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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 general formula for an amine?
Separating funnel
proton acceptor.
RNH2
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.

2. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Acids; HCOOCH3 is an ester
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
CN?
Soluble

3. What is the general formula for an acid?
RCOOH
Current - time and charge on ion (moles of e used in half cell reaction)
But S° of element is not zero (except at 0K)
Ionic compounds

4. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
brown volatile liquid
0.10M HCl (more ions)

5. halides
0.10M HCl (more ions)
Most are soluble except Ag - Pb
Insoluble except group 1 and ammonium
#ligands=charge x2

6. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Ksp = 108s5
CnH2n-2
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

7. What does the solubility of organic compounds depend on?
K2
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
bright yellow
More chaotic (ex: gases made)

8. How are primary alcohols turned into acids?
At half equivalence - pH=pKa
Most INsoluble except group 1 and ammonium
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
lighted splint (positive result=pop)

9. How many faradays of electric charge do you need to produce one mole of O2? H2?
White precipitate
Insoluble except group 1 and ammonium
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)
O2 needs 4F/mol H2 needs 2F/mol

10. thiosulfate
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
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
S2O3²?
Anode

11. What process do you use to separate two liquids with different boiling points?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Transition element compounds (except if it has a full or empty d shell)
O2 needs 4F/mol H2 needs 2F/mol
fractional distillation

12. What is the formula for percent error?
Trigonal pyramidal
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
|experimental - accepted|/accepted X 100
small size and high charge

13. What is the name of S2Cl2? (Know how to name others like this - too)
Insoluble except group 1 and ammonium
methyl formate
Soluble except Ag - Pb - Ca - Sr Ba)
Disulfur dichloride

14. When a cell is 'flat' What is its voltage?
bases
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
zero
Reduction always takes place at the cathode (RED CAT) In both types of cell!

15. What things should you remember to do when collecting gas over water?
Identity and purity (impure compounds usually have broad & low melting points)
allow for the vapor pressure of water and make sure to level levels
Pale yellow
Sulfur

16. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
S2O3²?
Purple
C4H10
Reduction always takes place at the cathode (RED CAT) In both types of cell!

17. At what point during titration do you have the perfect buffer - and what is the pH at this point?
metal oxides and hydrides are ionically bonded and basic
At half equivalence - pH=pKa
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Saturated - Substitution (which requires more radical conditions)

18. What is the test for oxygen?
0 and 14
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Glowing splint (positive result=relights)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

19. What is the word equation for condensation polymerisation ?
Graduated cylinder
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.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Monomer + monomer = polymer product + a simple molecule such as water or HCl

20. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
Suniverse increases for spontaneous processes
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
atoms

21. oxalate
C2O4²?
a-IMFs - b-molecular volume
Unsaturated - addition (ex: decolorize bromine solution)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

22. Name C7H16
same KE - but PEice<PEwater
Initiation energy (NOT Ea)
No - it depends on the number of ions produced on dissolving.
Heptane

23. Color is due to ______ _______ of light.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
OH- and NH3
Selective absorption
T increases exponentially the proportion of molecules with E > Ea

24. One mole of electrons carries 96500Coulombs - what is this quantity called?

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25. What is the formula of copper (II) phosphate?
R=8.31 J/mol/K
voltaic: + electrolytic: -
Cu3(PO4)2
Read the bottom of the meniscus

26. mercury (II) ion
Hg²?
bases
Big K=kf/kr
The one with most oxygen atoms (highest oxidation number)

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

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28. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Q=It (time in seconds)
Ksp = 4s³
neutralization: high K - H2O product dissociation: low K - H2O reactant
do not change

29. When is ?G zero?
It ceases - the circuit is broken.
Distillation
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
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

30. What electrons are lost/gained first in transition element ions?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
ns² electrons (first in-first out)
CnH2n+2
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

31. Alkanes are _________ and react by _________
Saturated - Substitution (which requires more radical conditions)
RCOOR
H+
H3PO4

32. lead compounds
Insoluble except nitrate and acetate
Most are soluble except Ag - Pb
Only temperature
Products - reactants (except for BDE when it's reactants - products)

33. What are two allotropes of carbon?
CnH2n-2
diamond and graphite
Acids; HCOOCH3 is an ester
Glacial acetic acid

34. What device would you use to measure a volume of gas?
Soluble
it's lower and occurs over less sharp a range
Eudiometer
are less dense than water

35. What type of solutions do small - highly charged cations tend to form?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
An active metal.
White precipitate

36. Give an example of a dilute strong acid.
fruit - fish - bases
blue
HClO4
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

37. What equipment do you need for a titration?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Greenish-yellow gas
ROH

38. bromothymol
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
redox reaction
blue (BTB)
Cr2O7²?

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

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40. 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.
CnH2n
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Distillation

41. lead iodide
blue (BTB)
Unsaturated - addition (ex: decolorize bromine solution)
bright yellow
OH- and NH3

42. Give an example of a concentrated weak acid.
zero-th: decreases - first: constant - second: increases
different forms of the same element
Glacial acetic acid
Q=It (time in seconds)

43. What causes the dramatic effect of T on rate?
proton acceptor.
ion pairing
T increases exponentially the proportion of molecules with E > Ea
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

44. What is the general formula for an alcohol?
ROH
Hg²?
CnH(2n+2)
zero-th: decreases - first: constant - second: increases

45. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
ClO2?
Sulfur

46. What are amphoteric oxides?
Soluble
Current - time and charge on ion (moles of e used in half cell reaction)
fractional distillation
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?)

47. What are the formulas for q?
OH- and NH3
Most are soluble except Ag - Pb
q=mc?T q=mL (or n x ?h)
Tetrahedral

48. What two types of substances are present in all redox reactions?
ROR
?G= -ve - E°= +ve
Sulfur
an oxidized and reduced substance

49. group 1 ions/compounds
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Soluble
OH- and NH3
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

50. What process do you use to obtain the precipitate from a solution?
?H-kJ - ?S-J - ?G-kJ
Orange
Pipette (burette if need repetition)
Filtration