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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. Give an example of a dilute strong acid.
Products - reactants (except for BDE when it's reactants - products)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
HClO4
Soluble

2. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
do not change
Ksp = 27s4
Purple
Mono; di; tri; tetra; penta; hexa.

3. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
voltaic: + electrolytic: -
Pale yellow
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
fractional distillation

4. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
The dilution effect when the solutions mix. M1V1 = M2V2
But S° of element is not zero (except at 0K)
HClO4

5. What are the signs of ?G and E° for spontaneous reactions?
Conjugate pair (one must be a weak base or acid)
?G=negative - E° must be positive
Pour liquids using a funnel or down a glass rod
ClO2?

6. What is the conjugate acid of H2PO4?
Ionic compounds
H3PO4
C2O4²?
Current - time and charge on ion (moles of e used in half cell reaction)

7. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
zero
CrO4²?
CnH2n+2

8. When combining half equations - what do you do to E° values when multiplying coefficients?
strong acids/bases are written as H+ or OH- ions
It ceases - the circuit is broken.
A salt solution.
Nothing

9. What is the general formula for an alcohol?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
ROH
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
lighted splint (positive result=pop)

10. What are isotopes?
They stay the same.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Time?¹ - (ex. s?¹ - hr?¹ - etc)
The compound with the lowest Ksp value.

11. What is the basic structure of an optical isomer?
voltaic: + electrolytic: -
Acid rain - dissolves marble buildings/statues and kills trees.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

12. What process do you use to separate two liquids with different boiling points?
A) any range. b) 8-10 c) 4-6
blue glass - it filters UV
bases
fractional distillation

13. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Greenish-yellow gas
red - green - blue
Identity and purity (impure compounds usually have broad & low melting points)
Ksp = s²

14. acetate
CH3COO?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Cr2O7²?
#ligands=charge x2

15. When a cell is 'flat' What is its voltage?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
methyl formate
look for changes in oxidation # - the one that goes up is oxidized and is the RA
zero

16. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Evaporation
proton donor base

17. Is the ?H formation of an element in standard state zero?
Synthesis - separation and purification of the product and its identification.
Conjugate pair (one must be a weak base or acid)
?H formation of an element in standard state=0
Greenish-yellow gas

18. What is the second law of thermodynamics?
zero
Unsaturated - addition (ex: decolorize bromine solution)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Suniverse increases for spontaneous processes

19. What is the third law of thermodynamics?
a-IMFs - b-molecular volume
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
S crystal at 0K=0
CN?

20. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
allow for the vapor pressure of water and make sure to level levels
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
S2O3²?
strong acids/bases are written as H+ or OH- ions

21. Esters smell like _______ and amines smell like _______ and are ______.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
H2PO4?
fruit - fish - bases
ionic and form hydrogen and hydroxide

22. If a weak acid is diluted more - what happens to its % dissociation value?
Initiation energy (NOT Ea)
Increases.
Salt and water
Kc=Kp

23. What do acids plus active metals form?
HClO4
Evaporation
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
a-IMFs - b-molecular volume

24. Give an example of a concentrated weak acid.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
same KE - but PEice<PEwater
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Glacial acetic acid

25. If Q > Ksp - then system shifts _______ and ppt ______
P2O5
Monomer + monomer = polymer product + a simple molecule such as water or HCl
boiling without losing volatile solvents/reactants
left - ppt will form

26. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
The dilution effect when the solutions mix. M1V1 = M2V2
voltaic: - electrolytic: +
Acids; HCOOCH3 is an ester

27. A Bronsted-Lowry acid is...
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)
proton donor base
CN?
same KE - but PEice<PEwater

28. A geometric (or cis-trans) isomer exists due to.....
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Clear
0.10M HCl (more ions)

29. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Soluble
Acid rain - dissolves marble buildings/statues and kills trees.
They stay the same.

30. What kind of bonding structure does benzene have?
0.10M HCl (more ions)
benzene has a delocalized pi ring structure
lighted splint (positive result=pop)
S crystal at 0K=0

31. What is H2CO3 (carbonate acid) usually written as?
|experimental - accepted|/accepted X 100
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
blue
H2O + CO2 (it decomposes readily)

32. When can supercooling occur? What does it look like on a cooling curve?

33. Alcohols and _______ are FG isomers
ethers
hydroxides (ex: Ba(OH)2)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

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

35. What is the formula for summation?

36. perchlorate
White precipitate
benzene has a delocalized pi ring structure
Synthetic condensation polymer (aka a polyamide)
ClO4?

37. What is the general formula of an alkane?
CnH(2n+2)
blue glass - it filters UV
red - green - blue
Iodine and CO2 (dry ice)

38. What are the formulas for q?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
q=mc?T q=mL (or n x ?h)
Decant
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

39. Ca - Sr - Ba
ethers
hydroxides (ex: Ba(OH)2)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
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

40. Which of the rates changes more when temperature is increased?
Sigma bonds are stronger than pi bonds
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
basic
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

41. What word is a clue for a redox reaction?
RCHO (carbonyl at end)
Acidified
acids
Selective absorption

42. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
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
Pour liquids using a funnel or down a glass rod
CO (poisonous)
Glacial acetic acid

43. Acidic gases like SO2 in the atmosphere cause what environmental problems?
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)
Graduated cylinder
Perform ICE BOX calculation based on K1
Acid rain - dissolves marble buildings/statues and kills trees.

44. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Anode
0.10M HCl (more ions)
H2O + CO2 (it decomposes readily)
water and substances with (s) less dense than

45. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
White precipitate
S crystal at 0K=0
Time?¹ - (ex. s?¹ - hr?¹ - etc)

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

47. How are more active metals reduced?
by electrolysis
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
0.10M HCl (more ions)
How grouped results are

48. group 1 ions/compounds
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
CnH2n
Soluble
Kc=Kp

49. How do you get the equation for a net electrolysis reaction?
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
A salt solution.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

50. What process do you use to obtain the precipitate from a solution?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Filtration
metal oxides and hydrides are ionically bonded and basic
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask