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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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.
?G=negative - E° must be positive
A) any range. b) 8-10 c) 4-6
Iodine and CO2 (dry ice)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

2. Is a graduated cylinder or beaker more accurate?
RCOOH
Graduated cylinder
Iodine and CO2 (dry ice)
The Faraday or Faraday's constant.

3. During a titration what is present in the beaker at the equivalence point?
Making sigma bonds and holding lone pairs
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
A salt solution.
water and substances with (s) less dense than

4. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
A) any range. b) 8-10 c) 4-6
PO4³?
Q=It (time in seconds)

5. 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?)
Both electrons come from the same atom (just as good as a regular bond)
neutralization: high K - H2O product dissociation: low K - H2O reactant
Transition element compounds (except if it has a full or empty d shell)

6. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
diamond and graphite
Trigonal pyramidal
RNH2

7. halides
Most are soluble except Ag - Pb
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
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
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

8. When the salt bridge is removed what happens to the cell reaction?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
It ceases - the circuit is broken.
proton donor base
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

9. When can supercooling occur? What does it look like on a cooling curve?

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10. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
left - ppt will form
Increases.
Most are soluble except Ag - Pb

11. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Add acid to water so that the acid doesn't boil and spit
Ppt will NOT form (unsaturated)
Molecules with the same molecular formulas - but different structural formulas

12. Nonmetals are good _____ agents. Metals are good _______ agents.
ClO3?
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)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
blue

13. thiosulfate
by electrolysis
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
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
S2O3²?

14. Does reactivity increase/decrease going down group 1 and group 17?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
An active metal.
Increases down group 1 decreases down group 17
voltaic: + electrolytic: -

15. Buffer capacity must contain decent amounts of a ________ ________
fruit - fish - bases
Conjugate pair (one must be a weak base or acid)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Check for air bubbles in the buret and remove the buret funnel from the buret

16. What is the formula for obtaining charge flowing in a cell?
Concentration
hydroxides (ex: Ba(OH)2)
Q=It (time in seconds)
Orange

17. Generally - which oxy acid is strongest?
Acidified
The one with most oxygen atoms (highest oxidation number)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Nothing

18. phosphates
brown volatile liquid
ROH
Most INsoluble except group 1 and ammonium
Cr2O7²?

19. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Pale purple - (orange)-yellow - red - blue - green.
CnH2n
bright yellow
Both electrons come from the same atom (just as good as a regular bond)

20. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
red - green - blue
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

21. What do you use for an acid spill? base spill?
left - ppt will form
allow for the vapor pressure of water and make sure to level levels
CN?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

22. hydroxides
H3PO4
Read the bottom of the meniscus
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Insoluble (except group 1 ammonium and Ba)

23. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
CrO4²?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

24. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
catalyst=conc H2SO4
Ksp = 4s³

25. How are more active metals reduced?
by electrolysis
RCHO (carbonyl at end)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

26. What changes Keq?
Only temperature
redox reaction
Big K=kf/kr
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

27. What equipment do you need for a titration?
Hg²?
Pale purple - (orange)-yellow - red - blue - green.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
it's lower and occurs over less sharp a range

28. Give an example of a concentrated weak acid.
blue (BTB)
Sigma bonds are stronger than pi bonds
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Glacial acetic acid

29. sulfate
SO4²?
A) any range. b) 8-10 c) 4-6
H2O + CO2 (it decomposes readily)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

30. What is HCOOCH3?
Acids; HCOOCH3 is an ester
Insoluble except nitrate and acetate
No - NH3 and HCl gases are extremely soluble
RCOOH

31. How do you get Ecell for spontaneous reactions?
Silvery gray solid - brown - purple
CO (poisonous)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
NH2?

32. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
CN?
Ksp = 108s5
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
fruit - fish - bases

33. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Most INsoluble except group 1 and ammonium
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

34. Is the standard entropy (S°) of an element zero?
Iodine and CO2 (dry ice)
But S° of element is not zero (except at 0K)
Both electrons come from the same atom (just as good as a regular bond)
Group I metals (soft metals) are stored under oil

35. What is the name of S2Cl2? (Know how to name others like this - too)
Soluble except Ag - Pb - Ca - Sr Ba)
Disulfur dichloride
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Heat a test tube at an angle at the side of the tube (not bottom)

36. What is the general formula for an alcohol?
blue (BTB)
Mn²? - Cr³? - Cr³
ROH
Hg2²?

37. What element is used to vulcanize rubber?
Sulfur
SO4²?
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)
#ligands=charge x2

38. Aromatic compounds contain what?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
H3PO4
Reduction always takes place at the cathode (RED CAT) In both types of cell!
The benzene ring (or more correctly the phenyl group - C6H5)

39. One mole of electrons carries 96500Coulombs - what is this quantity called?

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40. If a weak acid is diluted more - what happens to its % dissociation value?
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)
RCOOR
Synthetic condensation polymer (aka a polyamide)
Increases.

41. Acid plus base make?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Salt + water.
The Faraday or Faraday's constant.

42. carbonate
HClO4
CO3²?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

43. What are the prefixes for the naming of binary molecular compound formulas (up to six)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Mono; di; tri; tetra; penta; hexa.
atoms
'non-active' metals such as Cu - Ag - Au - Pt - etc.

44. What is the test for hydrogen?
At half equivalence - pH=pKa
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
They decrease (or could be the same if the solid has ONLY JUST disappeared)
lighted splint (positive result=pop)

45. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
T increases exponentially the proportion of molecules with E > Ea
Soluble
Add acid to water so that the acid doesn't boil and spit

46. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Heptane
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
O2 needs 4F/mol H2 needs 2F/mol

47. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Soluble except Ag - Pb - Ca - Sr Ba)
The dilution effect when the solutions mix. M1V1 = M2V2
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
CH3COO?

48. Colorless doesn't mean ______
H2PO4?
Clear
+4-covalent - +2-ionic
Initiation energy (NOT Ea)

49. Alkanes are _________ and react by _________
same KE - but PEice<PEwater
ClO2?
blue
Saturated - Substitution (which requires more radical conditions)

50. What process do you use to obtain a solvent from a solution?
Pour liquids using a funnel or down a glass rod
Distillation
Cr2O7²?
benzene has a delocalized pi ring structure