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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.
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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 Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
Synthesis - separation and purification of the product and its identification.
boiling without losing volatile solvents/reactants
10?8

2. What type of compounds do metals/non metals form?
ethers
Iodine and CO2 (dry ice)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Ionic compounds

3. What things should you remember to do when collecting gas over water?
a-IMFs - b-molecular volume
RX
allow for the vapor pressure of water and make sure to level levels
it is lower and occurs over less sharp a range

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

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5. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
R=8.31 J/mol/K
Increases.
[A?]/[HA] x 100 or [BH?]/[B] x 100

6. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Hg²?
ns² electrons (first in-first out)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

7. Is the standard entropy (S°) of an element zero?
OH- and NH3
Soluble
water and substances with (s) less dense than
But S° of element is not zero (except at 0K)

8. Name six characteristics of transition elements (or their compounds)
CH3COO?
Greenish-yellow gas
Anode
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)

9. chromate
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Most are soluble except Ag - Pb
diamond and graphite
CrO4²?

10. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Concentration
Add acid to water so that the acid doesn't boil and spit
H+

11. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
SO4²?
linear
CO (poisonous)
Insoluble (except group 1 ammonium and Ba)

12. What kind of bonding structure does benzene have?
Insoluble except for nitrate and acetate
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Mono; di; tri; tetra; penta; hexa.
benzene has a delocalized pi ring structure

13. What process do you use to separate two liquids with different boiling points?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
chemically (ex: with carbon)
C2O4²?
fractional distillation

14. What is the difference between equivalence point and end point of a titration.
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
Ksp = 4s³
No - NH3 and HCl gases are extremely soluble
T increases exponentially the proportion of molecules with E > Ea

15. copper sulfate
blue
Making sigma bonds and holding lone pairs
S crystal at 0K=0
blue (BTB)

16. What shape is water?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
bent
K1 x K2
Ksp = 27s4

17. oxalate
C2O4²?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Nothing
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

18. What do nonmetal oxides plus water form?
acids
Soluble
bent
SO4²?

19. What is a coordinate covalent bond?
ionic and form hydrogen and hydroxide
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Both electrons come from the same atom (just as good as a regular bond)
O2 needs 4F/mol H2 needs 2F/mol

20. Alcohols and _______ are FG isomers
ClO?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
ethers
+4-covalent - +2-ionic

21. perchlorate
Q=It (time in seconds)
ClO4?
Filtration
Evaporation

22. barium sulfate
Ksp = s²
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
White precipitate
The Faraday or Faraday's constant.

23. ________ are Lewis bases - because they can donate a lone pair of electrons.
Soluble except Ag - Pb - Ca - Sr Ba)
Conjugate pair (one must be a weak base or acid)
an oxidized and reduced substance
OH- and NH3

24. thiosulfate
The one with most oxygen atoms (highest oxidation number)
S2O3²?
Read the bottom of the meniscus
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

25. Is the freezing of ice endothermic or exothermic?
Exothermic
C2O4²?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Add acid to water so that the acid doesn't boil and spit

26. What do ions and electrons travel through in a voltaic/electrolytic cell?
Concentration
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Ksp = 4s³
+4-covalent - +2-ionic

27. Buffer capacity must contain decent amounts of a ________ ________
water and substances with (s) less dense than
C4H10
Conjugate pair (one must be a weak base or acid)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

28. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
small size and high charge
Kc=Kp

29. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
Check for air bubbles in the buret and remove the buret funnel from the buret
an oxidized and reduced substance
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

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

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31. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
CO (poisonous)
lighted splint (positive result=pop)
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

32. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
CnH2n+1 often designated 'R' ex C3H7 is propyl
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
CO (poisonous)

33. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
Saturated - Substitution (which requires more radical conditions)
Cu3(PO4)2
The dilution effect when the solutions mix. M1V1 = M2V2

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

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35. Alkanes are _________ and react by _________
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Tetrahedral
Decant
Saturated - Substitution (which requires more radical conditions)

36. What do you need to make a polymer?
different forms of the same element
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)
Pale purple - (orange)-yellow - red - blue - green.
acids

37. What is the general formula for an aldehyde?
RCHO (carbonyl at end)
S2O3²?
OH- and NH3
No - NH3 and HCl gases are extremely soluble

38. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
RNH2
Pale purple - (orange)-yellow - red - blue - green.
Transition element compounds (except if it has a full or empty d shell)
zero

39. What element is used to vulcanize rubber?
?G=negative - E° must be positive
Sulfur
Unsaturated - addition (ex: decolorize bromine solution)
Ppt will NOT form (unsaturated)

40. What is the third law of thermodynamics?
do not change
MnO4?
S crystal at 0K=0
'non-active' metals such as Cu - Ag - Au - Pt - etc.

41. What are isomers?
Experimental mass/theoretical mass X 100
Molecules with the same molecular formulas - but different structural formulas
At half equivalence - pH=pKa
Insoluble except group 1 and ammonium

42. What type of solutions do small - highly charged cations tend to form?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
ClO2?
0.10M HCl (more ions)

43. How do you explain trends in atomic properties using Coulomb's Law?
An active metal.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Acids; HCOOCH3 is an ester

44. How does the melting point of a mixture compare to the MP of a pure substance?
Pale yellow
non-metal oxides and hydrides are covalently bonded and are acidic.
Iodine and CO2 (dry ice)
it is lower and occurs over less sharp a range

45. What is the formula for percent error?
Filtration
basic
|experimental - accepted|/accepted X 100
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

46. How many ligands attach to a central ion in a complex ion?
Insoluble (except group 1 ammonium and Ba)
RCOOH
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
#ligands=charge x2

47. Is a graduated cylinder or beaker more accurate?
H2O + CO2 (it decomposes readily)
Perform ICE BOX calculation based on K1
Graduated cylinder
Most are soluble except Ag - Pb

48. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
fractional distillation
Trigonal pyramidal
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

49. Do anions flow to the cathode or anode?
Making sigma bonds and holding lone pairs
Anode
NH2?
look for changes in oxidation # - the one that goes up is oxidized and is the RA

50. nitrate
O2 needs 4F/mol H2 needs 2F/mol
Ksp = 27s4
Disulfur dichloride
NO3?