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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. What shape is carbon dioxide?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
linear
Pale purple - (orange)-yellow - red - blue - green.
CO3²?

2. If Q < Ksp a ppt ______
Ions go through the salt bridge - electrons go through metal wires in the external circuit
water and substances with (s) less dense than
R=8.31 J/mol/K
Ppt will NOT form (unsaturated)

3. chromate
zero
CrO4²?
different forms of the same element
Synthesis - separation and purification of the product and its identification.

4. What process do you use to obtain the precipitate from a solution?
Filtration
No - NH3 and HCl gases are extremely soluble
R=8.31 J/mol/K
They decrease (or could be the same if the solid has ONLY JUST disappeared)

5. What is the second law of thermodynamics?
left - ppt will form
Nothing
NO3?
Suniverse increases for spontaneous processes

6. What is the general formula for an amine?
CnH(2n+2)
RNH2
Increases down group 1 decreases down group 17
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

7. When combining half equations - what do you do to E° values when multiplying coefficients?
methyl formate
No - NH3 and HCl gases are extremely soluble
Pour liquids using a funnel or down a glass rod
Nothing

8. What is the relationship in strength between sigma and pi bonds?
same KE - but PEice<PEwater
red - green - blue
benzene is less reactive than alkenes
Sigma bonds are stronger than pi bonds

9. Generally - which oxy acid is strongest?
Soluble
The one with most oxygen atoms (highest oxidation number)
CnH2n
T increases exponentially the proportion of molecules with E > Ea

10. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
C4H10
RCOOR
Tetrahedral
No - it depends on the number of ions produced on dissolving.

11. If Q > Ksp - then system shifts _______ and ppt ______
Silvery gray solid - brown - purple
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
The one with most oxygen atoms (highest oxidation number)
left - ppt will form

12. What should you check for before you begin titrating?
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
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.
PO4³?

13. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
H2PO4?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Selective absorption

14. acetates
OH- and NH3
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Insoluble (except group 1 ammonium and Ba)
Soluble

15. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
ROR
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Pipette (burette if need repetition)
same KE - but PEice<PEwater

16. What is the general formula for an ester?
Big K=kf/kr
allow for the vapor pressure of water and make sure to level levels
RCOOR
H+

17. phosphate
PO4³?
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
R=8.31 J/mol/K
Orange

18. What type of solutions do small - highly charged cations tend to form?
ion pairing
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)
brown volatile liquid
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

19. Ca - Sr - Ba
0 and 14
Transition element compounds (except if it has a full or empty d shell)
How close results are to the accepted value
hydroxides (ex: Ba(OH)2)

20. What are two allotropes of carbon?
diamond and graphite
fruit - fish - bases
Soluble
Glowing splint (positive result=relights)

21. What is accuracy?
Most INsoluble except group 1 and ammonium
OH- and NH3
are less dense than water
How close results are to the accepted value

22. What process do you use to obtain the solute from a solution?
P2O5
Iodine and CO2 (dry ice)
Evaporation
C4H10

23. What is a dipeptide? polypeptide? protein?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
ethers
All except for lithium
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

24. What is the general formula for an aldehyde?
RCHO (carbonyl at end)
Ksp = 27s4
'non-active' metals such as Cu - Ag - Au - Pt - etc.
benzene is less reactive than alkenes

25. What is the general formula for alkyl halides?
water and substances with (s) less dense than
RX
RCOR
zero-th: decreases - first: constant - second: increases

26. How do you compute % dissociation?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
[A?]/[HA] x 100 or [BH?]/[B] x 100
catalyst=conc H2SO4

27. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
CN?
NO3?
CnH2n+1 often designated 'R' ex C3H7 is propyl

28. Which of the rates changes more when temperature is increased?
SO4²?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Tetrahedral

29. dihydrogen phosphate
H2PO4?
Only temperature
MnO4?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

30. Aromatic compounds contain what?
CnH(2n+2)
The benzene ring (or more correctly the phenyl group - C6H5)
?H formation of an element in standard state=0
Only temperature

31. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
diamond and graphite
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Trigonal pyramidal

32. If ?S is positive - are the products more or less chaotic than the reactants?
Suniverse increases for spontaneous processes
methyl formate
proton donor base
More chaotic (ex: gases made)

33. What do nonmetal oxides plus water form?
Increases down group 1 decreases down group 17
acids
Pale yellow
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

34. What do the 'a' and 'b' in Van Der Waal's equation allow for?
#ligands=charge x2
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
methyl formate
a-IMFs - b-molecular volume

35. What do acids plus active metals form?
0.10M HCl (more ions)
CN?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
H+

36. What is the formula for percent error?
Acid rain - dissolves marble buildings/statues and kills trees.
basic
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
|experimental - accepted|/accepted X 100

37. What type of compounds do Group 14 form?
MnO4?
+4-covalent - +2-ionic
#ligands=charge x2
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

38. phosphates
blue (BTB)
Most INsoluble except group 1 and ammonium
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Mn²? - Cr³? - Cr³

39. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
no - they're written undissociated (HAaq)
Insoluble except nitrate and acetate

40. What element is used to vulcanize rubber?
Sulfur
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
small size and high charge
neutralization: high K - H2O product dissociation: low K - H2O reactant

41. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
S crystal at 0K=0
linear

42. What is an Alkyl group?

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43. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
fractional distillation
They decrease (or could be the same if the solid has ONLY JUST disappeared)
More chaotic (ex: gases made)
Both electrons come from the same atom (just as good as a regular bond)

44. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Perform ICE BOX calculation based on K1
Iodine and CO2 (dry ice)
bent

45. What shape is water?
a-IMFs - b-molecular volume
RCHO (carbonyl at end)
bent
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

46. Why are noble gases stable?
MnO4?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ns² electrons (first in-first out)

47. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
RCOR
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Salt + water.
atoms

48. What is the conjugate acid of H2PO4?
Insoluble except nitrate and acetate
H3PO4
HClO4
OH?

49. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
0 and 14
More chaotic (ex: gases made)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

50. hydroxide
Nothing
OH?
Salts (ex: CaO + SO2 ? CaSO3)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O