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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. What causes the dramatic effect of T on rate?
RX
T increases exponentially the proportion of molecules with E > Ea
acid + alcohol
fruit - fish - bases

2. What are the units of the first order rate constant?
same KE - but PEice<PEwater
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Perform ICE BOX calculation based on K1
Trigonal pyramidal

3. ammonium
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Acids; HCOOCH3 is an ester
NH4?

4. What are isomers?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Molecules with the same molecular formulas - but different structural formulas
Salt and water
Heat a test tube at an angle at the side of the tube (not bottom)

5. Give an example of a concentrated weak acid.
Glacial acetic acid
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
it reacts by substitution NOT addition
#ligands=charge x2

6. What do group I/II metal oxides plus water form?
bases
Suniverse increases for spontaneous processes
Current - time and charge on ion (moles of e used in half cell reaction)
NO3?

7. How can metals like iron and zinc be reduced?
voltaic: + electrolytic: -
atoms
chemically (ex: with carbon)
CO (poisonous)

8. What device would you use to measure a volume of gas?
Evaporation
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Nothing
Eudiometer

9. If Q < Ksp a ppt ______
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Ppt will NOT form (unsaturated)
Iodine and CO2 (dry ice)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

10. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Mono; di; tri; tetra; penta; hexa.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
zero
CH3COO?

11. What value of R do you use for thermo calculations? gas calculations?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
The dilution effect when the solutions mix. M1V1 = M2V2
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Pipette (burette if need repetition)

12. What is the basic structure of an optical isomer?
proton acceptor.
It ceases - the circuit is broken.
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

13. What word is a clue for a redox reaction?
Salt and water
Purple
Acidified
RCOOR

14. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Concentration
They stay the same.
bases

15. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
NO3?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
White precipitate

16. What do metal oxides plus non- metal oxides form?
water and substances with (s) less dense than
The compound with the lowest Ksp value.
Salts (ex: CaO + SO2 ? CaSO3)
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

17. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
bases
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
zero-th: decreases - first: constant - second: increases

18. What is the general formula for an amine?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
q=mc?T q=mL (or n x ?h)
RNH2
Combine the equations for the half reactions in the non-spontaneous direction

19. What is an Alkyl group?

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20. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Current - time and charge on ion (moles of e used in half cell reaction)
Only temperature

21. What is the conjugate base of NH3?
Acids; HCOOCH3 is an ester
NH2?
Acidified
Purple

22. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
CO3²?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
P2O5

23. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Mn²? - Cr³? - Cr³
catalyst=conc H2SO4
Only temperature
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

24. Alkenes are ________ and react by __________
Acids; HCOOCH3 is an ester
strong acids/bases are written as H+ or OH- ions
Unsaturated - addition (ex: decolorize bromine solution)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

25. How do you clean a buret/pipette for a titration?
Concentration
do not change
Increases down group 1 decreases down group 17
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

26. hypochlorite
Pipette (burette if need repetition)
ClO?
a-IMFs - b-molecular volume
Graduated cylinder

27. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
#ligands=charge x2
Cr2O7²?
Heptane

28. hydroxide
atoms
OH?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

29. A geometric (or cis-trans) isomer exists due to.....
The benzene ring (or more correctly the phenyl group - C6H5)
Ionic compounds
Cu3(PO4)2
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

30. How do you identify which is oxidized or otherwise?
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)
-Ea/R
RCOOH

31. What part of a liquid do you look at to measure its volume?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
OH- and NH3
R=8.31 J/mol/K
Read the bottom of the meniscus

32. If Q > Ksp - then system shifts _______ and ppt ______
Tetrahedral
left - ppt will form
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.
Soluble

33. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
H3PO4
Saturated - Substitution (which requires more radical conditions)

34. When is ?G zero?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
do not change
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
yellow

35. When combining half equations - what do you do to E° values when multiplying coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Nothing
It ceases - the circuit is broken.
At half equivalence - pH=pKa

36. 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
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Perform ICE BOX calculation based on K1
blue glass - it filters UV

37. Name 2 ways in which you can create a buffer?
ClO4?
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)
q=mc?T q=mL (or n x ?h)
Nothing

38. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
bright yellow
Mn²? - Cr³? - Cr³
T increases exponentially the proportion of molecules with E > Ea

39. Which alkali metals float on water?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Kc=Kp
Cr2O7²?
All except for lithium

40. BaSO4
Insoluble
atoms
ion pairing
Hg2²?

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

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42. Both Acetic acid and ____________ are also functional isomers.
Pale yellow
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
methyl formate
Anode - oxygen. Cathode - hydrogen

43. What is the pH of 1.0M HCl? 1M NaOH?
same KE - but PEice<PEwater
Silvery gray solid - brown - purple
NH2?
0 and 14

44. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
hydroxides (ex: Ba(OH)2)
At half equivalence - pH=pKa
acids

45. How are metal oxides and hydrides bonded? are they acidic or basic?
bent
RCOOR
metal oxides and hydrides are ionically bonded and basic
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

46. What shape is methane?
Increases down group 1 decreases down group 17
Insoluble except nitrate and acetate
voltaic: - electrolytic: +
Tetrahedral

47. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Increases.
zero

48. What is the general formula for alkyl halides?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
RX
Exothermic (?H for ANY sa/sb = -57kJ/mol)
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)

49. What electrons are lost/gained first in transition element ions?
water and substances with (s) less dense than
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?)
it reacts by substitution NOT addition
ns² electrons (first in-first out)

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

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