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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 relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
acid + alcohol
More chaotic (ex: gases made)
ClO3?

2. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Big K=kf/kr
zero
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Iodine and CO2 (dry ice)

3. What is the formula for summation?

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4. ________ are Lewis bases - because they can donate a lone pair of electrons.
Suniverse increases for spontaneous processes
CN?
OH- and NH3
K2

5. What are two substances that sublime at 1 atm when heated?
by electrolysis
?H-kJ - ?S-J - ?G-kJ
linear
Iodine and CO2 (dry ice)

6. Esterification is...
Insoluble except nitrate and acetate
acid + alcohol
But S° of element is not zero (except at 0K)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

7. What is the first law of thermodynamics?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
E=q + w (negative is by system - positive is on system)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
are less dense than water

8. Does reactivity increase/decrease going down group 1 and group 17?
+4-covalent - +2-ionic
Increases down group 1 decreases down group 17
Making sigma bonds and holding lone pairs
Insoluble except group 1 and ammonium

9. Do you use J or kJ for ?H - ?S - and ?G?
q=mc?T q=mL (or n x ?h)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
?H-kJ - ?S-J - ?G-kJ
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?)

10. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
small size and high charge
neutralization: high K - H2O product dissociation: low K - H2O reactant
are less dense than water
it reacts by substitution NOT addition

11. How are strong ones written?
allow for the vapor pressure of water and make sure to level levels
Current - time and charge on ion (moles of e used in half cell reaction)
strong acids/bases are written as H+ or OH- ions
Most INsoluble except group 1 and ammonium

12. What do the 'a' and 'b' in Van Der Waal's equation allow for?
All except for lithium
a-IMFs - b-molecular volume
Pour liquids using a funnel or down a glass rod
Soluble

13. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Acid rain - dissolves marble buildings/statues and kills trees.
allow for the vapor pressure of water and make sure to level levels
It ceases - the circuit is broken.

14. What changes Keq?
Only temperature
P2O5
linear
S crystal at 0K=0

15. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Most are soluble except Ag - Pb
RCHO (carbonyl at end)
same KE - but PEice<PEwater

16. copper sulfate
proton acceptor.
blue
yellow
S2O3²?

17. carbonates
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
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Insoluble except group 1 and ammonium

18. What does a short - sharp melting point indicate?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
CnH2n-2
Identity and purity (impure compounds usually have broad & low melting points)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

19. What do you use for an acid spill? base spill?
Salt and water
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Synthetic condensation polymer (aka a polyamide)

20. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
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)
bases
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

21. What do you do to get rid of most of the solution from a precipitate?
Hg2²?
ClO?
Decant
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

22. What is the formula of copper (II) phosphate?
Sulfur
CH3COO?
Cu3(PO4)2
CO3²?

23. What shape is water?
NO3?
Soluble
bent
How grouped results are

24. permanganate
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Ksp = s²
RCOOH
MnO4?

25. Colorless doesn't mean ______
Increases down group 1 decreases down group 17
Insoluble except for nitrate and acetate
Clear
Soluble

26. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
Iodine and CO2 (dry ice)
Pale purple - (orange)-yellow - red - blue - green.
diamond and graphite

27. mercury (I) ion
H+
Hg2²?
Current - time and charge on ion (moles of e used in half cell reaction)
Nothing

28. How does half life change for zero-th order - first order - and second order processes?
hydroxides (ex: Ba(OH)2)
zero-th: decreases - first: constant - second: increases
are less dense than water
left - ppt will form

29. How do you get Ecell for spontaneous reactions?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
0 and 14
ethers
hydroxides (ex: Ba(OH)2)

30. At what point during titration do you have the perfect buffer - and what is the pH at this point?
CrO4²?
At half equivalence - pH=pKa
No - it depends on the number of ions produced on dissolving.
ClO4?

31. What part of a liquid do you look at to measure its volume?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
C4H10
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Read the bottom of the meniscus

32. What do you use to look at burning magnesium? why?
Heptane
SO4²?
blue glass - it filters UV
Suniverse increases for spontaneous processes

33. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
S2O3²?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Sulfur
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

34. mercury (II) ion
Cu3(PO4)2
+4-covalent - +2-ionic
Hg²?
Decant

35. Which of the rates changes more when temperature is increased?
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)
Cu3(PO4)2
zero
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

36. If Q > Ksp - then system shifts _______ and ppt ______
look for changes in oxidation # - the one that goes up is oxidized and is the RA
left - ppt will form
?G= -ve - E°= +ve
CrO4²?

37. What two compounds are great oxidizing agents?

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38. Nonmetals are good _____ agents. Metals are good _______ agents.
small size and high charge
'non-active' metals such as Cu - Ag - Au - Pt - etc.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
The benzene ring (or more correctly the phenyl group - C6H5)

39. What two types of substances are present in all redox reactions?
OH- and NH3
benzene has a delocalized pi ring structure
ion pairing
an oxidized and reduced substance

40. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
voltaic: - electrolytic: +
Concentration
same KE - but PEice<PEwater
an oxidized and reduced substance

41. Where are group I metals stored?
atoms
Salt + water
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Group I metals (soft metals) are stored under oil

42. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 27s4
Soluble except Ag - Pb - Ca - Sr Ba)
Ksp = 4s³
red - green - blue

43. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Sigma bonds are stronger than pi bonds
Soluble
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

44. How does the melting point of a mixture compare to the MP of a pure substance?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
it is lower and occurs over less sharp a range
Conjugate pair (one must be a weak base or acid)
blue (BTB)

45. What is the pH of 1.0M HCl? 1M NaOH?
P2O5
ROR
0 and 14
Only temperature

46. What are the formulas for q?
RCOR
Molecules with the same molecular formulas - but different structural formulas
q=mc?T q=mL (or n x ?h)
Filtration

47. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
brown volatile liquid
PO4³?
proton donor base

48. What type of solutions do small - highly charged cations tend to form?
S2O3²?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
catalyst=conc H2SO4
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

49. Alkanes are _________ and react by _________
10?8
Soluble
Saturated - Substitution (which requires more radical conditions)
Insoluble except group 1 and ammonium

50. What is the formula for obtaining charge flowing in a cell?
No - it depends on the number of ions produced on dissolving.
10?8
Iodine and CO2 (dry ice)
Q=It (time in seconds)