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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 an Alkyl group?

2. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
left - ppt will form
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Mn²? - Cr³? - Cr³
benzene has a delocalized pi ring structure

3. What do acids plus active metals form?
Exothermic
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Synthetic condensation polymer (aka a polyamide)
P2O5

4. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Soluble except Ag - Pb - Ca - Sr Ba)
a-IMFs - b-molecular volume
RCHO (carbonyl at end)
T increases exponentially the proportion of molecules with E > Ea

5. What is the catalyst for this reaction Ester + ?
Salt + water
CrO4²?
Insoluble except nitrate and acetate
catalyst=conc H2SO4

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

7. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Most are soluble except Ag - Pb
?H formation of an element in standard state=0

8. phosphate
ion pairing
PO4³?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
linear

9. What element is used to vulcanize rubber?
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
Sulfur
zero-th: decreases - first: constant - second: increases
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

10. What are the signs for ?G and E° for spontaneous reactions?
Pale purple - (orange)-yellow - red - blue - green.
?G= -ve - E°= +ve
Insoluble (except group 1 ammonium and Ba)
But S° of element is not zero (except at 0K)

11. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Suniverse increases for spontaneous processes
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Synthesis - separation and purification of the product and its identification.
Anode - oxygen. Cathode - hydrogen

12. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
Exothermic
Hg2²?
NH2?
The compound with the lowest Ksp value.

13. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Glowing splint (positive result=relights)
Heptane
same KE - but PEice<PEwater

14. If Q > Ksp - then system shifts _______ and ppt ______
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
RNH2
left - ppt will form
Monomer + monomer = polymer product + a simple molecule such as water or HCl

15. Generally - which oxy acid is strongest?
left - ppt will form
The one with most oxygen atoms (highest oxidation number)
But S° of element is not zero (except at 0K)
same KE - but PEice<PEwater

16. What reacts with an acid to create hydrogen gas?
An active metal.
K2
Salt + water
hydroxides (ex: Ba(OH)2)

17. oxalate
atoms
Insoluble (except group 1 ammonium and Ba)
C2O4²?
Acid rain - dissolves marble buildings/statues and kills trees.

18. 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)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
a-IMFs - b-molecular volume
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

19. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
?G=negative - E° must be positive
do not change
PO4³?
Ksp = 27s4

20. What is the test for oxygen?
They stay the same.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Glowing splint (positive result=relights)

21. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
chemically (ex: with carbon)
Insoluble except for nitrate and acetate

22. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Ksp = 27s4
do not change
Pale purple - (orange)-yellow - red - blue - green.

23. phosphates
Purple
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Most INsoluble except group 1 and ammonium
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

24. dichromate (soln + most solids)
Orange
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Filtration
H2PO4?

25. What process do you use to obtain the solute from a solution?
Making sigma bonds and holding lone pairs
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Saturated - Substitution (which requires more radical conditions)
Evaporation

26. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Glacial acetic acid
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

27. What process do you use to separate two liquids with different boiling points?
fractional distillation
Heptane
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Ppt will NOT form (unsaturated)

28. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Glacial acetic acid
Only temperature
Current - time and charge on ion (moles of e used in half cell reaction)
Salt + water.

29. What do you use to look at burning magnesium? why?
blue glass - it filters UV
Soluble
blue
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

30. Name six characteristics of transition elements (or their compounds)
lighted splint (positive result=pop)
E=q + w (negative is by system - positive is on system)
?H formation of an element in standard state=0
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)

31. What do you use for an acid spill? base spill?
Pale purple - (orange)-yellow - red - blue - green.
a-IMFs - b-molecular volume
RNH2
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

32. What type of polymer is nylon?
NH4?
Synthetic condensation polymer (aka a polyamide)
Iodine and CO2 (dry ice)
are less dense than water

33. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
Kc=Kp
Soluble
Heptane

34. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Pale purple - (orange)-yellow - red - blue - green.
OH- and NH3
a-IMFs - b-molecular volume
Q=It (time in seconds)

35. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
ClO3?
blue (BTB)
H+
red - green - blue

36. dihydrogen phosphate
H2PO4?
K2
White precipitate
fractional distillation

37. Which of the rates changes more when temperature is increased?
It ceases - the circuit is broken.
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

38. How many ligands attach to a central ion in a complex ion?
NO3?
CnH2n+2
#ligands=charge x2
an oxidized and reduced substance

39. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
ionic and form hydrogen and hydroxide
q=mc?T q=mL (or n x ?h)
Selective absorption

40. ________ are Lewis bases - because they can donate a lone pair of electrons.
Acids; HCOOCH3 is an ester
OH- and NH3
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
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

41. acetate
CH3COO?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

42. 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
voltaic: - electrolytic: +
All except for lithium
Synthetic condensation polymer (aka a polyamide)

43. Which would cause the bulb in a conductivity apparatus to be brightest?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Add acid to water so that the acid doesn't boil and spit
0.10M HCl (more ions)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

44. What are allotropes?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
different forms of the same element
P2O5
Insoluble except nitrate and acetate

45. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
red - green - blue
ClO4?
P2O5

46. For a dibasic acid (H2A) - [A²?]= ____ ?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
K2
water and substances with (s) less dense than

47. An amphiprotic (amphoteric) species is...
Insoluble
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
it's lower and occurs over less sharp a range

48. What is the formula for percent yield?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Experimental mass/theoretical mass X 100
Perform ICE BOX calculation based on K1
Most are soluble except Ag - Pb

49. What things should you remember to do when collecting gas over water?
Combine the equations for the half reactions in the non-spontaneous direction
Q=It (time in seconds)
allow for the vapor pressure of water and make sure to level levels
atoms

50. What is the formula for summation?