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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.
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. lead compounds
Pipette (burette if need repetition)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Insoluble except nitrate and acetate
Both electrons come from the same atom (just as good as a regular bond)

2. How are non-metal oxides and hydrides bonded? are they acidic or basic?
voltaic: - electrolytic: +
non-metal oxides and hydrides are covalently bonded and are acidic.
Synthesis - separation and purification of the product and its identification.
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

3. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
K1 x K2
Insoluble except group 1 and ammonium
Current - time and charge on ion (moles of e used in half cell reaction)
Unsaturated - addition (ex: decolorize bromine solution)

4. What is the word equation for condensation polymerisation ?
methyl formate
boiling without losing volatile solvents/reactants
redox reaction
Monomer + monomer = polymer product + a simple molecule such as water or HCl

5. What do you use to look at burning magnesium? why?
The one with most oxygen atoms (highest oxidation number)
water and substances with (s) less dense than
Saturated - Substitution (which requires more radical conditions)
blue glass - it filters UV

6. How are more active metals reduced?
O2 needs 4F/mol H2 needs 2F/mol
CnH2n
Salt and water
by electrolysis

7. What is the first law of thermodynamics?
Mn²? - Cr³? - Cr³
Clear
a-IMFs - b-molecular volume
E=q + w (negative is by system - positive is on system)

8. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Soluble
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
NO3?
E=q + w (negative is by system - positive is on system)

9. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
0 and 14
Products - reactants (except for BDE when it's reactants - products)
NH2?

10. acetate
CH3COO?
Transition element compounds (except if it has a full or empty d shell)
Soluble
Ions go through the salt bridge - electrons go through metal wires in the external circuit

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

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12. What is the test for hydrogen?
lighted splint (positive result=pop)
Glowing splint (positive result=relights)
do not change
0 and 14

13. During a titration what is present in the beaker at the equivalence point?
Salts (ex: CaO + SO2 ? CaSO3)
A salt solution.
Glacial acetic acid
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

14. When a cell is 'flat' What is its voltage?
zero
Insoluble
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

15. What is the difference between equivalence point and end point of a titration.
O2 needs 4F/mol H2 needs 2F/mol
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.
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
Saturated - Substitution (which requires more radical conditions)

16. What do you do to get rid of most of the solution from a precipitate?
Salt and water
Decant
Anode - oxygen. Cathode - hydrogen
The dilution effect when the solutions mix. M1V1 = M2V2

17. dichromate
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Cr2O7²?
Suniverse increases for spontaneous processes
Reduction always takes place at the cathode (RED CAT) In both types of cell!

18. What is the pH of 1.0M HCl? 1M NaOH?
All except for lithium
0 and 14
do not change
Exothermic (?H for ANY sa/sb = -57kJ/mol)

19. chromate
CrO4²?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
?H-kJ - ?S-J - ?G-kJ
ClO4?

20. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Mn²? - Cr³? - Cr³
0 and 14
#ligands=charge x2
At half equivalence - pH=pKa

21. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
H2O + CO2 (it decomposes readily)
Anode - oxygen. Cathode - hydrogen
Distillation

22. cyanide
K2
Iodine and CO2 (dry ice)
Group 1 hydroxides (ex: NaOH)
CN?

23. How does the melting point of a mixture compare to the MP of a pure substance?
acid + alcohol
Filtration
it is lower and occurs over less sharp a range
Glowing splint (positive result=relights)

24. phosphate
Most are soluble except Ag - Pb
PO4³?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
RCHO (carbonyl at end)

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

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26. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
The Faraday or Faraday's constant.
Ksp = 4s³
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

27. A Bronsted-Lowry base is...
zero
proton acceptor.
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.
They decrease (or could be the same if the solid has ONLY JUST disappeared)

28. What effect does increasing the size/surface area of a voltaic cell have on the cell?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
CN?
it reacts by substitution NOT addition
At half equivalence - pH=pKa

29. What is the formula for alkynes?
CnH2n-2
methyl formate
SO4²?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

30. chlorine
[A?]/[HA] x 100 or [BH?]/[B] x 100
Greenish-yellow gas
water and substances with (s) less dense than
linear

31. mercury (I) ion
Greenish-yellow gas
Hg2²?
They stay the same.
Big K=kf/kr

32. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
CH3COO?
No - it depends on the number of ions produced on dissolving.
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)
NH4?

33. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Greenish-yellow gas
Nothing
10?8

34. What is the general formula for an aldehyde?
Purple
RCHO (carbonyl at end)
White precipitate
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

35. lead iodide
+4-covalent - +2-ionic
A salt solution.
0 and 14
bright yellow

36. silver iodide
blue
Filtration
Pale yellow
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

37. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
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)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
diamond and graphite

38. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
benzene has a delocalized pi ring structure
Pale purple - (orange)-yellow - red - blue - green.
RCOOH
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

39. What device would you use to measure a volume of gas?
Eudiometer
OH- and NH3
non-metal oxides and hydrides are covalently bonded and are acidic.
metal oxides and hydrides are ionically bonded and basic

40. copper sulfate
by electrolysis
All except for lithium
blue
Molecules with the same molecular formulas - but different structural formulas

41. nitrate
NO3?
ROH
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Selective absorption

42. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Hg²?
redox reaction
Ksp = s²

43. What is the general formula for an ester?
RCOOR
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)
HClO4
Exothermic

44. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
OH- and NH3
Clear
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

45. Is the freezing of ice endothermic or exothermic?
The Faraday or Faraday's constant.
ionic and form hydrogen and hydroxide
Exothermic
?G=negative - E° must be positive

46. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Group 1 hydroxides (ex: NaOH)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
CnH2n+1 often designated 'R' ex C3H7 is propyl
water and substances with (s) less dense than

47. What are amphoteric oxides?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Synthetic condensation polymer (aka a polyamide)
Filtration
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?)

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

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49. The oxidation # for acid base reactions...
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
do not change
Conjugate pair (one must be a weak base or acid)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

50. carbonate
Separating funnel
Making sigma bonds and holding lone pairs
A salt solution.
CO3²?