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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 slope of the graph of lnk vs. 1/T?
do not change
Insoluble (except group 1 ammonium and Ba)
At half equivalence - pH=pKa
-Ea/R

2. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
allow for the vapor pressure of water and make sure to level levels
Hg2²?
#ligands=charge x2

3. What is H2CO3 (carbonate acid) usually written as?
neutralization: high K - H2O product dissociation: low K - H2O reactant
acid + alcohol
RCOOR
H2O + CO2 (it decomposes readily)

4. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
ns² electrons (first in-first out)
Anode - oxygen. Cathode - hydrogen
Eudiometer
ionic and form hydrogen and hydroxide

5. What process do you use to obtain the solute from a solution?
Cu3(PO4)2
Sulfur
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)
Evaporation

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

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7. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
RNH2
Increases.
Current - time and charge on ion (moles of e used in half cell reaction)

8. phosphates
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Most INsoluble except group 1 and ammonium
Increases.

9. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Ksp = 27s4
S2O3²?

10. Name 2 ways in which you can create a buffer?
CnH2n+2
E=q + w (negative is by system - positive is on system)
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)
different forms of the same element

11. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Making sigma bonds and holding lone pairs
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
No - it depends on the number of ions produced on dissolving.
by electrolysis

12. What kind of bonding structure does benzene have?
blue
benzene has a delocalized pi ring structure
Add acid to water so that the acid doesn't boil and spit
same KE - but PEice<PEwater

13. What is the general formula of an alkane?
Salt + water
catalyst=conc H2SO4
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CnH(2n+2)

14. What are the units of the first order rate constant?
R=8.31 J/mol/K
T increases exponentially the proportion of molecules with E > Ea
Time?¹ - (ex. s?¹ - hr?¹ - etc)
zero-th: decreases - first: constant - second: increases

15. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
RX
brown volatile liquid
They decrease (or could be the same if the solid has ONLY JUST disappeared)
zero

16. What is reflux?
boiling without losing volatile solvents/reactants
ROH
Suniverse increases for spontaneous processes
An active metal.

17. What is Big K in terms of kf and kr?
Big K=kf/kr
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
water and substances with (s) less dense than

18. Do anions flow to the cathode or anode?
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)
different forms of the same element
?G=negative - E° must be positive
Anode

19. What word is a clue for a redox reaction?
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)
Acidified
Experimental mass/theoretical mass X 100
boiling without losing volatile solvents/reactants

20. Name C7H16
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
K2
Heptane
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

21. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
it's lower and occurs over less sharp a range
NO3?
OH- and NH3

22. chlorite
ClO2?
boiling without losing volatile solvents/reactants
Suniverse increases for spontaneous processes
Pale purple - (orange)-yellow - red - blue - green.

23. What is the formula for alkynes?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
CnH2n-2
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

24. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
?G= -ve - E°= +ve
redox reaction
A salt solution.

25. What is the formula of butane?
K2
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
C4H10
Mn²? - Cr³? - Cr³

26. What shape is carbon dioxide?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
linear
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

27. What are allotropes?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
different forms of the same element
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Perform ICE BOX calculation based on K1

28. silver iodide
?G= -ve - E°= +ve
RCOR
CO2 and H2O
Pale yellow

29. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
A) any range. b) 8-10 c) 4-6
|experimental - accepted|/accepted X 100
Making sigma bonds and holding lone pairs
10?8

30. Generally - which oxy acid is strongest?
CnH2n+1 often designated 'R' ex C3H7 is propyl
RNH2
The one with most oxygen atoms (highest oxidation number)
Concentration

31. Ions are not ______.
Unsaturated - addition (ex: decolorize bromine solution)
atoms
left - ppt will form
methyl formate

32. Aromatic compounds contain what?
The benzene ring (or more correctly the phenyl group - C6H5)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
yellow
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

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

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34. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
benzene has a delocalized pi ring structure
blue
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

35. bromothymol
Acidified
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
basic
blue (BTB)

36. Alcohols and _______ are FG isomers
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Combine the equations for the half reactions in the non-spontaneous direction
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)
ethers

37. What is accuracy?
Iodine and CO2 (dry ice)
strong acids/bases are written as H+ or OH- ions
How close results are to the accepted value
Soluble

38. If a free element is involved - what type of reaction must be involved?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
The Faraday or Faraday's constant.
How close results are to the accepted value
redox reaction

39. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Combine the equations for the half reactions in the non-spontaneous direction
by electrolysis
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

40. Ca - Sr - Ba
diamond and graphite
brown volatile liquid
CO2 and H2O
hydroxides (ex: Ba(OH)2)

41. If ?S is positive - are the products more or less chaotic than the reactants?
Experimental mass/theoretical mass X 100
More chaotic (ex: gases made)
T increases exponentially the proportion of molecules with E > Ea
blue

42. What is the general formula for an ester?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
RCOOR
[A?]/[HA] x 100 or [BH?]/[B] x 100
R=8.31 J/mol/K

43. How does half life change for zero-th order - first order - and second order processes?
Mn²? - Cr³? - Cr³
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
by electrolysis
zero-th: decreases - first: constant - second: increases

44. What reacts with an acid to create hydrogen gas?
ROH
An active metal.
Experimental mass/theoretical mass X 100
No - it depends on the number of ions produced on dissolving.

45. When combining half equations - what do you do to E° values when multiplying coefficients?
allow for the vapor pressure of water and make sure to level levels
Nothing
Soluble
Acidified

46. What do nonmetal oxides plus water form?
The benzene ring (or more correctly the phenyl group - C6H5)
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
acids
Only temperature

47. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Eudiometer
Hg²?
water and substances with (s) less dense than
Combine the equations for the half reactions in the non-spontaneous direction

48. Give an example of a dilute strong acid.
proton donor base
an oxidized and reduced substance
Glowing splint (positive result=relights)
HClO4

49. How do you get the equation for a net electrolysis reaction?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Cr2O7²?
brown volatile liquid
Combine the equations for the half reactions in the non-spontaneous direction

50. How do you find the pH for a dibasic acid? (H2A)?
RX
Perform ICE BOX calculation based on K1
Ksp = 4s³
Read the bottom of the meniscus