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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. hydroxide
OH?
White precipitate
Soluble
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

2. How does the melting point of a mixture compare to the MP of a pure substance?

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3. What are the prefixes for the naming of binary molecular compound formulas (up to six)
-Ea/R
Mono; di; tri; tetra; penta; hexa.
a-IMFs - b-molecular volume
Sulfur

4. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
'non-active' metals such as Cu - Ag - Au - Pt - etc.
same KE - but PEice<PEwater
RCOR

5. What is the formula for percent yield?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Experimental mass/theoretical mass X 100
CnH(2n+2)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

6. What apparatus do you use to separate 2 immiscible liquids?
bent
Evaporation
Experimental mass/theoretical mass X 100
Separating funnel

7. How are strong ones written?
Pale yellow
strong acids/bases are written as H+ or OH- ions
Soluble
Soluble

8. What is the formula of butane?
C4H10
CnH2n+1 often designated 'R' ex C3H7 is propyl
bent
All except for lithium

9. Give an example of a concentrated weak acid.
allow for the vapor pressure of water and make sure to level levels
same KE - but PEice<PEwater
voltaic: + electrolytic: -
Glacial acetic acid

10. bromine
Acidified
At half equivalence - pH=pKa
brown volatile liquid
The Faraday or Faraday's constant.

11. What are two substances that sublime at 1 atm when heated?
bent
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
acids
Iodine and CO2 (dry ice)

12. What do nonmetal oxides plus water form?
Ionic compounds
acids
NO3?
?H formation of an element in standard state=0

13. Nonmetals are good _____ agents. Metals are good _______ agents.
methyl formate
Ksp = 27s4
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

14. What changes Keq?
proton donor base
#ligands=charge x2
K1 x K2
Only temperature

15. What process do you use to obtain the precipitate from a solution?
Filtration
RCOOR
Trigonal pyramidal
Decant

16. What is the slope of the graph of lnk vs. 1/T?
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?)
Ksp = 27s4
-Ea/R
Insoluble except for nitrate and acetate

17. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
benzene has a delocalized pi ring structure
Distillation
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Cu3(PO4)2

18. What do metal oxides plus acids form?
Acid rain - dissolves marble buildings/statues and kills trees.
HClO4
Salt + water
MnO4?

19. How do you clean a buret/pipette for a titration?
Insoluble except for nitrate and acetate
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
ClO4?
Pipette (burette if need repetition)

20. What do you use to look at burning magnesium? why?
But S° of element is not zero (except at 0K)
blue glass - it filters UV
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Soluble

21. Both Acetic acid and ____________ are also functional isomers.
[A?]/[HA] x 100 or [BH?]/[B] x 100
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
methyl formate
The benzene ring (or more correctly the phenyl group - C6H5)

22. lead compounds
Insoluble except nitrate and acetate
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Identity and purity (impure compounds usually have broad & low melting points)
?H formation of an element in standard state=0

23. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
K1 x K2
CO3²?
Soluble except Ag - Pb - Ca - Sr Ba)

24. phosphate
no - they're written undissociated (HAaq)
ClO4?
Concentration
PO4³?

25. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
A) any range. b) 8-10 c) 4-6
Heat a test tube at an angle at the side of the tube (not bottom)
same KE - but PEice<PEwater

26. What process do you use to obtain the solute from a solution?
10?8
no - they're written undissociated (HAaq)
ion pairing
Evaporation

27. What device would you use to measure a volume of gas?
Eudiometer
fractional distillation
Acid rain - dissolves marble buildings/statues and kills trees.
?H-kJ - ?S-J - ?G-kJ

28. bromothymol
Evaporation
NO3?
blue (BTB)
CO (poisonous)

29. lead iodide
0.10M HCl (more ions)
bright yellow
CnH2n
Soluble

30. Ions are not ______.
Concentration
Mn²? - Cr³? - Cr³
atoms
Iodine and CO2 (dry ice)

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

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32. What shape is water?
bent
Unsaturated - addition (ex: decolorize bromine solution)
CrO4²?
Trigonal pyramidal

33. Name some properties of Group 17
-Ea/R
RCOR
?G=negative - E° must be positive
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

34. Metal hydrides are _____ and form _______ and _______ when added to water
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
0.10M HCl (more ions)
ionic and form hydrogen and hydroxide
ClO2?

35. What element is used to vulcanize rubber?
Sulfur
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Molecules with the same molecular formulas - but different structural formulas
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

36. What do metal oxides plus non- metal oxides form?
ion pairing
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Salts (ex: CaO + SO2 ? CaSO3)
Only temperature

37. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
zero-th: decreases - first: constant - second: increases
0 and 14
?H-kJ - ?S-J - ?G-kJ

38. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
MnO4?
Mn²? - Cr³? - Cr³
Q=It (time in seconds)

39. carbonates
Anode
0.10M HCl (more ions)
water and substances with (s) less dense than
Insoluble except group 1 and ammonium

40. If ?S is positive - are the products more or less chaotic than the reactants?
Glowing splint (positive result=relights)
PO4³?
allow for the vapor pressure of water and make sure to level levels
More chaotic (ex: gases made)

41. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
a-IMFs - b-molecular volume
Cr2O7²?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

42. What is the formula for summation?

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43. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
RCOOH
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Salt and water

44. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Acids; HCOOCH3 is an ester
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

45. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
chemically (ex: with carbon)
blue
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
[A?]/[HA] x 100 or [BH?]/[B] x 100

46. permanganate
zero-th: decreases - first: constant - second: increases
Concentration
MnO4?
lighted splint (positive result=pop)

47. halides
Most are soluble except Ag - Pb
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
proton donor base
Insoluble except group 1 and ammonium

48. What is the formula of copper (II) phosphate?
Group I metals (soft metals) are stored under oil
blue (BTB)
Cu3(PO4)2
zero-th: decreases - first: constant - second: increases

49. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Only temperature
ethers
Salt and water
neutralization: high K - H2O product dissociation: low K - H2O reactant

50. What is the general formula for alkyl halides?
RX
White precipitate
ethers
A salt solution.