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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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. Colorless doesn't mean ______
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Clear
neutralization: high K - H2O product dissociation: low K - H2O reactant
CnH2n-2

2. What do hydrocarbons form when they burn in air (oxygen)?
CO2 and H2O
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
CnH2n+1 often designated 'R' ex C3H7 is propyl
acid + alcohol

3. What is the general formula for an aldehyde?
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)
CnH2n+2
RCHO (carbonyl at end)
H3PO4

4. Is the freezing of ice endothermic or exothermic?
Increases down group 1 decreases down group 17
Heptane
Exothermic
ns² electrons (first in-first out)

5. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
They stay the same.
lighted splint (positive result=pop)
The dilution effect when the solutions mix. M1V1 = M2V2
S crystal at 0K=0

6. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Both electrons come from the same atom (just as good as a regular bond)
?H formation of an element in standard state=0
CH3COO?

7. Does Kw increase or decrease with T? Why?
ion pairing
Eudiometer
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Current - time and charge on ion (moles of e used in half cell reaction)

8. What are amphoteric oxides?
catalyst=conc H2SO4
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?)
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.
yellow

9. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Acidified
RCOOH
K1 x K2
Synthetic condensation polymer (aka a polyamide)

10. What are the products of the reaction between group 1 metals and water?

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11. What is accuracy?
How close results are to the accepted value
?G= -ve - E°= +ve
fruit - fish - bases
Pale purple - (orange)-yellow - red - blue - green.

12. hydroxides
neutralization: high K - H2O product dissociation: low K - H2O reactant
Insoluble (except group 1 ammonium and Ba)
Identity and purity (impure compounds usually have broad & low melting points)
0 and 14

13. What is the third law of thermodynamics?
proton acceptor.
same KE - but PEice<PEwater
S crystal at 0K=0
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

14. What are allotropes?
RCHO (carbonyl at end)
different forms of the same element
|experimental - accepted|/accepted X 100
[A?]/[HA] x 100 or [BH?]/[B] x 100

15. What do metal oxides plus acids form?
Salt + water
Increases.
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

16. How many normal boiling points and boiling points are there?

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17. What steps do organic labs consist of?
NO3?
Synthesis - separation and purification of the product and its identification.
Ksp = 108s5
atoms

18. thiosulfate
benzene is less reactive than alkenes
S2O3²?
by electrolysis
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

19. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Pale yellow
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
red - green - blue
voltaic: + electrolytic: -

20. What things should you remember to do when collecting gas over water?
Exothermic
CnH2n
allow for the vapor pressure of water and make sure to level levels
Filtration

21. What type of compounds do metals/non metals form?
Filtration
Insoluble except group 1 and ammonium
Ionic compounds
Heptane

22. What is the basic structure of an optical isomer?
Orange
blue (BTB)
Experimental mass/theoretical mass X 100
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

23. What is the sign of the anode in voltaic cells? in electrolytic cells?
Graduated cylinder
voltaic: - electrolytic: +
An active metal.
Salt + water

24. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
C2O4²?
proton acceptor.
NO3?

25. What type of compounds do Group 14 form?
Soluble
left - ppt will form
+4-covalent - +2-ionic
Salt and water

26. What are the signs of ?G and E° for spontaneous reactions?
Unsaturated - addition (ex: decolorize bromine solution)
brown volatile liquid
SO4²?
?G=negative - E° must be positive

27. What electrons are lost/gained first in transition element ions?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
ns² electrons (first in-first out)
Soluble
?G=negative - E° must be positive

28. silver compounds
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Insoluble except for nitrate and acetate
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Add acid to water so that the acid doesn't boil and spit

29. dichromate (soln + most solids)
Orange
S crystal at 0K=0
Silvery gray solid - brown - purple
An active metal.

30. Why are i factors (Van't Hoff factors) often less than ideal?
Silvery gray solid - brown - purple
ion pairing
More chaotic (ex: gases made)
+4-covalent - +2-ionic

31. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
CnH2n+1 often designated 'R' ex C3H7 is propyl
H2O + CO2 (it decomposes readily)
The benzene ring (or more correctly the phenyl group - C6H5)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

32. What equipment do you need for a titration?
H3PO4
no - they're written undissociated (HAaq)
SO4²?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

33. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Pale yellow
Synthesis - separation and purification of the product and its identification.
At half equivalence - pH=pKa

34. Name six characteristics of transition elements (or their compounds)
Group 1 hydroxides (ex: NaOH)
CnH2n+2
K1 x K2
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)

35. What process do you use to obtain the precipitate from a solution?
O2 needs 4F/mol H2 needs 2F/mol
SO4²?
CH3COO?
Filtration

36. What are the signs for ?G and E° for spontaneous reactions?
Molecules with the same molecular formulas - but different structural formulas
Soluble
?G= -ve - E°= +ve
Reduction always takes place at the cathode (RED CAT) In both types of cell!

37. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
The benzene ring (or more correctly the phenyl group - C6H5)
The Faraday or Faraday's constant.
ClO2?

38. How does benzene compare in reactivity to alkenes?
Perform ICE BOX calculation based on K1
benzene is less reactive than alkenes
Increases down group 1 decreases down group 17
it reacts by substitution NOT addition

39. What is the formula of butane?
Cu3(PO4)2
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
C4H10
NH4?

40. What is the formula of copper (II) phosphate?
Cu3(PO4)2
It ceases - the circuit is broken.
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)
Increases down group 1 decreases down group 17

41. What are isotopes?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

42. What shape is methane?
Q=It (time in seconds)
ClO2?
Tetrahedral
basic

43. What things should you remember to do when collecting gas over water?
proton donor base
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
allow for the vapor pressure of water and make sure to level levels

44. phosphates
Pipette (burette if need repetition)
Ppt will NOT form (unsaturated)
Most INsoluble except group 1 and ammonium
OH- and NH3

45. chlorine
?G= -ve - E°= +ve
Greenish-yellow gas
it reacts by substitution NOT addition
different forms of the same element

46. carbonates
different forms of the same element
Insoluble except group 1 and ammonium
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

47. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
RCOOR
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

48. BaSO4
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Acid rain - dissolves marble buildings/statues and kills trees.
Insoluble
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

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

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50. What is the general formula for an amine?
RNH2
S2O3²?
acid + alcohol
0.10M HCl (more ions)