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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. How do you heat a test tube?
Perform ICE BOX calculation based on K1
Heat a test tube at an angle at the side of the tube (not bottom)
Salt + water.
ethers

2. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
Big K=kf/kr
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Increases.
P2O5

3. If Q > Ksp - then system shifts _______ and ppt ______
Exothermic (?H for ANY sa/sb = -57kJ/mol)
left - ppt will form
allow for the vapor pressure of water and make sure to level levels
The Faraday or Faraday's constant.

4. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
CrO4²?
Kc=Kp
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
At half equivalence - pH=pKa

5. If ?S is positive - are the products more or less chaotic than the reactants?
S crystal at 0K=0
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)
More chaotic (ex: gases made)
water and substances with (s) less dense than

6. What kind of bonding structure does benzene have?
Combine the equations for the half reactions in the non-spontaneous direction
benzene has a delocalized pi ring structure
Molecules with the same molecular formulas - but different structural formulas
fractional distillation

7. What is the formula for percent error?
left - ppt will form
a-IMFs - b-molecular volume
Trigonal pyramidal
|experimental - accepted|/accepted X 100

8. What are isomers?
Ppt will NOT form (unsaturated)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Molecules with the same molecular formulas - but different structural formulas
[A?]/[HA] x 100 or [BH?]/[B] x 100

9. What is the general formula for an ether?
ROR
C4H10
#ligands=charge x2
T increases exponentially the proportion of molecules with E > Ea

10. What is the word equation for condensation polymerisation ?
Filtration
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Only temperature

11. What part of a liquid do you look at to measure its volume?
PO4³?
Salt and water
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Read the bottom of the meniscus

12. Name six characteristics of transition elements (or their compounds)
Soluble
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)
Both electrons come from the same atom (just as good as a regular bond)
zero

13. During a titration what is present in the beaker at the equivalence point?
A salt solution.
ionic and form hydrogen and hydroxide
Pale purple - (orange)-yellow - red - blue - green.
RCOR

14. Is the ?H formation of an element in standard state zero?
linear
CO (poisonous)
?H formation of an element in standard state=0
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

15. Colorless doesn't mean ______
Clear
different forms of the same element
Soluble
The one with most oxygen atoms (highest oxidation number)

16. What is accuracy?
Nothing
How close results are to the accepted value
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
Anode

17. What is the charge on a chlorine atom?
Insoluble
different forms of the same element
White precipitate
zero

18. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
CnH(2n+2)
Mn²? - Cr³? - Cr³
Cr2O7²?
zero

19. What are the common strong bases?
Group 1 hydroxides (ex: NaOH)
Exothermic
Increases.
Add acid to water so that the acid doesn't boil and spit

20. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Anode - oxygen. Cathode - hydrogen
same KE - but PEice<PEwater
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

21. hypochlorite
Acids; HCOOCH3 is an ester
ClO?
it is lower and occurs over less sharp a range
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)

22. What do hydrocarbons form when they burn in air (oxygen)?
Conjugate pair (one must be a weak base or acid)
CO2 and H2O
Both electrons come from the same atom (just as good as a regular bond)
Initiation energy (NOT Ea)

23. What is Big K in terms of kf and kr?
RX
Big K=kf/kr
CnH2n-2
ns² electrons (first in-first out)

24. Generally - which oxy acid is strongest?
H2PO4?
RX
The one with most oxygen atoms (highest oxidation number)
?H-kJ - ?S-J - ?G-kJ

25. Do anions flow to the cathode or anode?
Concentration
Anode
Iodine and CO2 (dry ice)
Q=It (time in seconds)

26. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
NH4?
ionic and form hydrogen and hydroxide
zero
neutralization: high K - H2O product dissociation: low K - H2O reactant

27. Is the freezing of ice endothermic or exothermic?
OH?
Exothermic
Soluble
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

28. What is the slope of the graph of lnk vs. 1/T?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
How close results are to the accepted value
The benzene ring (or more correctly the phenyl group - C6H5)
-Ea/R

29. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
yellow
CO (poisonous)
Ksp = 108s5
A) any range. b) 8-10 c) 4-6

30. halides
Add acid to water so that the acid doesn't boil and spit
Most are soluble except Ag - Pb
ROH
Mn²? - Cr³? - Cr³

31. dichromate (soln + most solids)
Iodine and CO2 (dry ice)
Orange
an oxidized and reduced substance
H3PO4

32. What is HCOOCH3?
proton acceptor.
ethers
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Acids; HCOOCH3 is an ester

33. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Decant
Distillation
it's lower and occurs over less sharp a range
Acid rain - dissolves marble buildings/statues and kills trees.

34. What is the test for oxygen?
How close results are to the accepted value
More chaotic (ex: gases made)
Group I metals (soft metals) are stored under oil
Glowing splint (positive result=relights)

35. How are strong ones written?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
ClO?
acids
strong acids/bases are written as H+ or OH- ions

36. What is the pH of 1.0M HCl? 1M NaOH?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Mono; di; tri; tetra; penta; hexa.
0 and 14

37. What are allotropes?
Orange
different forms of the same element
An active metal.
fruit - fish - bases

38. Color is due to ______ _______ of light.
benzene has a delocalized pi ring structure
look for changes in oxidation # - the one that goes up is oxidized and is the RA
It ceases - the circuit is broken.
Selective absorption

39. What word is a clue for a redox reaction?
Acidified
small size and high charge
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
Read the bottom of the meniscus

40. iodine - iodine solution - iodine vapor
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Silvery gray solid - brown - purple
Most INsoluble except group 1 and ammonium
?G=negative - E° must be positive

41. 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?
Acid rain - dissolves marble buildings/statues and kills trees.
Unsaturated - addition (ex: decolorize bromine solution)
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
?G=negative - E° must be positive

42. hydroxides
Decant
bent
Group I metals (soft metals) are stored under oil
Insoluble (except group 1 ammonium and Ba)

43. What is the third law of thermodynamics?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
an oxidized and reduced substance
Identity and purity (impure compounds usually have broad & low melting points)
S crystal at 0K=0

44. What do nonmetal oxides plus water form?
C2O4²?
Identity and purity (impure compounds usually have broad & low melting points)
H3PO4
acids

45. What do group I/II metal oxides and acids form?
Salt and water
different forms of the same element
blue (BTB)
same KE - but PEice<PEwater

46. permanganate
MnO4?
RCOR
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Making sigma bonds and holding lone pairs

47. nitrates
Soluble
10?8
CnH(2n+2)
metal oxides and hydrides are ionically bonded and basic

48. How do you identify which is oxidized or otherwise?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
non-metal oxides and hydrides are covalently bonded and are acidic.
Trigonal pyramidal
Ppt will NOT form (unsaturated)

49. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Insoluble except for nitrate and acetate
a-IMFs - b-molecular volume
Pour liquids using a funnel or down a glass rod
Group 1 hydroxides (ex: NaOH)

50. Why are noble gases stable?
CN?
E=q + w (negative is by system - positive is on system)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
CH3COO?