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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. When the salt bridge is removed what happens to the cell reaction?
Disulfur dichloride
ClO4?
Decant
It ceases - the circuit is broken.

2. What value of R do you use for thermo calculations? gas calculations?
Transition element compounds (except if it has a full or empty d shell)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Acidified
Sigma bonds are stronger than pi bonds

3. What is the formula of copper (II) phosphate?
Cu3(PO4)2
No - it depends on the number of ions produced on dissolving.
Most are soluble except Ag - Pb
Ksp = 4s³

4. How do you dilute an acid?

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5. How are primary alcohols turned into acids?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

6. If Q < Ksp a ppt ______
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
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
It ceases - the circuit is broken.
Ppt will NOT form (unsaturated)

7. If Q > Ksp - then system shifts _______ and ppt ______
no - they're written undissociated (HAaq)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Mn²? - Cr³? - Cr³
left - ppt will form

8. 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
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
The benzene ring (or more correctly the phenyl group - C6H5)
brown volatile liquid

9. During a titration what is present in the beaker at the equivalence point?
A salt solution.
different forms of the same element
are less dense than water
NH2?

10. What is the formula for alkenes?
a-IMFs - b-molecular volume
ionic and form hydrogen and hydroxide
CnH2n
Iodine and CO2 (dry ice)

11. acetate
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.
acid + alcohol
CnH2n+1 often designated 'R' ex C3H7 is propyl
CH3COO?

12. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
by electrolysis
Soluble
linear
water and substances with (s) less dense than

13. When combining half equations - what do you do to E° values when multiplying coefficients?
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?)
Acid rain - dissolves marble buildings/statues and kills trees.
Kc=Kp
Nothing

14. What is precision?
CnH2n-2
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
How grouped results are
Eudiometer

15. permanganate
hydroxides (ex: Ba(OH)2)
MnO4?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
CO3²?

16. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
Iodine and CO2 (dry ice)
proton donor base
How grouped results are

17. What is the difference between equivalence point and end point of a titration.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
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
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
How grouped results are

18. Name six characteristics of transition elements (or their compounds)
A) any range. b) 8-10 c) 4-6
?H formation of an element in standard state=0
RX
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)

19. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
zero
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
proton acceptor.
Pale purple - (orange)-yellow - red - blue - green.

20. What do you do to get rid of most of the solution from a precipitate?
RCOOR
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)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Decant

21. What is the catalyst for this reaction Ester + ?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
catalyst=conc H2SO4
HClO4
voltaic: + electrolytic: -

22. What is the formula for percent error?
Eudiometer
water and substances with (s) less dense than
Ions go through the salt bridge - electrons go through metal wires in the external circuit
|experimental - accepted|/accepted X 100

23. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
CnH(2n+2)
Ksp = 27s4
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
atoms

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

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25. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
ClO?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
-Ea/R

26. What are the units of the first order rate constant?
Glacial acetic acid
zero
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Products - reactants (except for BDE when it's reactants - products)

27. primary colors
red - green - blue
RNH2
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
yellow

28. Ca - Sr - Ba
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
hydroxides (ex: Ba(OH)2)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

29. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
HClO4
Conjugate pair (one must be a weak base or acid)
same KE - but PEice<PEwater
a-IMFs - b-molecular volume

30. What is the general formula for an acid?
water and substances with (s) less dense than
non-metal oxides and hydrides are covalently bonded and are acidic.
RCOOH
CH3COO?

31. What do nonmetal oxides plus water form?
non-metal oxides and hydrides are covalently bonded and are acidic.
Salts (ex: CaO + SO2 ? CaSO3)
acids
a-IMFs - b-molecular volume

32. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
different forms of the same element
a-IMFs - b-molecular volume
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

33. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
They stay the same.
an oxidized and reduced substance
Increases down group 1 decreases down group 17

34. Both Acetic acid and ____________ are also functional isomers.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
voltaic: + electrolytic: -
methyl formate
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

35. Alkenes are ________ and react by __________
0 and 14
Disulfur dichloride
Unsaturated - addition (ex: decolorize bromine solution)
Iodine and CO2 (dry ice)

36. What reacts with an acid to create hydrogen gas?
An active metal.
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)
?H-kJ - ?S-J - ?G-kJ
Experimental mass/theoretical mass X 100

37. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
NH2?
Experimental mass/theoretical mass X 100
CH3COO?

38. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
do not change
Group 1 hydroxides (ex: NaOH)
The dilution effect when the solutions mix. M1V1 = M2V2
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

39. lead iodide
Hg²?
Synthesis - separation and purification of the product and its identification.
C2O4²?
bright yellow

40. Aromatic compounds contain what?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
yellow
Tetrahedral
The benzene ring (or more correctly the phenyl group - C6H5)

41. What process do you use to obtain a solvent from a solution?
How grouped results are
Distillation
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
H+

42. What is the test for hydrogen?
lighted splint (positive result=pop)
CH3COO?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
HClO4

43. What are the formulas for q?
ns² electrons (first in-first out)
q=mc?T q=mL (or n x ?h)
diamond and graphite
red - green - blue

44. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Silvery gray solid - brown - purple
They stay the same.
small size and high charge
basic

45. What process do you use to separate two liquids with different boiling points?
Mn²? - Cr³? - Cr³
CO (poisonous)
ClO2?
fractional distillation

46. What is the basic structure of an optical isomer?
Pale purple - (orange)-yellow - red - blue - green.
zero
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.

47. What is the conjugate base of NH3?
blue
Only temperature
NH2?
It ceases - the circuit is broken.

48. Which would cause the bulb in a conductivity apparatus to be brightest?
proton donor base
Group 1 hydroxides (ex: NaOH)
0.10M HCl (more ions)
fractional distillation

49. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
different forms of the same element
They stay the same.
Acid rain - dissolves marble buildings/statues and kills trees.
brown volatile liquid

50. How does the melting point of a mixture compare to the MP of a pure substance?
non-metal oxides and hydrides are covalently bonded and are acidic.
it is lower and occurs over less sharp a range
ns² electrons (first in-first out)
Q=It (time in seconds)