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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. How does the KE and PE of ice at 0C compare to the KE and PE of water at 0C?
strong acids/bases are written as H+ or OH- ions
same KE - but PEice<PEwater
Q=It (time in seconds)
Clear

2. Are weak acids (and bases) written dissociated?
Q=It (time in seconds)
Insoluble except for nitrate and acetate
no - they're written undissociated (HAaq)
How close results are to the accepted value

3. When a cell is 'flat' What is its voltage?
S crystal at 0K=0
Read the bottom of the meniscus
zero
Iodine and CO2 (dry ice)

4. Is the standard entropy (S) of an element zero?
fractional distillation
Products - reactants (except for BDE when it's reactants - products)
But S of element is not zero (except at 0K)
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.

5. What is the slope of the graph of lnk vs. 1/T?
NO3?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Identity and purity (impure compounds usually have broad & low melting points)
-Ea/R

6. What are allotropes?
blue glass - it filters UV
different forms of the same element
Heptane
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

7. What is HCOOCH3?
How grouped results are
Acids; HCOOCH3 is an ester
allow for the vapor pressure of water and make sure to level levels
Making sigma bonds and holding lone pairs

8. Color (absorbance) is proportional to ________
Concentration
catalyst=conc H2SO4
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
Soluble except Ag - Pb - Ca - Sr Ba)

9. Does Kw increase or decrease with T? Why?
?G=negative - E must be positive
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
#ligands=charge x2
r1/r2=(M2/M1)^ - v1/v2=(T1/T2)^ - E1/E2=T1/T2

10. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
Ppt will NOT form (unsaturated)
CO (poisonous)
ClO?

11. What complex ion does ammonia form with silver? copper? cadmium? zinc?
proton donor base
benzene is less reactive than alkenes
acid + alcohol
[Ag(NH3)2]? - [Cu(NH3)4]? - [Cd(NH3)4]? - [Zn(NH3)4]?

12. What do group I/II metal oxides plus water form?
A salt solution.
Big K=kf/kr
bases
fractional distillation

13. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
do not change
H3PO4
boiling without losing volatile solvents/reactants

14. What is the general formula of an alkane?
Big K=kf/kr
same KE - but PEice<PEwater
CnH(2n+2)
CnH2n+1 often designated 'R' ex C3H7 is propyl

15. Where are group I metals stored?
A salt solution.
Molecules with the same molecular formulas - but different structural formulas
Group I metals (soft metals) are stored under oil
Q=It (time in seconds)

16. acetates
Conjugate pair (one must be a weak base or acid)
The Faraday or Faraday's constant.
Soluble
+4-covalent - +2-ionic

17. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
NH4?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
benzene is less reactive than alkenes
Current - time and charge on ion (moles of e used in half cell reaction)

18. For a dibasic acid (H2A) - [A?]= ____ ?
Heat a test tube at an angle at the side of the tube (not bottom)
K2
Salt + water
Eudiometer

19. What two compounds are great oxidizing agents?
Group 1 hydroxides (ex: NaOH)
Soluble except Ag - Pb - Ca - Sr Ba)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
S crystal at 0K=0

20. chlorate
C2O4?
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)
ClO3?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

21. chlorite
an oxidized and reduced substance
Sigma bonds are stronger than pi bonds
ClO2?
Glowing splint (positive result=relights)

22. What is the conjugate acid of H2PO4?
?G= -ve - E= +ve
Anode - oxygen. Cathode - hydrogen
Products - reactants (except for BDE when it's reactants - products)
H3PO4

23. mercury (II) ion
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Most are soluble except Ag - Pb
Hg?
zero-th: decreases - first: constant - second: increases

24. What is the general formula for an amine?
blue
acids
RNH2
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

25. What are isomers?
benzene has a delocalized pi ring structure
ClO2?
Molecules with the same molecular formulas - but different structural formulas
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

26. What do metal oxides plus acids form?
Salt + water
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)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Big K=kf/kr

27. What is the formula of butane?
C4H10
Transition element compounds (except if it has a full or empty d shell)
Acidic solutions (Ex: [Fe(H2O)6]? + H2O = Fe(H2O)5OH]? + H3O?)
Ionic compounds

28. silver iodide
Pale yellow
No - it depends on the number of ions produced on dissolving.
Insoluble except for nitrate and acetate
The compound with the lowest Ksp value.

29. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
HClO4
They stay the same.
Pour liquids using a funnel or down a glass rod

30. What are the products of the reaction between group 1 metals and water?
Orange
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Ppt will NOT form (unsaturated)

31. How can metals like iron and zinc be reduced?
Increases.
chemically (ex: with carbon)
O2 needs 4F/mol H2 needs 2F/mol
Distillation

32. Esters smell like _______ and amines smell like _______ and are ______.
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
fruit - fish - bases
Heptane
Pale purple - (orange)-yellow - red - blue - green.

33. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
R=8.31 J/mol/K
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Glowing splint (positive result=relights)

34. How does group 1 metals' density compare to water's?
r1/r2=(M2/M1)^ - v1/v2=(T1/T2)^ - E1/E2=T1/T2
are less dense than water
proton donor base
K2

35. What do nonmetal oxides plus water form?
strong acids/bases are written as H+ or OH- ions
acids
Greenish-yellow gas
Kc=Kp

36. What do you do to get rid of most of the solution from a precipitate?
Pale purple - (orange)-yellow - red - blue - green.
Decant
benzene has a delocalized pi ring structure
Heptane

37. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Anode
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Acids; HCOOCH3 is an ester
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

38. What part of a liquid do you look at to measure its volume?
The one with most oxygen atoms (highest oxidation number)
Read the bottom of the meniscus
H2O + CO2 (it decomposes readily)
methyl formate

39. perchlorate
ClO4?
O2 needs 4F/mol H2 needs 2F/mol
Add acid to water so that the acid doesn't boil and spit
Most INsoluble except group 1 and ammonium

40. What is the general formula for an acid?
a-IMFs - b-molecular volume
RCOOH
Separating funnel
Identity and purity (impure compounds usually have broad & low melting points)

41. What is the test for oxygen?
CnH2n-2
fractional distillation
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Glowing splint (positive result=relights)

42. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
RCHO (carbonyl at end)
A) any range. b) 8-10 c) 4-6
r1/r2=(M2/M1)^ - v1/v2=(T1/T2)^ - E1/E2=T1/T2

43. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s
Soluble
Purple
How grouped results are

44. Name six characteristics of transition elements (or their compounds)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
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
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)
red - green - blue

45. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
They stay the same.
Mn? - Cr? - Cr
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)

46. What things should you remember to do when collecting gas over water?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
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.
Conjugate pair (one must be a weak base or acid)
allow for the vapor pressure of water and make sure to level levels

47. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
Unsaturated - addition (ex: decolorize bromine solution)
Separating funnel
An active metal.

48. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
Soluble except Ag - Pb - Ca - Sr Ba)
RCOR
How close results are to the accepted value

49. Neutralization is an ________ reaction.
Selective absorption
Exothermic (?H for ANY sa/sb = -57kJ/mol)
The dilution effect when the solutions mix. M1V1 = M2V2
Pipette (burette if need repetition)

50. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
Conjugate pair (one must be a weak base or acid)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
allow for the vapor pressure of water and make sure to level levels
A) any range. b) 8-10 c) 4-6

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AP Chemistry 2

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