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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 is the difference between equivalence point and end point of a titration.
NH2?
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
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
catalyst=conc H2SO4

2. What are the products of the reaction between group 1 metals and water?

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3. What is the formula of butane?
ClO4?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
C4H10
methyl formate

4. How does half life change for zero-th order - first order - and second order processes?
Add acid to water so that the acid doesn't boil and spit
CrO4²?
CO3²?
zero-th: decreases - first: constant - second: increases

5. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
RCOOR
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
The dilution effect when the solutions mix. M1V1 = M2V2

6. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Anode - oxygen. Cathode - hydrogen
Soluble
Experimental mass/theoretical mass X 100

7. What is the charge on a chlorine atom?
Group I metals (soft metals) are stored under oil
zero
Greenish-yellow gas
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

8. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
Acidified
Ionic compounds
CN?

9. What is the formula of copper (II) phosphate?
Conjugate pair (one must be a weak base or acid)
Iodine and CO2 (dry ice)
S2O3²?
Cu3(PO4)2

10. What is precision?
water and substances with (s) less dense than
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
How grouped results are
CnH2n-2

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

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12. What things should you remember to do when collecting gas over water?
Only temperature
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)
The compound with the lowest Ksp value.
allow for the vapor pressure of water and make sure to level levels

13. What apparatus do you use to pour liquids?
blue (BTB)
neutralization: high K - H2O product dissociation: low K - H2O reactant
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Pour liquids using a funnel or down a glass rod

14. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
Q=It (time in seconds)
E=q + w (negative is by system - positive is on system)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
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

15. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
H2O + CO2 (it decomposes readily)
RCHO (carbonyl at end)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Ksp = 27s4

16. What is the general formula for a ketone?
atoms
They stay the same.
RCOR
look for changes in oxidation # - the one that goes up is oxidized and is the RA

17. chlorite
by electrolysis
No - it depends on the number of ions produced on dissolving.
ClO2?
Soluble except Ag - Pb - Ca - Sr Ba)

18. chlorate
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
ClO3?
Filtration
zero-th: decreases - first: constant - second: increases

19. dihydrogen phosphate
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Salt + water
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
H2PO4?

20. oxalate
C2O4²?
Group I metals (soft metals) are stored under oil
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
catalyst=conc H2SO4

21. What is the sign of the anode in voltaic cells? in electrolytic cells?
The compound with the lowest Ksp value.
voltaic: - electrolytic: +
Mn²? - Cr³? - Cr³
benzene is less reactive than alkenes

22. What do you use to look at burning magnesium? why?
Heat a test tube at an angle at the side of the tube (not bottom)
an oxidized and reduced substance
Products - reactants (except for BDE when it's reactants - products)
blue glass - it filters UV

23. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Identity and purity (impure compounds usually have broad & low melting points)
At half equivalence - pH=pKa
Ppt will NOT form (unsaturated)
a-IMFs - b-molecular volume

24. Buffer capacity must contain decent amounts of a ________ ________
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
look for changes in oxidation # - the one that goes up is oxidized and is the RA
?H-kJ - ?S-J - ?G-kJ
Conjugate pair (one must be a weak base or acid)

25. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
small size and high charge
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
a-IMFs - b-molecular volume
bent

26. BaSO4
H2O + CO2 (it decomposes readily)
Insoluble
ClO?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

27. Does Kw increase or decrease with T? Why?
a-IMFs - b-molecular volume
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
proton acceptor.

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

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29. Color is due to ______ _______ of light.
Selective absorption
non-metal oxides and hydrides are covalently bonded and are acidic.
a-IMFs - b-molecular volume
yellow

30. What is the basic structure of an optical isomer?
RCOOH
hydroxides (ex: Ba(OH)2)
zero
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

31. lead compounds
How grouped results are
Hg²?
Insoluble except nitrate and acetate
benzene is less reactive than alkenes

32. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
ethers
Soluble except Ag - Pb - Ca - Sr Ba)
K1 x K2
A) any range. b) 8-10 c) 4-6

33. silver iodide
metal oxides and hydrides are ionically bonded and basic
Glacial acetic acid
Pale yellow
Eudiometer

34. perchlorate
by electrolysis
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
ClO4?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

35. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Current - time and charge on ion (moles of e used in half cell reaction)
red - green - blue
ethers
Experimental mass/theoretical mass X 100

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

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37. When the salt bridge is removed what happens to the cell reaction?
Selective absorption
It ceases - the circuit is broken.
benzene has a delocalized pi ring structure
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

38. Why are i factors (Van't Hoff factors) often less than ideal?
CnH2n-2
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
ion pairing
K2

39. Colorless doesn't mean ______
Clear
K2
Group 1 hydroxides (ex: NaOH)
ns² electrons (first in-first out)

40. How are strong ones written?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
strong acids/bases are written as H+ or OH- ions
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
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)

41. When is ?G zero?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
RNH2
More chaotic (ex: gases made)

42. What is the general formula for an ether?
How close results are to the accepted value
Time?¹ - (ex. s?¹ - hr?¹ - etc)
small size and high charge
ROR

43. Metal hydrides are _____ and form _______ and _______ when added to water
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
ionic and form hydrogen and hydroxide
|experimental - accepted|/accepted X 100
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

44. Which alkali metals float on water?
Greenish-yellow gas
CnH2n
All except for lithium
Most INsoluble except group 1 and ammonium

45. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
allow for the vapor pressure of water and make sure to level levels
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
A salt solution.

46. How do you find the pH for a dibasic acid? (H2A)?
Nothing
Perform ICE BOX calculation based on K1
10?8
blue glass - it filters UV

47. Name C7H16
Heptane
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
RX
Insoluble except group 1 and ammonium

48. acetates
allow for the vapor pressure of water and make sure to level levels
ionic and form hydrogen and hydroxide
They stay the same.
Soluble

49. Name 2 ways in which you can create a buffer?
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)
Big K=kf/kr
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

50. hydroxides
Trigonal pyramidal
Ppt will NOT form (unsaturated)
Insoluble (except group 1 ammonium and Ba)
zero