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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. If Q > Ksp - then system shifts _______ and ppt ______
CO3²?
left - ppt will form
0.10M HCl (more ions)
no - they're written undissociated (HAaq)

2. What do you use to look at burning magnesium? why?
Mono; di; tri; tetra; penta; hexa.
basic
blue glass - it filters UV
[A?]/[HA] x 100 or [BH?]/[B] x 100

3. Does reactivity increase/decrease going down group 1 and group 17?
The benzene ring (or more correctly the phenyl group - C6H5)
CO2 and H2O
Increases down group 1 decreases down group 17
C2O4²?

4. What is the general formula for an ether?
Increases down group 1 decreases down group 17
ROR
left - ppt will form
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

5. What are the units of the first order rate constant?
Insoluble except group 1 and ammonium
acid + alcohol
T increases exponentially the proportion of molecules with E > Ea
Time?¹ - (ex. s?¹ - hr?¹ - etc)

6. What is the formula for summation?

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7. Both Acetic acid and ____________ are also functional isomers.
q=mc?T q=mL (or n x ?h)
methyl formate
HClO4
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

8. 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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9. halides
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Most are soluble except Ag - Pb
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?)
Cr2O7²?

10. What do group I/II metal oxides and acids form?
voltaic: + electrolytic: -
Disulfur dichloride
it is lower and occurs over less sharp a range
Salt and water

11. The definition of acidic basic and neutral aqueous solutions is:
Eudiometer
ROR
Anode
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

12. nitrate
Salt + water
Cu3(PO4)2
NO3?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

13. Ions are not ______.
atoms
metal oxides and hydrides are ionically bonded and basic
A) any range. b) 8-10 c) 4-6
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

14. How are primary alcohols turned into acids?
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
Salts (ex: CaO + SO2 ? CaSO3)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

15. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
CnH2n-2
CnH(2n+2)
#ligands=charge x2

16. dichromate (soln + most solids)
Initiation energy (NOT Ea)
+4-covalent - +2-ionic
Orange
Clear

17. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
ROR
Evaporation
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
same KE - but PEice<PEwater

18. How are more active metals reduced?
The Faraday or Faraday's constant.
bases
Iodine and CO2 (dry ice)
by electrolysis

19. What is precision?
How grouped results are
Iodine and CO2 (dry ice)
ROR
?G=negative - E° must be positive

20. silver compounds
Eudiometer
Filtration
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Insoluble except for nitrate and acetate

21. 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.
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
Acid rain - dissolves marble buildings/statues and kills trees.
Perform ICE BOX calculation based on K1
A) any range. b) 8-10 c) 4-6

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

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23. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
diamond and graphite
No - it depends on the number of ions produced on dissolving.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

24. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
C2O4²?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
No - NH3 and HCl gases are extremely soluble
The compound with the lowest Ksp value.

25. Alkanes are _________ and react by _________
Saturated - Substitution (which requires more radical conditions)
Glacial acetic acid
diamond and graphite
RCHO (carbonyl at end)

26. What is the charge on a chlorine atom?
small size and high charge
water and substances with (s) less dense than
Purple
zero

27. What is the relationship in strength between sigma and pi bonds?
H2PO4?
voltaic: - electrolytic: +
zero-th: decreases - first: constant - second: increases
Sigma bonds are stronger than pi bonds

28. Name six characteristics of transition elements (or their compounds)
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)
CnH2n
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

29. What is reflux?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
boiling without losing volatile solvents/reactants
do not change

30. How are metal oxides and hydrides bonded? are they acidic or basic?
metal oxides and hydrides are ionically bonded and basic
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
allow for the vapor pressure of water and make sure to level levels
Monomer + monomer = polymer product + a simple molecule such as water or HCl

31. What do you do to get rid of most of the solution from a precipitate?
Conjugate pair (one must be a weak base or acid)
ns² electrons (first in-first out)
Decant
Concentration

32. chlorine
Big K=kf/kr
?G= -ve - E°= +ve
Greenish-yellow gas
allow for the vapor pressure of water and make sure to level levels

33. primary colors
CnH(2n+2)
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
red - green - blue
brown volatile liquid

34. What are the signs of ?G and E° for spontaneous reactions?
CrO4²?
Insoluble except group 1 and ammonium
atoms
?G=negative - E° must be positive

35. potassium permanganate
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
C2O4²?
Greenish-yellow gas
Purple

36. What should you check for before you begin titrating?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Ksp = 27s4
Check for air bubbles in the buret and remove the buret funnel from the buret
CnH2n+2

37. What type of polymer is nylon?
NH4?
OH- and NH3
non-metal oxides and hydrides are covalently bonded and are acidic.
Synthetic condensation polymer (aka a polyamide)

38. copper sulfate
Iodine and CO2 (dry ice)
Pour liquids using a funnel or down a glass rod
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
blue

39. What is the conjugate acid of H2PO4?
ns² electrons (first in-first out)
H3PO4
ClO4?
Greenish-yellow gas

40. What two compounds are great oxidizing agents?

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41. ammonium/ammonium compounds
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Group I metals (soft metals) are stored under oil
Soluble
Perform ICE BOX calculation based on K1

42. How do you get the equation for a net electrolysis reaction?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
NH4?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Combine the equations for the half reactions in the non-spontaneous direction

43. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Soluble
Ksp = 108s5
+4-covalent - +2-ionic

44. At what point during titration do you have the perfect buffer - and what is the pH at this point?
benzene is less reactive than alkenes
Hg²?
At half equivalence - pH=pKa
Increases.

45. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
Soluble
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
left - ppt will form

46. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Iodine and CO2 (dry ice)
a-IMFs - b-molecular volume
Eudiometer
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

47. What is the word equation for condensation polymerisation ?
ionic and form hydrogen and hydroxide
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Molecules with the same molecular formulas - but different structural formulas
are less dense than water

48. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
RCOOR
Pale purple - (orange)-yellow - red - blue - green.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
C4H10

49. How do you explain trends in atomic properties using Coulomb's Law?
P2O5
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Soluble
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

50. Buffer capacity must contain decent amounts of a ________ ________
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
voltaic: - electrolytic: +
Conjugate pair (one must be a weak base or acid)
different forms of the same element