AP Chemistry 2

Instructions:

• Answer 50 questions in 15 minutes.
• If you are not ready to take this test, you can study here.
• 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. dichromate
How grouped results are
Cr2O7²?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)


2. Esterification is...
acid + alcohol
CO (poisonous)
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)
Glacial acetic acid


3. Name six characteristics of transition elements (or their compounds)
proton acceptor.
look for changes in oxidation # - the one that goes up is oxidized and is the RA
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)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant


4. What is the general formula for an aldehyde?
yellow
RCHO (carbonyl at end)
RCOOH
ethers


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

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6. What is an Alkyl group?

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7. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
linear
Transition element compounds (except if it has a full or empty d shell)
It ceases - the circuit is broken.


8. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
0 and 14
Exothermic


9. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Eudiometer
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
linear
PO4³?


10. What changes Keq?
Ksp = 4s³
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Only temperature
Iodine and CO2 (dry ice)


11. What word is a clue for a redox reaction?
Anode
Acidified
it reacts by substitution NOT addition
Decant


12. 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
Unsaturated - addition (ex: decolorize bromine solution)
non-metal oxides and hydrides are covalently bonded and are acidic.
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp


13. What is the formula for percent error?
Increases down group 1 decreases down group 17
ClO4?
Most are soluble except Ag - Pb
|experimental - accepted|/accepted X 100


14. Is a graduated cylinder or beaker more accurate?
ion pairing
CO3²?
Salt and water
Graduated cylinder


15. Which alkali metals float on water?
Filtration
All except for lithium
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)
Insoluble except group 1 and ammonium


16. 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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17. Neutralization is an ________ reaction.
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)
Ppt will NOT form (unsaturated)
They stay the same.
Exothermic (?H for ANY sa/sb = -57kJ/mol)


18. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
?G=negative - E° must be positive
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Glowing splint (positive result=relights)
Current - time and charge on ion (moles of e used in half cell reaction)


19. What are the formulas for q?
Trigonal pyramidal
RX
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)
q=mc?T q=mL (or n x ?h)


20. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
strong acids/bases are written as H+ or OH- ions
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Insoluble except for nitrate and acetate


21. What is HCOOCH3?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Acids; HCOOCH3 is an ester
Filtration
Ksp = 27s4


22. A Bronsted-Lowry acid is...
It ceases - the circuit is broken.
water and substances with (s) less dense than
same KE - but PEice<PEwater
proton donor base


23. thiosulfate
Only temperature
S2O3²?
Salt and water
Combine the equations for the half reactions in the non-spontaneous direction


24. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
?H formation of an element in standard state=0
CO (poisonous)
benzene has a delocalized pi ring structure
They stay the same.


25. What type of compounds do metals/non metals form?
HClO4
How close results are to the accepted value
Filtration
Ionic compounds


26. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
K1 x K2
Acid rain - dissolves marble buildings/statues and kills trees.
RNH2


27. What process do you use to separate two liquids with different boiling points?
fractional distillation
NH4?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Distillation


28. hypochlorite
ClO?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Cr2O7²?
Ksp = 27s4


29. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
chemically (ex: with carbon)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask


30. How do you find the pH for a dibasic acid? (H2A)?
ionic and form hydrogen and hydroxide
Perform ICE BOX calculation based on K1
Heptane
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


31. Why are i factors (Van't Hoff factors) often less than ideal?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Suniverse increases for spontaneous processes
ion pairing
Pale purple - (orange)-yellow - red - blue - green.


32. How do you dilute an acid?

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33. ammonium
H3PO4
An active metal.
NH4?
redox reaction


34. Does the electrolyte with the lowest Ksp value have to be the least soluble? 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.
-Ea/R
No - it depends on the number of ions produced on dissolving.
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.


35. What is the formula of copper (II) phosphate?
Cu3(PO4)2
benzene has a delocalized pi ring structure
Evaporation
ROH


36. What shape is ammonia?
an oxidized and reduced substance
Trigonal pyramidal
water and substances with (s) less dense than
Unsaturated - addition (ex: decolorize bromine solution)


37. How does benzene compare in reactivity to alkenes?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
q=mc?T q=mL (or n x ?h)
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.
benzene is less reactive than alkenes


38. What do you do to get rid of most of the solution from a precipitate?
blue (BTB)
Soluble except Ag - Pb - Ca - Sr Ba)
Separating funnel
Decant


39. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
R=8.31 J/mol/K
Insoluble (except group 1 ammonium and Ba)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)


40. What is the formula for alkanes?
K1 x K2
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
CnH2n+2
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)


41. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
Tetrahedral
-Ea/R
P2O5
SO4²?


42. What is the word equation for addition polymerisation?
A) any range. b) 8-10 c) 4-6
H2O + CO2 (it decomposes readily)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
|experimental - accepted|/accepted X 100


43. What two compounds are great oxidizing agents?

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44. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
CH3COO?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
-Ea/R


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

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46. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
OH- and NH3
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
NH2?


47. If Q > Ksp - then system shifts _______ and ppt ______
Read the bottom of the meniscus
voltaic: + electrolytic: -
H3PO4
left - ppt will form


48. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
The dilution effect when the solutions mix. M1V1 = M2V2
Sigma bonds are stronger than pi bonds
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)


49. Does Kw increase or decrease with T? Why?
no - they're written undissociated (HAaq)
acid + alcohol
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)


50. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
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.
ns² electrons (first in-first out)
Soluble