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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. Which of the rates changes more when temperature is increased?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
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
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)
RCOR

2. What is the general formula for a ketone?
non-metal oxides and hydrides are covalently bonded and are acidic.
RCOR
RCOOH
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

3. A Bronsted-Lowry acid is...
How grouped results are
proton donor base
Filtration
Pale yellow

4. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
strong acids/bases are written as H+ or OH- ions
ion pairing

5. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
catalyst=conc H2SO4
Transition element compounds (except if it has a full or empty d shell)
[Ag(NH3)2]? - [Cu(NH3)4]? - [Cd(NH3)4]? - [Zn(NH3)4]?

6. Alkenes are ________ and react by __________
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
|experimental - accepted|/accepted X 100
Unsaturated - addition (ex: decolorize bromine solution)

7. chlorite
Iodine and CO2 (dry ice)
ClO2?
Acids; HCOOCH3 is an ester
Insoluble except group 1 and ammonium

8. What type of compounds are almost always colored?
Salt + water
Transition element compounds (except if it has a full or empty d shell)
Soluble
a-IMFs - b-molecular volume

9. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
bright yellow
Ksp = 108s5
E=q + w (negative is by system - positive is on system)
zero

10. What type of solutions do small - highly charged cations tend to form?
Separating funnel
Acidic solutions (Ex: [Fe(H2O)6]? + H2O = Fe(H2O)5OH]? + H3O?)
Exothermic
All single: sp - one double: sp - two doubles: sp - one triple: sp - two single and two lone pairs: sp - three single and one lone pair: sp

11. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
SO4?
Graduated cylinder
zero

12. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Acidified
basic
Most INsoluble except group 1 and ammonium
Nothing

13. Give an example of a concentrated weak acid.
Initiation energy (NOT Ea)
Glacial acetic acid
They stay the same.
same KE - but PEice<PEwater

14. What is HCOOCH3?
CnH2n
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Separating funnel
Acids; HCOOCH3 is an ester

15. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
voltaic: + electrolytic: -
Transition element compounds (except if it has a full or empty d shell)
The dilution effect when the solutions mix. M1V1 = M2V2

16. How do you explain trends in atomic properties using Coulomb's Law?
boiling without losing volatile solvents/reactants
Initiation energy (NOT Ea)
Suniverse increases for spontaneous processes
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

17. What do the 'a' and 'b' in Van Der Waal's equation allow for?
acid + alcohol
Ionic compounds
Saturated - Substitution (which requires more radical conditions)
a-IMFs - b-molecular volume

18. chlorine
CnH2n+1 often designated 'R' ex C3H7 is propyl
No - NH3 and HCl gases are extremely soluble
Greenish-yellow gas
#ligands=charge x2

19. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Acidic solutions (Ex: [Fe(H2O)6]? + H2O = Fe(H2O)5OH]? + H3O?)
Concentration
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
K1 x K2

20. What is Big K in terms of kf and kr?
Big K=kf/kr
proton donor base
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
HClO4

21. What kind of bonding structure does benzene have?
ionic and form hydrogen and hydroxide
benzene has a delocalized pi ring structure
Eudiometer
No - it depends on the number of ions produced on dissolving.

22. The definition of acidic basic and neutral aqueous solutions is:
MnO4?
RX
Soluble
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

23. phosphate
PO4?
CrO4?
Soluble
acid + alcohol

24. What is the formula for alkanes?
ClO4?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
CnH2n+2
Conjugate pair (one must be a weak base or acid)

25. What is the general formula for an amine?
S crystal at 0K=0
Iodine and CO2 (dry ice)
RNH2
RCHO (carbonyl at end)

26. Name C7H16
All single: sp - one double: sp - two doubles: sp - one triple: sp - two single and two lone pairs: sp - three single and one lone pair: sp
Heptane
brown volatile liquid
CO2 and H2O

27. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
blue
?H-kJ - ?S-J - ?G-kJ
They decrease (or could be the same if the solid has ONLY JUST disappeared)

28. 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)
The dilution effect when the solutions mix. M1V1 = M2V2
[Ag(NH3)2]? - [Cu(NH3)4]? - [Cd(NH3)4]? - [Zn(NH3)4]?
They stay the same.

29. What shape is ammonia?
Decant
C4H10
Glowing splint (positive result=relights)
Trigonal pyramidal

30. What is the general formula of an alkane?
Ionic compounds
RCOOH
CnH(2n+2)
fractional distillation

31. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Experimental mass/theoretical mass X 100
4 sigma bonds-109 - sp - one double bond-120 - sp two double bonds-180 - sp one triple bond-180 - sp
Synthetic condensation polymer (aka a polyamide)

32. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base
Time? - (ex. s? - hr? - etc)
Silvery gray solid - brown - purple
basic
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

33. What is the general formula for alkyl halides?
Most are soluble except Ag - Pb
Anode - oxygen. Cathode - hydrogen
RX
Clear

34. If a weak acid is diluted more - what happens to its % dissociation value?
Increases.
Anode
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Purple

35. During a titration what is present in the beaker at the equivalence point?
Ksp = 27s4
Cu3(PO4)2
Q=It (time in seconds)
A salt solution.

36. halides
Most are soluble except Ag - Pb
proton donor base
H2PO4?
Insoluble (except group 1 ammonium and Ba)

37. Color (absorbance) is proportional to ________
CO (poisonous)
Concentration
R=8.31 J/mol/K
Initiation energy (NOT Ea)

38. copper sulfate
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
+4-covalent - +2-ionic
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
blue

39. Color is due to ______ _______ of light.
diamond and graphite
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Transition element compounds (except if it has a full or empty d shell)
Selective absorption

40. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Synthetic condensation polymer (aka a polyamide)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
The dilution effect when the solutions mix. M1V1 = M2V2

41. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
CnH2n
No - it depends on the number of ions produced on dissolving.
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

42. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
Sigma bonds are stronger than pi bonds
Eudiometer
ion pairing

43. When combining half equations - what do you do to E values when multiplying coefficients?
Nothing
methyl formate
RCOOR
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

44. When can supercooling occur? What does it look like on a cooling curve?
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
RX
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
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.

45. mercury (II) ion
same KE - but PEice<PEwater
red - green - blue
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Hg?

46. What is the second law of thermodynamics?
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
NH2?
catalyst=conc H2SO4
Suniverse increases for spontaneous processes

47. What does the solubility of organic compounds depend on?
Soluble
CnH2n+1 often designated 'R' ex C3H7 is propyl
|experimental - accepted|/accepted X 100
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

48. Neutralization is an ________ reaction.
do not change
proton acceptor.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
ROR

49. How are primary alcohols turned into acids?
small size and high charge
yellow
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Acids; HCOOCH3 is an ester

50. How do you clean a buret/pipette for a titration?
Big K=kf/kr
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
PO4?

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