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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 is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
Trigonal pyramidal
?H-kJ - ?S-J - ?G-kJ
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
White precipitate

2. Do you use J or kJ for ?H - ?S - and ?G?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Exothermic
Ionic compounds
?H-kJ - ?S-J - ?G-kJ

3. What do nonmetal oxides plus water form?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
ClO3?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
acids

4. What is the formula of copper (II) phosphate?
Insoluble
Hg²?
Cu3(PO4)2
Cr2O7²?

5. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
All except for lithium
CnH2n
blue (BTB)

6. What is the test for oxygen?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
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
Glowing splint (positive result=relights)
allow for the vapor pressure of water and make sure to level levels

7. What do you need to make a polymer?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
0 and 14
Experimental mass/theoretical mass X 100
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)

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.
How grouped results are
zero-th: decreases - first: constant - second: increases
neutralization: high K - H2O product dissociation: low K - H2O reactant
C2O4²?

9. Is a graduated cylinder or beaker more accurate?
same KE - but PEice<PEwater
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
CnH2n-2
Graduated cylinder

10. What is the sign of the cathode in voltaic cells? in electrolytic cells?
+4-covalent - +2-ionic
do not change
bright yellow
voltaic: + electrolytic: -

11. Is the freezing of ice endothermic or exothermic?
Exothermic
Anode - oxygen. Cathode - hydrogen
PO4³?
Pale purple - (orange)-yellow - red - blue - green.

12. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
Group 1 hydroxides (ex: NaOH)
Graduated cylinder
Disulfur dichloride

13. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Read the bottom of the meniscus
CO (poisonous)
Synthetic condensation polymer (aka a polyamide)
NO3?

14. 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?)
H3PO4
it reacts by substitution NOT addition
S2O3²?

15. bromine
brown volatile liquid
S2O3²?
RNH2
CnH(2n+2)

16. How are non-metal oxides and hydrides bonded? are they acidic or basic?
do not change
non-metal oxides and hydrides are covalently bonded and are acidic.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Soluble

17. What is the second law of thermodynamics?
SO4²?
Insoluble
Suniverse increases for spontaneous processes
Salt and water

18. What process do you use to obtain the precipitate from a solution?
Both electrons come from the same atom (just as good as a regular bond)
Synthetic condensation polymer (aka a polyamide)
Filtration
At half equivalence - pH=pKa

19. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
An active metal.
MnO4?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
No - it depends on the number of ions produced on dissolving.

20. Alkenes are ________ and react by __________
ion pairing
Unsaturated - addition (ex: decolorize bromine solution)
Molecules with the same molecular formulas - but different structural formulas
Eudiometer

21. What is the catalyst for this reaction Ester + ?
Insoluble (except group 1 ammonium and Ba)
catalyst=conc H2SO4
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
brown volatile liquid

22. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
RCOOR
voltaic: + electrolytic: -
S crystal at 0K=0

23. ammonium/ammonium compounds
OH- and NH3
NH4?
Soluble
CO3²?

24. Aromatic compounds contain what?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Nothing
The benzene ring (or more correctly the phenyl group - C6H5)
atoms

25. What is reflux?
E=q + w (negative is by system - positive is on system)
Kc=Kp
The benzene ring (or more correctly the phenyl group - C6H5)
boiling without losing volatile solvents/reactants

26. How are primary alcohols turned into acids?
O2 needs 4F/mol H2 needs 2F/mol
CO (poisonous)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Insoluble except for nitrate and acetate

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

28. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
Separating funnel
C4H10
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

29. What is the relationship in strength between sigma and pi bonds?
Molecules with the same molecular formulas - but different structural formulas
Sigma bonds are stronger than pi bonds
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)
Synthesis - separation and purification of the product and its identification.

30. What is the general formula for alkyl halides?
ClO?
hydroxides (ex: Ba(OH)2)
RX
Synthesis - separation and purification of the product and its identification.

31. 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.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
OH- and NH3
Ksp = 108s5

32. Both Acetic acid and ____________ are also functional isomers.
a-IMFs - b-molecular volume
Mono; di; tri; tetra; penta; hexa.
Selective absorption
methyl formate

33. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
Most INsoluble except group 1 and ammonium
The one with most oxygen atoms (highest oxidation number)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

34. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Glowing splint (positive result=relights)
Ksp = s²
Exothermic (?H for ANY sa/sb = -57kJ/mol)

35. At what point during titration do you have the perfect buffer - and what is the pH at this point?
small size and high charge
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)
At half equivalence - pH=pKa
Heat a test tube at an angle at the side of the tube (not bottom)

36. mercury (II) ion
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
catalyst=conc H2SO4
Hg²?
Pale yellow

37. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
Making sigma bonds and holding lone pairs
Cu3(PO4)2
They stay the same.

38. Which value of R do you use for all energy and kinetics calculations?
MnO4?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
R=8.31 J/mol/K
Group I metals (soft metals) are stored under oil

39. How do you find the pH for a dibasic acid? (H2A)?
Group I metals (soft metals) are stored under oil
No - it depends on the number of ions produced on dissolving.
Soluble except Ag - Pb - Ca - Sr Ba)
Perform ICE BOX calculation based on K1

40. Why are i factors (Van't Hoff factors) often less than ideal?
blue
Group 1 hydroxides (ex: NaOH)
ion pairing
ns² electrons (first in-first out)

41. What effect does increasing the size/surface area of a voltaic cell have on the cell?
non-metal oxides and hydrides are covalently bonded and are acidic.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
ns² electrons (first in-first out)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

42. ammonium
Pale purple - (orange)-yellow - red - blue - green.
Exothermic
NH4?
Iodine and CO2 (dry ice)

43. phosphate
PO4³?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
No - NH3 and HCl gases are extremely soluble
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

44. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
?G=negative - E° must be positive
Ionic compounds
RCOOR

45. What word is a clue for a redox reaction?
Q=It (time in seconds)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
bright yellow
Acidified

46. primary colors
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
red - green - blue
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
The benzene ring (or more correctly the phenyl group - C6H5)

47. Which alkali metals float on water?
All except for lithium
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
PO4³?
H2O + CO2 (it decomposes readily)

48. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Insoluble (except group 1 ammonium and Ba)
C4H10

49. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
CN?
No - it depends on the number of ions produced on dissolving.
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

50. What is the formula for percent yield?
Ionic compounds
S2O3²?
Experimental mass/theoretical mass X 100
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)