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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. What equipment do you need for a titration?
Combine the equations for the half reactions in the non-spontaneous direction
HClO4
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

2. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Disulfur dichloride
CnH2n

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

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4. Name some properties of Group 17
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
White precipitate
K2
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

5. What is the general formula for an alcohol?
ROH
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)
Hg2²?
zero

6. What are the signs of ?G and E° for spontaneous reactions?
?G=negative - E° must be positive
water and substances with (s) less dense than
They stay the same.
diamond and graphite

7. Why are noble gases stable?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Ionic compounds
Soluble

8. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Nothing
More chaotic (ex: gases made)
Increases down group 1 decreases down group 17
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

9. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
water and substances with (s) less dense than
Exothermic (?H for ANY sa/sb = -57kJ/mol)
PO4³?

10. What is the general formula for an acid?
Ionic compounds
voltaic: - electrolytic: +
RCOOH
Distillation

11. Name C7H16
bases
do not change
Heptane
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

12. What are isotopes?
ethers
Acid rain - dissolves marble buildings/statues and kills trees.
Graduated cylinder
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

13. What is the word equation for addition polymerisation?
Insoluble (except group 1 ammonium and Ba)
[A?]/[HA] x 100 or [BH?]/[B] x 100
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
do not change

14. Esterification is...
q=mc?T q=mL (or n x ?h)
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
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

15. What type of compounds do metals/non metals form?
benzene has a delocalized pi ring structure
Filtration
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Ionic compounds

16. Which would cause the bulb in a conductivity apparatus to be brightest?
Identity and purity (impure compounds usually have broad & low melting points)
acid + alcohol
0.10M HCl (more ions)
fractional distillation

17. What do group I/II metal oxides plus water form?
bases
RCOOR
Ionic compounds
Insoluble except group 1 and ammonium

18. What two types of substances are present in all redox reactions?
it reacts by substitution NOT addition
0.10M HCl (more ions)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
an oxidized and reduced substance

19. How does the melting point of a mixture compare to the MP of a pure substance?
MnO4?
it is lower and occurs over less sharp a range
No - it depends on the number of ions produced on dissolving.
K2

20. What is an Alkyl group?

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21. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Synthesis - separation and purification of the product and its identification.
A) any range. b) 8-10 c) 4-6
Ksp = 108s5
fruit - fish - bases

22. What is the formula for percent yield?
Saturated - Substitution (which requires more radical conditions)
Ppt will NOT form (unsaturated)
Experimental mass/theoretical mass X 100
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

23. A Bronsted-Lowry base is...
C4H10
proton acceptor.
benzene is less reactive than alkenes
White precipitate

24. What are two allotropes of carbon?
It ceases - the circuit is broken.
Soluble
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
diamond and graphite

25. What shape is ammonia?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Trigonal pyramidal
bent
Insoluble

26. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
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)
it reacts by substitution NOT addition
Initiation energy (NOT Ea)

27. What is the formula of butane?
C4H10
K1 x K2
fractional distillation
Current - time and charge on ion (moles of e used in half cell reaction)

28. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
No - it depends on the number of ions produced on dissolving.
E=q + w (negative is by system - positive is on system)

29. What do ions and electrons travel through in a voltaic/electrolytic cell?
zero
Ions go through the salt bridge - electrons go through metal wires in the external circuit
small size and high charge
Glacial acetic acid

30. Acid plus base make?
Salt + water.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Only temperature
ClO3?

31. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
Ksp = 108s5
Hg2²?
Anode - oxygen. Cathode - hydrogen

32. What changes Keq?
Only temperature
Combine the equations for the half reactions in the non-spontaneous direction
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.
red - green - blue

33. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
Check for air bubbles in the buret and remove the buret funnel from the buret
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
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)

34. What is the conjugate acid of H2PO4?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
H3PO4
Graduated cylinder

35. What is reflux?
linear
Molecules with the same molecular formulas - but different structural formulas
boiling without losing volatile solvents/reactants
Q=It (time in seconds)

36. Color (absorbance) is proportional to ________
Group I metals (soft metals) are stored under oil
Identity and purity (impure compounds usually have broad & low melting points)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Concentration

37. BaSO4
Synthesis - separation and purification of the product and its identification.
Insoluble
water and substances with (s) less dense than
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

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

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39. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
The Faraday or Faraday's constant.
same KE - but PEice<PEwater
?H-kJ - ?S-J - ?G-kJ
No - NH3 and HCl gases are extremely soluble

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

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41. Is the freezing of ice endothermic or exothermic?
They stay the same.
Exothermic
it reacts by substitution NOT addition
How close results are to the accepted value

42. What process do you use to obtain the solute from a solution?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Evaporation
The dilution effect when the solutions mix. M1V1 = M2V2
RX

43. lead compounds
Decant
Ksp = s²
CO (poisonous)
Insoluble except nitrate and acetate

44. Alcohols and _______ are FG isomers
ethers
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

45. What is the test for hydrogen?
Synthesis - separation and purification of the product and its identification.
ClO3?
Unsaturated - addition (ex: decolorize bromine solution)
lighted splint (positive result=pop)

46. What are isomers?
K1 x K2
Molecules with the same molecular formulas - but different structural formulas
Products - reactants (except for BDE when it's reactants - products)
Soluble

47. potassium permanganate
non-metal oxides and hydrides are covalently bonded and are acidic.
Ionic compounds
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Purple

48. 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.
Soluble
CN?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
A) any range. b) 8-10 c) 4-6

49. 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
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
NO3?
Only temperature

50. hydroxides
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Synthetic condensation polymer (aka a polyamide)
Insoluble (except group 1 ammonium and Ba)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7