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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. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
RCOOH
Hg²?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

2. What are the signs of ?G and E° for spontaneous reactions?
H3PO4
ClO?
voltaic: + electrolytic: -
?G=negative - E° must be positive

3. Are weak acids (and bases) written dissociated?

4. Does reactivity increase/decrease going down group 1 and group 17?
by electrolysis
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Increases down group 1 decreases down group 17
it's lower and occurs over less sharp a range

5. What is an Alkyl group?

6. Name 2 ways in which you can create a buffer?
RNH2
White precipitate
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)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

7. What are allotropes?
Clear
different forms of the same element
O2 needs 4F/mol H2 needs 2F/mol
ROR

8. Why are noble gases stable?
Unsaturated - addition (ex: decolorize bromine solution)
S2O3²?
Q=It (time in seconds)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

9. permanganate
Insoluble except for nitrate and acetate
MnO4?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Most INsoluble except group 1 and ammonium

10. What is the difference between equivalence point and end point of a titration.
C2O4²?
O2 needs 4F/mol H2 needs 2F/mol
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
Iodine and CO2 (dry ice)

11. 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!
voltaic: - electrolytic: +
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Synthetic condensation polymer (aka a polyamide)

12. What do metal oxides plus non- metal oxides form?
Combine the equations for the half reactions in the non-spontaneous direction
yellow
Salts (ex: CaO + SO2 ? CaSO3)
red - green - blue

13. What is the general formula for a ketone?
MnO4?
RCOR
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
CnH(2n+2)

14. BaSO4
Group 1 hydroxides (ex: NaOH)
Graduated cylinder
Kc=Kp
Insoluble

15. What do hydrocarbons form when they burn in air (oxygen)?
CO2 and H2O
Both electrons come from the same atom (just as good as a regular bond)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
benzene has a delocalized pi ring structure

16. A Bronsted-Lowry acid is...
Disulfur dichloride
voltaic: - electrolytic: +
K1 x K2
proton donor base

17. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
H3PO4
Anode - oxygen. Cathode - hydrogen
Acids; HCOOCH3 is an ester
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

18. carbonates
red - green - blue
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
OH- and NH3
Insoluble except group 1 and ammonium

19. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
?G=negative - E° must be positive
They stay the same.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Exothermic

20. What process do you use to obtain the solute from a solution?
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)
Evaporation
-Ea/R
Saturated - Substitution (which requires more radical conditions)

21. What do you use for an acid spill? base spill?
non-metal oxides and hydrides are covalently bonded and are acidic.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
A) any range. b) 8-10 c) 4-6
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)

22. If a free element is involved - what type of reaction must be involved?
redox reaction
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
diamond and graphite
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

23. Ions are not ______.
atoms
bent
Most INsoluble except group 1 and ammonium
ns² electrons (first in-first out)

24. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
Hg2²?
P2O5
CnH2n-2
Ksp = 27s4

25. chromate ion (soln + most solids)
Identity and purity (impure compounds usually have broad & low melting points)
Perform ICE BOX calculation based on K1
yellow
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

26. What process do you use to separate two liquids with different boiling points?
?G=negative - E° must be positive
same KE - but PEice<PEwater
fractional distillation
[A?]/[HA] x 100 or [BH?]/[B] x 100

27. ________ are Lewis bases - because they can donate a lone pair of electrons.
OH- and NH3
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Synthetic condensation polymer (aka a polyamide)
Ksp = s²

28. What are the signs for ?G and E° for spontaneous reactions?
red - green - blue
?G= -ve - E°= +ve
Tetrahedral
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.

29. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
CO (poisonous)
A salt solution.
Heat a test tube at an angle at the side of the tube (not bottom)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

30. What process do you use to obtain a solvent from a solution?
do not change
Distillation
How grouped results are
CnH(2n+2)

31. chlorine
Q=It (time in seconds)
Kc=Kp
red - green - blue
Greenish-yellow gas

32. What shape is carbon dioxide?
Experimental mass/theoretical mass X 100
bent
Greenish-yellow gas
linear

33. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
Exothermic
fruit - fish - bases
S crystal at 0K=0

34. Do you use J or kJ for ?H - ?S - and ?G?
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.
ClO?
Graduated cylinder
?H-kJ - ?S-J - ?G-kJ

35. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
q=mc?T q=mL (or n x ?h)
same KE - but PEice<PEwater
red - green - blue

36. How does benzene compare in reactivity to alkenes?
Ksp = 27s4
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
bases
benzene is less reactive than alkenes

37. What reacts with an acid to create hydrogen gas?
An active metal.
Group 1 hydroxides (ex: NaOH)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Anode

38. What is the formula of copper (II) phosphate?
Exothermic
R=8.31 J/mol/K
Cu3(PO4)2
?H formation of an element in standard state=0

39. hydroxide
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
No - it depends on the number of ions produced on dissolving.
blue
OH?

40. Give an example of a dilute strong acid.
Ionic compounds
HClO4
#ligands=charge x2
Salt and water

41. Nonmetals are good _____ agents. Metals are good _______ agents.
Pale yellow
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
blue (BTB)
it reacts by substitution NOT addition

42. What is the conjugate base of NH3?
yellow
Glacial acetic acid
Conjugate pair (one must be a weak base or acid)
NH2?

43. If Q > Ksp - then system shifts _______ and ppt ______
OH?
ethers
left - ppt will form
R=8.31 J/mol/K

44. What apparatus do you use to separate 2 immiscible liquids?
Q=It (time in seconds)
-Ea/R
S crystal at 0K=0
Separating funnel

45. What is the formula for obtaining charge flowing in a cell?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Q=It (time in seconds)
blue
Synthesis - separation and purification of the product and its identification.

46. What is the formula for percent error?
How grouped results are
bent
|experimental - accepted|/accepted X 100
Hg²?

47. sulfates
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
strong acids/bases are written as H+ or OH- ions
Kc=Kp
Soluble except Ag - Pb - Ca - Sr Ba)

48. silver compounds
blue
Insoluble except for nitrate and acetate
Separating funnel
Hg²?

49. mercury (II) ion
Sigma bonds are stronger than pi bonds
RCHO (carbonyl at end)
Hg²?
S crystal at 0K=0

50. What is the second law of thermodynamics?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
blue
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Suniverse increases for spontaneous processes