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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.
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. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Both electrons come from the same atom (just as good as a regular bond)
Cu3(PO4)2
benzene is less reactive than alkenes

2. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Identity and purity (impure compounds usually have broad & low melting points)
Making sigma bonds and holding lone pairs
Anode - oxygen. Cathode - hydrogen

3. What is accuracy?
CO3²?
How close results are to the accepted value
Mono; di; tri; tetra; penta; hexa.
|experimental - accepted|/accepted X 100

4. group 1 ions/compounds
[A?]/[HA] x 100 or [BH?]/[B] x 100
Soluble
Exothermic
Add acid to water so that the acid doesn't boil and spit

5. What shape is methane?
Increases down group 1 decreases down group 17
T increases exponentially the proportion of molecules with E > Ea
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Tetrahedral

6. What reacts with an acid to create hydrogen gas?
Products - reactants (except for BDE when it's reactants - products)
An active metal.
ClO3?
blue

7. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
The compound with the lowest Ksp value.
CH3COO?
H3PO4

8. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
NH2?
water and substances with (s) less dense than
blue glass - it filters UV
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

9. silver compounds
C4H10
Read the bottom of the meniscus
Anode
Insoluble except for nitrate and acetate

10. Colorless doesn't mean ______
Ionic compounds
boiling without losing volatile solvents/reactants
Clear
ethers

11. What steps do organic labs consist of?
Acid rain - dissolves marble buildings/statues and kills trees.
bright yellow
ion pairing
Synthesis - separation and purification of the product and its identification.

12. What do group I/II metal oxides plus water form?
bases
NO3?
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
|experimental - accepted|/accepted X 100

13. If Q < Ksp a ppt ______
small size and high charge
Filtration
Ppt will NOT form (unsaturated)
Saturated - Substitution (which requires more radical conditions)

14. What process do you use to obtain the precipitate from a solution?
ion pairing
OH- and NH3
#ligands=charge x2
Filtration

15. What are allotropes?
methyl formate
Both electrons come from the same atom (just as good as a regular bond)
different forms of the same element
Salt and water

16. What type of metals don't react with water or acids to form H2?

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17. Can you collect soluble gases over water?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Suniverse increases for spontaneous processes
All single: sp³ - one double: sp² - two doubles: sp - one triple: sp - two single and two lone pairs: sp³ - three single and one lone pair: sp³
No - NH3 and HCl gases are extremely soluble

18. Give an example of a dilute strong acid.
Mono; di; tri; tetra; penta; hexa.
zero-th: decreases - first: constant - second: increases
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
HClO4

19. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
ClO3?
ClO4?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

20. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Synthesis - separation and purification of the product and its identification.
Ksp = 108s5
0.10M HCl (more ions)

21. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
do not change
catalyst=conc H2SO4
Separating funnel

22. What type of compounds are almost always colored?
Hg²?
acid + alcohol
Transition element compounds (except if it has a full or empty d shell)
RCOOR

23. What are the signs of ?G and E° for spontaneous reactions?
catalyst=conc H2SO4
red - green - blue
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
?G=negative - E° must be positive

24. What apparatus do you use to pour liquids?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
More chaotic (ex: gases made)
A salt solution.
Pour liquids using a funnel or down a glass rod

25. Do anions flow to the cathode or anode?
Cu3(PO4)2
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)
But S° of element is not zero (except at 0K)
Anode

26. During a titration what is present in the beaker at the equivalence point?
H2PO4?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
hydroxides (ex: Ba(OH)2)
A salt solution.

27. What is the general formula for an acid?
water and substances with (s) less dense than
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
A salt solution.
RCOOH

28. dihydrogen phosphate
Transition element compounds (except if it has a full or empty d shell)
CnH(2n+2)
H2PO4?
Filtration

29. What measuring device would you use for very small volumes of liquids?
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)
Pipette (burette if need repetition)
ClO4?
Reduction always takes place at the cathode (RED CAT) In both types of cell!

30. bromine
atoms
Exothermic
Suniverse increases for spontaneous processes
brown volatile liquid

31. How can metals like iron and zinc be reduced?
Soluble
chemically (ex: with carbon)
Anode - oxygen. Cathode - hydrogen
RCOOR

32. When combining half equations - what do you do to E° values when multiplying coefficients?
Nothing
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
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.
10?8

33. The oxidation # for acid base reactions...
Acidified
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
do not change
C2O4²?

34. What is the general formula for an alcohol?
ROH
Heat a test tube at an angle at the side of the tube (not bottom)
same KE - but PEice<PEwater
NH2?

35. What is the test for hydrogen?
lighted splint (positive result=pop)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
ion pairing
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

36. What is Big K in terms of kf and kr?
Suniverse increases for spontaneous processes
Salt + water.
Current - time and charge on ion (moles of e used in half cell reaction)
Big K=kf/kr

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

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38. What effect does increasing the size/surface area of a voltaic cell have on the cell?
fractional distillation
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.
Heptane
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

39. What is the charge on a chlorine atom?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
zero
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)
Identity and purity (impure compounds usually have broad & low melting points)

40. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
zero
They stay the same.
Products - reactants (except for BDE when it's reactants - products)
Read the bottom of the meniscus

41. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
R=8.31 J/mol/K
Anode - oxygen. Cathode - hydrogen

42. What apparatus do you use to separate 2 immiscible liquids?
?H-kJ - ?S-J - ?G-kJ
Separating funnel
H2O + CO2 (it decomposes readily)
ClO?

43. What two compounds are great oxidizing agents?

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

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45. chlorine
Increases.
Greenish-yellow gas
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?)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

46. BaSO4
Unsaturated - addition (ex: decolorize bromine solution)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
same KE - but PEice<PEwater
Insoluble

47. What are amphoteric oxides?
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?)
Decant
Making sigma bonds and holding lone pairs
same KE - but PEice<PEwater

48. acetates
Soluble
ion pairing
CrO4²?
Iodine and CO2 (dry ice)

49. How does group 1 metals' density compare to water's?
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.
No - it depends on the number of ions produced on dissolving.
RX
are less dense than water

50. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
blue
Ppt will NOT form (unsaturated)
basic
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?