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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 a dipeptide? polypeptide? protein?
Mono; di; tri; tetra; penta; hexa.
are less dense than water
HClO4
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

2. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Heptane
Ppt will NOT form (unsaturated)
Unsaturated - addition (ex: decolorize bromine solution)

3. What process do you use to obtain the precipitate from a solution?
Initiation energy (NOT Ea)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Orange
Filtration

4. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
water and substances with (s) less dense than
Mn²? - Cr³? - Cr³
Ionic compounds
ROH

5. What part of a liquid do you look at to measure its volume?
No - it depends on the number of ions produced on dissolving.
Anode - oxygen. Cathode - hydrogen
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Read the bottom of the meniscus

6. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
P2O5
fractional distillation
Ksp = 27s4
At half equivalence - pH=pKa

7. ammonium
?H formation of an element in standard state=0
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
NH4?
Soluble except Ag - Pb - Ca - Sr Ba)

8. What type of compounds do Group 14 form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Soluble
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
+4-covalent - +2-ionic

9. What is the general formula for a ketone?
Pale yellow
Conjugate pair (one must be a weak base or acid)
Mono; di; tri; tetra; penta; hexa.
RCOR

10. Both Acetic acid and ____________ are also functional isomers.
Ksp = 108s5
Salt + water.
methyl formate
0.10M HCl (more ions)

11. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Purple
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
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

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

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13. cyanide
Transition element compounds (except if it has a full or empty d shell)
Identity and purity (impure compounds usually have broad & low melting points)
Both electrons come from the same atom (just as good as a regular bond)
CN?

14. Does reactivity increase/decrease going down group 1 and group 17?
Synthesis - separation and purification of the product and its identification.
RNH2
an oxidized and reduced substance
Increases down group 1 decreases down group 17

15. 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
Filtration
proton acceptor.
S crystal at 0K=0

16. What is reflux?
Eudiometer
boiling without losing volatile solvents/reactants
non-metal oxides and hydrides are covalently bonded and are acidic.
water and substances with (s) less dense than

17. nitrates
ClO4?
Soluble
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Disulfur dichloride

18. chlorine
Greenish-yellow gas
?H formation of an element in standard state=0
Heptane
Decant

19. The definition of acidic basic and neutral aqueous solutions is:
OH?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
ClO?
it's lower and occurs over less sharp a range

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

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21. lead compounds
Glowing splint (positive result=relights)
Insoluble except nitrate and acetate
10?8
Ksp = 4s³

22. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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23. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Combine the equations for the half reactions in the non-spontaneous direction
All except for lithium
do not change
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

24. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
Evaporation
Hg²?
yellow

25. When a cell is 'flat' What is its voltage?
zero
same KE - but PEice<PEwater
?H formation of an element in standard state=0
A) any range. b) 8-10 c) 4-6

26. ammonium/ammonium compounds
proton acceptor.
Mono; di; tri; tetra; penta; hexa.
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Soluble

27. What are hybrid orbitals used for?
no - they're written undissociated (HAaq)
NH4?
Making sigma bonds and holding lone pairs
bases

28. What kind of bonding structure does benzene have?
Kc=Kp
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
benzene has a delocalized pi ring structure
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

29. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Ppt will NOT form (unsaturated)
linear
CN?
zero

30. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Mn²? - Cr³? - Cr³
Insoluble except for nitrate and acetate
a-IMFs - b-molecular volume
basic

31. Give an example of a concentrated weak acid.
T increases exponentially the proportion of molecules with E > Ea
Glacial acetic acid
The dilution effect when the solutions mix. M1V1 = M2V2
small size and high charge

32. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
ClO3?
Clear
HClO4
water and substances with (s) less dense than

33. Why are noble gases stable?
diamond and graphite
SO4²?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

34. Is the freezing of ice endothermic or exothermic?
hydroxides (ex: Ba(OH)2)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Exothermic
Insoluble except for nitrate and acetate

35. carbonate
Ksp = s²
Ksp = 108s5
O2 needs 4F/mol H2 needs 2F/mol
CO3²?

36. What is the general formula for alkyl halides?
RX
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)
Acid rain - dissolves marble buildings/statues and kills trees.
Soluble except Ag - Pb - Ca - Sr Ba)

37. dichromate
Pale yellow
K2
Cr2O7²?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

38. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
The dilution effect when the solutions mix. M1V1 = M2V2

39. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
CnH(2n+2)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
proton donor base

40. During a titration what is present in the beaker at the equivalence point?
Insoluble
A salt solution.
NH4?
RCOR

41. What shape is ammonia?
lighted splint (positive result=pop)
Trigonal pyramidal
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)
Decant

42. lead iodide
voltaic: + electrolytic: -
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
bright yellow
blue (BTB)

43. Acids + Carbonates (bicarbonates) make?
brown volatile liquid
CO2 and H2O
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
How grouped results are

44. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Glowing splint (positive result=relights)
NH4?
Identity and purity (impure compounds usually have broad & low melting points)

45. Acid plus base make?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Salt + water.
HClO4
NO3?

46. What do metal oxides plus acids form?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
More chaotic (ex: gases made)
K1 x K2
Salt + water

47. Alkenes are ________ and react by __________
Insoluble (except group 1 ammonium and Ba)
Suniverse increases for spontaneous processes
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Unsaturated - addition (ex: decolorize bromine solution)

48. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Group 1 hydroxides (ex: NaOH)
?G=negative - E° must be positive
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
fractional distillation

49. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
RCOOR
Group I metals (soft metals) are stored under oil

50. Which of the rates changes more when temperature is increased?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Distillation
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
metal oxides and hydrides are ionically bonded and basic