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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.
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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 is the formula for alkanes?
CnH2n+2
Sulfur
Hg2²?
Insoluble except nitrate and acetate

2. What is the word equation for addition polymerisation?
Group I metals (soft metals) are stored under oil
linear
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Exothermic

3. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
a-IMFs - b-molecular volume
acids
Graduated cylinder

4. What do group I/II metal oxides and acids form?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Salt and water
Only temperature
Both electrons come from the same atom (just as good as a regular bond)

5. barium sulfate
Disulfur dichloride
+4-covalent - +2-ionic
Pale yellow
White precipitate

6. What steps do organic labs consist of?
NO3?
Synthesis - separation and purification of the product and its identification.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Hg²?

7. How many faradays of electric charge do you need to produce one mole of O2? H2?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
O2 needs 4F/mol H2 needs 2F/mol
-Ea/R
Both electrons come from the same atom (just as good as a regular bond)

8. What does saturated mean? Unsaturated?
NH4?
Mono; di; tri; tetra; penta; hexa.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

9. Why are i factors (Van't Hoff factors) often less than ideal?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Most are soluble except Ag - Pb
ion pairing
Nothing

10. What does the solubility of organic compounds depend on?
Perform ICE BOX calculation based on K1
No - NH3 and HCl gases are extremely soluble
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

11. What reacts with an acid to create hydrogen gas?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
An active metal.
ClO3?
Insoluble except for nitrate and acetate

12. What should you check for before you begin titrating?
Iodine and CO2 (dry ice)
Check for air bubbles in the buret and remove the buret funnel from the buret
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

13. Lattice energy is high for ions with _____ size and _____ charge
Soluble except Ag - Pb - Ca - Sr Ba)
E=q + w (negative is by system - positive is on system)
small size and high charge
Decant

14. How do you dilute an acid?

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15. oxalate
C2O4²?
Only temperature
Increases down group 1 decreases down group 17
Conjugate pair (one must be a weak base or acid)

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

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17. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
Nothing
The one with most oxygen atoms (highest oxidation number)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

18. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
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)
Selective absorption
H+

19. copper sulfate
Ksp = 27s4
blue
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
?H-kJ - ?S-J - ?G-kJ

20. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Q=It (time in seconds)
are less dense than water
R=8.31 J/mol/K

21. If a free element is involved - what type of reaction must be involved?
no - they're written undissociated (HAaq)
redox reaction
H+
blue glass - it filters UV

22. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
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?)
fruit - fish - bases
Ksp = 108s5
Only temperature

23. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
Pipette (burette if need repetition)
R=8.31 J/mol/K
10?8
Filtration

24. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Nothing
Insoluble except for nitrate and acetate

25. How do you compute % dissociation?
OH?
Add acid to water so that the acid doesn't boil and spit
Evaporation
[A?]/[HA] x 100 or [BH?]/[B] x 100

26. Which value of R do you use for all energy and kinetics calculations?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
0.10M HCl (more ions)
R=8.31 J/mol/K
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.

27. What is the conjugate acid of H2PO4?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
RNH2
atoms
H3PO4

28. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
C4H10
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Filtration
it's lower and occurs over less sharp a range

29. What do you do to get rid of most of the solution from a precipitate?
Soluble
CO (poisonous)
Decant
Salts (ex: CaO + SO2 ? CaSO3)

30. When driving off water from a hydrate - how do you tell you're done?
How close results are to the accepted value
White precipitate
E=q + w (negative is by system - positive is on system)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

31. Buffer capacity must contain decent amounts of a ________ ________
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Conjugate pair (one must be a weak base or acid)
An active metal.
different forms of the same element

32. What are hybrid orbitals used for?
Making sigma bonds and holding lone pairs
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
blue
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)

33. Esters smell like _______ and amines smell like _______ and are ______.
Eudiometer
Kc=Kp
fruit - fish - bases
Ksp = 27s4

34. What shape is methane?
Tetrahedral
H+
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
The benzene ring (or more correctly the phenyl group - C6H5)

35. Give an example of a dilute strong acid.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
same KE - but PEice<PEwater
HClO4
Insoluble except nitrate and acetate

36. What type of compounds do metals/non metals form?
zero
Exothermic
NH2?
Ionic compounds

37. acetates
same KE - but PEice<PEwater
Soluble
0 and 14
CN?

38. How do you get Ecell for spontaneous reactions?
An active metal.
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

39. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
SO4²?
Hg2²?
Group I metals (soft metals) are stored under oil

40. What are the products of the reaction between group 1 metals and water?

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41. How do you find the pH for a dibasic acid? (H2A)?
Orange
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Ksp = s²
Perform ICE BOX calculation based on K1

42. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
CH3COO?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
?H formation of an element in standard state=0
Salts (ex: CaO + SO2 ? CaSO3)

43. What process do you use to obtain the solute from a solution?
Evaporation
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
How grouped results are
They decrease (or could be the same if the solid has ONLY JUST disappeared)

44. dichromate
Cr2O7²?
left - ppt will form
No - it depends on the number of ions produced on dissolving.
CnH2n+1 often designated 'R' ex C3H7 is propyl

45. Acids + Carbonates (bicarbonates) make?
CnH2n+1 often designated 'R' ex C3H7 is propyl
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Ksp = 108s5
ion pairing

46. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
-Ea/R
Decant
Kc=Kp
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

47. dichromate (soln + most solids)
CO3²?
red - green - blue
diamond and graphite
Orange

48. How are primary alcohols turned into acids?
Acidified
RCOOR
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Graduated cylinder

49. 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
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
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Heptane

50. If ?S is positive - are the products more or less chaotic than the reactants?
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.
CnH2n+2
More chaotic (ex: gases made)
ClO4?