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 reacts with an acid to create hydrogen gas?
Both electrons come from the same atom (just as good as a regular bond)
An active metal.
Iodine and CO2 (dry ice)
Silvery gray solid - brown - purple


2. What device would you use to measure a volume of gas?
Eudiometer
ClO?
chemically (ex: with carbon)
ClO3?


3. What is the conjugate base of NH3?
0.10M HCl (more ions)
NH2?
yellow
Only temperature


4. What is the third law of thermodynamics?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
HClO4
S crystal at 0K=0
Increases.


5. What are the names and formulas of the 6 strong acids?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
No - it depends on the number of ions produced on dissolving.
fruit - fish - bases


6. What two types of substances are present in all redox reactions?
RCOR
[A?]/[HA] x 100 or [BH?]/[B] x 100
an oxidized and reduced substance
ClO4?


7. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
CO3²?
Concentration
Group 1 hydroxides (ex: NaOH)


8. thiosulfate
S2O3²?
ethers
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)


9. copper sulfate
blue
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
linear
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell


10. How do you compute % dissociation?
Perform ICE BOX calculation based on K1
[A?]/[HA] x 100 or [BH?]/[B] x 100
MnO4?
water and substances with (s) less dense than


11. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
CH3COO?
Insoluble except group 1 and ammonium
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties


12. What does saturated mean? Unsaturated?
Acid rain - dissolves marble buildings/statues and kills trees.
Selective absorption
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
CO2 and H2O


13. Alkenes are ________ and react by __________
ClO2?
CO3²?
Unsaturated - addition (ex: decolorize bromine solution)
it's lower and occurs over less sharp a range


14. What do you use for an acid spill? base spill?
zero
E=q + w (negative is by system - positive is on system)
benzene is less reactive than alkenes
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)


15. What do you do to get rid of most of the solution from a precipitate?
Decant
NO3?
H2PO4?
a-IMFs - b-molecular volume


16. What is the sign of the cathode in voltaic cells? in electrolytic cells?
NH2?
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)
C2O4²?
voltaic: + electrolytic: -


17. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Perform ICE BOX calculation based on K1


18. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Exothermic
non-metal oxides and hydrides are covalently bonded and are acidic.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Experimental mass/theoretical mass X 100


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

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20. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
benzene has a delocalized pi ring structure
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
Kc=Kp
Iodine and CO2 (dry ice)


21. mercury (II) ion
catalyst=conc H2SO4
Hg²?
atoms
'non-active' metals such as Cu - Ag - Au - Pt - etc.


22. What shape is water?
bent
Only temperature
CrO4²?
P2O5


23. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
non-metal oxides and hydrides are covalently bonded and are acidic.
HClO4
zero
proton donor base


24. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
Suniverse increases for spontaneous processes
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
ion pairing


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

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26. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
chemically (ex: with carbon)
no - they're written undissociated (HAaq)
acids


27. For a dibasic acid (H2A) - [A²?]= ____ ?
Orange
lighted splint (positive result=pop)
K2
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.


28. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
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)
T increases exponentially the proportion of molecules with E > Ea


29. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Salt + water.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
?H formation of an element in standard state=0


30. 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
acid + alcohol
OH- and NH3
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.


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

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32. sulfates
All except for lithium
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Soluble except Ag - Pb - Ca - Sr Ba)
Insoluble except nitrate and acetate


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

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34. What process do you use to obtain the solute from a solution?
Evaporation
same KE - but PEice<PEwater
do not change
P2O5


35. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Ionic compounds
hydroxides (ex: Ba(OH)2)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
No - it depends on the number of ions produced on dissolving.


36. bromine
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
brown volatile liquid
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)


37. What kind of bonding structure does benzene have?
metal oxides and hydrides are ionically bonded and basic
benzene has a delocalized pi ring structure
methyl formate
Graduated cylinder


38. What are the signs for ?G and E° for spontaneous reactions?
ns² electrons (first in-first out)
SO4²?
boiling without losing volatile solvents/reactants
?G= -ve - E°= +ve


39. What is the general formula for an alcohol?
proton acceptor.
ROH
Insoluble except nitrate and acetate
Ppt will NOT form (unsaturated)


40. What is the general formula for an ester?
Ksp = s²
RCOOR
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Heptane


41. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
The one with most oxygen atoms (highest oxidation number)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
no - they're written undissociated (HAaq)


42. What do nonmetal oxides plus water form?
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
Separating funnel
Ksp = 27s4
acids


43. What is the slope of the graph of lnk vs. 1/T?
Nothing
Check for air bubbles in the buret and remove the buret funnel from the buret
it reacts by substitution NOT addition
-Ea/R


44. chromate
Insoluble except for nitrate and acetate
CrO4²?
Pale yellow
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?)


45. Give an example of a dilute strong acid.
HClO4
Ksp = 108s5
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
RCOOH


46. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Experimental mass/theoretical mass X 100
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
a-IMFs - b-molecular volume
proton acceptor.


47. chlorite
Kc=Kp
0.10M HCl (more ions)
ClO2?
ROR


48. A Bronsted-Lowry acid is...
Greenish-yellow gas
H3PO4
proton donor base
H2PO4?


49. phosphates
Most INsoluble except group 1 and ammonium
zero
A salt solution.
Most are soluble except Ag - Pb


50. What are the products of the reaction between group 1 metals and water?

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