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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. Do anions flow to the cathode or anode?
Anode
Soluble
Evaporation
Pale purple - (orange)-yellow - red - blue - green.

2. What are two allotropes of carbon?
diamond and graphite
CnH2n+1 often designated 'R' ex C3H7 is propyl
an oxidized and reduced substance
CrO4²?

3. permanganate
blue (BTB)
diamond and graphite
Insoluble except group 1 and ammonium
MnO4?

4. What do hydrocarbons form when they burn in air (oxygen)?
CO2 and H2O
The compound with the lowest Ksp value.
acids
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

5. silver iodide
Decant
bright yellow
Pale yellow
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

6. Why are noble gases stable?
OH?
Sigma bonds are stronger than pi bonds
'non-active' metals such as Cu - Ag - Au - Pt - etc.
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

7. silver compounds
Insoluble except for nitrate and acetate
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Ionic compounds
benzene is less reactive than alkenes

8. perchlorate
How grouped results are
NO3?
ClO4?
Orange

9. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
voltaic: - electrolytic: +
How close results are to the accepted value

10. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
NO3?
Kc=Kp
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

11. Give an example of a concentrated weak acid.
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.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Glacial acetic acid
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

12. What type of compounds do Group 14 form?
Only temperature
Decant
+4-covalent - +2-ionic
Nothing

13. At what point during titration do you have the perfect buffer - and what is the pH at this point?
#ligands=charge x2
Salts (ex: CaO + SO2 ? CaSO3)
Evaporation
At half equivalence - pH=pKa

14. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
RX
|experimental - accepted|/accepted X 100
No - it depends on the number of ions produced on dissolving.
Iodine and CO2 (dry ice)

15. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
S crystal at 0K=0
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Purple
Reduction always takes place at the cathode (RED CAT) In both types of cell!

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

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17. For a dibasic acid (H2A) - [A²?]= ____ ?
CnH2n-2
+4-covalent - +2-ionic
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
K2

18. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Perform ICE BOX calculation based on K1
It ceases - the circuit is broken.
+4-covalent - +2-ionic
water and substances with (s) less dense than

19. What does the solubility of organic compounds depend on?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
OH- and NH3
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

20. What is precision?
Iodine and CO2 (dry ice)
No - it depends on the number of ions produced on dissolving.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
How grouped results are

21. Metal hydrides are _____ and form _______ and _______ when added to water
CO2 and H2O
zero-th: decreases - first: constant - second: increases
ionic and form hydrogen and hydroxide
diamond and graphite

22. What word is a clue for a redox reaction?
Selective absorption
K2
Acidified
Orange

23. What are amphoteric oxides?
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?)
Silvery gray solid - brown - purple
PO4³?
Insoluble

24. What is the formula for alkanes?
methyl formate
CnH2n+2
different forms of the same element
Insoluble

25. What are two substances that sublime at 1 atm when heated?
Glacial acetic acid
look for changes in oxidation # - the one that goes up is oxidized and is the RA
q=mc?T q=mL (or n x ?h)
Iodine and CO2 (dry ice)

26. If ?S is positive - are the products more or less chaotic than the reactants?
Kc=Kp
More chaotic (ex: gases made)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

27. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
non-metal oxides and hydrides are covalently bonded and are acidic.
Insoluble except for nitrate and acetate
Read the bottom of the meniscus

28. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
NH2?
Big K=kf/kr
by electrolysis
Pale purple - (orange)-yellow - red - blue - green.

29. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Check for air bubbles in the buret and remove the buret funnel from the buret
allow for the vapor pressure of water and make sure to level levels
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
How close results are to the accepted value

30. Where are group I metals stored?
Soluble
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Group I metals (soft metals) are stored under oil
Salt + water.

31. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Identity and purity (impure compounds usually have broad & low melting points)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
small size and high charge

32. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
But S° of element is not zero (except at 0K)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
H2PO4?

33. What is the general formula of an alkane?
CO (poisonous)
Selective absorption
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
CnH(2n+2)

34. Ca - Sr - Ba
R=8.31 J/mol/K
A) any range. b) 8-10 c) 4-6
hydroxides (ex: Ba(OH)2)
NH4?

35. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Initiation energy (NOT Ea)
neutralization: high K - H2O product dissociation: low K - H2O reactant

36. What reacts with an acid to create hydrogen gas?
H3PO4
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
No - it depends on the number of ions produced on dissolving.
An active metal.

37. Name C7H16
The one with most oxygen atoms (highest oxidation number)
PO4³?
Heptane
The Faraday or Faraday's constant.

38. How many ligands attach to a central ion in a complex ion?
ClO2?
Synthesis - separation and purification of the product and its identification.
#ligands=charge x2
Cu3(PO4)2

39. What is the general formula for an ether?
it's lower and occurs over less sharp a range
proton donor base
yellow
ROR

40. What is the general formula for a ketone?
redox reaction
RCOR
?H-kJ - ?S-J - ?G-kJ
They decrease (or could be the same if the solid has ONLY JUST disappeared)

41. barium sulfate
'non-active' metals such as Cu - Ag - Au - Pt - etc.
CrO4²?
White precipitate
No - it depends on the number of ions produced on dissolving.

42. What things should you remember to do when collecting gas over water?
hydroxides (ex: Ba(OH)2)
Cu3(PO4)2
Purple
allow for the vapor pressure of water and make sure to level levels

43. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Anode - oxygen. Cathode - hydrogen
Mn²? - Cr³? - Cr³
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Big K=kf/kr

44. A Bronsted-Lowry acid is...
proton donor base
ClO?
Separating funnel
Suniverse increases for spontaneous processes

45. What are the units of the first order rate constant?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
K2
Time?¹ - (ex. s?¹ - hr?¹ - etc)
ClO2?

46. What do you use to look at burning magnesium? why?
ClO4?
ion pairing
Ksp = s²
blue glass - it filters UV

47. What is reflux?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
No - NH3 and HCl gases are extremely soluble
?H-kJ - ?S-J - ?G-kJ
boiling without losing volatile solvents/reactants

48. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
CO (poisonous)
an oxidized and reduced substance
Anode - oxygen. Cathode - hydrogen
Transition element compounds (except if it has a full or empty d shell)

49. What is the name of S2Cl2? (Know how to name others like this - too)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Combine the equations for the half reactions in the non-spontaneous direction
Disulfur dichloride
Sigma bonds are stronger than pi bonds

50. Do you use J or kJ for ?H - ?S - and ?G?
?H-kJ - ?S-J - ?G-kJ
brown volatile liquid
?G= -ve - E°= +ve
Time?¹ - (ex. s?¹ - hr?¹ - etc)