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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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1. bromine
RCOOH
it reacts by substitution NOT addition
brown volatile liquid
RCOR

2. What shape is methane?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Soluble
Tetrahedral
All except for lithium

3. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
linear
ionic and form hydrogen and hydroxide
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
The dilution effect when the solutions mix. M1V1 = M2V2

4. 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?
The compound with the lowest Ksp value.
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)
Insoluble
All except for lithium

5. dihydrogen phosphate
H2PO4?
CN?
it reacts by substitution NOT addition
Soluble

6. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Soluble
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
proton donor base

7. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Glowing splint (positive result=relights)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
?H-kJ - ?S-J - ?G-kJ
The benzene ring (or more correctly the phenyl group - C6H5)

8. Alcohols and _______ are FG isomers
Trigonal pyramidal
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Pipette (burette if need repetition)
ethers

9. What do you use to look at burning magnesium? why?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
-Ea/R
blue glass - it filters UV
atoms

10. silver iodide
do not change
Pale yellow
Salt and water
Saturated - Substitution (which requires more radical conditions)

11. What is the slope of the graph of lnk vs. 1/T?
Increases.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
-Ea/R

12. What do nonmetal oxides plus water form?
proton acceptor.
NO3?
10?8
acids

13. Which alkali metals float on water?
CrO4²?
All except for lithium
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
zero-th: decreases - first: constant - second: increases

14. What is the difference between equivalence point and end point of a titration.
ionic and form hydrogen and hydroxide
acids
R=8.31 J/mol/K
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

15. What apparatus do you use to pour liquids?
CnH2n+2
Pour liquids using a funnel or down a glass rod
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
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?)

16. What is the third law of thermodynamics?
S crystal at 0K=0
basic
Anode - oxygen. Cathode - hydrogen
NO3?

17. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Hg2²?
basic
'non-active' metals such as Cu - Ag - Au - Pt - etc.
zero

18. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
Decant
it is lower and occurs over less sharp a range
H2O + CO2 (it decomposes readily)

19. Generally - which oxy acid is strongest?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
A) any range. b) 8-10 c) 4-6
Greenish-yellow gas
The one with most oxygen atoms (highest oxidation number)

20. What is the second law of thermodynamics?
Pale yellow
Exothermic
Suniverse increases for spontaneous processes
Exothermic (?H for ANY sa/sb = -57kJ/mol)

21. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Sigma bonds are stronger than pi bonds
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
strong acids/bases are written as H+ or OH- ions

22. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
HClO4
Ksp = s²
NH2?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

23. sulfates
P2O5
But S° of element is not zero (except at 0K)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Soluble except Ag - Pb - Ca - Sr Ba)

24. What are the formulas for q?
Ksp = 4s³
ionic and form hydrogen and hydroxide
q=mc?T q=mL (or n x ?h)
Acids; HCOOCH3 is an ester

25. How do you explain trends in atomic properties using Coulomb's Law?
At half equivalence - pH=pKa
Ppt will NOT form (unsaturated)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

26. Why are i factors (Van't Hoff factors) often less than ideal?
ClO2?
Ppt will NOT form (unsaturated)
ion pairing
NO3?

27. What do hydrocarbons form when they burn in air (oxygen)?
zero
Glowing splint (positive result=relights)
Soluble
CO2 and H2O

28. Alkenes are ________ and react by __________
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
ethers
Heat a test tube at an angle at the side of the tube (not bottom)
Unsaturated - addition (ex: decolorize bromine solution)

29. Is the standard entropy (S°) of an element zero?
0 and 14
allow for the vapor pressure of water and make sure to level levels
Most INsoluble except group 1 and ammonium
But S° of element is not zero (except at 0K)

30. What is the formula for obtaining charge flowing in a cell?
ClO?
Q=It (time in seconds)
Suniverse increases for spontaneous processes
Products - reactants (except for BDE when it's reactants - products)

31. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Salt + water.
Current - time and charge on ion (moles of e used in half cell reaction)
small size and high charge
proton acceptor.

32. What is Big K in terms of kf and kr?
?H-kJ - ?S-J - ?G-kJ
How grouped results are
Big K=kf/kr
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

33. What is reflux?
Saturated - Substitution (which requires more radical conditions)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
blue (BTB)
boiling without losing volatile solvents/reactants

34. Ca - Sr - Ba
Making sigma bonds and holding lone pairs
hydroxides (ex: Ba(OH)2)
proton acceptor.
Salt + water

35. What element is used to vulcanize rubber?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Sulfur
same KE - but PEice<PEwater
Experimental mass/theoretical mass X 100

36. What is the general formula for an amine?
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
How close results are to the accepted value
zero-th: decreases - first: constant - second: increases
RNH2

37. What is the pH of 1.0M HCl? 1M NaOH?
Clear
0 and 14
different forms of the same element
White precipitate

38. If Q < Ksp a ppt ______
Insoluble except nitrate and acetate
no - they're written undissociated (HAaq)
Ppt will NOT form (unsaturated)
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.

39. What is the test for oxygen?
Cr2O7²?
Mn²? - Cr³? - Cr³
Glowing splint (positive result=relights)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

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

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41. ________ are Lewis bases - because they can donate a lone pair of electrons.
OH?
OH- and NH3
Mn²? - Cr³? - Cr³
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

42. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
catalyst=conc H2SO4
q=mc?T q=mL (or n x ?h)
P2O5
Identity and purity (impure compounds usually have broad & low melting points)

43. When driving off water from a hydrate - how do you tell you're done?
Transition element compounds (except if it has a full or empty d shell)
Trigonal pyramidal
Q=It (time in seconds)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

44. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
same KE - but PEice<PEwater
are less dense than water

45. How can metals like iron and zinc be reduced?
Acid rain - dissolves marble buildings/statues and kills trees.
chemically (ex: with carbon)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

46. What are allotropes?
Synthesis - separation and purification of the product and its identification.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Exothermic (?H for ANY sa/sb = -57kJ/mol)
different forms of the same element

47. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Anode - oxygen. Cathode - hydrogen
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)
CO3²?

48. What are the common strong bases?
Group 1 hydroxides (ex: NaOH)
ClO3?
bent
look for changes in oxidation # - the one that goes up is oxidized and is the RA

49. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
S crystal at 0K=0
Cu3(PO4)2
left - ppt will form

50. What is the general formula for an acid?
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)
RCOOH
Decant
a-IMFs - b-molecular volume

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AP Chemistry 2

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