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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 does the solubility of organic compounds depend on?
The dilution effect when the solutions mix. M1V1 = M2V2
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

2. A Bronsted-Lowry acid is...
How grouped results are
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
proton donor base

3. What changes Keq?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Soluble
Only temperature
allow for the vapor pressure of water and make sure to level levels

4. What are isomers?
Hg2²?
Molecules with the same molecular formulas - but different structural formulas
Insoluble except group 1 and ammonium
RCOOR

5. What shape is methane?
Tetrahedral
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
small size and high charge
RCOOH

6. Give an example of a concentrated weak acid.
catalyst=conc H2SO4
different forms of the same element
Glacial acetic acid
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

7. What is the formula for alkanes?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Group 1 hydroxides (ex: NaOH)
CnH2n+2
NH4?

8. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
Ions go through the salt bridge - electrons go through metal wires in the external circuit
ethers
[A?]/[HA] x 100 or [BH?]/[B] x 100

9. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
Insoluble except group 1 and ammonium
Pale purple - (orange)-yellow - red - blue - green.
CN?

10. What is the slope of the graph of lnk vs. 1/T?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
-Ea/R
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

11. bromothymol
strong acids/bases are written as H+ or OH- ions
Decant
blue (BTB)
Orange

12. Why are i factors (Van't Hoff factors) often less than ideal?
atoms
ion pairing
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Insoluble except group 1 and ammonium

13. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Heat a test tube at an angle at the side of the tube (not bottom)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
boiling without losing volatile solvents/reactants
CO (poisonous)

14. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
K2
HClO4

15. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
ethers
same KE - but PEice<PEwater
Iodine and CO2 (dry ice)
CrO4²?

16. What causes the dramatic effect of T on rate?
Heptane
T increases exponentially the proportion of molecules with E > Ea
Pale purple - (orange)-yellow - red - blue - green.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

17. When the salt bridge is removed what happens to the cell reaction?
Ksp = 27s4
It ceases - the circuit is broken.
Soluble except Ag - Pb - Ca - Sr Ba)
The one with most oxygen atoms (highest oxidation number)

18. group 1 ions/compounds
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Soluble
acids
Products - reactants (except for BDE when it's reactants - products)

19. What is accuracy?
Anode - oxygen. Cathode - hydrogen
How close results are to the accepted value
Glowing splint (positive result=relights)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

20. thiosulfate
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
S2O3²?

21. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Sigma bonds are stronger than pi bonds
Ksp = s²
blue glass - it filters UV
Decant

22. Is the standard entropy (S°) of an element zero?
CO (poisonous)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
The dilution effect when the solutions mix. M1V1 = M2V2
But S° of element is not zero (except at 0K)

23. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
0.10M HCl (more ions)
Mono; di; tri; tetra; penta; hexa.
Insoluble except group 1 and ammonium

24. What are isotopes?
Pale purple - (orange)-yellow - red - blue - green.
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
blue

25. What reacts with an acid to create hydrogen gas?
proton acceptor.
a-IMFs - b-molecular volume
P2O5
An active metal.

26. bromine
Current - time and charge on ion (moles of e used in half cell reaction)
brown volatile liquid
Making sigma bonds and holding lone pairs
Anode - oxygen. Cathode - hydrogen

27. When combining half equations - what do you do to E° values when multiplying coefficients?
Disulfur dichloride
Nothing
Synthesis - separation and purification of the product and its identification.
a-IMFs - b-molecular volume

28. What is the formula for obtaining charge flowing in a cell?
zero
CnH2n
non-metal oxides and hydrides are covalently bonded and are acidic.
Q=It (time in seconds)

29. What is the formula of butane?
C4H10
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Sulfur
bright yellow

30. dichromate (soln + most solids)
Orange
[A?]/[HA] x 100 or [BH?]/[B] x 100
C4H10
OH?

31. What is a coordinate covalent bond?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Both electrons come from the same atom (just as good as a regular bond)
zero
catalyst=conc H2SO4

32. oxalate
C2O4²?
fruit - fish - bases
Initiation energy (NOT Ea)
ClO3?

33. silver iodide
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)
All except for lithium
Anode

34. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Mono; di; tri; tetra; penta; hexa.
Group 1 hydroxides (ex: NaOH)

35. What steps do organic labs consist of?
blue glass - it filters UV
Synthesis - separation and purification of the product and its identification.
a-IMFs - b-molecular volume
benzene has a delocalized pi ring structure

36. barium sulfate
CH3COO?
Current - time and charge on ion (moles of e used in half cell reaction)
ion pairing
White precipitate

37. What is an Alkyl group?

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38. How are metal oxides and hydrides bonded? are they acidic or basic?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
metal oxides and hydrides are ionically bonded and basic
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

39. What do you use to look at burning magnesium? why?
blue glass - it filters UV
?G= -ve - E°= +ve
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
ion pairing

40. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
catalyst=conc H2SO4
?H formation of an element in standard state=0
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

41. iodine - iodine solution - iodine vapor
Ksp = s²
K2
Silvery gray solid - brown - purple
CH3COO?

42. What is the general formula for an alcohol?
a-IMFs - b-molecular volume
RCOOR
ROH
Group I metals (soft metals) are stored under oil

43. What do you do to get rid of most of the solution from a precipitate?
Decant
Insoluble (except group 1 ammonium and Ba)
are less dense than water
basic

44. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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45. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
They decrease (or could be the same if the solid has ONLY JUST disappeared)
same KE - but PEice<PEwater
Salt + water

46. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
The compound with the lowest Ksp value.
Only temperature
Unsaturated - addition (ex: decolorize bromine solution)
OH?

47. What do you use for an acid spill? base spill?
How grouped results are
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Purple
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

48. Acids + Carbonates (bicarbonates) make?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Experimental mass/theoretical mass X 100
Salt and water

49. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
allow for the vapor pressure of water and make sure to level levels
bent
#ligands=charge x2

50. Ions are not ______.
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)
Acid rain - dissolves marble buildings/statues and kills trees.
atoms
Making sigma bonds and holding lone pairs

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AP Chemistry 2

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