (s) less dense than

40. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Saturated - Substitution (which requires more radical conditions)
diamond and graphite
Selective absorption

41. What do you need to make a polymer?
benzene has a delocalized pi ring structure
White precipitate
Cr2O7²?
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)

42. Color is due to ______ _______ of light.
Read the bottom of the meniscus
Decant
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Selective absorption

43. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
No - it depends on the number of ions produced on dissolving.
boiling without losing volatile solvents/reactants
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Silvery gray solid - brown - purple

44. Acids + Carbonates (bicarbonates) make?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Nothing
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

45. When combining half equations - what do you do to E° values when multiplying coefficients?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
benzene is less reactive than alkenes
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Nothing

46. A geometric (or cis-trans) isomer exists due to.....
OH?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Pale yellow
HClO4

47. What apparatus do you use to separate 2 immiscible liquids?
Soluble
Synthesis - separation and purification of the product and its identification.
Group I metals (soft metals) are stored under oil
Separating funnel

48. What is reflux?
boiling without losing volatile solvents/reactants
proton donor base
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.
Ksp = 27s4

49. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
linear
Eudiometer
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
benzene is less reactive than alkenes

50. dihydrogen phosphate
H2PO4?
A salt solution.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Soluble

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AP Chemistry 2

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