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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. acetate
do not change
CH3COO?
All except for lithium
?H-kJ - ?S-J - ?G-kJ

2. What is the slope of the graph of lnk vs. 1/T?
ns² electrons (first in-first out)
Hg2²?
-Ea/R
Ksp = 108s5

3. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
ion pairing
Ksp = s²

4. What shape is methane?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
P2O5
Tetrahedral
Ksp = 4s³

5. Esters smell like _______ and amines smell like _______ and are ______.
Current - time and charge on ion (moles of e used in half cell reaction)
Synthesis - separation and purification of the product and its identification.
fruit - fish - bases
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

6. For a dibasic acid (H2A) - [A²?]= ____ ?
Exothermic
K2
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
0 and 14

7. How do you compute % dissociation?
water and substances with (s) less dense than
blue glass - it filters UV
atoms
[A?]/[HA] x 100 or [BH?]/[B] x 100

8. What do nonmetal oxides plus water form?
CnH2n-2
ClO4?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
acids

9. What equipment do you need for a titration?
zero
A) any range. b) 8-10 c) 4-6
allow for the vapor pressure of water and make sure to level levels
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

10. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
do not change
yellow
H2PO4?

11. dihydrogen phosphate
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)
CO3²?
H2PO4?
Combine the equations for the half reactions in the non-spontaneous direction

12. What electrons are lost/gained first in transition element ions?
benzene is less reactive than alkenes
ns² electrons (first in-first out)
HClO4
small size and high charge

13. silver iodide
Most are soluble except Ag - Pb
Pale yellow
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
S2O3²?

14. What are the units of the first order rate constant?
Soluble except Ag - Pb - Ca - Sr Ba)
Pale yellow
Time?¹ - (ex. s?¹ - hr?¹ - etc)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

15. Acidic gases like SO2 in the atmosphere cause what environmental problems?
How close results are to the accepted value
Acid rain - dissolves marble buildings/statues and kills trees.
+4-covalent - +2-ionic
no - they're written undissociated (HAaq)

16. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Glacial acetic acid
neutralization: high K - H2O product dissociation: low K - H2O reactant
Conjugate pair (one must be a weak base or acid)
H3PO4

17. Ions are not ______.
different forms of the same element
Salt and water
atoms
Clear

18. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
No - NH3 and HCl gases are extremely soluble
zero-th: decreases - first: constant - second: increases
Pale purple - (orange)-yellow - red - blue - green.
Insoluble

19. mercury (I) ion
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
same KE - but PEice<PEwater
Pipette (burette if need repetition)
Hg2²?

20. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Glowing splint (positive result=relights)
allow for the vapor pressure of water and make sure to level levels
The dilution effect when the solutions mix. M1V1 = M2V2
Ksp = 4s³

21. Why are i factors (Van't Hoff factors) often less than ideal?
Purple
ion pairing
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

22. Nonmetals are good _____ agents. Metals are good _______ agents.
Tetrahedral
ClO2?
Acid rain - dissolves marble buildings/statues and kills trees.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

23. The oxidation # for acid base reactions...
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
catalyst=conc H2SO4
do not change
They decrease (or could be the same if the solid has ONLY JUST disappeared)

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

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25. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
H2O + CO2 (it decomposes readily)
How close results are to the accepted value
by electrolysis
Ksp = 108s5

26. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
The dilution effect when the solutions mix. M1V1 = M2V2
The one with most oxygen atoms (highest oxidation number)
Q=It (time in seconds)
Decant

27. What is the formula of butane?
Soluble
no - they're written undissociated (HAaq)
C4H10
yellow

28. What is the general formula for an acid?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
RCOOH
Cu3(PO4)2
Time?¹ - (ex. s?¹ - hr?¹ - etc)

29. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
yellow
Initiation energy (NOT Ea)
Heptane

30. perchlorate
How close results are to the accepted value
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
ClO4?
diamond and graphite

31. What should you check for before you begin titrating?
a-IMFs - b-molecular volume
Check for air bubbles in the buret and remove the buret funnel from the buret
bright yellow
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

32. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Graduated cylinder
CrO4²?
At half equivalence - pH=pKa
Soluble except Ag - Pb - Ca - Sr Ba)

33. chlorate
ClO3?
Filtration
Pale yellow
small size and high charge

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

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35. What is the test for hydrogen?
Q=It (time in seconds)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
boiling without losing volatile solvents/reactants
lighted splint (positive result=pop)

36. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
MnO4?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
catalyst=conc H2SO4

37. What are amphoteric oxides?
metal oxides and hydrides are ionically bonded and basic
zero
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?)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

38. What are the names and formulas of the 6 strong acids?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
CnH2n
are less dense than water

39. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Anode - oxygen. Cathode - hydrogen
acid + alcohol
Separating funnel
Decant

40. What does the solubility of organic compounds depend on?
No - NH3 and HCl gases are extremely soluble
Soluble
CN?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

41. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
Salt + water
Pipette (burette if need repetition)
Anode - oxygen. Cathode - hydrogen

42. ammonium
NH4?
acids
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
?H formation of an element in standard state=0

43. chlorine
acid + alcohol
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
Anode - oxygen. Cathode - hydrogen
Greenish-yellow gas

44. Name 2 ways in which you can create a buffer?
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)
acids
Conjugate pair (one must be a weak base or acid)
NH4?

45. What are two allotropes of carbon?
proton acceptor.
diamond and graphite
Anode - oxygen. Cathode - hydrogen
Ksp = 27s4

46. Is the standard entropy (S°) of an element zero?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
But S° of element is not zero (except at 0K)
H2PO4?

47. Do you use J or kJ for ?H - ?S - and ?G?
ClO2?
?H-kJ - ?S-J - ?G-kJ
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)
ionic and form hydrogen and hydroxide

48. Why are noble gases stable?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Sigma bonds are stronger than pi bonds
#ligands=charge x2
Add acid to water so that the acid doesn't boil and spit

49. nitrate
H2O + CO2 (it decomposes readily)
Insoluble
NO3?
Kc=Kp

50. What is the formula for summation?

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