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. Color is due to ______ _______ of light.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
benzene is less reactive than alkenes
Selective absorption
Ksp = s²

2. Why are i factors (Van't Hoff factors) often less than ideal?
do not change
Heptane
non-metal oxides and hydrides are covalently bonded and are acidic.
ion pairing

3. What is the formula for alkanes?
P2O5
+4-covalent - +2-ionic
CnH2n+2
proton acceptor.

4. Give an example of a dilute strong acid.
Most are soluble except Ag - Pb
do not change
metal oxides and hydrides are ionically bonded and basic
HClO4

5. What is the charge on a chlorine atom?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Distillation
zero
White precipitate

6. What is the general formula for an ester?
ROR
RCOOR
Kc=Kp
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

7. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
Insoluble except group 1 and ammonium
methyl formate
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

8. What shape is water?
Group I metals (soft metals) are stored under oil
Pale yellow
bent
No - NH3 and HCl gases are extremely soluble

9. How do you get Ecell for spontaneous reactions?
Initiation energy (NOT Ea)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Greenish-yellow gas
Concentration

10. primary colors
Both electrons come from the same atom (just as good as a regular bond)
red - green - blue
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Exothermic

11. What is the catalyst for this reaction Ester + ?
catalyst=conc H2SO4
H2O + CO2 (it decomposes readily)
CnH(2n+2)
?G=negative - E° must be positive

12. Ca - Sr - Ba
zero
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
hydroxides (ex: Ba(OH)2)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

13. Neutralization is an ________ reaction.
ROH
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Silvery gray solid - brown - purple
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

14. How does the melting point of a mixture compare to the MP of a pure substance?
Unsaturated - addition (ex: decolorize bromine solution)
it is lower and occurs over less sharp a range
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
0 and 14

15. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Q=It (time in seconds)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
a-IMFs - b-molecular volume

16. What process do you use to obtain the solute from a solution?
Evaporation
All except for lithium
proton donor base
Both electrons come from the same atom (just as good as a regular bond)

17. Metal hydrides are _____ and form _______ and _______ when added to water
But S° of element is not zero (except at 0K)
O2 needs 4F/mol H2 needs 2F/mol
ionic and form hydrogen and hydroxide
Anode

18. When combining half equations - what do you do to E° values when multiplying coefficients?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Nothing
Cu3(PO4)2
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)

19. An amphiprotic (amphoteric) species is...
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
red - green - blue
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

20. What is the test for oxygen?
Sulfur
Glowing splint (positive result=relights)
Mono; di; tri; tetra; penta; hexa.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

21. A Bronsted-Lowry base is...
SO4²?
proton acceptor.
H2PO4?
basic

22. What is the difference between equivalence point and end point of a titration.
A) any range. b) 8-10 c) 4-6
an oxidized and reduced substance
Time?¹ - (ex. s?¹ - hr?¹ - etc)
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

23. What are hybrid orbitals used for?
Making sigma bonds and holding lone pairs
left - ppt will form
The one with most oxygen atoms (highest oxidation number)
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

24. If a free element is involved - what type of reaction must be involved?
0.10M HCl (more ions)
CnH(2n+2)
redox reaction
Filtration

25. What is the general formula for alkyl halides?
-Ea/R
All single: sp³ - one double: sp² - two doubles: sp - one triple: sp - two single and two lone pairs: sp³ - three single and one lone pair: sp³
RX
Insoluble except group 1 and ammonium

26. chlorine
atoms
do not change
Greenish-yellow gas
RX

27. Alcohols and _______ are FG isomers
blue (BTB)
ethers
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Saturated - Substitution (which requires more radical conditions)

28. What is the conjugate base of NH3?
Read the bottom of the meniscus
NH2?
10?8
Time?¹ - (ex. s?¹ - hr?¹ - etc)

29. What is the formula for summation?

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

30. A Bronsted-Lowry acid is...
Acid rain - dissolves marble buildings/statues and kills trees.
different forms of the same element
Increases down group 1 decreases down group 17
proton donor base

31. Aromatic compounds contain what?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Tetrahedral
The benzene ring (or more correctly the phenyl group - C6H5)
S2O3²?

32. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
O2 needs 4F/mol H2 needs 2F/mol
Current - time and charge on ion (moles of e used in half cell reaction)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Cr2O7²?

33. Name 2 ways in which you can create a buffer?
a-IMFs - b-molecular volume
red - green - blue
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)
NO3?

34. What does saturated mean? Unsaturated?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
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.
0.10M HCl (more ions)

35. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Check for air bubbles in the buret and remove the buret funnel from the buret

36. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
A) any range. b) 8-10 c) 4-6
Iodine and CO2 (dry ice)
Saturated - Substitution (which requires more radical conditions)
ion pairing

37. group 1 ions/compounds
Tetrahedral
Soluble
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Pipette (burette if need repetition)

38. What is a dipeptide? polypeptide? protein?
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?)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Mn²? - Cr³? - Cr³
acid + alcohol

39. Name C7H16
Salt + water
They stay the same.
Heptane
A) any range. b) 8-10 c) 4-6

40. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
Acid rain - dissolves marble buildings/statues and kills trees.
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Salt and water

41. Acidic gases like SO2 in the atmosphere cause what environmental problems?
The dilution effect when the solutions mix. M1V1 = M2V2
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
OH- and NH3
Acid rain - dissolves marble buildings/statues and kills trees.

42. oxalate
proton acceptor.
C2O4²?
Only temperature
voltaic: - electrolytic: +

43. ammonium/ammonium compounds
Insoluble except for nitrate and acetate
Glowing splint (positive result=relights)
Soluble
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)

44. Alkanes are _________ and react by _________
voltaic: + electrolytic: -
Saturated - Substitution (which requires more radical conditions)
No - NH3 and HCl gases are extremely soluble
Soluble

45. The oxidation # for acid base reactions...
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Synthesis - separation and purification of the product and its identification.
do not change
Decant

46. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
bases
Acids; HCOOCH3 is an ester
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

47. Is the standard entropy (S°) of an element zero?
Insoluble except group 1 and ammonium
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
But S° of element is not zero (except at 0K)
RX

48. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
-Ea/R
Heat a test tube at an angle at the side of the tube (not bottom)
Anode - oxygen. Cathode - hydrogen
benzene is less reactive than alkenes

49. What device would you use to measure a volume of gas?
atoms
redox reaction
basic
Eudiometer

50. copper sulfate
a-IMFs - b-molecular volume
C4H10
Synthetic condensation polymer (aka a polyamide)
blue