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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. nitrate
Q=It (time in seconds)
NO3?
The dilution effect when the solutions mix. M1V1 = M2V2
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

2. What is the first law of thermodynamics?
#ligands=charge x2
E=q + w (negative is by system - positive is on system)
H2O + CO2 (it decomposes readily)
Soluble except Ag - Pb - Ca - Sr Ba)

3. What value of R do you use for thermo calculations? gas calculations?
by electrolysis
RCHO (carbonyl at end)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
benzene is less reactive than alkenes

4. 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.
A) any range. b) 8-10 c) 4-6
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
a-IMFs - b-molecular volume
'non-active' metals such as Cu - Ag - Au - Pt - etc.

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

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6. permanganate
MnO4?
Synthesis - separation and purification of the product and its identification.
do not change
catalyst=conc H2SO4

7. Why are noble gases stable?
CN?
benzene has a delocalized pi ring structure
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
But S° of element is not zero (except at 0K)

8. The oxidation # for acid base reactions...
chemically (ex: with carbon)
do not change
Read the bottom of the meniscus
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

9. What is the general formula for an acid?
Soluble
RCOOH
do not change
[A?]/[HA] x 100 or [BH?]/[B] x 100

10. What is the formula for alkynes?
acid + alcohol
CnH2n-2
Disulfur dichloride
K2

11. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
voltaic: - electrolytic: +
Salt + water.
Saturated - Substitution (which requires more radical conditions)

12. Do anions flow to the cathode or anode?
proton acceptor.
ROR
Anode
C2O4²?

13. If ?S is positive - are the products more or less chaotic than the reactants?
Synthesis - separation and purification of the product and its identification.
bright yellow
More chaotic (ex: gases made)
0 and 14

14. How do you find the pH for a dibasic acid? (H2A)?
red - green - blue
Pipette (burette if need repetition)
Perform ICE BOX calculation based on K1
S2O3²?

15. What is the catalyst for this reaction Ester + ?
catalyst=conc H2SO4
Transition element compounds (except if it has a full or empty d shell)
H2PO4?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

16. What is the formula of copper (II) phosphate?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Trigonal pyramidal
Cu3(PO4)2
Acids; HCOOCH3 is an ester

17. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
They stay the same.
linear
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

18. What is precision?
linear
How grouped results are
metal oxides and hydrides are ionically bonded and basic
blue glass - it filters UV

19. silver compounds
Salt + water.
Insoluble except for nitrate and acetate
Ionic compounds
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

20. Which value of R do you use for all energy and kinetics calculations?
?G= -ve - E°= +ve
R=8.31 J/mol/K
water and substances with (s) less dense than
CO (poisonous)

21. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
ClO3?
They stay the same.
How close results are to the accepted value
All except for lithium

22. What are the signs for ?G and E° for spontaneous reactions?
Making sigma bonds and holding lone pairs
?G= -ve - E°= +ve
Initiation energy (NOT Ea)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

23. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
ethers
Pale purple - (orange)-yellow - red - blue - green.
Group I metals (soft metals) are stored under oil
Mn²? - Cr³? - Cr³

24. Ions are not ______.
The compound with the lowest Ksp value.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
non-metal oxides and hydrides are covalently bonded and are acidic.
atoms

25. What is the general formula of an alkane?
CnH(2n+2)
zero
CO3²?
zero

26. What is the basic structure of an optical isomer?
Ionic compounds
Mono; di; tri; tetra; penta; hexa.
Initiation energy (NOT Ea)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

27. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
0 and 14
Read the bottom of the meniscus
left - ppt will form

28. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
it's lower and occurs over less sharp a range
Concentration
Ionic compounds

29. How do you compute % dissociation?
Identity and purity (impure compounds usually have broad & low melting points)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Big K=kf/kr
Increases down group 1 decreases down group 17

30. phosphate
Soluble except Ag - Pb - Ca - Sr Ba)
PO4³?
CrO4²?
lighted splint (positive result=pop)

31. Where are group I metals stored?
Transition element compounds (except if it has a full or empty d shell)
red - green - blue
Group I metals (soft metals) are stored under oil
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

32. Name C7H16
by electrolysis
H2O + CO2 (it decomposes readily)
left - ppt will form
Heptane

33. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
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.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
do not change
a-IMFs - b-molecular volume

34. What things should you remember to do when collecting gas over water?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
allow for the vapor pressure of water and make sure to level levels
+4-covalent - +2-ionic
left - ppt will form

35. What is HCOOCH3?
Saturated - Substitution (which requires more radical conditions)
acid + alcohol
Acids; HCOOCH3 is an ester
metal oxides and hydrides are ionically bonded and basic

36. What type of compounds are almost always colored?
Purple
Transition element compounds (except if it has a full or empty d shell)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
basic

37. dichromate (soln + most solids)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Orange
Trigonal pyramidal
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

38. sulfate
SO4²?
an oxidized and reduced substance
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

39. What are two substances that sublime at 1 atm when heated?
CO2 and H2O
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Iodine and CO2 (dry ice)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

40. What is the general formula for an alcohol?
ClO4?
ROH
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
MnO4?

41. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
Anode
CO3²?
ion pairing

42. What do group I/II metal oxides plus water form?
bases
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Nothing
Saturated - Substitution (which requires more radical conditions)

43. Colorless doesn't mean ______
How close results are to the accepted value
NO3?
Clear
CrO4²?

44. Acid plus base make?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Salt + water.
O2 needs 4F/mol H2 needs 2F/mol
non-metal oxides and hydrides are covalently bonded and are acidic.

45. chlorate
ClO3?
Ksp = 27s4
Cr2O7²?
10?8

46. What is reflux?
boiling without losing volatile solvents/reactants
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
methyl formate
CO (poisonous)

47. What causes the dramatic effect of T on rate?
Mn²? - Cr³? - Cr³
T increases exponentially the proportion of molecules with E > Ea
Salt + water
Glowing splint (positive result=relights)

48. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
#ligands=charge x2
Products - reactants (except for BDE when it's reactants - products)
Acid rain - dissolves marble buildings/statues and kills trees.

49. What are the signs of ?G and E° for spontaneous reactions?
Selective absorption
proton acceptor.
?G=negative - E° must be positive
Nothing

50. What two compounds are great oxidizing agents?

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