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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 is the slope of the graph of lnk vs. 1/T?
-Ea/R
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Identity and purity (impure compounds usually have broad & low melting points)
Anode

2. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
PO4³?
H2PO4?
a-IMFs - b-molecular volume

3. What are two allotropes of carbon?
Only temperature
catalyst=conc H2SO4
bright yellow
diamond and graphite

4. sulfate
How grouped results are
SO4²?
zero
At half equivalence - pH=pKa

5. What steps do organic labs consist of?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
fruit - fish - bases
CnH2n
Synthesis - separation and purification of the product and its identification.

6. copper sulfate
Hg2²?
[A?]/[HA] x 100 or [BH?]/[B] x 100
brown volatile liquid
blue

7. What things should you remember to do when collecting gas over water?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
[A?]/[HA] x 100 or [BH?]/[B] x 100
allow for the vapor pressure of water and make sure to level levels
Pale purple - (orange)-yellow - red - blue - green.

8. ammonium
NH4?
CO (poisonous)
zero
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

9. If a weak acid is diluted more - what happens to its % dissociation value?
Add acid to water so that the acid doesn't boil and spit
HClO4
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)
Increases.

10. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Tetrahedral
Ksp = 27s4
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
allow for the vapor pressure of water and make sure to level levels

11. What is precision?
Exothermic
An active metal.
How grouped results are
Pale yellow

12. Lattice energy is high for ions with _____ size and _____ charge
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Sulfur
Identity and purity (impure compounds usually have broad & low melting points)
small size and high charge

13. How many ligands attach to a central ion in a complex ion?
Insoluble except for nitrate and acetate
bases
All except for lithium
#ligands=charge x2

14. What is the general formula for an acid?
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?)
Ksp = s²
Separating funnel
RCOOH

15. What do you use to look at burning magnesium? why?
Transition element compounds (except if it has a full or empty d shell)
Identity and purity (impure compounds usually have broad & low melting points)
blue glass - it filters UV
it reacts by substitution NOT addition

16. What do group I/II metal oxides plus water form?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Synthetic condensation polymer (aka a polyamide)
bases

17. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
'non-active' metals such as Cu - Ag - Au - Pt - etc.
S crystal at 0K=0
CO2 and H2O

18. What is the formula of copper (II) phosphate?
Cu3(PO4)2
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Acidified
RCOOH

19. Color (absorbance) is proportional to ________
The compound with the lowest Ksp value.
Concentration
Insoluble
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

20. What is the catalyst for this reaction Ester + ?
?G=negative - E° must be positive
Ksp = 4s³
catalyst=conc H2SO4
Hg²?

21. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
H3PO4
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
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

22. What is the conjugate acid of H2PO4?
The Faraday or Faraday's constant.
H3PO4
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.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

23. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Soluble
10?8
Ions go through the salt bridge - electrons go through metal wires in the external circuit
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

24. What is HCOOCH3?
Trigonal pyramidal
Unsaturated - addition (ex: decolorize bromine solution)
Acids; HCOOCH3 is an ester
C4H10

25. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Current - time and charge on ion (moles of e used in half cell reaction)
water and substances with (s) less dense than
Salt and water
RNH2

26. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
ClO4?
Kc=Kp
Initiation energy (NOT Ea)

27. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
hydroxides (ex: Ba(OH)2)
Purple
CO (poisonous)
q=mc?T q=mL (or n x ?h)

28. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Acid rain - dissolves marble buildings/statues and kills trees.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
bent
Anode

29. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Initiation energy (NOT Ea)
Soluble
Filtration

30. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
CnH2n+1 often designated 'R' ex C3H7 is propyl
look for changes in oxidation # - the one that goes up is oxidized and is the RA
voltaic: - electrolytic: +

31. How do you get the equation for a net electrolysis reaction?
But S° of element is not zero (except at 0K)
Combine the equations for the half reactions in the non-spontaneous direction
proton acceptor.
water and substances with (s) less dense than

32. iodine - iodine solution - iodine vapor
Ksp = 108s5
Hg2²?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Silvery gray solid - brown - purple

33. What is the general formula for a ketone?
a-IMFs - b-molecular volume
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
RCOR
ROR

34. sulfates
T increases exponentially the proportion of molecules with E > Ea
ion pairing
Soluble except Ag - Pb - Ca - Sr Ba)
zero-th: decreases - first: constant - second: increases

35. Give an example of a dilute strong acid.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
P2O5
The benzene ring (or more correctly the phenyl group - C6H5)
HClO4

36. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
boiling without losing volatile solvents/reactants
CrO4²?
The one with most oxygen atoms (highest oxidation number)

37. What is the test for oxygen?
Glowing splint (positive result=relights)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
water and substances with (s) less dense than
Group I metals (soft metals) are stored under oil

38. What is the general formula for an aldehyde?
Purple
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
RCHO (carbonyl at end)
Initiation energy (NOT Ea)

39. What things should you remember to do when collecting gas over water?
catalyst=conc H2SO4
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Hg2²?
allow for the vapor pressure of water and make sure to level levels

40. cyanide
R=8.31 J/mol/K
CN?
Ionic compounds
K1 x K2

41. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Distillation
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
The benzene ring (or more correctly the phenyl group - C6H5)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

42. A geometric (or cis-trans) isomer exists due to.....
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
But S° of element is not zero (except at 0K)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Acidified

43. A Bronsted-Lowry base is...
Only temperature
Acid rain - dissolves marble buildings/statues and kills trees.
proton acceptor.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

44. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Group I metals (soft metals) are stored under oil

45. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Mn²? - Cr³? - Cr³
ClO?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
At half equivalence - pH=pKa

46. What is the general formula for an alcohol?
bases
Concentration
Molecules with the same molecular formulas - but different structural formulas
ROH

47. What are the prefixes for the naming of binary molecular compound formulas (up to six)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
S2O3²?
H2O + CO2 (it decomposes readily)
Mono; di; tri; tetra; penta; hexa.

48. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Graduated cylinder
Filtration
NO3?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

49. How many normal boiling points and boiling points are there?

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50. How can metals like iron and zinc be reduced?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Salt + water
H2PO4?
chemically (ex: with carbon)