Test your basic knowledge |

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 compounds are almost always colored?
blue glass - it filters UV
CnH(2n+2)
Transition element compounds (except if it has a full or empty d shell)
acid + alcohol

2. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
ion pairing
Increases.
Eudiometer
CO (poisonous)

3. What do metal oxides plus non- metal oxides form?
Ksp = s²
Increases down group 1 decreases down group 17
Salts (ex: CaO + SO2 ? CaSO3)
zero

4. hydroxides
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Insoluble (except group 1 ammonium and Ba)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Clear

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

6. Does Benzene react by addition or substitution?
Selective absorption
linear
it reacts by substitution NOT addition
PO4³?

7. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
H3PO4
Separating funnel
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

8. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
NO3?
Mn²? - Cr³? - Cr³
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Pale purple - (orange)-yellow - red - blue - green.

9. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
H2PO4?
The dilution effect when the solutions mix. M1V1 = M2V2
yellow
Current - time and charge on ion (moles of e used in half cell reaction)

10. What two compounds are great oxidizing agents?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

11. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
proton donor base
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
The compound with the lowest Ksp value.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

12. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
CO2 and H2O
All except for lithium
Synthetic condensation polymer (aka a polyamide)

13. How do you identify which is oxidized or otherwise?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
it is lower and occurs over less sharp a range
catalyst=conc H2SO4

14. group 1 ions/compounds
Soluble
#ligands=charge x2
Cr2O7²?
benzene is less reactive than alkenes

15. What are hybrid orbitals used for?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Greenish-yellow gas
basic
Making sigma bonds and holding lone pairs

16. 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)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Sulfur
Transition element compounds (except if it has a full or empty d shell)

17. Both Acetic acid and ____________ are also functional isomers.
+4-covalent - +2-ionic
Exothermic (?H for ANY sa/sb = -57kJ/mol)
methyl formate
look for changes in oxidation # - the one that goes up is oxidized and is the RA

18. carbonates
by electrolysis
Acid rain - dissolves marble buildings/statues and kills trees.
Insoluble except group 1 and ammonium
O2 needs 4F/mol H2 needs 2F/mol

19. The definition of acidic basic and neutral aqueous solutions is:
Filtration
Cr2O7²?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

20. What is the third law of thermodynamics?
do not change
Pale yellow
Insoluble (except group 1 ammonium and Ba)
S crystal at 0K=0

21. dichromate
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Cr2O7²?
Ksp = 108s5
are less dense than water

22. What is the formula for alkenes?
CnH2n
RCOOH
blue (BTB)
acids

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

24. What is the first law of thermodynamics?
proton acceptor.
Separating funnel
E=q + w (negative is by system - positive is on system)
Glowing splint (positive result=relights)

25. How do you compute % dissociation?
acids
Insoluble except group 1 and ammonium
ClO3?
[A?]/[HA] x 100 or [BH?]/[B] x 100

26. Why are i factors (Van't Hoff factors) often less than ideal?
redox reaction
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
ion pairing
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

28. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
Time?¹ - (ex. s?¹ - hr?¹ - etc)
catalyst=conc H2SO4
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

29. Is the standard entropy (S°) of an element zero?
A salt solution.
fractional distillation
But S° of element is not zero (except at 0K)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

30. silver iodide
Pale yellow
Sulfur
Both electrons come from the same atom (just as good as a regular bond)
by electrolysis

31. Give an example of a concentrated weak acid.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Glacial acetic acid
Acidified

32. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
RNH2
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
basic
same KE - but PEice<PEwater

33. Acid plus base make?
CnH2n+2
Salt + water.
Soluble except Ag - Pb - Ca - Sr Ba)
Iodine and CO2 (dry ice)

34. Alcohols and _______ are FG isomers
Current - time and charge on ion (moles of e used in half cell reaction)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Acid rain - dissolves marble buildings/statues and kills trees.
ethers

35. Buffer capacity must contain decent amounts of a ________ ________
water and substances with (s) less dense than
redox reaction
Conjugate pair (one must be a weak base or acid)
are less dense than water

36. How do you explain trends in atomic properties using Coulomb's Law?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
non-metal oxides and hydrides are covalently bonded and are acidic.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
RNH2

37. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
bright yellow

38. What is the formula of butane?
Saturated - Substitution (which requires more radical conditions)
C4H10
it is lower and occurs over less sharp a range
A) any range. b) 8-10 c) 4-6

39. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
E=q + w (negative is by system - positive is on system)
chemically (ex: with carbon)
Synthetic condensation polymer (aka a polyamide)

40. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Sigma bonds are stronger than pi bonds
Suniverse increases for spontaneous processes
Insoluble except nitrate and acetate

41. lead compounds
White precipitate
ROR
Insoluble except nitrate and acetate
[A?]/[HA] x 100 or [BH?]/[B] x 100

42. Colorless doesn't mean ______
The benzene ring (or more correctly the phenyl group - C6H5)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Clear
CrO4²?

43. What is the formula for alkanes?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
CnH2n+2
S2O3²?
No - NH3 and HCl gases are extremely soluble

44. What is the general formula for a ketone?
catalyst=conc H2SO4
RX
Tetrahedral
RCOR

45. ammonium/ammonium compounds
q=mc?T q=mL (or n x ?h)
same KE - but PEice<PEwater
Ksp = 108s5
Soluble

46. What type of solutions do small - highly charged cations tend to form?
ethers
SO4²?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Glowing splint (positive result=relights)

47. phosphates
Trigonal pyramidal
Most INsoluble except group 1 and ammonium
'non-active' metals such as Cu - Ag - Au - Pt - etc.
diamond and graphite

48. Does Kw increase or decrease with T? Why?
Orange
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
do not change
Greenish-yellow gas

49. What apparatus do you use to separate 2 immiscible liquids?
NO3?
neutralization: high K - H2O product dissociation: low K - H2O reactant
They stay the same.
Separating funnel

50. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
RNH2
The one with most oxygen atoms (highest oxidation number)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.