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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. acetate
Pipette (burette if need repetition)
0 and 14
fruit - fish - bases
CH3COO?

2. oxalate
C2O4²?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CrO4²?
water and substances with (s) less dense than

3. What type of solutions do small - highly charged cations tend to form?
zero
#ligands=charge x2
Kc=Kp
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

4. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
?G= -ve - E°= +ve
different forms of the same element
Ppt will NOT form (unsaturated)

5. What complex ion does ammonia form with silver? copper? cadmium? zinc?
+4-covalent - +2-ionic
Anode - oxygen. Cathode - hydrogen
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Experimental mass/theoretical mass X 100

6. How do you find the pH for a dibasic acid? (H2A)?
atoms
Perform ICE BOX calculation based on K1
CrO4²?
?H formation of an element in standard state=0

7. What are allotropes?
Disulfur dichloride
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
different forms of the same element
?H-kJ - ?S-J - ?G-kJ

8. What is the formula of butane?
S2O3²?
C4H10
Heptane
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

9. hydroxide
They stay the same.
OH?
Heat a test tube at an angle at the side of the tube (not bottom)
|experimental - accepted|/accepted X 100

10. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
?H formation of an element in standard state=0
R=8.31 J/mol/K
Combine the equations for the half reactions in the non-spontaneous direction

11. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
ion pairing
Pour liquids using a funnel or down a glass rod
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

12. What shape is ammonia?
Salts (ex: CaO + SO2 ? CaSO3)
Heat a test tube at an angle at the side of the tube (not bottom)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Trigonal pyramidal

13. How are primary alcohols turned into acids?
ClO3?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Transition element compounds (except if it has a full or empty d shell)
Filtration

14. What is the formula for percent yield?
Soluble
zero-th: decreases - first: constant - second: increases
0.10M HCl (more ions)
Experimental mass/theoretical mass X 100

15. What is the general formula for an amine?
?G=negative - E° must be positive
RNH2
Exothermic
Initiation energy (NOT Ea)

16. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
MnO4?
Ksp = 27s4
benzene has a delocalized pi ring structure
Reduction always takes place at the cathode (RED CAT) In both types of cell!

17. Do anions flow to the cathode or anode?
H2O + CO2 (it decomposes readily)
small size and high charge
Anode
Conjugate pair (one must be a weak base or acid)

18. If a free element is involved - what type of reaction must be involved?
redox reaction
OH- and NH3
Clear
A salt solution.

19. Which of the rates changes more when temperature is increased?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Identity and purity (impure compounds usually have broad & low melting points)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Distillation

20. copper sulfate
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
catalyst=conc H2SO4
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
blue

21. What are isomers?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Disulfur dichloride
Molecules with the same molecular formulas - but different structural formulas
catalyst=conc H2SO4

22. lead iodide
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)
bright yellow
blue glass - it filters UV
brown volatile liquid

23. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
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.
Pale purple - (orange)-yellow - red - blue - green.
CO (poisonous)
allow for the vapor pressure of water and make sure to level levels

24. chlorite
H2PO4?
Clear
ClO2?
They stay the same.

25. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
ion pairing
Insoluble
Pale yellow

26. How many faradays of electric charge do you need to produce one mole of O2? H2?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
an oxidized and reduced substance
O2 needs 4F/mol H2 needs 2F/mol

27. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
neutralization: high K - H2O product dissociation: low K - H2O reactant
How grouped results are
same KE - but PEice<PEwater
Saturated - Substitution (which requires more radical conditions)

28. What two types of substances are present in all redox reactions?
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.
RCOOH
Cu3(PO4)2
an oxidized and reduced substance

29. How do you get Ecell for spontaneous reactions?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
small size and high charge
bright yellow
Exothermic

30. ammonium/ammonium compounds
blue glass - it filters UV
The compound with the lowest Ksp value.
Soluble
ionic and form hydrogen and hydroxide

31. If Q > Ksp - then system shifts _______ and ppt ______
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
left - ppt will form
Salt + water.
?G= -ve - E°= +ve

32. For a dibasic acid (H2A) - [A²?]= ____ ?
acids
The dilution effect when the solutions mix. M1V1 = M2V2
Mono; di; tri; tetra; penta; hexa.
K2

33. Is the standard entropy (S°) of an element zero?
Kc=Kp
But S° of element is not zero (except at 0K)
E=q + w (negative is by system - positive is on system)
PO4³?

34. What is the general formula for an ester?
Pale yellow
Suniverse increases for spontaneous processes
RCOOR
acids

35. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Only temperature
Combine the equations for the half reactions in the non-spontaneous direction
bases

36. Nonmetals are good _____ agents. Metals are good _______ agents.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
hydroxides (ex: Ba(OH)2)
Conjugate pair (one must be a weak base or acid)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

37. Why are noble gases stable?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Increases.
Glacial acetic acid
fractional distillation

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

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39. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Check for air bubbles in the buret and remove the buret funnel from the buret
Ksp = s²
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

40. What is the word equation for condensation polymerisation ?
do not change
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Soluble except Ag - Pb - Ca - Sr Ba)
HClO4

41. group 1 ions/compounds
RCOOH
Read the bottom of the meniscus
Soluble
bright yellow

42. What is the general formula of an alkane?
CnH(2n+2)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
different forms of the same element
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

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

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44. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Increases.
Insoluble except nitrate and acetate
Group I metals (soft metals) are stored under oil
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

45. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
bent
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
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

46. What is the test for oxygen?
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)
Glowing splint (positive result=relights)
Hg²?
Exothermic (?H for ANY sa/sb = -57kJ/mol)

47. What word is a clue for a redox reaction?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
OH- and NH3
Acidified
q=mc?T q=mL (or n x ?h)

48. How do you clean a buret/pipette for a titration?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Current - time and charge on ion (moles of e used in half cell reaction)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
ClO3?

49. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Insoluble except nitrate and acetate
The dilution effect when the solutions mix. M1V1 = M2V2
Check for air bubbles in the buret and remove the buret funnel from the buret
#ligands=charge x2

50. sulfates
Synthesis - separation and purification of the product and its identification.
Soluble
Soluble except Ag - Pb - Ca - Sr Ba)
Hg²?