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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 things should you remember to do when collecting gas over water?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
methyl formate
allow for the vapor pressure of water and make sure to level levels
Increases down group 1 decreases down group 17

2. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
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)
Selective absorption
NO3?

3. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
How close results are to the accepted value
The compound with the lowest Ksp value.
same KE - but PEice<PEwater
Iodine and CO2 (dry ice)

4. What do you need to make a polymer?
it reacts by substitution NOT addition
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)
Greenish-yellow gas
Acid rain - dissolves marble buildings/statues and kills trees.

5. Name some properties of Group 17
?H-kJ - ?S-J - ?G-kJ
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
0.10M HCl (more ions)
Heptane

6. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
Glacial acetic acid
Increases down group 1 decreases down group 17
redox reaction

7. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
Disulfur dichloride
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Perform ICE BOX calculation based on K1

8. Give an example of a dilute strong acid.
RCOR
H3PO4
HClO4
Orange

9. cyanide
methyl formate
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
CN?
0 and 14

10. How does group 1 metals' density compare to water's?
are less dense than water
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
-Ea/R
?H formation of an element in standard state=0

11. chlorate
Add acid to water so that the acid doesn't boil and spit
Sigma bonds are stronger than pi bonds
look for changes in oxidation # - the one that goes up is oxidized and is the RA
ClO3?

12. What shape is carbon dioxide?
voltaic: - electrolytic: +
linear
Unsaturated - addition (ex: decolorize bromine solution)
SO4²?

13. Does reactivity increase/decrease going down group 1 and group 17?
H+
Increases down group 1 decreases down group 17
Hg2²?
ClO?

14. How do you dilute an acid?

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15. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
metal oxides and hydrides are ionically bonded and basic
same KE - but PEice<PEwater
redox reaction

16. What is the formula for alkenes?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Cu3(PO4)2
H2O + CO2 (it decomposes readily)
CnH2n

17. What steps do organic labs consist of?
|experimental - accepted|/accepted X 100
Synthesis - separation and purification of the product and its identification.
ClO3?
Trigonal pyramidal

18. What does a short - sharp melting point indicate?
?H formation of an element in standard state=0
voltaic: - electrolytic: +
acids
Identity and purity (impure compounds usually have broad & low melting points)

19. What device would you use to measure a volume of gas?
Mn²? - Cr³? - Cr³
atoms
Eudiometer
Salt + water.

20. What equipment do you need for a titration?
metal oxides and hydrides are ionically bonded and basic
They stay the same.
?H-kJ - ?S-J - ?G-kJ
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

21. Name six characteristics of transition elements (or their compounds)
same KE - but PEice<PEwater
Silvery gray solid - brown - purple
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)
fruit - fish - bases

22. 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.
A) any range. b) 8-10 c) 4-6
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
left - ppt will form
ClO2?

23. What is the general formula for an ether?
The benzene ring (or more correctly the phenyl group - C6H5)
ns² electrons (first in-first out)
The dilution effect when the solutions mix. M1V1 = M2V2
ROR

24. What is the difference between equivalence point and end point of a titration.
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
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
CH3COO?
Filtration

25. Neutralization is an ________ reaction.
it is lower and occurs over less sharp a range
NO3?
Soluble
Exothermic (?H for ANY sa/sb = -57kJ/mol)

26. What is a dipeptide? polypeptide? protein?
Ksp = s²
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
|experimental - accepted|/accepted X 100

27. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Add acid to water so that the acid doesn't boil and spit
Big K=kf/kr
K1 x K2

28. Why are i factors (Van't Hoff factors) often less than ideal?
Mn²? - Cr³? - Cr³
Conjugate pair (one must be a weak base or acid)
Mono; di; tri; tetra; penta; hexa.
ion pairing

29. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
allow for the vapor pressure of water and make sure to level levels

30. Which alkali metals float on water?
q=mc?T q=mL (or n x ?h)
All except for lithium
Graduated cylinder
CnH2n+1 often designated 'R' ex C3H7 is propyl

31. chlorine
The dilution effect when the solutions mix. M1V1 = M2V2
Selective absorption
Greenish-yellow gas
OH- and NH3

32. What is an Alkyl group?

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

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34. Colorless doesn't mean ______
zero-th: decreases - first: constant - second: increases
Salt and water
Clear
Purple

35. What is the general formula for an aldehyde?
No - it depends on the number of ions produced on dissolving.
Glowing splint (positive result=relights)
RCHO (carbonyl at end)
Hg²?

36. What are the units of the first order rate constant?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

37. What do group I/II metal oxides plus water form?
Molecules with the same molecular formulas - but different structural formulas
They stay the same.
benzene has a delocalized pi ring structure
bases

38. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
lighted splint (positive result=pop)
ClO4?
Making sigma bonds and holding lone pairs

39. How do you identify which is oxidized or otherwise?
water and substances with (s) less dense than
look for changes in oxidation # - the one that goes up is oxidized and is the RA
CnH2n+1 often designated 'R' ex C3H7 is propyl
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.

40. How do you compute % dissociation?
Current - time and charge on ion (moles of e used in half cell reaction)
Anode
[A?]/[HA] x 100 or [BH?]/[B] x 100
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

41. How are metal oxides and hydrides bonded? are they acidic or basic?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Cu3(PO4)2
Insoluble except nitrate and acetate
metal oxides and hydrides are ionically bonded and basic

42. nitrate
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
ionic and form hydrogen and hydroxide
?H formation of an element in standard state=0
NO3?

43. How do you get Ecell for spontaneous reactions?
CnH2n+2
Soluble
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
#ligands=charge x2

44. What is the general formula for an amine?
Salt + water
Evaporation
Greenish-yellow gas
RNH2

45. Esterification is...
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
RCOOR
acid + alcohol
Sigma bonds are stronger than pi bonds

46. nitrates
Soluble
|experimental - accepted|/accepted X 100
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

47. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
OH- and NH3
no - they're written undissociated (HAaq)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

48. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
do not change
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
No - it depends on the number of ions produced on dissolving.
zero

49. What is the slope of the graph of lnk vs. 1/T?
O2 needs 4F/mol H2 needs 2F/mol
-Ea/R
Pour liquids using a funnel or down a glass rod
Add acid to water so that the acid doesn't boil and spit

50. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
a-IMFs - b-molecular volume
RCHO (carbonyl at end)
Iodine and CO2 (dry ice)