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 process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
?H formation of an element in standard state=0
Salt + water
Add acid to water so that the acid doesn't boil and spit


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

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3. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Silvery gray solid - brown - purple
blue glass - it filters UV
a-IMFs - b-molecular volume
Disulfur dichloride


4. dichromate (soln + most solids)
Hg2²?
+4-covalent - +2-ionic
voltaic: - electrolytic: +
Orange


5. One mole of electrons carries 96500Coulombs - what is this quantity called?

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6. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
ionic and form hydrogen and hydroxide
Acidified
H+
H3PO4


7. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
do not change
S crystal at 0K=0
Mn²? - Cr³? - Cr³
But S° of element is not zero (except at 0K)


8. What is the name of S2Cl2? (Know how to name others like this - too)
ion pairing
Disulfur dichloride
q=mc?T q=mL (or n x ?h)
Acid rain - dissolves marble buildings/statues and kills trees.


9. What is the formula for alkynes?
Products - reactants (except for BDE when it's reactants - products)
do not change
CnH2n-2
linear


10. If Q > Ksp - then system shifts _______ and ppt ______
a-IMFs - b-molecular volume
left - ppt will form
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Mn²? - Cr³? - Cr³


11. What apparatus do you use to separate 2 immiscible liquids?
0 and 14
Separating funnel
bases
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)


12. Aromatic compounds contain what?
The benzene ring (or more correctly the phenyl group - C6H5)
ion pairing
CrO4²?
an oxidized and reduced substance


13. Which would cause the bulb in a conductivity apparatus to be brightest?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Iodine and CO2 (dry ice)
Most INsoluble except group 1 and ammonium
0.10M HCl (more ions)


14. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Ksp = 27s4
P2O5
a-IMFs - b-molecular volume
Acid rain - dissolves marble buildings/statues and kills trees.


15. nitrates
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Soluble
do not change
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)


16. What do nonmetal oxides plus water form?
acids
Concentration
ion pairing
small size and high charge


17. What is precision?
Heat a test tube at an angle at the side of the tube (not bottom)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
How grouped results are


18. What is the formula for summation?

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19. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
by electrolysis
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble


20. What are two substances that sublime at 1 atm when heated?
Eudiometer
Iodine and CO2 (dry ice)
do not change
Ksp = 4s³


21. What is the test for hydrogen?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Saturated - Substitution (which requires more radical conditions)
lighted splint (positive result=pop)


22. What steps do organic labs consist of?
Synthesis - separation and purification of the product and its identification.
Ksp = 4s³
Distillation
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.


23. What reacts with an acid to create hydrogen gas?
An active metal.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
NH4?
+4-covalent - +2-ionic


24. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
different forms of the same element
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Greenish-yellow gas


25. Does reactivity increase/decrease going down group 1 and group 17?
Heptane
Synthetic condensation polymer (aka a polyamide)
Increases down group 1 decreases down group 17
small size and high charge


26. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Iodine and CO2 (dry ice)
They stay the same.
OH- and NH3
Nothing


27. What shape is methane?
Tetrahedral
left - ppt will form
Decant
Molecules with the same molecular formulas - but different structural formulas


28. Color (absorbance) is proportional to ________
Graduated cylinder
are less dense than water
Concentration
Orange


29. chlorate
ClO3?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
yellow
blue


30. What complex ion does ammonia form with silver? copper? cadmium? zinc?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
A) any range. b) 8-10 c) 4-6
Acids; HCOOCH3 is an ester


31. What apparatus do you use to pour liquids?
O2 needs 4F/mol H2 needs 2F/mol
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia
ClO3?
Pour liquids using a funnel or down a glass rod


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

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33. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Distillation
redox reaction


34. What causes the dramatic effect of T on rate?
Soluble
T increases exponentially the proportion of molecules with E > Ea
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Mono; di; tri; tetra; penta; hexa.


35. What electrons are lost/gained first in transition element ions?
Check for air bubbles in the buret and remove the buret funnel from the buret
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
ns² electrons (first in-first out)
O2 needs 4F/mol H2 needs 2F/mol


36. chromate ion (soln + most solids)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
yellow
Acids; HCOOCH3 is an ester
metal oxides and hydrides are ionically bonded and basic


37. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
water and substances with (s) less dense than
same KE - but PEice<PEwater
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia


38. What is the general formula for an ester?
RCOOR
Insoluble except for nitrate and acetate
Hg2²?
Salt + water


39. What process do you use to separate two liquids with different boiling points?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
fractional distillation
brown volatile liquid
Ionic compounds


40. group 1 ions/compounds
Making sigma bonds and holding lone pairs
An active metal.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Soluble


41. What are the formulas for q?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
q=mc?T q=mL (or n x ?h)
water and substances with (s) less dense than
Suniverse increases for spontaneous processes


42. chromate
Initiation energy (NOT Ea)
CrO4²?
S crystal at 0K=0
To ensure Ptot = Plab and that Pgas = Ptot-PH2O


43. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
An active metal.
P2O5
CH3COO?
benzene has a delocalized pi ring structure


44. What do group I/II metal oxides plus water form?
Insoluble
Hg²?
All except for lithium
bases


45. What is the general formula for an acid?
Insoluble except for nitrate and acetate
RCOOH
CO3²?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)


46. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia
Most are soluble except Ag - Pb


47. What two compounds are great oxidizing agents?

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48. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
water and substances with (s) less dense than


49. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
The Faraday or Faraday's constant.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble


50. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
At half equivalence - pH=pKa
water and substances with (s) less dense than
?H-kJ - ?S-J - ?G-kJ
basic