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. Are weak acids (and bases) written dissociated?

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2. phosphate
PO4³?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Separating funnel
methyl formate


3. What value of R do you use for thermo calculations? gas calculations?
Glowing splint (positive result=relights)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
0 and 14


4. What is accuracy?
Concentration
How close results are to the accepted value
redox reaction
Salts (ex: CaO + SO2 ? CaSO3)


5. What are isotopes?
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
Ksp = 4s³
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
+4 and +2 (+4 dominates top of group and +2 at bottom of group)


6. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
PO4³?
Heat a test tube at an angle at the side of the tube (not bottom)


7. What is the formula of butane?
diamond and graphite
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
RCOOR
C4H10


8. What is the formula for percent error?
|experimental - accepted|/accepted X 100
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
bright yellow
O2 needs 4F/mol H2 needs 2F/mol


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

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10. What apparatus do you use to separate 2 immiscible liquids?
No - NH3 and HCl gases are extremely soluble
Separating funnel
voltaic: - electrolytic: +
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)


11. sulfate
SO4²?
red - green - blue
Current - time and charge on ion (moles of e used in half cell reaction)
RCHO (carbonyl at end)


12. What should you check for before you begin titrating?
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?)
Check for air bubbles in the buret and remove the buret funnel from the buret
Tetrahedral
Suniverse increases for spontaneous processes


13. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
redox reaction
ClO3?
blue
same KE - but PEice<PEwater


14. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
P2O5
Identity and purity (impure compounds usually have broad & low melting points)
zero


15. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
boiling without losing volatile solvents/reactants
OH- and NH3
C4H10
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7


16. What do you use to look at burning magnesium? why?
blue glass - it filters UV
CrO4²?
Soluble
Graduated cylinder


17. What is the test for hydrogen?
proton acceptor.
lighted splint (positive result=pop)
water and substances with (s) less dense than
MnO4?


18. How many faradays of electric charge do you need to produce one mole of O2? H2?
Tetrahedral
O2 needs 4F/mol H2 needs 2F/mol
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
allow for the vapor pressure of water and make sure to level levels


19. Esters smell like _______ and amines smell like _______ and are ______.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
fruit - fish - bases
Nothing
NH4?


20. Colorless doesn't mean ______
Clear
voltaic: + electrolytic: -
Insoluble (except group 1 ammonium and Ba)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)


21. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
are less dense than water
No - NH3 and HCl gases are extremely soluble
No - it depends on the number of ions produced on dissolving.
water and substances with (s) less dense than


22. The oxidation # for acid base reactions...
How grouped results are
K2
do not change
lighted splint (positive result=pop)


23. hydroxides
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
Insoluble (except group 1 ammonium and Ba)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
At half equivalence - pH=pKa


24. Do you use J or kJ for ?H - ?S - and ?G?
Insoluble except group 1 and ammonium
Synthesis - separation and purification of the product and its identification.
Nothing
?H-kJ - ?S-J - ?G-kJ


25. What type of compounds do Group 14 form?
Salts (ex: CaO + SO2 ? CaSO3)
+4-covalent - +2-ionic
acid + alcohol
Read the bottom of the meniscus


26. What is reflux?
An active metal.
CrO4²?
boiling without losing volatile solvents/reactants
Heptane


27. What is the word equation for condensation polymerisation ?
Transition element compounds (except if it has a full or empty d shell)
voltaic: - electrolytic: +
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Monomer + monomer = polymer product + a simple molecule such as water or HCl


28. What is the conjugate base of NH3?
fractional distillation
NH2?
CN?
basic


29. What is precision?
Cu3(PO4)2
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
How grouped results are
Q=It (time in seconds)


30. ________ are Lewis bases - because they can donate a lone pair of electrons.
Heptane
small size and high charge
zero-th: decreases - first: constant - second: increases
OH- and NH3


31. ammonium/ammonium compounds
Soluble
RCOOH
Synthetic condensation polymer (aka a polyamide)
Selective absorption


32. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
neutralization: high K - H2O product dissociation: low K - H2O reactant
no - they're written undissociated (HAaq)
The benzene ring (or more correctly the phenyl group - C6H5)


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

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34. If a weak acid is diluted more - what happens to its % dissociation value?
Clear
Increases.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Suniverse increases for spontaneous processes


35. What type of metals don't react with water or acids to form H2?

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36. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
CnH(2n+2)
Trigonal pyramidal
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Ksp = 4s³


37. What shape is water?
ClO3?
CnH2n+2
PO4³?
bent


38. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
small size and high charge
Hg²?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
neutralization: high K - H2O product dissociation: low K - H2O reactant


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

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40. What are the units of the first order rate constant?
Insoluble except group 1 and ammonium
White precipitate
Time?¹ - (ex. s?¹ - hr?¹ - etc)
same KE - but PEice<PEwater


41. Give an example of a dilute strong acid.
Ksp = 4s³
it reacts by substitution NOT addition
boiling without losing volatile solvents/reactants
HClO4


42. Why are noble gases stable?
Cr2O7²?
Acidified
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
H2PO4?


43. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
ionic and form hydrogen and hydroxide
All except for lithium
Distillation


44. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Iodine and CO2 (dry ice)
Nothing
NH2?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec


45. chromate ion (soln + most solids)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
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?)
yellow
Ksp = 108s5


46. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Heat a test tube at an angle at the side of the tube (not bottom)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
#ligands=charge x2
+4 and +2 (+4 dominates top of group and +2 at bottom of group)


47. What do the 'a' and 'b' in Van Der Waal's equation allow for?
10?8
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
a-IMFs - b-molecular volume
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)


48. What is the difference between equivalence point and end point of a titration.
blue glass - it filters UV
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
CN?
Cu3(PO4)2


49. What are the prefixes for the naming of binary molecular compound formulas (up to six)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Synthesis - separation and purification of the product and its identification.
Mono; di; tri; tetra; penta; hexa.
left - ppt will form


50. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
by electrolysis
OH?
Insoluble (except group 1 ammonium and Ba)
Mn²? - Cr³? - Cr³