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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. nitrate
NO3?
10?8
Decant
Glacial acetic acid

2. What is HCOOCH3?
The benzene ring (or more correctly the phenyl group - C6H5)
non-metal oxides and hydrides are covalently bonded and are acidic.
Acids; HCOOCH3 is an ester
Pale yellow

3. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Group I metals (soft metals) are stored under oil
do not change
by electrolysis
Salt and water

4. What is the difference between equivalence point and end point of a titration.
Experimental mass/theoretical mass X 100
The compound with the lowest Ksp value.
NO3?
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

5. When driving off water from a hydrate - how do you tell you're done?
CH3COO?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
CN?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

6. What is the general formula for an ether?
Pipette (burette if need repetition)
C4H10
|experimental - accepted|/accepted X 100
ROR

7. A Bronsted-Lowry acid is...
Group I metals (soft metals) are stored under oil
proton donor base
ClO2?
redox reaction

8. Metal hydrides are _____ and form _______ and _______ when added to water
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=mc?T q=mL (or n x ?h)
ionic and form hydrogen and hydroxide
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

9. If a weak acid is diluted more - what happens to its % dissociation value?
diamond and graphite
Iodine and CO2 (dry ice)
Increases.
a-IMFs - b-molecular volume

10. Lattice energy is high for ions with _____ size and _____ charge
Big K=kf/kr
The Faraday or Faraday's constant.
small size and high charge
proton acceptor.

11. The oxidation # for acid base reactions...
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
do not change
same KE - but PEice<PEwater

12. What things should you remember to do when collecting gas over water?
Trigonal pyramidal
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
allow for the vapor pressure of water and make sure to level levels
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

13. hypochlorite
Separating funnel
ClO?
CH3COO?
Ksp = 27s4

14. What are two substances that sublime at 1 atm when heated?
Both electrons come from the same atom (just as good as a regular bond)
Making sigma bonds and holding lone pairs
Iodine and CO2 (dry ice)
bent

15. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
bright yellow
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Concentration
water and substances with (s) less dense than

16. What do acids plus active metals form?
A salt solution.
Saturated - Substitution (which requires more radical conditions)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
MnO4?

17. dichromate (soln + most solids)
proton acceptor.
Orange
blue glass - it filters UV
Graduated cylinder

18. What should you check for before you begin titrating?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
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.
Check for air bubbles in the buret and remove the buret funnel from the buret
lighted splint (positive result=pop)

19. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
0.10M HCl (more ions)
ROH
No - it depends on the number of ions produced on dissolving.
ClO3?

20. How does group 1 metals' density compare to water's?
are less dense than water
benzene is less reactive than alkenes
Kc=Kp
SO4²?

21. hydroxide
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
OH?
an oxidized and reduced substance
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

22. What process do you use to obtain the solute from a solution?
allow for the vapor pressure of water and make sure to level levels
How close results are to the accepted value
White precipitate
Evaporation

23. Does Kw increase or decrease with T? Why?
Iodine and CO2 (dry ice)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
RCOOR

24. What is the general formula for an alcohol?
The compound with the lowest Ksp value.
ROH
It ceases - the circuit is broken.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

25. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
T increases exponentially the proportion of molecules with E > Ea
Insoluble except nitrate and acetate

26. phosphate
PO4³?
atoms
H+
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

27. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Salts (ex: CaO + SO2 ? CaSO3)
Synthesis - separation and purification of the product and its identification.
OH- and NH3
non-metal oxides and hydrides are covalently bonded and are acidic.

28. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
ethers
ClO?
Concentration

29. What is the formula for alkynes?
Anode - oxygen. Cathode - hydrogen
CnH2n-2
Silvery gray solid - brown - purple
boiling without losing volatile solvents/reactants

30. What reacts with an acid to create hydrogen gas?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
An active metal.
Soluble
allow for the vapor pressure of water and make sure to level levels

31. Aromatic compounds contain what?
H2PO4?
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 benzene ring (or more correctly the phenyl group - C6H5)
All except for lithium

32. bromine
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
10?8
non-metal oxides and hydrides are covalently bonded and are acidic.
brown volatile liquid

33. What kind of bonding structure does benzene have?
fractional distillation
Soluble except Ag - Pb - Ca - Sr Ba)
benzene has a delocalized pi ring structure
by electrolysis

34. What is an Alkyl group?

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35. What part of a liquid do you look at to measure its volume?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Most are soluble except Ag - Pb
Read the bottom of the meniscus
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

36. What changes Keq?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
The dilution effect when the solutions mix. M1V1 = M2V2
Only temperature
The one with most oxygen atoms (highest oxidation number)

37. lead compounds
#ligands=charge x2
Insoluble except nitrate and acetate
Insoluble except for nitrate and acetate
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

38. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
Initiation energy (NOT Ea)
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.
Most INsoluble except group 1 and ammonium

39. What is the relationship in strength between sigma and pi bonds?
Disulfur dichloride
Sigma bonds are stronger than pi bonds
OH- and NH3
Mn²? - Cr³? - Cr³

40. What do you use for an acid spill? base spill?
redox reaction
Anode
Glacial acetic acid
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

41. What shape is carbon dioxide?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
red - green - blue
linear

42. What is the general formula for an amine?
RNH2
The Faraday or Faraday's constant.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Selective absorption

43. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Acids; HCOOCH3 is an ester
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Decant
Insoluble except nitrate and acetate

44. What do you need to make a polymer?
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)
Tetrahedral
C2O4²?
Cu3(PO4)2

45. Give an example of a concentrated weak acid.
But S° of element is not zero (except at 0K)
Salt + water
S crystal at 0K=0
Glacial acetic acid

46. What complex ion does ammonia form with silver? copper? cadmium? zinc?
bases
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

47. thiosulfate
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
S2O3²?
E=q + w (negative is by system - positive is on system)
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?)

48. A geometric (or cis-trans) isomer exists due to.....
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
same KE - but PEice<PEwater
small size and high charge

49. chlorate
zero-th: decreases - first: constant - second: increases
CO3²?
ClO3?
Soluble

50. 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.
Mono; di; tri; tetra; penta; hexa.
A) any range. b) 8-10 c) 4-6
Big K=kf/kr
+4 and +2 (+4 dominates top of group and +2 at bottom of group)