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 are the names and formulas of the 6 strong acids?
Products - reactants (except for BDE when it's reactants - products)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
proton acceptor.
Insoluble


2. What is the general formula for an ether?
ROR
Ksp = 4s³
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Reduction always takes place at the cathode (RED CAT) In both types of cell!


3. What is reflux?
Kc=Kp
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
boiling without losing volatile solvents/reactants


4. What are isotopes?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
CnH2n
Acid rain - dissolves marble buildings/statues and kills trees.
Combine the equations for the half reactions in the non-spontaneous direction


5. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Heptane
Increases.
Acid rain - dissolves marble buildings/statues and kills trees.
it's lower and occurs over less sharp a range


6. sulfate
proton donor base
SO4²?
Iodine and CO2 (dry ice)
Sulfur


7. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
#ligands=charge x2
?H-kJ - ?S-J - ?G-kJ
Increases.


8. group 1 ions/compounds
lighted splint (positive result=pop)
zero
voltaic: + electrolytic: -
Soluble


9. How are strong ones written?
same KE - but PEice<PEwater
strong acids/bases are written as H+ or OH- ions
an oxidized and reduced substance
Sulfur


10. dihydrogen phosphate
All except for lithium
Experimental mass/theoretical mass X 100
Orange
H2PO4?


11. What does saturated mean? Unsaturated?
P2O5
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.
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Perform ICE BOX calculation based on K1


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

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13. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
At half equivalence - pH=pKa
Synthetic condensation polymer (aka a polyamide)
K1 x K2


14. What do the 'a' and 'b' in Van Der Waal's equation allow for?
The dilution effect when the solutions mix. M1V1 = M2V2
Products - reactants (except for BDE when it's reactants - products)
ion pairing
a-IMFs - b-molecular volume


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

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16. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
The dilution effect when the solutions mix. M1V1 = M2V2
neutralization: high K - H2O product dissociation: low K - H2O reactant
Big K=kf/kr


17. What word is a clue for a redox reaction?
Hg2²?
White precipitate
Acidified
At half equivalence - pH=pKa


18. What are two allotropes of carbon?
ns² electrons (first in-first out)
benzene is less reactive than alkenes
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
diamond and graphite


19. What is the general formula for alkyl halides?
Increases down group 1 decreases down group 17
Increases.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
RX


20. What is the first law of thermodynamics?
zero
E=q + w (negative is by system - positive is on system)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
All except for lithium


21. iodine - iodine solution - iodine vapor
CnH2n+2
Silvery gray solid - brown - purple
ClO3?
T increases exponentially the proportion of molecules with E > Ea


22. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
it reacts by substitution NOT addition
A) any range. b) 8-10 c) 4-6
Mono; di; tri; tetra; penta; hexa.


23. How do you get Ecell for spontaneous reactions?
It ceases - the circuit is broken.
catalyst=conc H2SO4
At half equivalence - pH=pKa
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)


24. Name six characteristics of transition elements (or their compounds)
O2 needs 4F/mol H2 needs 2F/mol
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)
methyl formate
ns² electrons (first in-first out)


25. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
Check for air bubbles in the buret and remove the buret funnel from the buret
Cu3(PO4)2
Trigonal pyramidal


26. What is the formula for summation?

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27. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Pale purple - (orange)-yellow - red - blue - green.
?H-kJ - ?S-J - ?G-kJ
CO2 and H2O


28. Is the freezing of ice endothermic or exothermic?
Exothermic
S crystal at 0K=0
A salt solution.
Current - time and charge on ion (moles of e used in half cell reaction)


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

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30. What two types of substances are present in all redox reactions?
Initiation energy (NOT Ea)
Suniverse increases for spontaneous processes
Synthesis - separation and purification of the product and its identification.
an oxidized and reduced substance


31. halides
Most are soluble except Ag - Pb
do not change
Molecules with the same molecular formulas - but different structural formulas
[A?]/[HA] x 100 or [BH?]/[B] x 100


32. What is the general formula for an aldehyde?
RCHO (carbonyl at end)
Check for air bubbles in the buret and remove the buret funnel from the buret
same KE - but PEice<PEwater
acid + alcohol


33. What is the formula for alkenes?
Salt + water.
zero-th: decreases - first: constant - second: increases
Graduated cylinder
CnH2n


34. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
CnH2n
left - ppt will form
chemically (ex: with carbon)


35. If a free element is involved - what type of reaction must be involved?
ClO?
redox reaction
Graduated cylinder
RX


36. What is the general formula for an acid?
An active metal.
RCOOH
Group I metals (soft metals) are stored under oil
Hg²?


37. hydroxide
An active metal.
OH?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
They decrease (or could be the same if the solid has ONLY JUST disappeared)


38. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Glowing splint (positive result=relights)
water and substances with (s) less dense than
Increases.
How grouped results are


39. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
acid + alcohol
H2O + CO2 (it decomposes readily)
All except for lithium


40. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
Ksp = 108s5
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -


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

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42. Does Kw increase or decrease with T? Why?
Identity and purity (impure compounds usually have broad & low melting points)
Cu3(PO4)2
fruit - fish - bases
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.


43. What do metal oxides plus non- metal oxides form?
All except for lithium
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Salts (ex: CaO + SO2 ? CaSO3)


44. Which alkali metals float on water?
RNH2
catalyst=conc H2SO4
All except for lithium
linear


45. What are amphoteric oxides?
OH?
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?)
Q=It (time in seconds)
Hg2²?


46. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
Exothermic (?H for ANY sa/sb = -57kJ/mol)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
bent


47. The oxidation # for acid base reactions...
voltaic: + electrolytic: -
MnO4?
C2O4²?
do not change


48. What is an Alkyl group?

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49. What apparatus do you use to separate 2 immiscible liquids?
voltaic: + electrolytic: -
HClO4
Separating funnel
Clear


50. bromine
Acid rain - dissolves marble buildings/statues and kills trees.
brown volatile liquid
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
+4-covalent - +2-ionic