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. How are primary alcohols turned into acids?
Pale purple - (orange)-yellow - red - blue - green.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Both electrons come from the same atom (just as good as a regular bond)

2. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
The one with most oxygen atoms (highest oxidation number)
Selective absorption
OH?

3. What is the formula of butane?
Purple
C4H10
Pale purple - (orange)-yellow - red - blue - green.
RCOOR

4. Is the freezing of ice endothermic or exothermic?
Initiation energy (NOT Ea)
Exothermic
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
All except for lithium

5. How do you get the equation for a net electrolysis reaction?
Mn²? - Cr³? - Cr³
Combine the equations for the half reactions in the non-spontaneous direction
O2 needs 4F/mol H2 needs 2F/mol
linear

6. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
lighted splint (positive result=pop)
neutralization: high K - H2O product dissociation: low K - H2O reactant
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Ions go through the salt bridge - electrons go through metal wires in the external circuit

7. What is the general formula for an amine?
RNH2
Separating funnel
H2PO4?
Soluble

8. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
ROR
At half equivalence - pH=pKa

9. How do you compute % dissociation?
blue
[A?]/[HA] x 100 or [BH?]/[B] x 100
allow for the vapor pressure of water and make sure to level levels
P2O5

10. Give an example of a dilute strong acid.
#ligands=charge x2
|experimental - accepted|/accepted X 100
Ksp = 27s4
HClO4

11. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Silvery gray solid - brown - purple
E=q + w (negative is by system - positive is on system)
Decant

12. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Trigonal pyramidal
water and substances with (s) less dense than
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
CnH2n+1 often designated 'R' ex C3H7 is propyl

13. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Greenish-yellow gas
Pour liquids using a funnel or down a glass rod

14. dichromate
lighted splint (positive result=pop)
Trigonal pyramidal
blue glass - it filters UV
Cr2O7²?

15. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
0.10M HCl (more ions)
Transition element compounds (except if it has a full or empty d shell)
bent

16. Which value of R do you use for all energy and kinetics calculations?
Cr2O7²?
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
R=8.31 J/mol/K
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

17. When combining half equations - what do you do to E° values when multiplying coefficients?
P2O5
Nothing
The compound with the lowest Ksp value.
Sulfur

18. What is the conjugate base of NH3?
|experimental - accepted|/accepted X 100
Perform ICE BOX calculation based on K1
NH2?
by electrolysis

19. What does the solubility of organic compounds depend on?
Only temperature
bases
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
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

20. What is the energy you must put into a reaction to make it start called?
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?)
Initiation energy (NOT Ea)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
HClO4

21. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Ksp = 27s4
basic

22. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
Iodine and CO2 (dry ice)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

23. How do you clean a buret/pipette for a titration?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
brown volatile liquid
basic

24. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Making sigma bonds and holding lone pairs
Products - reactants (except for BDE when it's reactants - products)

25. copper sulfate
proton donor base
blue
Acid rain - dissolves marble buildings/statues and kills trees.
Ions go through the salt bridge - electrons go through metal wires in the external circuit

26. halides
Sulfur
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Initiation energy (NOT Ea)
Most are soluble except Ag - Pb

27. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Anode - oxygen. Cathode - hydrogen
zero
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Q=It (time in seconds)

28. What is the test for oxygen?
O2 needs 4F/mol H2 needs 2F/mol
left - ppt will form
ion pairing
Glowing splint (positive result=relights)

29. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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

30. silver compounds
OH?
MnO4?
Insoluble except for nitrate and acetate
Salt + water.

31. How many faradays of electric charge do you need to produce one mole of O2? H2?
CO3²?
O2 needs 4F/mol H2 needs 2F/mol
same KE - but PEice<PEwater
-Ea/R

32. chlorate
Exothermic
RX
ClO3?
0 and 14

33. Acidic gases like SO2 in the atmosphere cause what environmental problems?
blue (BTB)
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)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Acid rain - dissolves marble buildings/statues and kills trees.

34. What are amphoteric oxides?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
fractional distillation
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?)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

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

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

36. What is the difference between equivalence point and end point of a titration.
ClO3?
How grouped results are
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
0 and 14

37. What type of compounds do metals/non metals form?
Ionic compounds
Synthesis - separation and purification of the product and its identification.
bases
Ksp = 27s4

38. How are more active metals reduced?
by electrolysis
Current - time and charge on ion (moles of e used in half cell reaction)
An active metal.
Glowing splint (positive result=relights)

39. Alcohols and _______ are FG isomers
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
ClO3?
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?)
ethers

40. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
Silvery gray solid - brown - purple
They stay the same.
small size and high charge

41. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
Saturated - Substitution (which requires more radical conditions)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Big K=kf/kr

42. How many ligands attach to a central ion in a complex ion?
bases
#ligands=charge x2
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
All except for lithium

43. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
Read the bottom of the meniscus
Sulfur
Glacial acetic acid

44. What do hydrocarbons form when they burn in air (oxygen)?
+4-covalent - +2-ionic
Ions go through the salt bridge - electrons go through metal wires in the external circuit
All except for lithium
CO2 and H2O

45. During a titration what is present in the beaker at the equivalence point?
Identity and purity (impure compounds usually have broad & low melting points)
fruit - fish - bases
A salt solution.
CO (poisonous)

46. What do you use to look at burning magnesium? why?
0.10M HCl (more ions)
Group 1 hydroxides (ex: NaOH)
Q=It (time in seconds)
blue glass - it filters UV

47. Why are i factors (Van't Hoff factors) often less than ideal?
+4-covalent - +2-ionic
ion pairing
blue
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

48. Alkanes are _________ and react by _________
Synthetic condensation polymer (aka a polyamide)
Hg²?
?H-kJ - ?S-J - ?G-kJ
Saturated - Substitution (which requires more radical conditions)

49. What do ions and electrons travel through in a voltaic/electrolytic cell?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
strong acids/bases are written as H+ or OH- ions
Group I metals (soft metals) are stored under oil

50. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
methyl formate
Hg2²?
red - green - blue