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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.
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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. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
Only temperature
Disulfur dichloride
CH3COO?

2. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
MnO4?
Ionic compounds
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
NO3?

3. 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.
do not change
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

4. dichromate
Cr2O7²?
Molecules with the same molecular formulas - but different structural formulas
q=mc?T q=mL (or n x ?h)
CO2 and H2O

5. Which alkali metals float on water?
Products - reactants (except for BDE when it's reactants - products)
lighted splint (positive result=pop)
ClO?
All except for lithium

6. potassium permanganate
Purple
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Anode
voltaic: + electrolytic: -

7. bromothymol
blue (BTB)
ClO2?
zero
Read the bottom of the meniscus

8. Is a graduated cylinder or beaker more accurate?
The benzene ring (or more correctly the phenyl group - C6H5)
Soluble
Graduated cylinder
ionic and form hydrogen and hydroxide

9. dichromate (soln + most solids)
?G= -ve - E°= +ve
Orange
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

10. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
CO2 and H2O
Salt and water
NH2?

11. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
CO (poisonous)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Cu3(PO4)2
Big K=kf/kr

12. How can metals like iron and zinc be reduced?
S crystal at 0K=0
chemically (ex: with carbon)
At half equivalence - pH=pKa
Silvery gray solid - brown - purple

13. Give an example of a concentrated weak acid.
|experimental - accepted|/accepted X 100
same KE - but PEice<PEwater
PO4³?
Glacial acetic acid

14. What do metal oxides plus non- metal oxides form?
Separating funnel
H2PO4?
Salts (ex: CaO + SO2 ? CaSO3)
0.10M HCl (more ions)

15. Does reactivity increase/decrease going down group 1 and group 17?
R=8.31 J/mol/K
Increases down group 1 decreases down group 17
ethers
by electrolysis

16. How does half life change for zero-th order - first order - and second order processes?
chemically (ex: with carbon)
Increases.
zero-th: decreases - first: constant - second: increases
Reduction always takes place at the cathode (RED CAT) In both types of cell!

17. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
Suniverse increases for spontaneous processes
Transition element compounds (except if it has a full or empty d shell)
?H formation of an element in standard state=0

18. What device would you use to measure a volume of gas?
ClO3?
Eudiometer
But S° of element is not zero (except at 0K)
C2O4²?

19. Alkenes are ________ and react by __________
ion pairing
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
metal oxides and hydrides are ionically bonded and basic
Unsaturated - addition (ex: decolorize bromine solution)

20. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Glacial acetic acid
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
CrO4²?

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

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22. Do anions flow to the cathode or anode?
Only temperature
Anode
do not change
proton donor base

23. 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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24. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Pipette (burette if need repetition)
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
CnH2n
Perform ICE BOX calculation based on K1

25. What is the general formula for an alcohol?
ROH
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)
Experimental mass/theoretical mass X 100
0 and 14

26. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
yellow
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
CnH2n+1 often designated 'R' ex C3H7 is propyl

27. What is a coordinate covalent bond?
Perform ICE BOX calculation based on K1
Both electrons come from the same atom (just as good as a regular bond)
Synthetic condensation polymer (aka a polyamide)
0.10M HCl (more ions)

28. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
RCHO (carbonyl at end)
it's lower and occurs over less sharp a range
Heat a test tube at an angle at the side of the tube (not bottom)

29. Ca - Sr - Ba
0 and 14
Sigma bonds are stronger than pi bonds
Ksp = 108s5
hydroxides (ex: Ba(OH)2)

30. Name six characteristics of transition elements (or their compounds)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
different forms of the same element
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)
Combine the equations for the half reactions in the non-spontaneous direction

31. Aromatic compounds contain what?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
blue glass - it filters UV
The benzene ring (or more correctly the phenyl group - C6H5)
chemically (ex: with carbon)

32. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
q=mc?T q=mL (or n x ?h)
do not change
Acids; HCOOCH3 is an ester
Ksp = 27s4

33. Alkanes are _________ and react by _________
Saturated - Substitution (which requires more radical conditions)
Distillation
Salt + water
Conjugate pair (one must be a weak base or acid)

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

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35. cyanide
CN?
acid + alcohol
Only temperature
Filtration

36. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
do not change
Anode - oxygen. Cathode - hydrogen
no - they're written undissociated (HAaq)

37. 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
K2
Pale purple - (orange)-yellow - red - blue - green.
Soluble

38. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
?G= -ve - E°= +ve
The dilution effect when the solutions mix. M1V1 = M2V2
K1 x K2
Decant

39. What does saturated mean? Unsaturated?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
it reacts by substitution NOT addition

40. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
a-IMFs - b-molecular volume
P2O5
ns² electrons (first in-first out)
Mono; di; tri; tetra; penta; hexa.

41. copper sulfate
blue
Both electrons come from the same atom (just as good as a regular bond)
same KE - but PEice<PEwater
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

42. Neutralization is an ________ reaction.
0 and 14
small size and high charge
RCOOR
Exothermic (?H for ANY sa/sb = -57kJ/mol)

43. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Disulfur dichloride
zero
Ksp = 4s³

44. 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?)
Silvery gray solid - brown - purple
OH?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

45. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
zero
10?8
CO3²?
Ksp = s²

46. What type of metals don't react with water or acids to form H2?

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47. A Bronsted-Lowry base is...
Both electrons come from the same atom (just as good as a regular bond)
The benzene ring (or more correctly the phenyl group - C6H5)
proton acceptor.
methyl formate

48. What is the third law of thermodynamics?
Sigma bonds are stronger than pi bonds
Increases.
S crystal at 0K=0
?G= -ve - E°= +ve

49. What is accuracy?
How close results are to the accepted value
'non-active' metals such as Cu - Ag - Au - Pt - etc.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Pale purple - (orange)-yellow - red - blue - green.

50. What are the formulas for q?
All except for lithium
q=mc?T q=mL (or n x ?h)
Pale purple - (orange)-yellow - red - blue - green.
OH?