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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. dichromate (soln + most solids)
Orange
Ionic compounds
H+
do not change

2. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
K2
?H-kJ - ?S-J - ?G-kJ
+4-covalent - +2-ionic

3. What do the 'a' and 'b' in Van Der Waal's equation allow for?
different forms of the same element
Disulfur dichloride
a-IMFs - b-molecular volume
C4H10

4. What word is a clue for a redox reaction?
ionic and form hydrogen and hydroxide
ethers
Acidified
Products - reactants (except for BDE when it's reactants - products)

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

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6. What is the second law of thermodynamics?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Ksp = s²
+4-covalent - +2-ionic
Suniverse increases for spontaneous processes

7. sulfates
catalyst=conc H2SO4
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
CnH2n+2
Soluble except Ag - Pb - Ca - Sr Ba)

8. Color (absorbance) is proportional to ________
blue
CH3COO?
Anode - oxygen. Cathode - hydrogen
Concentration

9. What do metal oxides plus non- metal oxides form?
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.
CN?
Salts (ex: CaO + SO2 ? CaSO3)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

10. What do you need to make a polymer?
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)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Evaporation
Soluble

11. What are the products of the reaction between group 1 metals and water?

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12. What are allotropes?
different forms of the same element
CnH(2n+2)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
bent

13. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Greenish-yellow gas
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
yellow
Decant

14. primary colors
Soluble
Group 1 hydroxides (ex: NaOH)
red - green - blue
ClO4?

15. Both Acetic acid and ____________ are also functional isomers.
?G= -ve - E°= +ve
by electrolysis
methyl formate
CnH2n-2

16. How are metal oxides and hydrides bonded? are they acidic or basic?
voltaic: + electrolytic: -
More chaotic (ex: gases made)
bases
metal oxides and hydrides are ionically bonded and basic

17. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
Salts (ex: CaO + SO2 ? CaSO3)
Kc=Kp
Acidified
The compound with the lowest Ksp value.

18. What does the solubility of organic compounds depend on?
benzene has a delocalized pi ring structure
K2
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Tetrahedral

19. group 1 ions/compounds
Soluble
Clear
Decant
T increases exponentially the proportion of molecules with E > Ea

20. What is the slope of the graph of lnk vs. 1/T?
Q=It (time in seconds)
Eudiometer
-Ea/R
by electrolysis

21. silver iodide
K2
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
ethers
Pale yellow

22. 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
Soluble
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Heptane

23. What is the formula for percent error?
Acid rain - dissolves marble buildings/statues and kills trees.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
|experimental - accepted|/accepted X 100
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

24. Does Benzene react by addition or substitution?
Insoluble
it reacts by substitution NOT addition
Decant
CO3²?

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

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26. How do you get the equation for a net electrolysis reaction?
?G=negative - E° must be positive
Combine the equations for the half reactions in the non-spontaneous direction
a-IMFs - b-molecular volume
bases

27. What kind of bonding structure does benzene have?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
How close results are to the accepted value
benzene has a delocalized pi ring structure

28. The oxidation # for acid base reactions...
a-IMFs - b-molecular volume
RNH2
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
do not change

29. ________ are Lewis bases - because they can donate a lone pair of electrons.
OH- and NH3
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)
CH3COO?
Acidified

30. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
[A?]/[HA] x 100 or [BH?]/[B] x 100
H2O + CO2 (it decomposes readily)
Insoluble except nitrate and acetate
do not change

31. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
ROH
voltaic: + electrolytic: -
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

32. lead iodide
bright yellow
Most INsoluble except group 1 and ammonium
S2O3²?
Perform ICE BOX calculation based on K1

33. What is the general formula for an ether?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
boiling without losing volatile solvents/reactants
ROR
?H-kJ - ?S-J - ?G-kJ

34. Which alkali metals float on water?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
All except for lithium
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

35. chromate ion (soln + most solids)
Selective absorption
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
yellow
catalyst=conc H2SO4

36. What shape is water?
?G=negative - E° must be positive
bent
+4-covalent - +2-ionic
Insoluble except group 1 and ammonium

37. Acid plus base make?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Salt + water.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
q=mc?T q=mL (or n x ?h)

38. What do group I/II metal oxides plus water form?
bases
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
by electrolysis

39. chlorine
blue glass - it filters UV
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.
Greenish-yellow gas
RNH2

40. Can you collect soluble gases over water?
Ksp = 27s4
E=q + w (negative is by system - positive is on system)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
No - NH3 and HCl gases are extremely soluble

41. What are two substances that sublime at 1 atm when heated?
Decant
Suniverse increases for spontaneous processes
diamond and graphite
Iodine and CO2 (dry ice)

42. What is a coordinate covalent bond?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Both electrons come from the same atom (just as good as a regular bond)
Cu3(PO4)2
Glowing splint (positive result=relights)

43. What two types of substances are present in all redox reactions?
The benzene ring (or more correctly the phenyl group - C6H5)
Glowing splint (positive result=relights)
CnH2n+2
an oxidized and reduced substance

44. What type of metals don't react with water or acids to form H2?

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45. What is the conjugate acid of H2PO4?
Glacial acetic acid
H3PO4
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Ksp = 108s5

46. bromine
How close results are to the accepted value
Disulfur dichloride
chemically (ex: with carbon)
brown volatile liquid

47. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
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
CnH2n+1 often designated 'R' ex C3H7 is propyl
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

48. How are more active metals reduced?
RCOOH
Soluble
by electrolysis
Acidified

49. ammonium/ammonium compounds
Soluble
0 and 14
by electrolysis
allow for the vapor pressure of water and make sure to level levels

50. Which of the rates changes more when temperature is increased?
blue glass - it filters UV
More chaotic (ex: gases made)
OH- and NH3
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)