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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.
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 two compounds are great oxidizing agents?

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2. What complex ion does ammonia form with silver? copper? cadmium? zinc?
?G=negative - E° must be positive
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Disulfur dichloride
No - NH3 and HCl gases are extremely soluble

3. What type of compounds do Group 14 form?
+4-covalent - +2-ionic
do not change
Sulfur
q=mc?T q=mL (or n x ?h)

4. primary colors
Pour liquids using a funnel or down a glass rod
No - NH3 and HCl gases are extremely soluble
red - green - blue
Silvery gray solid - brown - purple

5. BaSO4
Iodine and CO2 (dry ice)
Insoluble
redox reaction
The benzene ring (or more correctly the phenyl group - C6H5)

6. How are metal oxides and hydrides bonded? are they acidic or basic?
No - it depends on the number of ions produced on dissolving.
Insoluble
metal oxides and hydrides are ionically bonded and basic
Most INsoluble except group 1 and ammonium

7. Aromatic compounds contain what?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
How close results are to the accepted value
Salts (ex: CaO + SO2 ? CaSO3)
The benzene ring (or more correctly the phenyl group - C6H5)

8. What are the signs for ?G and E° for spontaneous reactions?
Pipette (burette if need repetition)
voltaic: + electrolytic: -
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= -ve - E°= +ve

9. What does saturated mean? Unsaturated?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Synthesis - separation and purification of the product and its identification.
NH2?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

10. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
No - it depends on the number of ions produced on dissolving.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
it reacts by substitution NOT addition
?G= -ve - E°= +ve

11. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Add acid to water so that the acid doesn't boil and spit
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Suniverse increases for spontaneous processes

12. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
zero
Pale purple - (orange)-yellow - red - blue - green.
Check for air bubbles in the buret and remove the buret funnel from the buret
Graduated cylinder

13. What is HCOOCH3?
ion pairing
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
benzene has a delocalized pi ring structure
Acids; HCOOCH3 is an ester

14. Nonmetals are good _____ agents. Metals are good _______ agents.
Exothermic
But S° of element is not zero (except at 0K)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Identity and purity (impure compounds usually have broad & low melting points)

15. Are weak acids (and bases) written dissociated?

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16. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
No - it depends on the number of ions produced on dissolving.
PO4³?
same KE - but PEice<PEwater
Reduction always takes place at the cathode (RED CAT) In both types of cell!

17. Name C7H16
The one with most oxygen atoms (highest oxidation number)
Heptane
|experimental - accepted|/accepted X 100
Group I metals (soft metals) are stored under oil

18. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
Combine the equations for the half reactions in the non-spontaneous direction
R=8.31 J/mol/K
RCHO (carbonyl at end)

19. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
allow for the vapor pressure of water and make sure to level levels
Soluble
A) any range. b) 8-10 c) 4-6
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

20. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
ClO?
Iodine and CO2 (dry ice)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

21. What is the first law of thermodynamics?
blue (BTB)
E=q + w (negative is by system - positive is on system)
OH?
diamond and graphite

22. Esters smell like _______ and amines smell like _______ and are ______.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
fruit - fish - bases
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

23. mercury (I) ion
Unsaturated - addition (ex: decolorize bromine solution)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Hg2²?
Only temperature

24. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
ion pairing
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Trigonal pyramidal

25. bromothymol
Salts (ex: CaO + SO2 ? CaSO3)
Current - time and charge on ion (moles of e used in half cell reaction)
MnO4?
blue (BTB)

26. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
Unsaturated - addition (ex: decolorize bromine solution)
R=8.31 J/mol/K
CO3²?

27. How can metals like iron and zinc be reduced?
Cr2O7²?
The benzene ring (or more correctly the phenyl group - C6H5)
chemically (ex: with carbon)
Increases down group 1 decreases down group 17

28. Which of the rates changes more when temperature is increased?
O2 needs 4F/mol H2 needs 2F/mol
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
More chaotic (ex: gases made)
Add acid to water so that the acid doesn't boil and spit

29. Why are i factors (Van't Hoff factors) often less than ideal?
blue glass - it filters UV
ion pairing
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
ethers

30. phosphate
proton donor base
PO4³?
diamond and graphite
Pipette (burette if need repetition)

31. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
benzene is less reactive than alkenes

32. Is the ?H formation of an element in standard state zero?
zero-th: decreases - first: constant - second: increases
?H formation of an element in standard state=0
Cu3(PO4)2
HClO4

33. perchlorate
-Ea/R
Ksp = 108s5
ClO4?
Combine the equations for the half reactions in the non-spontaneous direction

34. What is the general formula for an acid?
RCOOH
fractional distillation
look for changes in oxidation # - the one that goes up is oxidized and is the RA
'non-active' metals such as Cu - Ag - Au - Pt - etc.

35. What is precision?
Insoluble (except group 1 ammonium and Ba)
allow for the vapor pressure of water and make sure to level levels
How grouped results are
CN?

36. What device would you use to measure a volume of gas?
CN?
water and substances with (s) less dense than
Q=It (time in seconds)
Eudiometer

37. bromine
But S° of element is not zero (except at 0K)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
ClO3?
brown volatile liquid

38. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
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
bright yellow
HClO4

39. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Filtration
ns² electrons (first in-first out)
?G=negative - E° must be positive
K1 x K2

40. What is the formula for percent error?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
|experimental - accepted|/accepted X 100
Ions go through the salt bridge - electrons go through metal wires in the external circuit
ClO?

41. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
The compound with the lowest Ksp value.
non-metal oxides and hydrides are covalently bonded and are acidic.
Saturated - Substitution (which requires more radical conditions)
brown volatile liquid

42. How do you heat a test tube?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Separating funnel
Heat a test tube at an angle at the side of the tube (not bottom)
same KE - but PEice<PEwater

43. What two types of substances are present in all redox reactions?
Anode - oxygen. Cathode - hydrogen
CH3COO?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
an oxidized and reduced substance

44. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
#ligands=charge x2
H+
The dilution effect when the solutions mix. M1V1 = M2V2
water and substances with (s) less dense than

45. lead iodide
bright yellow
Soluble
Most are soluble except Ag - Pb
do not change

46. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
voltaic: - electrolytic: +
H+
water and substances with (s) less dense than
Synthesis - separation and purification of the product and its identification.

47. What are the products of the reaction between group 1 metals and water?

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48. What does a short - sharp melting point indicate?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Identity and purity (impure compounds usually have broad & low melting points)
Cr2O7²?
Increases down group 1 decreases down group 17

49. A Bronsted-Lowry base is...
do not change
proton acceptor.
SO4²?
Read the bottom of the meniscus

50. What is reflux?
boiling without losing volatile solvents/reactants
Pipette (burette if need repetition)
CO2 and H2O
CrO4²?