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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. dichromate
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Trigonal pyramidal
Cr2O7²?
it's lower and occurs over less sharp a range

2. What word is a clue for a redox reaction?
Acidified
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
bases
Soluble

3. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
non-metal oxides and hydrides are covalently bonded and are acidic.
Most are soluble except Ag - Pb
Ksp = s²
Synthesis - separation and purification of the product and its identification.

4. How do you heat a test tube?
by electrolysis
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Heat a test tube at an angle at the side of the tube (not bottom)
benzene has a delocalized pi ring structure

5. Alkanes are _________ and react by _________
?H-kJ - ?S-J - ?G-kJ
yellow
Saturated - Substitution (which requires more radical conditions)
Exothermic

6. At what point during titration do you have the perfect buffer - and what is the pH at this point?
RNH2
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
H3PO4
At half equivalence - pH=pKa

7. What type of compounds do metals/non metals form?
it reacts by substitution NOT addition
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Ionic compounds
0 and 14

8. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Soluble
NO3?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
RCOR

9. What is the formula of copper (II) phosphate?
are less dense than water
Molecules with the same molecular formulas - but different structural formulas
Cu3(PO4)2
CrO4²?

10. What is HCOOCH3?
Acids; HCOOCH3 is an ester
Hg²?
Saturated - Substitution (which requires more radical conditions)
More chaotic (ex: gases made)

11. What is the pH of 1.0M HCl? 1M NaOH?
Combine the equations for the half reactions in the non-spontaneous direction
0 and 14
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
S2O3²?

12. What is an Alkyl group?

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13. potassium permanganate
ClO3?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
The one with most oxygen atoms (highest oxidation number)
Purple

14. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Salt + water
R=8.31 J/mol/K
Big K=kf/kr

15. How are strong ones written?
allow for the vapor pressure of water and make sure to level levels
Anode - oxygen. Cathode - hydrogen
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
strong acids/bases are written as H+ or OH- ions

16. chlorate
Salt + water
atoms
ClO3?
CO2 and H2O

17. A Bronsted-Lowry base is...
+4-covalent - +2-ionic
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Sigma bonds are stronger than pi bonds
proton acceptor.

18. Nonmetals are good _____ agents. Metals are good _______ agents.
Silvery gray solid - brown - purple
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
ethers
Salt + water

19. Alkenes are ________ and react by __________
Pipette (burette if need repetition)
CO (poisonous)
Unsaturated - addition (ex: decolorize bromine solution)
The one with most oxygen atoms (highest oxidation number)

20. What is the basic structure of an optical isomer?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
?G= -ve - E°= +ve
Salt and water

21. dihydrogen phosphate
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
H2PO4?
red - green - blue
All single: sp³ - one double: sp² - two doubles: sp - one triple: sp - two single and two lone pairs: sp³ - three single and one lone pair: sp³

22. What do you use for an acid spill? base spill?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
RCOR
zero-th: decreases - first: constant - second: increases
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

23. oxalate
it reacts by substitution NOT addition
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
C2O4²?
ClO2?

24. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
bright yellow
Mn²? - Cr³? - Cr³
All except for lithium
Pour liquids using a funnel or down a glass rod

25. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
by electrolysis
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

26. What type of compounds do Group 14 form?
Heat a test tube at an angle at the side of the tube (not bottom)
Experimental mass/theoretical mass X 100
No - NH3 and HCl gases are extremely soluble
+4-covalent - +2-ionic

27. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
an oxidized and reduced substance
Increases.
Current - time and charge on ion (moles of e used in half cell reaction)
bent

28. What is a coordinate covalent bond?
Transition element compounds (except if it has a full or empty d shell)
RCOOR
Acid rain - dissolves marble buildings/statues and kills trees.
Both electrons come from the same atom (just as good as a regular bond)

29. What is the catalyst for this reaction Ester + ?
CH3COO?
The benzene ring (or more correctly the phenyl group - C6H5)
Perform ICE BOX calculation based on K1
catalyst=conc H2SO4

30. Which value of R do you use for all energy and kinetics calculations?
bases
R=8.31 J/mol/K
Mn²? - Cr³? - Cr³
Nothing

31. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
brown volatile liquid
zero
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

32. What is the test for hydrogen?
brown volatile liquid
redox reaction
lighted splint (positive result=pop)
Time?¹ - (ex. s?¹ - hr?¹ - etc)

33. What do group I/II metal oxides plus water form?
bases
T increases exponentially the proportion of molecules with E > Ea
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
S crystal at 0K=0

34. copper sulfate
Most INsoluble except group 1 and ammonium
blue
0.10M HCl (more ions)
Pour liquids using a funnel or down a glass rod

35. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Nothing
Experimental mass/theoretical mass X 100
neutralization: high K - H2O product dissociation: low K - H2O reactant
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)

36. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
lighted splint (positive result=pop)
RCHO (carbonyl at end)
No - it depends on the number of ions produced on dissolving.
basic

37. sulfate
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
SO4²?
Acidified
No - NH3 and HCl gases are extremely soluble

38. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
CrO4²?
Group I metals (soft metals) are stored under oil
H+

39. What is the formula for percent yield?
K2
Experimental mass/theoretical mass X 100
Add acid to water so that the acid doesn't boil and spit
CnH(2n+2)

40. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
blue glass - it filters UV
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
by electrolysis

41. What do you need to make a polymer?
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)
Experimental mass/theoretical mass X 100
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
benzene has a delocalized pi ring structure

42. dichromate (soln + most solids)
Pipette (burette if need repetition)
blue (BTB)
Orange
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

43. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
yellow
Ksp = 27s4
Soluble
Exothermic

44. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
[A?]/[HA] x 100 or [BH?]/[B] x 100
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Glacial acetic acid

45. acetates
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
acids
Selective absorption
Soluble

46. Is the ?H formation of an element in standard state zero?
ion pairing
Purple
?H formation of an element in standard state=0
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

47. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
no - they're written undissociated (HAaq)
CnH(2n+2)
zero

48. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Mn²? - Cr³? - Cr³
They stay the same.
K1 x K2
Ions go through the salt bridge - electrons go through metal wires in the external circuit

49. group 1 ions/compounds
an oxidized and reduced substance
diamond and graphite
Soluble
Concentration

50. 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
no - they're written undissociated (HAaq)
boiling without losing volatile solvents/reactants
OH?