Test your basic knowledge |

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. How can metals like iron and zinc be reduced?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
chemically (ex: with carbon)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
|experimental - accepted|/accepted X 100

2. What are the signs for ?G and E° for spontaneous reactions?
PO4³?
CH3COO?
strong acids/bases are written as H+ or OH- ions
?G= -ve - E°= +ve

3. chlorate
blue glass - it filters UV
ClO3?
Ksp = 27s4
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

5. acetate
different forms of the same element
CH3COO?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
CrO4²?

6. chlorite
ClO2?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
OH?
Soluble

7. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
allow for the vapor pressure of water and make sure to level levels
Identity and purity (impure compounds usually have broad & low melting points)
q=mc?T q=mL (or n x ?h)
The compound with the lowest Ksp value.

8. What is the general formula of an alkane?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
CnH(2n+2)
RNH2
10?8

9. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
redox reaction
Ksp = 27s4
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
P2O5

10. Ca - Sr - Ba
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.
ionic and form hydrogen and hydroxide
hydroxides (ex: Ba(OH)2)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

11. 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.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
no - they're written undissociated (HAaq)
ROH
A) any range. b) 8-10 c) 4-6

12. perchlorate
CN?
Pipette (burette if need repetition)
same KE - but PEice<PEwater
ClO4?

13. hypochlorite
CN?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Distillation
ClO?

14. What is the formula for alkenes?
Ppt will NOT form (unsaturated)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
CnH2n

15. What electrons are lost/gained first in transition element ions?
Iodine and CO2 (dry ice)
ns² electrons (first in-first out)
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)
RX

16. Acid plus base make?
Salt + water.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
No - it depends on the number of ions produced on dissolving.

17. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
do not change
RNH2
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Most are soluble except Ag - Pb

18. Ions are not ______.
Glowing splint (positive result=relights)
atoms
do not change
Evaporation

19. What type of compounds do Group 14 form?
q=mc?T q=mL (or n x ?h)
blue
+4-covalent - +2-ionic
ClO3?

20. If ?S is positive - are the products more or less chaotic than the reactants?
Salt + water
ClO2?
A salt solution.
More chaotic (ex: gases made)

21. What are hybrid orbitals used for?
CnH2n+1 often designated 'R' ex C3H7 is propyl
a-IMFs - b-molecular volume
No - it depends on the number of ions produced on dissolving.
Making sigma bonds and holding lone pairs

22. What type of solutions do small - highly charged cations tend to form?
different forms of the same element
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
NH4?

23. What reacts with an acid to create hydrogen gas?
An active metal.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
T increases exponentially the proportion of molecules with E > Ea

24. How do you compute % dissociation?
CH3COO?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
[A?]/[HA] x 100 or [BH?]/[B] x 100
small size and high charge

25. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Insoluble except nitrate and acetate
Q=It (time in seconds)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

26. What are the signs of ?G and E° for spontaneous reactions?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
S crystal at 0K=0
ion pairing
?G=negative - E° must be positive

27. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Pale purple - (orange)-yellow - red - blue - green.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Insoluble except group 1 and ammonium

28. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
H2O + CO2 (it decomposes readily)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
no - they're written undissociated (HAaq)
Salt + water.

29. What is the difference between equivalence point and end point of a titration.
CnH(2n+2)
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
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
same KE - but PEice<PEwater

30. What is the general formula for a ketone?
More chaotic (ex: gases made)
it is lower and occurs over less sharp a range
All except for lithium
RCOR

31. carbonate
CO3²?
a-IMFs - b-molecular volume
The benzene ring (or more correctly the phenyl group - C6H5)
ClO?

32. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Anode - oxygen. Cathode - hydrogen
No - NH3 and HCl gases are extremely soluble
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Ksp = 4s³

33. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
Evaporation
No - NH3 and HCl gases are extremely soluble
Group I metals (soft metals) are stored under oil

34. Aromatic compounds contain what?
Heat a test tube at an angle at the side of the tube (not bottom)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
blue
The benzene ring (or more correctly the phenyl group - C6H5)

35. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
Most are soluble except Ag - Pb
Hg2²?
Ksp = s²

36. nitrate
lighted splint (positive result=pop)
NO3?
NH2?
benzene is less reactive than alkenes

37. How do you heat a test tube?
The Faraday or Faraday's constant.
Heat a test tube at an angle at the side of the tube (not bottom)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
RNH2

38. What is precision?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
K2
How grouped results are
OH- and NH3

39. What element is used to vulcanize rubber?
MnO4?
Salt and water
Sulfur
NH4?

40. silver iodide
ROR
H+
How grouped results are
Pale yellow

41. What is a coordinate covalent bond?
OH- and NH3
A) any range. b) 8-10 c) 4-6
Insoluble
Both electrons come from the same atom (just as good as a regular bond)

42. What is the general formula for an alcohol?
ROH
boiling without losing volatile solvents/reactants
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Conjugate pair (one must be a weak base or acid)

43. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Insoluble
K1 x K2

44. What type of compounds do metals/non metals form?
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)
How grouped results are
Ionic compounds
left - ppt will form

45. How are more active metals reduced?
Group I metals (soft metals) are stored under oil
by electrolysis
The benzene ring (or more correctly the phenyl group - C6H5)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

46. What are two allotropes of carbon?
ClO3?
diamond and graphite
Sulfur
Add acid to water so that the acid doesn't boil and spit

47. Esterification is...
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
acid + alcohol
do not change
E=q + w (negative is by system - positive is on system)

48. Both Acetic acid and ____________ are also functional isomers.
brown volatile liquid
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Big K=kf/kr
methyl formate

49. Alkanes are _________ and react by _________
C4H10
Saturated - Substitution (which requires more radical conditions)
Read the bottom of the meniscus
Graduated cylinder

50. When driving off water from a hydrate - how do you tell you're done?
ClO3?
blue
K2
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant