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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. bromine
brown volatile liquid
by electrolysis
ClO?
basic

2. Why are i factors (Van't Hoff factors) often less than ideal?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
ion pairing
q=mc?T q=mL (or n x ?h)
Only temperature

3. What is the conjugate base of NH3?
CO2 and H2O
NH2?
Orange
linear

4. Do anions flow to the cathode or anode?
Insoluble (except group 1 ammonium and Ba)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
boiling without losing volatile solvents/reactants
Anode

5. Acid plus base make?
Salt + water.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

6. Does Benzene react by addition or substitution?
Salt + water
The one with most oxygen atoms (highest oxidation number)
linear
it reacts by substitution NOT addition

7. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
Insoluble (except group 1 ammonium and Ba)
neutralization: high K - H2O product dissociation: low K - H2O reactant
No - it depends on the number of ions produced on dissolving.

8. nitrates
it's lower and occurs over less sharp a range
Soluble
The compound with the lowest Ksp value.
No - NH3 and HCl gases are extremely soluble

9. What do group I/II metal oxides plus water form?
bases
The Faraday or Faraday's constant.
How close results are to the accepted value
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

10. Which would cause the bulb in a conductivity apparatus to be brightest?
water and substances with (s) less dense than
MnO4?
0.10M HCl (more ions)
ClO?

11. Does Kw increase or decrease with T? Why?
Suniverse increases for spontaneous processes
brown volatile liquid
non-metal oxides and hydrides are covalently bonded and are acidic.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

12. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Read the bottom of the meniscus
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
OH?

13. chlorate
ClO3?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Hg²?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

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

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15. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
S2O3²?
Initiation energy (NOT Ea)
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.

16. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
small size and high charge
basic
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Iodine and CO2 (dry ice)

17. What is the relationship in strength between sigma and pi bonds?
More chaotic (ex: gases made)
How grouped results are
Sigma bonds are stronger than pi bonds
R=8.31 J/mol/K

18. What is HCOOCH3?
Identity and purity (impure compounds usually have broad & low melting points)
Acids; HCOOCH3 is an ester
All except for lithium
neutralization: high K - H2O product dissociation: low K - H2O reactant

19. What is the general formula for an aldehyde?
CO2 and H2O
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Synthetic condensation polymer (aka a polyamide)
RCHO (carbonyl at end)

20. lead compounds
brown volatile liquid
are less dense than water
Insoluble except nitrate and acetate
The one with most oxygen atoms (highest oxidation number)

21. Name C7H16
red - green - blue
Heptane
a-IMFs - b-molecular volume
C2O4²?

22. hydroxides
small size and high charge
Insoluble (except group 1 ammonium and Ba)
bright yellow
CO2 and H2O

23. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
No - it depends on the number of ions produced on dissolving.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Unsaturated - addition (ex: decolorize bromine solution)
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)

24. Lattice energy is high for ions with _____ size and _____ charge
Pale purple - (orange)-yellow - red - blue - green.
CnH2n+1 often designated 'R' ex C3H7 is propyl
OH- and NH3
small size and high charge

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

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26. How do you get Ecell for spontaneous reactions?
Big K=kf/kr
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
MnO4?
yellow

27. bromothymol
?G= -ve - E°= +ve
Kc=Kp
blue (BTB)
Pale purple - (orange)-yellow - red - blue - green.

28. What is reflux?
Exothermic
boiling without losing volatile solvents/reactants
it reacts by substitution NOT addition
CN?

29. Where are group I metals stored?
Glowing splint (positive result=relights)
Concentration
ClO2?
Group I metals (soft metals) are stored under oil

30. What is the general formula for an ether?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
E=q + w (negative is by system - positive is on system)
ROR
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

31. How do you compute % dissociation?
CO2 and H2O
Heptane
Eudiometer
[A?]/[HA] x 100 or [BH?]/[B] x 100

32. What do you use for an acid spill? base spill?
H2PO4?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
RCOR
All except for lithium

33. chlorite
Insoluble (except group 1 ammonium and Ba)
CnH2n-2
ClO2?
Products - reactants (except for BDE when it's reactants - products)

34. What causes the dramatic effect of T on rate?
RCOR
T increases exponentially the proportion of molecules with E > Ea
fractional distillation
The dilution effect when the solutions mix. M1V1 = M2V2

35. How do you clean a buret/pipette for a titration?
Salt and water
Big K=kf/kr
The dilution effect when the solutions mix. M1V1 = M2V2
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

36. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Anode - oxygen. Cathode - hydrogen
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Pour liquids using a funnel or down a glass rod

37. How does group 1 metals' density compare to water's?
CH3COO?
are less dense than water
ionic and form hydrogen and hydroxide
The compound with the lowest Ksp value.

38. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
benzene is less reactive than alkenes
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
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

39. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
same KE - but PEice<PEwater
Mn²? - Cr³? - Cr³
Current - time and charge on ion (moles of e used in half cell reaction)
Big K=kf/kr

40. The definition of acidic basic and neutral aqueous solutions is:
Salt + water.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
a-IMFs - b-molecular volume

41. mercury (II) ion
No - it depends on the number of ions produced on dissolving.
RCOR
yellow
Hg²?

42. Can you collect soluble gases over water?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
H2O + CO2 (it decomposes readily)
No - NH3 and HCl gases are extremely soluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

43. hypochlorite
ion pairing
ClO?
Increases down group 1 decreases down group 17
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

44. When is ?G zero?
C4H10
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Pale purple - (orange)-yellow - red - blue - green.
it is lower and occurs over less sharp a range

45. What does the solubility of organic compounds depend on?
An active metal.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Perform ICE BOX calculation based on K1
acids

46. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
RCOR
Initiation energy (NOT Ea)
CrO4²?

47. ammonium
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Iodine and CO2 (dry ice)
NH4?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

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

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49. Both Acetic acid and ____________ are also functional isomers.
Increases.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
methyl formate

50. copper sulfate
CH3COO?
benzene is less reactive than alkenes
Silvery gray solid - brown - purple
blue