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. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
The compound with the lowest Ksp value.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
CO (poisonous)

2. silver iodide
diamond and graphite
Ksp = s²
fruit - fish - bases
Pale yellow

3. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
But S° of element is not zero (except at 0K)
H+
fruit - fish - bases

4. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
red - green - blue
Soluble
OH?

5. lead iodide
Insoluble except nitrate and acetate
Greenish-yellow gas
bright yellow
Ions go through the salt bridge - electrons go through metal wires in the external circuit

6. How do you identify which is oxidized or otherwise?
NH4?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
q=mc?T q=mL (or n x ?h)
Heptane

7. Why are noble gases stable?
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)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Ionic compounds
Ions go through the salt bridge - electrons go through metal wires in the external circuit

8. Lattice energy is high for ions with _____ size and _____ charge
Purple
small size and high charge
do not change
?H formation of an element in standard state=0

9. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Ksp = s²
red - green - blue

10. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
ion pairing
Current - time and charge on ion (moles of e used in half cell reaction)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

11. Name 2 ways in which you can create a buffer?
?H-kJ - ?S-J - ?G-kJ
K1 x K2
Time?¹ - (ex. s?¹ - hr?¹ - etc)
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)

12. What process do you use to separate two liquids with different boiling points?
Salt + water.
H2O + CO2 (it decomposes readily)
fractional distillation
CO2 and H2O

13. What do metal oxides plus acids form?
Salt + water
lighted splint (positive result=pop)
brown volatile liquid
Heptane

14. What is accuracy?
Greenish-yellow gas
All except for lithium
How close results are to the accepted value
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

15. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Glacial acetic acid
Salt + water

16. Colorless doesn't mean ______
Soluble
Clear
Salt + water.
Ksp = s²

17. bromine
A salt solution.
Soluble
Nothing
brown volatile liquid

18. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
All except for lithium
basic
CnH2n+2

19. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Insoluble except for nitrate and acetate
water and substances with (s) less dense than
bright yellow
Only temperature

20. How do you compute % dissociation?
T increases exponentially the proportion of molecules with E > Ea
[A?]/[HA] x 100 or [BH?]/[B] 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.
|experimental - accepted|/accepted X 100

21. What is the formula for obtaining charge flowing in a cell?
Add acid to water so that the acid doesn't boil and spit
Q=It (time in seconds)
CnH(2n+2)
It ceases - the circuit is broken.

22. What are the units of the first order rate constant?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
CO (poisonous)
Perform ICE BOX calculation based on K1
Time?¹ - (ex. s?¹ - hr?¹ - etc)

23. How does the melting point of a mixture compare to the MP of a pure substance?
Soluble
'non-active' metals such as Cu - Ag - Au - Pt - etc.
it is lower and occurs over less sharp a range
ethers

24. Why are i factors (Van't Hoff factors) often less than ideal?
lighted splint (positive result=pop)
proton acceptor.
ion pairing
benzene has a delocalized pi ring structure

25. dihydrogen phosphate
C4H10
H2PO4?
water and substances with (s) less dense than
No - NH3 and HCl gases are extremely soluble

26. If a free element is involved - what type of reaction must be involved?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
blue
redox reaction
MnO4?

27. Do you use J or kJ for ?H - ?S - and ?G?
CnH2n+2
voltaic: + electrolytic: -
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
?H-kJ - ?S-J - ?G-kJ

28. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
No - it depends on the number of ions produced on dissolving.
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
Ksp = s²
Eudiometer

29. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
Glacial acetic acid
CnH2n+1 often designated 'R' ex C3H7 is propyl
NO3?

30. When the salt bridge is removed what happens to the cell reaction?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
It ceases - the circuit is broken.
acids
ClO4?

31. Both Acetic acid and ____________ are also functional isomers.
fractional distillation
'non-active' metals such as Cu - Ag - Au - Pt - etc.
methyl formate
proton acceptor.

32. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Sulfur

33. Do anions flow to the cathode or anode?
Anode
OH?
ClO2?
ethers

34. What causes the dramatic effect of T on rate?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
basic
Glacial acetic acid
T increases exponentially the proportion of molecules with E > Ea

35. One mole of electrons carries 96500Coulombs - what is this quantity called?

36. During a titration what is present in the beaker at the equivalence point?
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
Glowing splint (positive result=relights)
A salt solution.
RCOOR

37. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
diamond and graphite
|experimental - accepted|/accepted X 100
Group 1 hydroxides (ex: NaOH)

38. What is the third law of thermodynamics?
Iodine and CO2 (dry ice)
OH?
voltaic: + electrolytic: -
S crystal at 0K=0

39. How are more active metals reduced?
by electrolysis
Nothing
water and substances with (s) less dense than
voltaic: - electrolytic: +

40. What is the test for hydrogen?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Salt and water
lighted splint (positive result=pop)
non-metal oxides and hydrides are covalently bonded and are acidic.

41. What do ions and electrons travel through in a voltaic/electrolytic cell?
Greenish-yellow gas
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Ions go through the salt bridge - electrons go through metal wires in the external circuit

42. chlorite
metal oxides and hydrides are ionically bonded and basic
Insoluble except nitrate and acetate
ClO2?
proton acceptor.

43. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
CnH2n
zero
q=mc?T q=mL (or n x ?h)
Q=It (time in seconds)

44. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Read the bottom of the meniscus

45. What do you use for an acid spill? base spill?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Pale purple - (orange)-yellow - red - blue - green.
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

46. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Synthetic condensation polymer (aka a polyamide)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

47. Acid plus base make?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Hg²?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Salt + water.

48. Why are i factors (Van't Hoff factors) often less than ideal?
lighted splint (positive result=pop)
Acidified
ion pairing
CO2 and H2O

49. iodine - iodine solution - iodine vapor
OH?
Silvery gray solid - brown - purple
bent
K2

50. cyanide
Trigonal pyramidal
Pour liquids using a funnel or down a glass rod
CN?
brown volatile liquid