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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. If Q < Ksp a ppt ______
K1 x K2
voltaic: + electrolytic: -
CnH2n
Ppt will NOT form (unsaturated)

2. oxalate
Combine the equations for the half reactions in the non-spontaneous direction
C2O4²?
Soluble
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?)

3. Name C7H16
Add acid to water so that the acid doesn't boil and spit
Heptane
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
diamond and graphite

4. nitrate
NO3?
More chaotic (ex: gases made)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
CH3COO?

5. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
CH3COO?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
H+

6. Buffer capacity must contain decent amounts of a ________ ________
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
They stay the same.
Conjugate pair (one must be a weak base or acid)
voltaic: - electrolytic: +

7. What does saturated mean? Unsaturated?
lighted splint (positive result=pop)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

8. What is the conjugate acid of H2PO4?
H3PO4
Acid rain - dissolves marble buildings/statues and kills trees.
Ionic compounds
linear

9. What is the word equation for addition polymerisation?
CN?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Iodine and CO2 (dry ice)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

10. Do anions flow to the cathode or anode?
brown volatile liquid
diamond and graphite
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Anode

11. What do acids plus active metals form?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
|experimental - accepted|/accepted X 100

12. What do you use to look at burning magnesium? why?
White precipitate
blue glass - it filters UV
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

13. What is the general formula for an acid?
benzene has a delocalized pi ring structure
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
RCOOH
|experimental - accepted|/accepted X 100

14. Name six characteristics of transition elements (or their compounds)
Transition element compounds (except if it has a full or empty d shell)
Most INsoluble except group 1 and ammonium
Iodine and CO2 (dry ice)
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)

15. Which of the rates changes more when temperature is increased?
Soluble
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
No - NH3 and HCl gases are extremely soluble
Insoluble

16. What is the general formula for a ketone?
RCOR
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
small size and high charge
But S° of element is not zero (except at 0K)

17. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
Sulfur
voltaic: - electrolytic: +
H2O + CO2 (it decomposes readily)

18. primary colors
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Iodine and CO2 (dry ice)
Iodine and CO2 (dry ice)
red - green - blue

19. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
Hg2²?
bent
NO3?

20. How does the melting point of a mixture compare to the MP of a pure substance?

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21. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
zero
Purple
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

22. hypochlorite
ethers
hydroxides (ex: Ba(OH)2)
ClO?
Purple

23. What device would you use to measure a volume of gas?
yellow
ROR
proton donor base
Eudiometer

24. What is the formula for summation?

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25. What is precision?
PO4³?
How grouped results are
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
HClO4

26. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
ns² electrons (first in-first out)
Acid rain - dissolves marble buildings/statues and kills trees.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
CrO4²?

27. What is an Alkyl group?

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28. hydroxides
Mono; di; tri; tetra; penta; hexa.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Insoluble (except group 1 ammonium and Ba)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

29. What changes Keq?
Tetrahedral
Cr2O7²?
Conjugate pair (one must be a weak base or acid)
Only temperature

30. How do you get Ecell for spontaneous reactions?
RCOR
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
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)
Big K=kf/kr

31. What is the formula for alkenes?
CnH2n
zero
bases
Hg²?

32. What is reflux?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
boiling without losing volatile solvents/reactants
do not change
diamond and graphite

33. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
CO2 and H2O
ns² electrons (first in-first out)
Ksp = 4s³
ROR

34. What do you use for an acid spill? base spill?
The dilution effect when the solutions mix. M1V1 = M2V2
CH3COO?
CnH2n+2
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

35. What process do you use to obtain the solute from a solution?
catalyst=conc H2SO4
0.10M HCl (more ions)
Evaporation
zero

36. If a free element is involved - what type of reaction must be involved?
MnO4?
redox reaction
atoms
How grouped results are

37. What is the pH of 1.0M HCl? 1M NaOH?
RX
0 and 14
-Ea/R
But S° of element is not zero (except at 0K)

38. Is the standard entropy (S°) of an element zero?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
CO2 and H2O
bases
But S° of element is not zero (except at 0K)

39. What is the general formula of an alkane?
Insoluble except nitrate and acetate
Anode
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
CnH(2n+2)

40. What do you need to make a polymer?
Filtration
neutralization: high K - H2O product dissociation: low K - H2O reactant
10?8
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)

41. When the salt bridge is removed what happens to the cell reaction?
a-IMFs - b-molecular volume
redox reaction
It ceases - the circuit is broken.
atoms

42. Name some properties of Group 17
Trigonal pyramidal
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Hg²?
PO4³?

43. Alkenes are ________ and react by __________
a-IMFs - b-molecular volume
Glowing splint (positive result=relights)
Acid rain - dissolves marble buildings/statues and kills trees.
Unsaturated - addition (ex: decolorize bromine solution)

44. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
it reacts by substitution NOT addition
Reduction always takes place at the cathode (RED CAT) In both types of cell!
The compound with the lowest Ksp value.
basic

45. silver iodide
Pale yellow
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

46. halides
Ksp = s²
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
Most are soluble except Ag - Pb
CnH2n

47. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
C2O4²?
H2PO4?
methyl formate

48. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
0.10M HCl (more ions)
basic
Salt + water

49. What is accuracy?
OH- and NH3
blue (BTB)
How close results are to the accepted value
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.

50. Give an example of a dilute strong acid.
Eudiometer
bright yellow
R=8.31 J/mol/K
HClO4