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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 happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
no - they're written undissociated (HAaq)
Trigonal pyramidal
They decrease (or could be the same if the solid has ONLY JUST disappeared)

2. Alcohols and _______ are FG isomers
?H-kJ - ?S-J - ?G-kJ
H+
CN?
ethers

3. Do you use J or kJ for ?H - ?S - and ?G?
Combine the equations for the half reactions in the non-spontaneous direction
voltaic: - electrolytic: +
?H-kJ - ?S-J - ?G-kJ
?G=negative - E° must be positive

4. 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
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Most are soluble except Ag - Pb

5. What is the formula for percent error?
|experimental - accepted|/accepted X 100
ionic and form hydrogen and hydroxide
Soluble except Ag - Pb - Ca - Sr Ba)
Clear

6. What is precision?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
How grouped results are
Cu3(PO4)2
zero

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

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8. chlorite
Check for air bubbles in the buret and remove the buret funnel from the buret
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
Trigonal pyramidal
ClO2?

9. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
ClO?
fractional distillation
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

10. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Iodine and CO2 (dry ice)
left - ppt will form
Acidified
Reduction always takes place at the cathode (RED CAT) In both types of cell!

11. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
voltaic: - electrolytic: +
Perform ICE BOX calculation based on K1
zero
Sigma bonds are stronger than pi bonds

12. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
Distillation
redox reaction
Ksp = 108s5

13. What do you use to look at burning magnesium? why?
blue glass - it filters UV
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
E=q + w (negative is by system - positive is on system)
Acids; HCOOCH3 is an ester

14. What is H2CO3 (carbonate acid) usually written as?
NH2?
Filtration
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
H2O + CO2 (it decomposes readily)

15. What word is a clue for a redox reaction?
zero
allow for the vapor pressure of water and make sure to level levels
small size and high charge
Acidified

16. ammonium/ammonium compounds
Soluble
Filtration
brown volatile liquid
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

17. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
Insoluble except nitrate and acetate
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Tetrahedral

18. What is an Alkyl group?

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19. What are isotopes?
RNH2
acid + alcohol
Conjugate pair (one must be a weak base or acid)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

20. dichromate
do not change
Decant
Unsaturated - addition (ex: decolorize bromine solution)
Cr2O7²?

21. 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
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Ions go through the salt bridge - electrons go through metal wires in the external circuit
ClO2?

22. What do acids plus active metals form?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
T increases exponentially the proportion of molecules with E > Ea

23. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
proton donor base
No - it depends on the number of ions produced on dissolving.
Transition element compounds (except if it has a full or empty d shell)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

24. What shape is water?
White precipitate
blue (BTB)
bent
boiling without losing volatile solvents/reactants

25. How do you compute % dissociation?
Selective absorption
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
[A?]/[HA] x 100 or [BH?]/[B] x 100
A salt solution.

26. What is the test for hydrogen?
Acidified
Greenish-yellow gas
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
lighted splint (positive result=pop)

27. Which value of R do you use for all energy and kinetics calculations?
Concentration
Identity and purity (impure compounds usually have broad & low melting points)
benzene is less reactive than alkenes
R=8.31 J/mol/K

28. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Identity and purity (impure compounds usually have broad & low melting points)
blue
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Acidified

29. What are the signs of ?G and E° for spontaneous reactions?
strong acids/bases are written as H+ or OH- ions
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Soluble
?G=negative - E° must be positive

30. Generally - which oxy acid is strongest?
Glowing splint (positive result=relights)
The one with most oxygen atoms (highest oxidation number)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
small size and high charge

31. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
CH3COO?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
ion pairing

32. What two types of substances are present in all redox reactions?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
an oxidized and reduced substance
same KE - but PEice<PEwater
Saturated - Substitution (which requires more radical conditions)

33. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
OH?
OH- and NH3
T increases exponentially the proportion of molecules with E > Ea

34. What is accuracy?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
How close results are to the accepted value
[A?]/[HA] x 100 or [BH?]/[B] x 100
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

35. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Kc=Kp
zero
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
benzene has a delocalized pi ring structure

36. What do you do to get rid of most of the solution from a precipitate?
No - NH3 and HCl gases are extremely soluble
Decant
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
ion pairing

37. What process do you use to separate two liquids with different boiling points?
Salt and water
fractional distillation
by electrolysis
basic

38. What is HCOOCH3?
Acids; HCOOCH3 is an ester
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Combine the equations for the half reactions in the non-spontaneous direction
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

39. mercury (I) ion
MnO4?
different forms of the same element
Hg2²?
|experimental - accepted|/accepted X 100

40. During a titration what is present in the beaker at the equivalence point?
Increases down group 1 decreases down group 17
A salt solution.
Mono; di; tri; tetra; penta; hexa.
E=q + w (negative is by system - positive is on system)

41. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
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
Pale purple - (orange)-yellow - red - blue - green.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

42. Give an example of a dilute strong acid.
Evaporation
HClO4
ROH
acid + alcohol

43. hydroxide
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
metal oxides and hydrides are ionically bonded and basic
OH?
fractional distillation

44. What is the conjugate base of NH3?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
NH2?
K1 x K2
K2

45. How do you clean a buret/pipette for a titration?
?G= -ve - E°= +ve
Concentration
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

46. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
Transition element compounds (except if it has a full or empty d shell)
bent
A) any range. b) 8-10 c) 4-6
Group 1 hydroxides (ex: NaOH)

47. What type of compounds do Group 14 form?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Most are soluble except Ag - Pb
+4-covalent - +2-ionic
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

48. What do the 'a' and 'b' in Van Der Waal's equation allow for?
An active metal.
CnH2n
a-IMFs - b-molecular volume
RCOR

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

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50. sulfate
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Combine the equations for the half reactions in the non-spontaneous direction
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
SO4²?