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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. Color (absorbance) is proportional to ________
Concentration
The compound with the lowest Ksp value.
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.
They decrease (or could be the same if the solid has ONLY JUST disappeared)

2. Which of the rates changes more when temperature is increased?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Pour liquids using a funnel or down a glass rod

3. Name 2 ways in which you can create a buffer?
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)
Pour liquids using a funnel or down a glass rod
RNH2
basic

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

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5. A Bronsted-Lowry base is...
zero-th: decreases - first: constant - second: increases
Pour liquids using a funnel or down a glass rod
An active metal.
proton acceptor.

6. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Q=It (time in seconds)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

7. How do you heat a test tube?
Evaporation
K2
Heat a test tube at an angle at the side of the tube (not bottom)
Eudiometer

8. What do group I/II metal oxides plus water form?
SO4²?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
bases
Ksp = 27s4

9. What shape is carbon dioxide?
More chaotic (ex: gases made)
q=mc?T q=mL (or n x ?h)
A salt solution.
linear

10. silver iodide
Most are soluble except Ag - Pb
They stay the same.
Pale yellow
At half equivalence - pH=pKa

11. primary colors
red - green - blue
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
HClO4
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

12. How are more active metals reduced?
by electrolysis
Pour liquids using a funnel or down a glass rod
methyl formate
Separating funnel

13. What is the third law of thermodynamics?
S crystal at 0K=0
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Unsaturated - addition (ex: decolorize bromine solution)
Acids; HCOOCH3 is an ester

14. What two compounds are great oxidizing agents?

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15. What are the prefixes for the naming of binary molecular compound formulas (up to six)
ion pairing
+4-covalent - +2-ionic
Perform ICE BOX calculation based on K1
Mono; di; tri; tetra; penta; hexa.

16. If Q < Ksp a ppt ______
Kc=Kp
Ppt will NOT form (unsaturated)
Hg2²?
Cr2O7²?

17. What value of R do you use for thermo calculations? gas calculations?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
E=q + w (negative is by system - positive is on system)
Soluble except Ag - Pb - Ca - Sr Ba)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

18. Name six characteristics of transition elements (or their compounds)
fruit - fish - bases
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Cu3(PO4)2
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)

19. What is H2CO3 (carbonate acid) usually written as?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
H2O + CO2 (it decomposes readily)
allow for the vapor pressure of water and make sure to level levels
A) any range. b) 8-10 c) 4-6

20. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Tetrahedral
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Reduction always takes place at the cathode (RED CAT) In both types of cell!
acids

21. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
H+
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Evaporation

22. What do group I/II metal oxides and acids form?
Salt and water
CN?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
PO4³?

23. What is the word equation for addition polymerisation?
NH2?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Distillation
different forms of the same element

24. 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)
P2O5
?G= -ve - E°= +ve
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

25. What is the formula for summation?

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26. What is the formula for alkanes?
CnH2n+2
Filtration
ROH
Anode - oxygen. Cathode - hydrogen

27. How does the melting point of a mixture compare to the MP of a pure substance?

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28. Do you use J or kJ for ?H - ?S - and ?G?
?H-kJ - ?S-J - ?G-kJ
Trigonal pyramidal
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Soluble

29. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
CnH2n-2
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
The dilution effect when the solutions mix. M1V1 = M2V2

30. What type of compounds are almost always colored?
Ionic compounds
PO4³?
Decant
Transition element compounds (except if it has a full or empty d shell)

31. 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?
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?)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Purple
The compound with the lowest Ksp value.

32. Which alkali metals float on water?
ClO4?
All except for lithium
Eudiometer
H3PO4

33. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Pale yellow
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Evaporation
diamond and graphite

34. What is the difference between equivalence point and end point of a titration.
Salts (ex: CaO + SO2 ? CaSO3)
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
?H formation of an element in standard state=0
Ppt will NOT form (unsaturated)

35. When is ?G zero?
Orange
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Group I metals (soft metals) are stored under oil
atoms

36. What kind of bonding structure does benzene have?
fruit - fish - bases
White precipitate
benzene has a delocalized pi ring structure
Group 1 hydroxides (ex: NaOH)

37. What do you use for an acid spill? base spill?
PO4³?
by electrolysis
benzene is less reactive than alkenes
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

38. Esters smell like _______ and amines smell like _______ and are ______.
are less dense than water
CnH(2n+2)
fruit - fish - bases
Both electrons come from the same atom (just as good as a regular bond)

39. What complex ion does ammonia form with silver? copper? cadmium? zinc?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Check for air bubbles in the buret and remove the buret funnel from the buret
Transition element compounds (except if it has a full or empty d shell)
zero

40. halides
Most are soluble except Ag - Pb
CrO4²?
brown volatile liquid
Suniverse increases for spontaneous processes

41. How do you get Ecell for spontaneous reactions?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
voltaic: - electrolytic: +
zero-th: decreases - first: constant - second: increases
benzene is less reactive than alkenes

42. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
basic
bases
same KE - but PEice<PEwater
bright yellow

43. When combining half equations - what do you do to E° values when multiplying coefficients?
The benzene ring (or more correctly the phenyl group - C6H5)
Nothing
Both electrons come from the same atom (just as good as a regular bond)
#ligands=charge x2

44. What is Big K in terms of kf and kr?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Big K=kf/kr
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)
HClO4

45. Neutralization is an ________ reaction.
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Unsaturated - addition (ex: decolorize bromine solution)
metal oxides and hydrides are ionically bonded and basic

46. Lattice energy is high for ions with _____ size and _____ charge
Eudiometer
Hg²?
water and substances with (s) less dense than
small size and high charge

47. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
CN?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
benzene is less reactive than alkenes
it is lower and occurs over less sharp a range

48. How do you find the pH for a dibasic acid? (H2A)?
ClO2?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Perform ICE BOX calculation based on K1
are less dense than water

49. oxalate
CO3²?
C2O4²?
water and substances with (s) less dense than
Making sigma bonds and holding lone pairs

50. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
CrO4²?
Ksp = 4s³
Cr2O7²?