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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. Give an example of a dilute strong acid.
All except for lithium
HClO4
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Soluble

2. nitrates
Iodine and CO2 (dry ice)
Soluble
Salt + water.
Anode

3. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Pale purple - (orange)-yellow - red - blue - green.
zero
a-IMFs - b-molecular volume
CnH(2n+2)

4. How are more active metals reduced?
by electrolysis
zero
Evaporation
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

5. How does group 1 metals' density compare to water's?
?G= -ve - E°= +ve
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
are less dense than water
left - ppt will form

6. Which would cause the bulb in a conductivity apparatus to be brightest?
10?8
0.10M HCl (more ions)
RCOOR
Conjugate pair (one must be a weak base or acid)

7. barium sulfate
S2O3²?
RCOOH
Glowing splint (positive result=relights)
White precipitate

8. What process do you use to obtain a solvent from a solution?
Distillation
RCOR
small size and high charge
hydroxides (ex: Ba(OH)2)

9. chromate ion (soln + most solids)
CnH2n+2
RCOR
ClO?
yellow

10. What do you do to get rid of most of the solution from a precipitate?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
a-IMFs - b-molecular volume
Decant
CO2 and H2O

11. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Big K=kf/kr
CnH2n+1 often designated 'R' ex C3H7 is propyl

12. What is reflux?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
boiling without losing volatile solvents/reactants
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
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

13. What do nonmetal oxides plus water form?
acids
boiling without losing volatile solvents/reactants
Pale purple - (orange)-yellow - red - blue - green.
bright yellow

14. thiosulfate
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Tetrahedral
Big K=kf/kr
S2O3²?

15. What are amphoteric oxides?
Ksp = s²
Add acid to water so that the acid doesn't boil and spit
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?)
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)

16. What is H2CO3 (carbonate acid) usually written as?
voltaic: + electrolytic: -
Ksp = 108s5
H2O + CO2 (it decomposes readily)
boiling without losing volatile solvents/reactants

17. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
C2O4²?
Conjugate pair (one must be a weak base or acid)
No - it depends on the number of ions produced on dissolving.

18. What is the general formula for an alcohol?
Soluble except Ag - Pb - Ca - Sr Ba)
ROH
Clear
They decrease (or could be the same if the solid has ONLY JUST disappeared)

19. What is the general formula for an ester?
RCOOR
acid + alcohol
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

20. A Bronsted-Lowry acid is...
proton donor base
10?8
fruit - fish - bases
Exothermic

21. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
Sigma bonds are stronger than pi bonds
Ions go through the salt bridge - electrons go through metal wires in the external circuit
metal oxides and hydrides are ionically bonded and basic

22. Are weak acids (and bases) written dissociated?

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23. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
More chaotic (ex: gases made)
+4-covalent - +2-ionic

24. What is the formula for alkanes?
ethers
atoms
CnH2n+2
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

25. ammonium/ammonium compounds
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
NH2?
Soluble
neutralization: high K - H2O product dissociation: low K - H2O reactant

26. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
Selective absorption
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Products - reactants (except for BDE when it's reactants - products)

27. What do acids plus active metals form?
fractional distillation
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Ppt will NOT form (unsaturated)

28. Esters smell like _______ and amines smell like _______ and are ______.
RCOR
Soluble except Ag - Pb - Ca - Sr Ba)
fruit - fish - bases
ClO2?

29. What are two allotropes of carbon?
blue glass - it filters UV
diamond and graphite
Unsaturated - addition (ex: decolorize bromine solution)
ClO3?

30. During a titration what is present in the beaker at the equivalence point?
NH4?
ClO2?
A salt solution.
Iodine and CO2 (dry ice)

31. If a free element is involved - what type of reaction must be involved?
redox reaction
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Evaporation
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

32. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
ClO3?
Anode - oxygen. Cathode - hydrogen
An active metal.

33. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
no - they're written undissociated (HAaq)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
zero

34. How does half life change for zero-th order - first order - and second order processes?
left - ppt will form
Ions go through the salt bridge - electrons go through metal wires in the external circuit
zero-th: decreases - first: constant - second: increases
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

35. Generally - which oxy acid is strongest?
benzene is less reactive than alkenes
The one with most oxygen atoms (highest oxidation number)
zero
small size and high charge

36. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
H2PO4?
voltaic: - electrolytic: +
Reduction always takes place at the cathode (RED CAT) In both types of cell!

37. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
blue glass - it filters UV
Increases.

38. What is the slope of the graph of lnk vs. 1/T?
left - ppt will form
Separating funnel
-Ea/R
hydroxides (ex: Ba(OH)2)

39. What is the sign of the cathode in voltaic cells? in electrolytic cells?
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)
RCHO (carbonyl at end)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
voltaic: + electrolytic: -

40. How do you heat a test tube?
White precipitate
Heat a test tube at an angle at the side of the tube (not bottom)
basic
The compound with the lowest Ksp value.

41. Both Acetic acid and ____________ are also functional isomers.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
methyl formate
Experimental mass/theoretical mass X 100
benzene has a delocalized pi ring structure

42. Metal hydrides are _____ and form _______ and _______ when added to water
?G= -ve - E°= +ve
Distillation
ionic and form hydrogen and hydroxide
Both electrons come from the same atom (just as good as a regular bond)

43. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Orange
Synthesis - separation and purification of the product and its identification.
blue

44. What is the charge on a chlorine atom?
Ksp = s²
zero
CnH2n+2
are less dense than water

45. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
Increases down group 1 decreases down group 17
Silvery gray solid - brown - purple
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

46. What is the formula for summation?

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47. What are the formulas for q?
bright yellow
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
q=mc?T q=mL (or n x ?h)

48. What is an Alkyl group?

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49. The definition of acidic basic and neutral aqueous solutions is:
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
|experimental - accepted|/accepted X 100
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

50. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
fractional distillation
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.