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

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2. cyanide
CN?
brown volatile liquid
water and substances with (s) less dense than
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

3. What shape is carbon dioxide?
H+
different forms of the same element
linear
H3PO4

4. Is the standard entropy (S°) of an element zero?
CO2 and H2O
But S° of element is not zero (except at 0K)
Orange
zero

5. Alkenes are ________ and react by __________
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Anode
Unsaturated - addition (ex: decolorize bromine solution)
Initiation energy (NOT Ea)

6. What device would you use to measure a volume of gas?
Iodine and CO2 (dry ice)
Eudiometer
ionic and form hydrogen and hydroxide
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

7. Colorless doesn't mean ______
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Disulfur dichloride
proton donor base
Clear

8. What is the general formula of an alkane?
CO2 and H2O
Disulfur dichloride
Group I metals (soft metals) are stored under oil
CnH(2n+2)

9. Acid plus base make?
The Faraday or Faraday's constant.
Salt + water.
Iodine and CO2 (dry ice)
a-IMFs - b-molecular volume

10. What is the formula for alkynes?
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.
Iodine and CO2 (dry ice)
CnH2n-2
bent

11. Name some properties of Group 17
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
a-IMFs - b-molecular volume
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
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)

12. When the salt bridge is removed what happens to the cell reaction?
CN?
Salt + water.
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
It ceases - the circuit is broken.

13. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
ethers
NO3?
0 and 14

14. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Insoluble except nitrate and acetate
a-IMFs - b-molecular volume
CrO4²?
Ksp = 4s³

15. What are the common strong bases?
Molecules with the same molecular formulas - but different structural formulas
T increases exponentially the proportion of molecules with E > Ea
Group 1 hydroxides (ex: NaOH)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

16. Esterification is...
yellow
Soluble
Check for air bubbles in the buret and remove the buret funnel from the buret
acid + alcohol

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

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18. What word is a clue for a redox reaction?
RCOOH
Insoluble except for nitrate and acetate
Soluble
Acidified

19. What type of compounds are almost always colored?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
blue glass - it filters UV
Transition element compounds (except if it has a full or empty d shell)
H2O + CO2 (it decomposes readily)

20. What do hydrocarbons form when they burn in air (oxygen)?
All except for lithium
Clear
CO2 and H2O
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

21. Does reactivity increase/decrease going down group 1 and group 17?
Disulfur dichloride
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Increases down group 1 decreases down group 17
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

22. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
Pipette (burette if need repetition)
Salts (ex: CaO + SO2 ? CaSO3)
Soluble except Ag - Pb - Ca - Sr Ba)

23. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
CN?
Graduated cylinder

24. What do you use to look at burning magnesium? why?
blue glass - it filters UV
Evaporation
it is lower and occurs over less sharp a range
acid + alcohol

25. 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.
CnH2n-2
diamond and graphite
A) any range. b) 8-10 c) 4-6
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

26. chlorine
Greenish-yellow gas
?G=negative - E° must be positive
Filtration
All except for lithium

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

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28. What does saturated mean? Unsaturated?
CnH(2n+2)
Exothermic
Cr2O7²?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

29. What do ions and electrons travel through in a voltaic/electrolytic cell?
Synthetic condensation polymer (aka a polyamide)
acids
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Ions go through the salt bridge - electrons go through metal wires in the external circuit

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

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31. What is accuracy?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Orange
How close results are to the accepted value
acid + alcohol

32. How do you get Ecell for spontaneous reactions?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
bases
metal oxides and hydrides are ionically bonded and basic
CN?

33. What kind of bonding structure does benzene have?
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?)
benzene has a delocalized pi ring structure
CnH2n+2
OH- and NH3

34. When is ?G zero?
diamond and graphite
small size and high charge
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
bases

35. Give an example of a dilute strong acid.
SO4²?
HClO4
allow for the vapor pressure of water and make sure to level levels
Acids; HCOOCH3 is an ester

36. What is the general formula for an amine?
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
RNH2
Selective absorption
S crystal at 0K=0

37. chromate
red - green - blue
Monomer + monomer = polymer product + a simple molecule such as water or HCl
CrO4²?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

38. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
boiling without losing volatile solvents/reactants
ROH
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

39. acetates
Selective absorption
PO4³?
Insoluble except nitrate and acetate
Soluble

40. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
Cu3(PO4)2
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
?G= -ve - E°= +ve

41. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
MnO4?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

42. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
acids
Soluble
CO2 and H2O

43. bromothymol
-Ea/R
blue (BTB)
The benzene ring (or more correctly the phenyl group - C6H5)
Insoluble

44. halides
Most are soluble except Ag - Pb
metal oxides and hydrides are ionically bonded and basic
NH2?
ns² electrons (first in-first out)

45. What is the difference between equivalence point and end point of a titration.
it is lower and occurs over less sharp a range
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
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

46. What type of polymer is nylon?
benzene has a delocalized pi ring structure
Most are soluble except Ag - Pb
Ksp = s²
Synthetic condensation polymer (aka a polyamide)

47. How do you clean a buret/pipette for a titration?
bright yellow
T increases exponentially the proportion of molecules with E > Ea
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
benzene has a delocalized pi ring structure

48. Nonmetals are good _____ agents. Metals are good _______ agents.
red - green - blue
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?)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

49. nitrates
?G= -ve - E°= +ve
Transition element compounds (except if it has a full or empty d shell)
Soluble
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

50. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
Sulfur
by electrolysis
More chaotic (ex: gases made)