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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. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
Soluble
methyl formate
Decant

2. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Heptane
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Synthesis - separation and purification of the product and its identification.

3. What is the general formula for an aldehyde?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Synthesis - separation and purification of the product and its identification.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
RCHO (carbonyl at end)

4. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Acids; HCOOCH3 is an ester
CnH2n+1 often designated 'R' ex C3H7 is propyl

5. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
H+
Unsaturated - addition (ex: decolorize bromine solution)
10?8

6. carbonate
Add acid to water so that the acid doesn't boil and spit
CO3²?
Soluble
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.

7. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
zero
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
RX
Mn²? - Cr³? - Cr³

8. Name six characteristics of transition elements (or their compounds)
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)
same KE - but PEice<PEwater
neutralization: high K - H2O product dissociation: low K - H2O reactant
Big K=kf/kr

9. What is the formula for obtaining charge flowing in a cell?
Heat a test tube at an angle at the side of the tube (not bottom)
Iodine and CO2 (dry ice)
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?)
Q=It (time in seconds)

10. What is the general formula for alkyl halides?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
A) any range. b) 8-10 c) 4-6
RX
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

11. acetate
CH3COO?
Acid rain - dissolves marble buildings/statues and kills trees.
CnH2n
Transition element compounds (except if it has a full or empty d shell)

12. Why are i factors (Van't Hoff factors) often less than ideal?
MnO4?
voltaic: - electrolytic: +
H3PO4
ion pairing

13. A Bronsted-Lowry acid is...
OH- and NH3
A) any range. b) 8-10 c) 4-6
Making sigma bonds and holding lone pairs
proton donor base

14. What is the test for oxygen?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Products - reactants (except for BDE when it's reactants - products)
voltaic: + electrolytic: -
Glowing splint (positive result=relights)

15. A Bronsted-Lowry base is...
proton acceptor.
CnH(2n+2)
+4-covalent - +2-ionic
P2O5

16. halides
Most are soluble except Ag - Pb
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Salt + water
Increases down group 1 decreases down group 17

17. For a dibasic acid (H2A) - [A²?]= ____ ?
A) any range. b) 8-10 c) 4-6
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
K2
Orange

18. Color is due to ______ _______ of light.
Selective absorption
+4-covalent - +2-ionic
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
The one with most oxygen atoms (highest oxidation number)

19. How do you clean a buret/pipette for a titration?
?H formation of an element in standard state=0
CnH(2n+2)
Soluble
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

20. What are amphoteric oxides?
Glowing splint (positive result=relights)
an oxidized and reduced substance
do not change
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?)

21. dichromate (soln + most solids)
Only temperature
Orange
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?)
water and substances with (s) less dense than

22. What are two substances that sublime at 1 atm when heated?
Acid rain - dissolves marble buildings/statues and kills trees.
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Iodine and CO2 (dry ice)
The benzene ring (or more correctly the phenyl group - C6H5)

23. potassium permanganate
ROR
S2O3²?
Purple
S crystal at 0K=0

24. copper sulfate
blue
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
Q=It (time in seconds)
Soluble

25. How are more active metals reduced?
How close results are to the accepted value
Soluble
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
by electrolysis

26. A geometric (or cis-trans) isomer exists due to.....
Group I metals (soft metals) are stored under oil
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Soluble
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

27. Metal hydrides are _____ and form _______ and _______ when added to water
Glowing splint (positive result=relights)
ionic and form hydrogen and hydroxide
Tetrahedral
Exothermic (?H for ANY sa/sb = -57kJ/mol)

28. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
ion pairing
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

29. What shape is methane?
Trigonal pyramidal
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Tetrahedral
voltaic: + electrolytic: -

30. What is an Alkyl group?

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31. An amphiprotic (amphoteric) species is...
Hg2²?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
zero
Transition element compounds (except if it has a full or empty d shell)

32. mercury (II) ion
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Hg²?
q=mc?T q=mL (or n x ?h)
'non-active' metals such as Cu - Ag - Au - Pt - etc.

33. What is the catalyst for this reaction Ester + ?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Acidified
catalyst=conc H2SO4
Soluble

34. What is a coordinate covalent bond?
are less dense than water
an oxidized and reduced substance
Eudiometer
Both electrons come from the same atom (just as good as a regular bond)

35. How are strong ones written?
Ppt will NOT form (unsaturated)
strong acids/bases are written as H+ or OH- ions
do not change
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

36. What process do you use to obtain a solvent from a solution?
Distillation
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Group I metals (soft metals) are stored under oil

37. What is the third law of thermodynamics?
yellow
S crystal at 0K=0
ionic and form hydrogen and hydroxide
E=q + w (negative is by system - positive is on system)

38. What is the general formula for an amine?
Ksp = s²
RNH2
ionic and form hydrogen and hydroxide
hydroxides (ex: Ba(OH)2)

39. What is the sign of the cathode in voltaic cells? in electrolytic cells?
No - it depends on the number of ions produced on dissolving.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
voltaic: + electrolytic: -
How grouped results are

40. chromate ion (soln + most solids)
yellow
Increases.
ROR
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

41. What are the names and formulas of the 6 strong acids?
same KE - but PEice<PEwater
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
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?)

42. oxalate
Identity and purity (impure compounds usually have broad & low melting points)
C2O4²?
different forms of the same element
Only temperature

43. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Mn²? - Cr³? - Cr³
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Monomer + monomer = polymer product + a simple molecule such as water or HCl

44. When a cell is 'flat' What is its voltage?
zero
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
catalyst=conc H2SO4
Tetrahedral

45. What reacts with an acid to create hydrogen gas?
Ksp = 4s³
ClO4?
An active metal.
allow for the vapor pressure of water and make sure to level levels

46. sulfates
10?8
Soluble except Ag - Pb - Ca - Sr Ba)
Group I metals (soft metals) are stored under oil
CO2 and H2O

47. Which alkali metals float on water?
it's lower and occurs over less sharp a range
voltaic: + electrolytic: -
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
All except for lithium

48. What electrons are lost/gained first in transition element ions?
ClO4?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
ns² electrons (first in-first out)
it is lower and occurs over less sharp a range

49. Nonmetals are good _____ agents. Metals are good _______ agents.
ionic and form hydrogen and hydroxide
Soluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Group I metals (soft metals) are stored under oil

50. What is Big K in terms of kf and kr?
Suniverse increases for spontaneous processes
Acids; HCOOCH3 is an ester
acid + alcohol
Big K=kf/kr