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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. What is the test for hydrogen?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
RCOOH
neutralization: high K - H2O product dissociation: low K - H2O reactant
lighted splint (positive result=pop)

2. What does the solubility of organic compounds depend on?
ROH
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
by electrolysis

3. What is the general formula for an ester?
Evaporation
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
CO3²?
RCOOR

4. What are allotropes?
CnH2n
fractional distillation
different forms of the same element
?G= -ve - E°= +ve

5. Alkenes are ________ and react by __________
ion pairing
Concentration
Unsaturated - addition (ex: decolorize bromine solution)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

6. What steps do organic labs consist of?
lighted splint (positive result=pop)
More chaotic (ex: gases made)
H+
Synthesis - separation and purification of the product and its identification.

7. What are the signs for ?G and E° for spontaneous reactions?
RX
?G= -ve - E°= +ve
Heat a test tube at an angle at the side of the tube (not bottom)
Anode

8. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Glacial acetic acid
Reduction always takes place at the cathode (RED CAT) In both types of cell!
No - NH3 and HCl gases are extremely soluble
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

9. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
ROH
Decant
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

10. What electrons are lost/gained first in transition element ions?
boiling without losing volatile solvents/reactants
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.
ns² electrons (first in-first out)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

11. What is the general formula for an acid?
SO4²?
benzene is less reactive than alkenes
it is lower and occurs over less sharp a range
RCOOH

12. halides
Hg²?
Making sigma bonds and holding lone pairs
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Most are soluble except Ag - Pb

13. Which alkali metals float on water?
Ppt will NOT form (unsaturated)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
All except for lithium
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

14. What does saturated mean? Unsaturated?
Anode - oxygen. Cathode - hydrogen
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
P2O5
Kc=Kp

15. lead iodide
bright yellow
Glacial acetic acid
Pipette (burette if need repetition)
It ceases - the circuit is broken.

16. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Molecules with the same molecular formulas - but different structural formulas
Filtration
[A?]/[HA] x 100 or [BH?]/[B] x 100
No - it depends on the number of ions produced on dissolving.

17. What is the formula for alkenes?
Most INsoluble except group 1 and ammonium
ROR
Big K=kf/kr
CnH2n

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

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19. What is Big K in terms of kf and kr?
Trigonal pyramidal
Big K=kf/kr
blue (BTB)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

20. thiosulfate
blue glass - it filters UV
#ligands=charge x2
S2O3²?
OH?

21. How are primary alcohols turned into acids?
Combine the equations for the half reactions in the non-spontaneous direction
catalyst=conc H2SO4
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
fruit - fish - bases

22. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
CnH2n
Kc=Kp
S crystal at 0K=0
A salt solution.

23. Lattice energy is high for ions with _____ size and _____ charge
Only temperature
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
water and substances with (s) less dense than
small size and high charge

24. What is the basic structure of an optical isomer?
voltaic: - electrolytic: +
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
CO3²?

25. If Q > Ksp - then system shifts _______ and ppt ______
R=8.31 J/mol/K
Orange
q=mc?T q=mL (or n x ?h)
left - ppt will form

26. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
red - green - blue
water and substances with (s) less dense than
Increases.
It ceases - the circuit is broken.

27. What do group I/II metal oxides and acids form?
Purple
Salt and water
bright yellow
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

28. 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?)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Add acid to water so that the acid doesn't boil and spit
Increases down group 1 decreases down group 17

29. perchlorate
water and substances with (s) less dense than
A salt solution.
PO4³?
ClO4?

30. If ?S is positive - are the products more or less chaotic than the reactants?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
All except for lithium
More chaotic (ex: gases made)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

31. The oxidation # for acid base reactions...
do not change
[A?]/[HA] x 100 or [BH?]/[B] x 100
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Mono; di; tri; tetra; penta; hexa.

32. ammonium/ammonium compounds
They stay the same.
ClO?
The dilution effect when the solutions mix. M1V1 = M2V2
Soluble

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

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34. What are two substances that sublime at 1 atm when heated?
methyl formate
Iodine and CO2 (dry ice)
Orange
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

35. copper sulfate
Pour liquids using a funnel or down a glass rod
blue
Anode - oxygen. Cathode - hydrogen
it is lower and occurs over less sharp a range

36. 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.
bent
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Pipette (burette if need repetition)

37. What complex ion does ammonia form with silver? copper? cadmium? zinc?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
fruit - fish - bases
At half equivalence - pH=pKa
No - NH3 and HCl gases are extremely soluble

38. Generally - which oxy acid is strongest?
Transition element compounds (except if it has a full or empty d shell)
zero
Pour liquids using a funnel or down a glass rod
The one with most oxygen atoms (highest oxidation number)

39. Name some properties of Group 17
?G=negative - E° must be positive
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
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.
acids

40. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Saturated - Substitution (which requires more radical conditions)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
do not change
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

41. What do you do to get rid of most of the solution from a precipitate?
Decant
zero
RX
redox reaction

42. What is H2CO3 (carbonate acid) usually written as?
CnH2n+1 often designated 'R' ex C3H7 is propyl
H2O + CO2 (it decomposes readily)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Increases down group 1 decreases down group 17

43. What is the formula for alkanes?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
CnH2n+2
Ksp = 27s4
E=q + w (negative is by system - positive is on system)

44. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
?H-kJ - ?S-J - ?G-kJ
No - NH3 and HCl gases are extremely soluble
Orange
The compound with the lowest Ksp value.

45. What are the prefixes for the naming of binary molecular compound formulas (up to six)
ethers
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Mono; di; tri; tetra; penta; hexa.
Ppt will NOT form (unsaturated)

46. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
C4H10
P2O5
More chaotic (ex: gases made)

47. chlorine
Greenish-yellow gas
#ligands=charge x2
10?8
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

48. Nonmetals are good _____ agents. Metals are good _______ agents.
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
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.
?H-kJ - ?S-J - ?G-kJ

49. Is the freezing of ice endothermic or exothermic?
Soluble
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Exothermic
Pour liquids using a funnel or down a glass rod

50. What is the charge on a chlorine atom?
?H formation of an element in standard state=0
ROR
The dilution effect when the solutions mix. M1V1 = M2V2
zero