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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. The oxidation # for acid base reactions...
do not change
Glacial acetic acid
PO4³?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

2. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
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)
water and substances with (s) less dense than
Exothermic
RCHO (carbonyl at end)

3. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
CrO4²?
The benzene ring (or more correctly the phenyl group - C6H5)
Current - time and charge on ion (moles of e used in half cell reaction)
Orange

4. What are the units of the first order rate constant?
NH2?
Glowing splint (positive result=relights)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
voltaic: + electrolytic: -

5. acetate
OH?
CO3²?
Q=It (time in seconds)
CH3COO?

6. 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?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
CnH2n-2
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
bright yellow

7. chromate
Concentration
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
CrO4²?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

8. BaSO4
methyl formate
H3PO4
Insoluble
blue

9. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
ClO?
Check for air bubbles in the buret and remove the buret funnel from the buret
neutralization: high K - H2O product dissociation: low K - H2O reactant

10. What is the slope of the graph of lnk vs. 1/T?
same KE - but PEice<PEwater
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
-Ea/R
[A?]/[HA] x 100 or [BH?]/[B] x 100

11. Does reactivity increase/decrease going down group 1 and group 17?
ClO?
Increases down group 1 decreases down group 17
|experimental - accepted|/accepted X 100
Kc=Kp

12. What causes the dramatic effect of T on rate?
ClO4?
atoms
T increases exponentially the proportion of molecules with E > Ea
ethers

13. What element is used to vulcanize rubber?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Making sigma bonds and holding lone pairs
Sulfur
Selective absorption

14. oxalate
An active metal.
C2O4²?
Concentration
brown volatile liquid

15. What are the signs of ?G and E° for spontaneous reactions?
CnH2n+2
+4-covalent - +2-ionic
Soluble
?G=negative - E° must be positive

16. What is the relationship in strength between sigma and pi bonds?
A salt solution.
?H-kJ - ?S-J - ?G-kJ
Ppt will NOT form (unsaturated)
Sigma bonds are stronger than pi bonds

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

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18. Which of the rates changes more when temperature is increased?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
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
Conjugate pair (one must be a weak base or acid)

19. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
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.
CO (poisonous)
[A?]/[HA] x 100 or [BH?]/[B] x 100
fruit - fish - bases

20. What is a dipeptide? polypeptide? protein?
RCOOH
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
linear
Synthetic condensation polymer (aka a polyamide)

21. Alkanes are _________ and react by _________
SO4²?
Saturated - Substitution (which requires more radical conditions)
Selective absorption
Initiation energy (NOT Ea)

22. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Iodine and CO2 (dry ice)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
At half equivalence - pH=pKa
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

23. Neutralization is an ________ reaction.
different forms of the same element
[A?]/[HA] x 100 or [BH?]/[B] x 100
Exothermic (?H for ANY sa/sb = -57kJ/mol)
bases

24. The definition of acidic basic and neutral aqueous solutions is:
Increases down group 1 decreases down group 17
ion pairing
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
RNH2

25. chlorite
allow for the vapor pressure of water and make sure to level levels
The benzene ring (or more correctly the phenyl group - C6H5)
ClO2?
H2O + CO2 (it decomposes readily)

26. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
A) any range. b) 8-10 c) 4-6
C4H10
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

27. What apparatus do you use to separate 2 immiscible liquids?
ion pairing
CnH2n-2
Separating funnel
Group 1 hydroxides (ex: NaOH)

28. A Bronsted-Lowry base is...
proton acceptor.
H3PO4
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
non-metal oxides and hydrides are covalently bonded and are acidic.

29. perchlorate
ClO4?
Soluble
Salt and water
Orange

30. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
|experimental - accepted|/accepted X 100
They stay the same.

31. How does group 1 metals' density compare to water's?
How close results are to the accepted value
are less dense than water
Most are soluble except Ag - Pb
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

32. How are strong ones written?
ROH
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
strong acids/bases are written as H+ or OH- ions

33. When a cell is 'flat' What is its voltage?
Synthetic condensation polymer (aka a polyamide)
-Ea/R
RCOOR
zero

34. lead iodide
NH2?
linear
Sulfur
bright yellow

35. mercury (II) ion
CrO4²?
CH3COO?
Making sigma bonds and holding lone pairs
Hg²?

36. Does Benzene react by addition or substitution?
Iodine and CO2 (dry ice)
ClO2?
it reacts by substitution NOT addition
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

37. What are hybrid orbitals used for?
Tetrahedral
Ksp = 4s³
Making sigma bonds and holding lone pairs
Saturated - Substitution (which requires more radical conditions)

38. Is a graduated cylinder or beaker more accurate?
Hg2²?
?G= -ve - E°= +ve
Graduated cylinder
it reacts by substitution NOT addition

39. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
hydroxides (ex: Ba(OH)2)
The dilution effect when the solutions mix. M1V1 = M2V2
neutralization: high K - H2O product dissociation: low K - H2O reactant
|experimental - accepted|/accepted X 100

40. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Ionic compounds
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
catalyst=conc H2SO4
The compound with the lowest Ksp value.

41. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
Sulfur
Salts (ex: CaO + SO2 ? CaSO3)
RNH2

42. acetates
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Ksp = s²
Soluble
Read the bottom of the meniscus

43. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Most INsoluble except group 1 and ammonium
Exothermic (?H for ANY sa/sb = -57kJ/mol)
K2

44. What is the conjugate base of NH3?
NH2?
bright yellow
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Check for air bubbles in the buret and remove the buret funnel from the buret

45. When combining half equations - what do you do to E° values when multiplying coefficients?
ROH
small size and high charge
|experimental - accepted|/accepted X 100
Nothing

46. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Identity and purity (impure compounds usually have broad & low melting points)
metal oxides and hydrides are ionically bonded and basic
H3PO4

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

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48. silver compounds
ethers
benzene has a delocalized pi ring structure
Insoluble except for nitrate and acetate
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

49. permanganate
a-IMFs - b-molecular volume
CH3COO?
MnO4?
S crystal at 0K=0

50. sulfates
bent
Soluble except Ag - Pb - Ca - Sr Ba)
ion pairing
[A?]/[HA] x 100 or [BH?]/[B] x 100