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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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1. Name six characteristics of transition elements (or their compounds)
#ligands=charge x2
same KE - but PEice<PEwater
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)
K1 x K2

2. What do you use for an acid spill? base spill?
non-metal oxides and hydrides are covalently bonded and are acidic.
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
CnH2n-2

3. What should you check for before you begin titrating?
Mn²? - Cr³? - Cr³
Tetrahedral
Check for air bubbles in the buret and remove the buret funnel from the buret
Acid rain - dissolves marble buildings/statues and kills trees.

4. Neutralization is an ________ reaction.
At half equivalence - pH=pKa
water and substances with (s) less dense than
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Exothermic (?H for ANY sa/sb = -57kJ/mol)

5. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Ksp = 27s4
CH3COO?

6. If ?S is positive - are the products more or less chaotic than the reactants?
Kc=Kp
Soluble except Ag - Pb - Ca - Sr Ba)
?G=negative - E° must be positive
More chaotic (ex: gases made)

7. How does the melting point of a mixture compare to the MP of a pure substance?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
it is lower and occurs over less sharp a range
The dilution effect when the solutions mix. M1V1 = M2V2
Pale yellow

8. Does reactivity increase/decrease going down group 1 and group 17?
methyl formate
The dilution effect when the solutions mix. M1V1 = M2V2
Increases down group 1 decreases down group 17
Iodine and CO2 (dry ice)

9. What shape is water?
are less dense than water
blue
bent
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

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

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11. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
K2
left - ppt will form
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
do not change

12. phosphates
benzene has a delocalized pi ring structure
Soluble except Ag - Pb - Ca - Sr Ba)
Most INsoluble except group 1 and ammonium
How grouped results are

13. What is the word equation for condensation polymerisation ?
Current - time and charge on ion (moles of e used in half cell reaction)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Combine the equations for the half reactions in the non-spontaneous direction
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

14. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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15. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
P2O5
CN?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
zero

16. What device would you use to measure a volume of gas?
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.
T increases exponentially the proportion of molecules with E > Ea
At half equivalence - pH=pKa
Eudiometer

17. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Group I metals (soft metals) are stored under oil
ionic and form hydrogen and hydroxide
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Big K=kf/kr

18. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
HClO4
Soluble
K1 x K2
Disulfur dichloride

19. What changes Keq?
?G= -ve - E°= +ve
S2O3²?
The compound with the lowest Ksp value.
Only temperature

20. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
do not change
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Pale purple - (orange)-yellow - red - blue - green.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

21. ammonium
NH4?
Anode
T increases exponentially the proportion of molecules with E > Ea
Unsaturated - addition (ex: decolorize bromine solution)

22. carbonates
Ksp = 108s5
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Insoluble except group 1 and ammonium
No - NH3 and HCl gases are extremely soluble

23. What things should you remember to do when collecting gas over water?
benzene has a delocalized pi ring structure
allow for the vapor pressure of water and make sure to level levels
MnO4?
zero-th: decreases - first: constant - second: increases

24. chromate ion (soln + most solids)
bright yellow
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
yellow
Silvery gray solid - brown - purple

25. silver iodide
?H-kJ - ?S-J - ?G-kJ
Pale yellow
0 and 14
#ligands=charge x2

26. silver compounds
How close results are to the accepted value
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
K1 x K2
Insoluble except for nitrate and acetate

27. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Products - reactants (except for BDE when it's reactants - products)
C2O4²?
same KE - but PEice<PEwater

28. What is the catalyst for this reaction Ester + ?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Exothermic (?H for ANY sa/sb = -57kJ/mol)
methyl formate
catalyst=conc H2SO4

29. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
H3PO4
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Ksp = 108s5
Filtration

30. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
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)
yellow

31. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Acids; HCOOCH3 is an ester
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

32. What do acids plus active metals form?
Both electrons come from the same atom (just as good as a regular bond)
Insoluble except group 1 and ammonium
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Mono; di; tri; tetra; penta; hexa.

33. Which of the rates changes more when temperature is increased?
Unsaturated - addition (ex: decolorize bromine solution)
Concentration
K1 x K2
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

34. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Disulfur dichloride
MnO4?

35. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
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?)
Experimental mass/theoretical mass X 100
Ksp = s²

36. What type of compounds do Group 14 form?
zero-th: decreases - first: constant - second: increases
0 and 14
+4-covalent - +2-ionic
blue glass - it filters UV

37. What do you do to get rid of most of the solution from a precipitate?
allow for the vapor pressure of water and make sure to level levels
NH4?
Decant
benzene has a delocalized pi ring structure

38. What is Big K in terms of kf and kr?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Q=It (time in seconds)
The one with most oxygen atoms (highest oxidation number)
Big K=kf/kr

39. What is the formula for percent error?
C4H10
|experimental - accepted|/accepted X 100
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
same KE - but PEice<PEwater

40. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
benzene has a delocalized pi ring structure
All except for lithium
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

41. What do metal oxides plus acids form?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Salt + water
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Sigma bonds are stronger than pi bonds

42. dichromate (soln + most solids)
Heptane
Clear
CnH2n-2
Orange

43. What are the common strong bases?
Big K=kf/kr
Group 1 hydroxides (ex: NaOH)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

44. Give an example of a concentrated weak acid.
MnO4?
Glacial acetic acid
Tetrahedral
An active metal.

45. If Q < Ksp a ppt ______
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ClO3?
Ppt will NOT form (unsaturated)
Salts (ex: CaO + SO2 ? CaSO3)

46. ammonium/ammonium compounds
Soluble
chemically (ex: with carbon)
Purple
yellow

47. What is the difference between equivalence point and end point of a titration.
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
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
RX
How close results are to the accepted value

48. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
CnH2n+1 often designated 'R' ex C3H7 is propyl
Soluble except Ag - Pb - Ca - Sr Ba)
|experimental - accepted|/accepted X 100

49. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Ksp = s²
Selective absorption
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

50. When combining half equations - what do you do to E° values when multiplying coefficients?
strong acids/bases are written as H+ or OH- ions
blue (BTB)
Nothing
Monomer + monomer = polymer product + a simple molecule such as water or HCl

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AP Chemistry 2

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