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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 element is used to vulcanize rubber?
Glacial acetic acid
Increases.
ethers
Sulfur

2. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
10?8
A salt solution.
C2O4²?
Reduction always takes place at the cathode (RED CAT) In both types of cell!

3. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Add acid to water so that the acid doesn't boil and spit
Eudiometer
Making sigma bonds and holding lone pairs

4. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
Pipette (burette if need repetition)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Decant
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

5. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
|experimental - accepted|/accepted X 100
no - they're written undissociated (HAaq)
Soluble

6. What process do you use to obtain a solvent from a solution?
Distillation
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Add acid to water so that the acid doesn't boil and spit

7. What are the signs of ?G and E° for spontaneous reactions?
NH4?
Pale yellow
voltaic: + electrolytic: -
?G=negative - E° must be positive

8. If ?S is positive - are the products more or less chaotic than the reactants?
Silvery gray solid - brown - purple
More chaotic (ex: gases made)
Both electrons come from the same atom (just as good as a regular bond)
NO3?

9. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Transition element compounds (except if it has a full or empty d shell)
water and substances with (s) less dense than
Heat a test tube at an angle at the side of the tube (not bottom)
Acidified

10. What is the test for hydrogen?
Disulfur dichloride
lighted splint (positive result=pop)
same KE - but PEice<PEwater
All except for lithium

11. Why are i factors (Van't Hoff factors) often less than ideal?
Insoluble (except group 1 ammonium and Ba)
neutralization: high K - H2O product dissociation: low K - H2O reactant
ion pairing
NH4?

12. What measuring device would you use for very small volumes of liquids?
OH?
ClO3?
Selective absorption
Pipette (burette if need repetition)

13. What is the test for oxygen?
Glowing splint (positive result=relights)
allow for the vapor pressure of water and make sure to level levels
Transition element compounds (except if it has a full or empty d shell)
O2 needs 4F/mol H2 needs 2F/mol

14. Ca - Sr - Ba
hydroxides (ex: Ba(OH)2)
MnO4?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Ksp = 108s5

15. What process do you use to obtain the solute from a solution?
Evaporation
RCOR
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
ethers

16. Do you use J or kJ for ?H - ?S - and ?G?
Ksp = s²
?H-kJ - ?S-J - ?G-kJ
C4H10
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

17. Does Kw increase or decrease with T? Why?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Check for air bubbles in the buret and remove the buret funnel from the buret
fruit - fish - bases
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

18. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Synthetic condensation polymer (aka a polyamide)
They stay the same.
proton donor base
non-metal oxides and hydrides are covalently bonded and are acidic.

19. How are primary alcohols turned into acids?
O2 needs 4F/mol H2 needs 2F/mol
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

20. The definition of acidic basic and neutral aqueous solutions is:
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
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.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
zero-th: decreases - first: constant - second: increases

21. What is the difference between equivalence point and end point of a titration.
Mn²? - Cr³? - Cr³
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
H+
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

22. 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)
Increases.
Heat a test tube at an angle at the side of the tube (not bottom)
ClO4?

23. iodine - iodine solution - iodine vapor
allow for the vapor pressure of water and make sure to level levels
Silvery gray solid - brown - purple
strong acids/bases are written as H+ or OH- ions
CnH2n+1 often designated 'R' ex C3H7 is propyl

24. permanganate
Suniverse increases for spontaneous processes
bases
MnO4?
How close results are to the accepted value

25. carbonate
Insoluble
CO3²?
Unsaturated - addition (ex: decolorize bromine solution)
Separating funnel

26. What two compounds are great oxidizing agents?

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

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28. What steps do organic labs consist of?
ROH
allow for the vapor pressure of water and make sure to level levels
benzene has a delocalized pi ring structure
Synthesis - separation and purification of the product and its identification.

29. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
ROH
A salt solution.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

30. What are allotropes?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
different forms of the same element
Tetrahedral

31. Color (absorbance) is proportional to ________
Soluble
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
voltaic: + electrolytic: -
Concentration

32. phosphates
?G=negative - E° must be positive
ionic and form hydrogen and hydroxide
Group I metals (soft metals) are stored under oil
Most INsoluble except group 1 and ammonium

33. How does group 1 metals' density compare to water's?
C4H10
same KE - but PEice<PEwater
How grouped results are
are less dense than water

34. How do you dilute an acid?

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35. silver compounds
Cr2O7²?
ClO2?
Insoluble except for nitrate and acetate
zero

36. Can you collect soluble gases over water?
Insoluble except nitrate and acetate
Acid rain - dissolves marble buildings/statues and kills trees.
No - NH3 and HCl gases are extremely soluble
do not change

37. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Acidified
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.
K2

38. Which value of R do you use for all energy and kinetics calculations?
Ksp = 27s4
R=8.31 J/mol/K
allow for the vapor pressure of water and make sure to level levels
it's lower and occurs over less sharp a range

39. What do you use to look at burning magnesium? why?
boiling without losing volatile solvents/reactants
blue glass - it filters UV
atoms
Iodine and CO2 (dry ice)

40. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Soluble
ClO3?
Kc=Kp
Identity and purity (impure compounds usually have broad & low melting points)

41. How many ligands attach to a central ion in a complex ion?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Separating funnel
an oxidized and reduced substance
#ligands=charge x2

42. What shape is methane?
Tetrahedral
P2O5
All except for lithium
do not change

43. Buffer capacity must contain decent amounts of a ________ ________
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
diamond and graphite
Conjugate pair (one must be a weak base or acid)

44. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Acid rain - dissolves marble buildings/statues and kills trees.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
a-IMFs - b-molecular volume
by electrolysis

45. If Q < Ksp a ppt ______
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Ppt will NOT form (unsaturated)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

46. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Greenish-yellow gas
zero
[A?]/[HA] x 100 or [BH?]/[B] x 100

47. What are the common strong bases?
NH4?
CN?
Group 1 hydroxides (ex: NaOH)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

48. Generally - which oxy acid is strongest?
RX
S2O3²?
The one with most oxygen atoms (highest oxidation number)
Heat a test tube at an angle at the side of the tube (not bottom)

49. dichromate (soln + most solids)
[A?]/[HA] x 100 or [BH?]/[B] x 100
methyl formate
Orange
it is lower and occurs over less sharp a range

50. What is the word equation for addition polymerisation?
Making sigma bonds and holding lone pairs
RNH2
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Most INsoluble except group 1 and ammonium