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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 things should you remember to do when collecting gas over water?
The dilution effect when the solutions mix. M1V1 = M2V2
allow for the vapor pressure of water and make sure to level levels
Increases.
Kc=Kp

2. Ions are not ______.
MnO4?
Making sigma bonds and holding lone pairs
atoms
Insoluble except for nitrate and acetate

3. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
MnO4?
Iodine and CO2 (dry ice)
water and substances with (s) less dense than
Both electrons come from the same atom (just as good as a regular bond)

4. What electrons are lost/gained first in transition element ions?
White precipitate
ns² electrons (first in-first out)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Soluble

5. iodine - iodine solution - iodine vapor
Exothermic
zero
Silvery gray solid - brown - purple
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

6. The definition of acidic basic and neutral aqueous solutions is:
Sulfur
S crystal at 0K=0
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Nothing

7. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Pale purple - (orange)-yellow - red - blue - green.
Clear
Ksp = 27s4
Pour liquids using a funnel or down a glass rod

8. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
How close results are to the accepted value
They stay the same.
-Ea/R

9. Aromatic compounds contain what?
Anode
A) any range. b) 8-10 c) 4-6
lighted splint (positive result=pop)
The benzene ring (or more correctly the phenyl group - C6H5)

10. What does a short - sharp melting point indicate?
Iodine and CO2 (dry ice)
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?)
benzene has a delocalized pi ring structure
Identity and purity (impure compounds usually have broad & low melting points)

11. Why are i factors (Van't Hoff factors) often less than ideal?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
ion pairing
P2O5
strong acids/bases are written as H+ or OH- ions

12. What is the general formula for alkyl halides?
yellow
methyl formate
H3PO4
RX

13. 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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14. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
A) any range. b) 8-10 c) 4-6
Heat a test tube at an angle at the side of the tube (not bottom)

15. What measuring device would you use for very small volumes of liquids?
Heptane
They stay the same.
Insoluble except group 1 and ammonium
Pipette (burette if need repetition)

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

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17. What shape is ammonia?
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
C4H10
Iodine and CO2 (dry ice)
Trigonal pyramidal

18. When the salt bridge is removed what happens to the cell reaction?
Cr2O7²?
It ceases - the circuit is broken.
-Ea/R
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

19. What is the formula for summation?

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20. bromine
blue glass - it filters UV
It ceases - the circuit is broken.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
brown volatile liquid

21. What is HCOOCH3?
White precipitate
diamond and graphite
Acids; HCOOCH3 is an ester
CN?

22. phosphates
Products - reactants (except for BDE when it's reactants - products)
Most INsoluble except group 1 and ammonium
Soluble
CO (poisonous)

23. How are primary alcohols turned into acids?
Tetrahedral
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
do not change
Ksp = 108s5

24. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Selective absorption
Products - reactants (except for BDE when it's reactants - products)
voltaic: + electrolytic: -
Graduated cylinder

25. permanganate
Nothing
MnO4?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
ROR

26. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
The benzene ring (or more correctly the phenyl group - C6H5)

27. How do you dilute an acid?

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28. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
Soluble
Acids; HCOOCH3 is an ester
ClO?

29. If Q > Ksp - then system shifts _______ and ppt ______
Heat a test tube at an angle at the side of the tube (not bottom)
left - ppt will form
S2O3²?
do not change

30. acetates
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
T increases exponentially the proportion of molecules with E > Ea
P2O5
Soluble

31. What are two allotropes of carbon?
it is lower and occurs over less sharp a range
Trigonal pyramidal
do not change
diamond and graphite

32. 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)
ion pairing
neutralization: high K - H2O product dissociation: low K - H2O reactant
An active metal.

33. A Bronsted-Lowry base is...
RX
-Ea/R
proton acceptor.
acid + alcohol

34. mercury (I) ion
More chaotic (ex: gases made)
Hg2²?
No - it depends on the number of ions produced on dissolving.
small size and high charge

35. What steps do organic labs consist of?
Synthesis - separation and purification of the product and its identification.
zero
RNH2
The compound with the lowest Ksp value.

36. barium sulfate
Ionic compounds
Evaporation
At half equivalence - pH=pKa
White precipitate

37. During a titration what is present in the beaker at the equivalence point?
diamond and graphite
A salt solution.
it reacts by substitution NOT addition
blue (BTB)

38. What kind of bonding structure does benzene have?
Check for air bubbles in the buret and remove the buret funnel from the buret
Q=It (time in seconds)
benzene has a delocalized pi ring structure
Ksp = 108s5

39. What is the name of S2Cl2? (Know how to name others like this - too)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Disulfur dichloride
No - it depends on the number of ions produced on dissolving.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

40. A geometric (or cis-trans) isomer exists due to.....
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Saturated - Substitution (which requires more radical conditions)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
chemically (ex: with carbon)

41. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Disulfur dichloride
The one with most oxygen atoms (highest oxidation number)
More chaotic (ex: gases made)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

42. If Q < Ksp a ppt ______
Salts (ex: CaO + SO2 ? CaSO3)
Salt + water.
Ppt will NOT form (unsaturated)
C2O4²?

43. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Orange
allow for the vapor pressure of water and make sure to level levels
Pipette (burette if need repetition)
non-metal oxides and hydrides are covalently bonded and are acidic.

44. When is ?G zero?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Decant
ROH

45. What is Big K in terms of kf and kr?
Big K=kf/kr
Cu3(PO4)2
Greenish-yellow gas
it's lower and occurs over less sharp a range

46. What is the general formula for an ether?
non-metal oxides and hydrides are covalently bonded and are acidic.
Soluble except Ag - Pb - Ca - Sr Ba)
Glowing splint (positive result=relights)
ROR

47. Why are i factors (Van't Hoff factors) often less than ideal?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Anode - oxygen. Cathode - hydrogen
CnH2n+1 often designated 'R' ex C3H7 is propyl
ion pairing

48. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
same KE - but PEice<PEwater
no - they're written undissociated (HAaq)
R=8.31 J/mol/K
The dilution effect when the solutions mix. M1V1 = M2V2

49. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
S crystal at 0K=0
0.10M HCl (more ions)

50. What is the first law of thermodynamics?
RCOOR
Clear
q=mc?T q=mL (or n x ?h)
E=q + w (negative is by system - positive is on system)