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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 word equation for addition polymerisation?
T increases exponentially the proportion of molecules with E > Ea
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
CnH2n+1 often designated 'R' ex C3H7 is propyl
Pale purple - (orange)-yellow - red - blue - green.

2. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
H3PO4
Soluble
Group I metals (soft metals) are stored under oil
neutralization: high K - H2O product dissociation: low K - H2O reactant

3. What process do you use to obtain a solvent from a solution?
?G=negative - E° must be positive
left - ppt will form
S2O3²?
Distillation

4. What is the first law of thermodynamics?
left - ppt will form
'non-active' metals such as Cu - Ag - Au - Pt - etc.
E=q + w (negative is by system - positive is on system)
O2 needs 4F/mol H2 needs 2F/mol

5. What is the third law of thermodynamics?
blue glass - it filters UV
Iodine and CO2 (dry ice)
S crystal at 0K=0
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

6. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
it reacts by substitution NOT addition
CH3COO?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
They stay the same.

7. When is ?G zero?
CO2 and H2O
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Both electrons come from the same atom (just as good as a regular bond)

8. The oxidation # for acid base reactions...
Clear
?H-kJ - ?S-J - ?G-kJ
do not change
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

9. What is the name of S2Cl2? (Know how to name others like this - too)
Initiation energy (NOT Ea)
Glacial acetic acid
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Disulfur dichloride

10. What is the charge on a chlorine atom?
E=q + w (negative is by system - positive is on system)
zero
red - green - blue
Insoluble except nitrate and acetate

11. What steps do organic labs consist of?
Big K=kf/kr
Synthesis - separation and purification of the product and its identification.
Suniverse increases for spontaneous processes
OH?

12. What are allotropes?
different forms of the same element
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
acids
More chaotic (ex: gases made)

13. Name C7H16
Only temperature
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Heptane

14. sulfate
linear
SO4²?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
The one with most oxygen atoms (highest oxidation number)

15. A Bronsted-Lowry base is...
proton acceptor.
No - NH3 and HCl gases are extremely soluble
by electrolysis
Exothermic

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

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17. How do you dilute an acid?

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18. 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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19. Alcohols and _______ are FG isomers
At half equivalence - pH=pKa
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
ethers
Nothing

20. mercury (II) ion
0 and 14
Hg²?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

21. If a weak acid is diluted more - what happens to its % dissociation value?
10?8
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Increases.
metal oxides and hydrides are ionically bonded and basic

22. Alkenes are ________ and react by __________
Filtration
chemically (ex: with carbon)
Unsaturated - addition (ex: decolorize bromine solution)
Eudiometer

23. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
RCOOR
ROH
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?)

24. What is an Alkyl group?

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25. Ions are not ______.
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 = 4s³
catalyst=conc H2SO4
atoms

26. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
More chaotic (ex: gases made)
Most INsoluble except group 1 and ammonium
q=mc?T q=mL (or n x ?h)

27. Ca - Sr - Ba
CnH2n-2
Anode - oxygen. Cathode - hydrogen
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
hydroxides (ex: Ba(OH)2)

28. Acid plus base make?
Salt + water.
blue (BTB)
Separating funnel
allow for the vapor pressure of water and make sure to level levels

29. Give an example of a concentrated weak acid.
Glacial acetic acid
Nothing
Group 1 hydroxides (ex: NaOH)
ClO3?

30. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
S2O3²?
|experimental - accepted|/accepted X 100
PO4³?

31. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Pale purple - (orange)-yellow - red - blue - green.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Read the bottom of the meniscus

32. What do group I/II metal oxides and acids form?
Exothermic
Salt and water
are less dense than water
Hg2²?

33. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
redox reaction
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
The dilution effect when the solutions mix. M1V1 = M2V2

34. How can metals like iron and zinc be reduced?
R=8.31 J/mol/K
chemically (ex: with carbon)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
?H-kJ - ?S-J - ?G-kJ

35. What is the general formula for an alcohol?
Insoluble except for nitrate and acetate
ROR
ROH
The benzene ring (or more correctly the phenyl group - C6H5)

36. What do you use to look at burning magnesium? why?
Initiation energy (NOT Ea)
Saturated - Substitution (which requires more radical conditions)
blue glass - it filters UV
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

37. What is the general formula for a ketone?
Ksp = 27s4
brown volatile liquid
Pipette (burette if need repetition)
RCOR

38. Where are group I metals stored?
fractional distillation
Increases.
Ksp = 108s5
Group I metals (soft metals) are stored under oil

39. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
ClO?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

40. How do you find the pH for a dibasic acid? (H2A)?
P2O5
A salt solution.
Perform ICE BOX calculation based on K1
allow for the vapor pressure of water and make sure to level levels

41. Do you use J or kJ for ?H - ?S - and ?G?
NO3?
?H-kJ - ?S-J - ?G-kJ
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
T increases exponentially the proportion of molecules with E > Ea

42. What is the formula of butane?
But S° of element is not zero (except at 0K)
Soluble
it's lower and occurs over less sharp a range
C4H10

43. silver iodide
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Pale yellow
No - it depends on the number of ions produced on dissolving.
Soluble except Ag - Pb - Ca - Sr Ba)

44. What is the general formula of an alkane?
They stay the same.
CnH(2n+2)
C2O4²?
The benzene ring (or more correctly the phenyl group - C6H5)

45. What two types of substances are present in all redox reactions?
Only temperature
an oxidized and reduced substance
ionic and form hydrogen and hydroxide
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

46. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
Soluble except Ag - Pb - Ca - Sr Ba)
Iodine and CO2 (dry ice)
Group I metals (soft metals) are stored under oil

47. When combining half equations - what do you do to E° values when multiplying coefficients?
Nothing
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
ROH
0 and 14

48. Neutralization is an ________ reaction.
Experimental mass/theoretical mass X 100
Unsaturated - addition (ex: decolorize bromine solution)
ClO4?
Exothermic (?H for ANY sa/sb = -57kJ/mol)

49. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Exothermic
Sigma bonds are stronger than pi bonds
No - it depends on the number of ions produced on dissolving.

50. Why are i factors (Van't Hoff factors) often less than ideal?
Cu3(PO4)2
ion pairing
0 and 14
?H-kJ - ?S-J - ?G-kJ