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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. During a titration what is present in the beaker at the equivalence point?
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.
Glacial acetic acid
hydroxides (ex: Ba(OH)2)
A salt solution.

2. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Pale purple - (orange)-yellow - red - blue - green.
?H formation of an element in standard state=0
K1 x K2

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

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4. What are hybrid orbitals used for?
CO2 and H2O
Insoluble except nitrate and acetate
Making sigma bonds and holding lone pairs
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

5. phosphate
acid + alcohol
metal oxides and hydrides are ionically bonded and basic
ClO4?
PO4³?

6. What is H2CO3 (carbonate acid) usually written as?
same KE - but PEice<PEwater
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)
H2O + CO2 (it decomposes readily)
Iodine and CO2 (dry ice)

7. Is the freezing of ice endothermic or exothermic?
Exothermic
But S° of element is not zero (except at 0K)
neutralization: high K - H2O product dissociation: low K - H2O reactant
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

8. If a free element is involved - what type of reaction must be involved?
redox reaction
Greenish-yellow gas
by electrolysis
non-metal oxides and hydrides are covalently bonded and are acidic.

9. What is HCOOCH3?
Acids; HCOOCH3 is an ester
The dilution effect when the solutions mix. M1V1 = M2V2
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Iodine and CO2 (dry ice)

10. What is the formula for alkenes?
They stay the same.
CnH2n
a-IMFs - b-molecular volume
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

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

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12. If a weak acid is diluted more - what happens to its % dissociation value?
?H formation of an element in standard state=0
Increases.
H+
are less dense than water

13. What is the test for oxygen?
Anode - oxygen. Cathode - hydrogen
S2O3²?
Glowing splint (positive result=relights)
NO3?

14. ammonium/ammonium compounds
Soluble
Salt + water.
Insoluble except for nitrate and acetate
a-IMFs - b-molecular volume

15. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
-Ea/R
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Mono; di; tri; tetra; penta; hexa.

16. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
S crystal at 0K=0
allow for the vapor pressure of water and make sure to level levels
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

17. How can metals like iron and zinc be reduced?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
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)
chemically (ex: with carbon)
ethers

18. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
It ceases - the circuit is broken.
Time?¹ - (ex. s?¹ - hr?¹ - etc)
are less dense than water

19. An amphiprotic (amphoteric) species is...
bent
Evaporation
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
proton donor base

20. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
water and substances with (s) less dense than
CnH(2n+2)
Cr2O7²?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

21. What do hydrocarbons form when they burn in air (oxygen)?
non-metal oxides and hydrides are covalently bonded and are acidic.
RX
All except for lithium
CO2 and H2O

22. Metal hydrides are _____ and form _______ and _______ when added to water
bent
-Ea/R
Synthesis - separation and purification of the product and its identification.
ionic and form hydrogen and hydroxide

23. mercury (II) ion
a-IMFs - b-molecular volume
T increases exponentially the proportion of molecules with E > Ea
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Hg²?

24. What element is used to vulcanize rubber?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Sulfur

25. What things should you remember to do when collecting gas over water?
CrO4²?
allow for the vapor pressure of water and make sure to level levels
Soluble
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

26. What should you check for before you begin titrating?
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
C4H10
Check for air bubbles in the buret and remove the buret funnel from the buret
ClO4?

27. How do you heat a test tube?
RCOOR
RNH2
zero
Heat a test tube at an angle at the side of the tube (not bottom)

28. 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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29. dihydrogen phosphate
Decant
Disulfur dichloride
H2PO4?
HClO4

30. What do the 'a' and 'b' in Van Der Waal's equation allow for?
More chaotic (ex: gases made)
proton donor base
No - NH3 and HCl gases are extremely soluble
a-IMFs - b-molecular volume

31. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
non-metal oxides and hydrides are covalently bonded and are acidic.
Perform ICE BOX calculation based on K1
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)

32. Name some properties of Group 17
by electrolysis
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Sigma bonds are stronger than pi bonds
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

33. Both Acetic acid and ____________ are also functional isomers.
methyl formate
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)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Soluble except Ag - Pb - Ca - Sr Ba)

34. lead iodide
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)
bright yellow
acids
They stay the same.

35. thiosulfate
Saturated - Substitution (which requires more radical conditions)
OH- and NH3
S2O3²?
same KE - but PEice<PEwater

36. phosphates
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
A salt solution.
H2PO4?
Most INsoluble except group 1 and ammonium

37. How do you compute % dissociation?
CH3COO?
H2PO4?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
[A?]/[HA] x 100 or [BH?]/[B] x 100

38. lead compounds
Insoluble except nitrate and acetate
bent
water and substances with (s) less dense than
benzene is less reactive than alkenes

39. When is ?G zero?
Orange
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
CnH(2n+2)
Ksp = s²

40. acetates
acids
CO (poisonous)
P2O5
Soluble

41. What is the test for hydrogen?
water and substances with (s) less dense than
The Faraday or Faraday's constant.
lighted splint (positive result=pop)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

42. How many ligands attach to a central ion in a complex ion?
0.10M HCl (more ions)
CnH(2n+2)
#ligands=charge x2
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)

43. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Big K=kf/kr
Ksp = s²
atoms
They decrease (or could be the same if the solid has ONLY JUST disappeared)

44. What is the formula of butane?
redox reaction
C4H10
0 and 14
Suniverse increases for spontaneous processes

45. Esterification is...
CnH2n+1 often designated 'R' ex C3H7 is propyl
Graduated cylinder
Identity and purity (impure compounds usually have broad & low melting points)
acid + alcohol

46. chlorine
acids
Greenish-yellow gas
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

47. What shape is methane?
bases
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Tetrahedral

48. What shape is carbon dioxide?
do not change
P2O5
linear
Ksp = 27s4

49. What are two allotropes of carbon?
diamond and graphite
proton donor base
allow for the vapor pressure of water and make sure to level levels
catalyst=conc H2SO4

50. What does saturated mean? Unsaturated?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Heat a test tube at an angle at the side of the tube (not bottom)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)