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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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 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.
E=q + w (negative is by system - positive is on system)
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)
The compound with the lowest Ksp value.
A) any range. b) 8-10 c) 4-6

2. Does Benzene react by addition or substitution?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Add acid to water so that the acid doesn't boil and spit
it reacts by substitution NOT addition
Group 1 hydroxides (ex: NaOH)

3. What is H2CO3 (carbonate acid) usually written as?
Selective absorption
H2O + CO2 (it decomposes readily)
Sulfur
H2PO4?

4. What do metal oxides plus acids form?
Current - time and charge on ion (moles of e used in half cell reaction)
Salt + water
Ions go through the salt bridge - electrons go through metal wires in the external circuit
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

5. What apparatus do you use to pour liquids?
non-metal oxides and hydrides are covalently bonded and are acidic.
zero
Pour liquids using a funnel or down a glass rod
But S° of element is not zero (except at 0K)

6. Name C7H16
voltaic: + electrolytic: -
Heptane
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Purple

7. What is the general formula for an aldehyde?
blue (BTB)
RCHO (carbonyl at end)
Increases down group 1 decreases down group 17
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

8. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
PO4³?
Glowing splint (positive result=relights)
10?8

9. What is the general formula for an ether?
ROR
Glacial acetic acid
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
blue

10. permanganate
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Only temperature
MnO4?
Soluble

11. A Bronsted-Lowry base is...
proton acceptor.
benzene has a delocalized pi ring structure
Initiation energy (NOT Ea)
it reacts by substitution NOT addition

12. ammonium
water and substances with (s) less dense than
NH4?
?H formation of an element in standard state=0
Making sigma bonds and holding lone pairs

13. Why are noble gases stable?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ROH
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

14. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
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
Group I metals (soft metals) are stored under oil
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
different forms of the same element

15. iodine - iodine solution - iodine vapor
ionic and form hydrogen and hydroxide
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Silvery gray solid - brown - purple
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

16. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
linear
Molecules with the same molecular formulas - but different structural formulas
Ksp = s²
same KE - but PEice<PEwater

17. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
10?8
are less dense than water
Concentration

18. What process do you use to separate two liquids with different boiling points?
bright yellow
Ksp = 108s5
How grouped results are
fractional distillation

19. Nonmetals are good _____ agents. Metals are good _______ agents.
acid + alcohol
Separating funnel
blue
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

20. thiosulfate
Soluble
do not change
The Faraday or Faraday's constant.
S2O3²?

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

22. What is the formula of copper (II) phosphate?
They stay the same.
hydroxides (ex: Ba(OH)2)
Cu3(PO4)2
Nothing

23. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 27s4
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
linear
Ksp = 4s³

24. Is the freezing of ice endothermic or exothermic?
Cr2O7²?
Exothermic
Separating funnel
CnH2n-2

25. ________ are Lewis bases - because they can donate a lone pair of electrons.
hydroxides (ex: Ba(OH)2)
OH- and NH3
OH?
?H-kJ - ?S-J - ?G-kJ

26. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
blue (BTB)
zero
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
bent

27. What is the general formula for an amine?
Sigma bonds are stronger than pi bonds
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
RNH2
Anode - oxygen. Cathode - hydrogen

28. What is the word equation for addition polymerisation?
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)
Transition element compounds (except if it has a full or empty d shell)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Ppt will NOT form (unsaturated)

29. halides
Clear
Most are soluble except Ag - Pb
Filtration
lighted splint (positive result=pop)

30. oxalate
-Ea/R
Kc=Kp
C2O4²?
Glacial acetic acid

31. What shape is methane?
Mn²? - Cr³? - Cr³
voltaic: + electrolytic: -
CH3COO?
Tetrahedral

32. When combining half equations - what do you do to E° values when multiplying coefficients?
metal oxides and hydrides are ionically bonded and basic
Clear
Nothing
?H formation of an element in standard state=0

33. What is the test for oxygen?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Glowing splint (positive result=relights)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

34. What do you do to get rid of most of the solution from a precipitate?
Decant
Ions go through the salt bridge - electrons go through metal wires in the external circuit
fruit - fish - bases
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

35. What are isotopes?
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)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
small size and high charge
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

36. What is the first law of thermodynamics?
fruit - fish - bases
E=q + w (negative is by system - positive is on system)
basic
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?)

37. What are two substances that sublime at 1 atm when heated?
ion pairing
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Acid rain - dissolves marble buildings/statues and kills trees.
Iodine and CO2 (dry ice)

38. When is ?G zero?
Ksp = 27s4
zero
CN?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

39. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
No - NH3 and HCl gases are extremely soluble
Unsaturated - addition (ex: decolorize bromine solution)
H2PO4?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

40. What are hybrid orbitals used for?
Making sigma bonds and holding lone pairs
Acids; HCOOCH3 is an ester
Acidified
acids

41. chromate ion (soln + most solids)
Decant
catalyst=conc H2SO4
S crystal at 0K=0
yellow

42. Can you collect soluble gases over water?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
No - NH3 and HCl gases are extremely soluble
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

43. What kind of bonding structure does benzene have?
0 and 14
|experimental - accepted|/accepted X 100
Pour liquids using a funnel or down a glass rod
benzene has a delocalized pi ring structure

44. What type of compounds do Group 14 form?
voltaic: + electrolytic: -
hydroxides (ex: Ba(OH)2)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
+4-covalent - +2-ionic

45. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Ksp = 108s5
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.
CO (poisonous)
Insoluble (except group 1 ammonium and Ba)

46. What is the formula for percent error?
Concentration
|experimental - accepted|/accepted X 100
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
lighted splint (positive result=pop)

47. Acid plus base make?
More chaotic (ex: gases made)
by electrolysis
Salt + water.
Graduated cylinder

48. Alcohols and _______ are FG isomers
ethers
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)
K1 x K2
no - they're written undissociated (HAaq)

49. What is the formula of butane?
?H formation of an element in standard state=0
Pale yellow
C4H10
Nothing

50. How do you get Ecell for spontaneous reactions?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Pour liquids using a funnel or down a glass rod
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)