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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. What two types of substances are present in all redox reactions?
CnH2n
an oxidized and reduced substance
Salt + water.
[A?]/[HA] x 100 or [BH?]/[B] x 100

2. Name six characteristics of transition elements (or their compounds)
ion pairing
Saturated - Substitution (which requires more radical conditions)
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)
Group 1 hydroxides (ex: NaOH)

3. What process do you use to obtain a solvent from a solution?
?H-kJ - ?S-J - ?G-kJ
Distillation
Experimental mass/theoretical mass X 100
T increases exponentially the proportion of molecules with E > Ea

4. Generally - which oxy acid is strongest?
Acids; HCOOCH3 is an ester
water and substances with (s) less dense than
The one with most oxygen atoms (highest oxidation number)
catalyst=conc H2SO4

5. What steps do organic labs consist of?
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
Soluble
CH3COO?
Synthesis - separation and purification of the product and its identification.

6. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
chemically (ex: with carbon)
zero
Glacial acetic acid
S crystal at 0K=0

7. What reacts with an acid to create hydrogen gas?
Insoluble except group 1 and ammonium
An active metal.
0 and 14
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

8. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Glacial acetic acid
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Unsaturated - addition (ex: decolorize bromine solution)
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.

9. chlorate
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)
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.
bright yellow
ClO3?

10. Color is due to ______ _______ of light.
Both electrons come from the same atom (just as good as a regular bond)
Selective absorption
No - NH3 and HCl gases are extremely soluble
CO (poisonous)

11. phosphate
[Ag(NH3)2]? - [Cu(NH3)4]? - [Cd(NH3)4]? - [Zn(NH3)4]?
|experimental - accepted|/accepted X 100
PO4?
CnH(2n+2)

12. What element is used to vulcanize rubber?
catalyst=conc H2SO4
SO4?
Sulfur
Hg?

13. The oxidation # for acid base reactions...
Ionic compounds
0 and 14
PO4?
do not change

14. What is the general formula for a ketone?
Both electrons come from the same atom (just as good as a regular bond)
RCOR
Anode - oxygen. Cathode - hydrogen
yellow

15. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
benzene has a delocalized pi ring structure
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
10?8
Kc=Kp

16. thiosulfate
?H formation of an element in standard state=0
No - NH3 and HCl gases are extremely soluble
acids
S2O3?

17. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
CrO4?
O2 needs 4F/mol H2 needs 2F/mol
Pipette (burette if need repetition)

18. What is reflux?
boiling without losing volatile solvents/reactants
Group I metals (soft metals) are stored under oil
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
How close results are to the accepted value

19. chromate ion (soln + most solids)
brown volatile liquid
Salts (ex: CaO + SO2 ? CaSO3)
Synthesis - separation and purification of the product and its identification.
yellow

20. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
Cr2O7?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
It ceases - the circuit is broken.

21. How do you dilute an acid?
water and substances with (s) less dense than
bent
Kc=Kp
Add acid to water so that the acid doesn't boil and spit

22. Can you collect soluble gases over water?
Cu3(PO4)2
a-IMFs - b-molecular volume
No - it depends on the number of ions produced on dissolving.
No - NH3 and HCl gases are extremely soluble

23. What two compounds are great oxidizing agents?
Acidic solutions (Ex: [Fe(H2O)6]? + H2O = Fe(H2O)5OH]? + H3O?)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Synthesis - separation and purification of the product and its identification.

24. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
?G=negative - E must be positive
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Iodine and CO2 (dry ice)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

25. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Products - reactants (except for BDE when it's reactants - products)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
At half equivalence - pH=pKa
Transition element compounds (except if it has a full or empty d shell)

26. What is the first law of thermodynamics?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
E=q + w (negative is by system - positive is on system)
Increases down group 1 decreases down group 17
fruit - fish - bases

27. oxalate
No - NH3 and HCl gases are extremely soluble
Cr2O7?
|experimental - accepted|/accepted X 100
C2O4?

28. What is the word equation for condensation polymerisation ?
left - ppt will form
Most INsoluble except group 1 and ammonium
CH3COO?
Monomer + monomer = polymer product + a simple molecule such as water or HCl

29. What do ions and electrons travel through in a voltaic/electrolytic cell?
+4-covalent - +2-ionic
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Both electrons come from the same atom (just as good as a regular bond)

30. What is the formula for alkynes?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
CnH2n-2
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
C4H10

31. Name 2 ways in which you can create a buffer?
S crystal at 0K=0
White precipitate
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)
?H formation of an element in standard state=0

32. What is the conjugate base of NH3?
NH2?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ClO2?
The compound with the lowest Ksp value.

33. What is Big K in terms of kf and kr?
H+
bright yellow
Big K=kf/kr
Salt + water.

34. What is the catalyst for this reaction Ester + ?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
catalyst=conc H2SO4
Most are soluble except Ag - Pb
Cr2O7?

35. Alcohols and _______ are FG isomers
ethers
Clear
T increases exponentially the proportion of molecules with E > Ea
Trigonal pyramidal

36. Give an example of a concentrated weak acid.
Glacial acetic acid
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Molecules with the same molecular formulas - but different structural formulas
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)

37. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
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
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Mono; di; tri; tetra; penta; hexa.

38. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Ppt will NOT form (unsaturated)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
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
neutralization: high K - H2O product dissociation: low K - H2O reactant

39. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
Products - reactants (except for BDE when it's reactants - products)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

40. Aromatic compounds contain what?
strong acids/bases are written as H+ or OH- ions
Perform ICE BOX calculation based on K1
The benzene ring (or more correctly the phenyl group - C6H5)
left - ppt will form

41. What process do you use to separate two liquids with different boiling points?
fractional distillation
Group 1 hydroxides (ex: NaOH)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Perform ICE BOX calculation based on K1

42. Ca - Sr - Ba
NH2?
hydroxides (ex: Ba(OH)2)
?H formation of an element in standard state=0
?G=negative - E must be positive

43. Why are noble gases stable?
H2PO4?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Concentration
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

44. What are two allotropes of carbon?
Saturated - Substitution (which requires more radical conditions)
diamond and graphite
Salts (ex: CaO + SO2 ? CaSO3)
Suniverse increases for spontaneous processes

45. What word is a clue for a redox reaction?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Suniverse increases for spontaneous processes
Mn? - Cr? - Cr
Acidified

46. cyanide
CN?
Eudiometer
10?8
chemically (ex: with carbon)

47. What type of polymer is nylon?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
P2O5
Synthetic condensation polymer (aka a polyamide)
Ksp = s

48. Color (absorbance) is proportional to ________
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Concentration
Only temperature
zero-th: decreases - first: constant - second: increases

49. How does group 1 metals' density compare to water's?
are less dense than water
Eudiometer
Nothing
Suniverse increases for spontaneous processes

50. What is the second law of thermodynamics?
Suniverse increases for spontaneous processes
R=8.31 J/mol/K
atoms
OH- and NH3

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