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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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. perchlorate
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
ClO4?
Initiation energy (NOT Ea)
RNH2

2. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
blue
Distillation
same KE - but PEice<PEwater

3. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
allow for the vapor pressure of water and make sure to level levels
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia
Q=It (time in seconds)
q=mc?T q=mL (or n x ?h)

4. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
The benzene ring (or more correctly the phenyl group - C6H5)
RX
The one with most oxygen atoms (highest oxidation number)
Ksp = 4s³

5. What are the common strong bases?
Group 1 hydroxides (ex: NaOH)
Initiation energy (NOT Ea)
Ksp = 108s5
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

6. What are the signs for ?G and E° for spontaneous reactions?
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)
10?8
?G= -ve - E°= +ve
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

7. What value of R do you use for thermo calculations? gas calculations?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Increases.
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)

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

9. How do you get the equation for a net electrolysis reaction?
Insoluble
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Combine the equations for the half reactions in the non-spontaneous direction
non-metal oxides and hydrides are covalently bonded and are acidic.

10. lead compounds
ClO4?
Insoluble except nitrate and acetate
linear
Both electrons come from the same atom (just as good as a regular bond)

11. What are two allotropes of carbon?
Graduated cylinder
diamond and graphite
S crystal at 0K=0
10?8

12. oxalate
?H formation of an element in standard state=0
Big K=kf/kr
C2O4²?
O2 needs 4F/mol H2 needs 2F/mol

13. What type of polymer is nylon?
Unsaturated - addition (ex: decolorize bromine solution)
Synthetic condensation polymer (aka a polyamide)
CnH2n
fractional distillation

14. What type of solutions do small - highly charged cations tend to form?
Concentration
Ksp = 4s³
No - it depends on the number of ions produced on dissolving.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

15. halides
Acidified
Ksp = 4s³
Most are soluble except Ag - Pb
At half equivalence - pH=pKa

16. The oxidation # for acid base reactions...
do not change
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 + alcohol
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

17. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
CrO4²?
red - green - blue
?G=negative - E° must be positive
Anode - oxygen. Cathode - hydrogen

18. mercury (I) ion
Hg2²?
q=mc?T q=mL (or n x ?h)
Hg²?
How grouped results are

19. What electrons are lost/gained first in transition element ions?
Anode
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
ns² electrons (first in-first out)
Increases down group 1 decreases down group 17

20. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
+4-covalent - +2-ionic
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Heat a test tube at an angle at the side of the tube (not bottom)

21. What is the general formula for alkyl halides?
RX
catalyst=conc H2SO4
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Pipette (burette if need repetition)

22. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
ion pairing
Transition element compounds (except if it has a full or empty d shell)
ClO3?
P2O5

23. What device would you use to measure a volume of gas?
Add acid to water so that the acid doesn't boil and spit
Eudiometer
The one with most oxygen atoms (highest oxidation number)
CO (poisonous)

24. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
ethers
Ksp = 108s5
Current - time and charge on ion (moles of e used in half cell reaction)
H+

25. How do you compute % dissociation?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
[A?]/[HA] x 100 or [BH?]/[B] x 100
blue glass - it filters UV
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

26. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
An active metal.
Iodine and CO2 (dry ice)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

27. chromate ion (soln + most solids)
CO (poisonous)
yellow
#ligands=charge x2
They decrease (or could be the same if the solid has ONLY JUST disappeared)

28. When the salt bridge is removed what happens to the cell reaction?
Soluble
ionic and form hydrogen and hydroxide
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
It ceases - the circuit is broken.

29. If ?S is positive - are the products more or less chaotic than the reactants?
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)
More chaotic (ex: gases made)
Exothermic
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

30. What is the catalyst for this reaction Ester + ?
RCOR
red - green - blue
catalyst=conc H2SO4
ethers

31. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
same KE - but PEice<PEwater
neutralization: high K - H2O product dissociation: low K - H2O reactant
Acid rain - dissolves marble buildings/statues and kills trees.
Reduction always takes place at the cathode (RED CAT) In both types of cell!

32. Do anions flow to the cathode or anode?
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)
strong acids/bases are written as H+ or OH- ions
Kc=Kp
Anode

33. Alkanes are _________ and react by _________
fractional distillation
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Saturated - Substitution (which requires more radical conditions)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

34. Does Kw increase or decrease with T? Why?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
E=q + w (negative is by system - positive is on system)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
ns² electrons (first in-first out)

35. Alkenes are ________ and react by __________
All except for lithium
RCOOR
Identity and purity (impure compounds usually have broad & low melting points)
Unsaturated - addition (ex: decolorize bromine solution)

36. What is the word equation for addition polymerisation?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
linear
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

37. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
PO4³?
RCHO (carbonyl at end)
Exothermic (?H for ANY sa/sb = -57kJ/mol)

38. potassium permanganate
Eudiometer
ROR
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Purple

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

40. What is the general formula for an acid?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
it reacts by substitution NOT addition
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
RCOOH

41. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
No - NH3 and HCl gases are extremely soluble
lighted splint (positive result=pop)
Distillation
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

42. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
Most are soluble except Ag - Pb
Current - time and charge on ion (moles of e used in half cell reaction)
Experimental mass/theoretical mass X 100

43. What is the pH of 1.0M HCl? 1M NaOH?
Acid rain - dissolves marble buildings/statues and kills trees.
0 and 14
At half equivalence - pH=pKa
Mn²? - Cr³? - Cr³

44. What is the first law of thermodynamics?
small size and high charge
Greenish-yellow gas
Only temperature
E=q + w (negative is by system - positive is on system)

45. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
The Faraday or Faraday's constant.
But S° of element is not zero (except at 0K)

46. When is ?G zero?
H+
ROH
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

47. bromine
Disulfur dichloride
no - they're written undissociated (HAaq)
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)
brown volatile liquid

48. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Tetrahedral
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
All except for lithium
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

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

50. hydroxides
Selective absorption
Insoluble (except group 1 ammonium and Ba)
methyl formate
No - it depends on the number of ions produced on dissolving.