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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. BaSO4
Insoluble
Initiation energy (NOT Ea)
red - green - blue
acid + alcohol

2. Neutralization is an ________ reaction.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Cr2O7²?
Ksp = 4s³

3. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
q=mc?T q=mL (or n x ?h)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

4. What is a dipeptide? polypeptide? protein?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Group 1 hydroxides (ex: NaOH)
The compound with the lowest Ksp value.

5. Esterification is...
Mn²? - Cr³? - Cr³
acid + alcohol
a-IMFs - b-molecular volume
RCOR

6. What is precision?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
0 and 14
How grouped results are
But S° of element is not zero (except at 0K)

7. What two compounds are great oxidizing agents?

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8. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
They stay the same.
Soluble
E=q + w (negative is by system - positive is on system)

9. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
water and substances with (s) less dense than
0 and 14
Kc=Kp

10. What is the catalyst for this reaction Ester + ?
boiling without losing volatile solvents/reactants
catalyst=conc H2SO4
Filtration
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

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

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12. What is the test for hydrogen?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
same KE - but PEice<PEwater
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
lighted splint (positive result=pop)

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

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14. What is HCOOCH3?
Purple
Acids; HCOOCH3 is an ester
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Conjugate pair (one must be a weak base or acid)

15. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
ClO3?
Mn²? - Cr³? - Cr³
proton acceptor.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

16. What is the formula for summation?

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17. What is the name of S2Cl2? (Know how to name others like this - too)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
chemically (ex: with carbon)
CrO4²?
Disulfur dichloride

18. What is the general formula of an alkane?
CnH(2n+2)
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)
RCHO (carbonyl at end)
Iodine and CO2 (dry ice)

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

20. What do the 'a' and 'b' in Van Der Waal's equation allow for?
The Faraday or Faraday's constant.
Trigonal pyramidal
look for changes in oxidation # - the one that goes up is oxidized and is the RA
a-IMFs - b-molecular volume

21. What do nonmetal oxides plus water form?
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?)
acids
ethers
proton acceptor.

22. Buffer capacity must contain decent amounts of a ________ ________
ion pairing
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Conjugate pair (one must be a weak base or acid)
?G= -ve - E°= +ve

23. What is the test for oxygen?
Silvery gray solid - brown - purple
Pipette (burette if need repetition)
Glowing splint (positive result=relights)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

24. mercury (II) ion
CH3COO?
Glowing splint (positive result=relights)
E=q + w (negative is by system - positive is on system)
Hg²?

25. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
red - green - blue
RNH2
CnH2n

26. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
H+
?G=negative - E° must be positive
Concentration

27. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
zero
The benzene ring (or more correctly the phenyl group - C6H5)
blue (BTB)

28. What element is used to vulcanize rubber?
?H formation of an element in standard state=0
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Sulfur
catalyst=conc H2SO4

29. What do group I/II metal oxides and acids form?
Salt and water
RNH2
by electrolysis
Anode

30. Color (absorbance) is proportional to ________
[A?]/[HA] x 100 or [BH?]/[B] x 100
voltaic: + electrolytic: -
Concentration
The benzene ring (or more correctly the phenyl group - C6H5)

31. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
SO4²?
The dilution effect when the solutions mix. M1V1 = M2V2
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?)

32. What is the general formula for alkyl halides?
RX
it's lower and occurs over less sharp a range
T increases exponentially the proportion of molecules with E > Ea
It ceases - the circuit is broken.

33. hypochlorite
ClO?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Molecules with the same molecular formulas - but different structural formulas
boiling without losing volatile solvents/reactants

34. What things should you remember to do when collecting gas over water?
CnH2n+2
do not change
allow for the vapor pressure of water and make sure to level levels
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

35. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Acids; HCOOCH3 is an ester
Increases down group 1 decreases down group 17
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Glacial acetic acid

36. Give an example of a concentrated weak acid.
strong acids/bases are written as H+ or OH- ions
fractional distillation
Glacial acetic acid
Silvery gray solid - brown - purple

37. 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
do not change
atoms
benzene is less reactive than alkenes

38. What do group I/II metal oxides plus water form?
bases
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.
basic
Combine the equations for the half reactions in the non-spontaneous direction

39. cyanide
Decant
CN?
Conjugate pair (one must be a weak base or acid)
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)

40. A Bronsted-Lowry acid is...
neutralization: high K - H2O product dissociation: low K - H2O reactant
Mn²? - Cr³? - Cr³
proton donor base
Exothermic (?H for ANY sa/sb = -57kJ/mol)

41. Where are group I metals stored?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Group I metals (soft metals) are stored under oil
Graduated cylinder
Insoluble except group 1 and ammonium

42. What are the signs of ?G and E° for spontaneous reactions?
Iodine and CO2 (dry ice)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
RCOOR
?G=negative - E° must be positive

43. How do you explain trends in atomic properties using Coulomb's Law?
Ksp = 108s5
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
RCOOR

44. Is the freezing of ice endothermic or exothermic?
left - ppt will form
A) any range. b) 8-10 c) 4-6
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Exothermic

45. What type of polymer is nylon?
methyl formate
An active metal.
Synthetic condensation polymer (aka a polyamide)
Conjugate pair (one must be a weak base or acid)

46. What is the pH of 1.0M HCl? 1M NaOH?
?G= -ve - E°= +ve
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Salt and water
0 and 14

47. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
it's lower and occurs over less sharp a range
Check for air bubbles in the buret and remove the buret funnel from the buret
ClO4?
They decrease (or could be the same if the solid has ONLY JUST disappeared)

48. Does reactivity increase/decrease going down group 1 and group 17?
Orange
Mn²? - Cr³? - Cr³
Pale purple - (orange)-yellow - red - blue - green.
Increases down group 1 decreases down group 17

49. What word is a clue for a redox reaction?
CnH2n
A) any range. b) 8-10 c) 4-6
Insoluble except nitrate and acetate
Acidified

50. What is the general formula for an ester?
RCOOR
Ppt will NOT form (unsaturated)
acid + alcohol
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?