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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 hybrid orbitals used for?
Making sigma bonds and holding lone pairs
Insoluble except nitrate and acetate
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Kc=Kp

2. What type of solutions do small - highly charged cations tend to form?
White precipitate
are less dense than water
Products - reactants (except for BDE when it's reactants - products)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

3. What is the general formula of an alkane?
CH3COO?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Increases.
CnH(2n+2)

4. What are two substances that sublime at 1 atm when heated?
it's lower and occurs over less sharp a range
Iodine and CO2 (dry ice)
An active metal.
Eudiometer

5. Colorless doesn't mean ______
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Selective absorption
Clear
Most are soluble except Ag - Pb

6. Is the freezing of ice endothermic or exothermic?
Ksp = s²
The benzene ring (or more correctly the phenyl group - C6H5)
Exothermic
non-metal oxides and hydrides are covalently bonded and are acidic.

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

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8. What do metal oxides plus non- metal oxides form?
CO2 and H2O
O2 needs 4F/mol H2 needs 2F/mol
Clear
Salts (ex: CaO + SO2 ? CaSO3)

9. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Anode
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

10. What is the catalyst for this reaction Ester + ?
catalyst=conc H2SO4
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
H+
strong acids/bases are written as H+ or OH- ions

11. An amphiprotic (amphoteric) species is...
Perform ICE BOX calculation based on K1
CH3COO?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

12. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
OH- and NH3
10?8
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Check for air bubbles in the buret and remove the buret funnel from the buret

13. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
Decant
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Most INsoluble except group 1 and ammonium

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

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15. What is the difference between equivalence point and end point of a titration.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
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
Sigma bonds are stronger than pi bonds
Separating funnel

16. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Mn²? - Cr³? - Cr³
benzene is less reactive than alkenes
A) any range. b) 8-10 c) 4-6

17. What is the general formula for an alcohol?
Iodine and CO2 (dry ice)
Hg2²?
hydroxides (ex: Ba(OH)2)
ROH

18. What shape is methane?
RNH2
Tetrahedral
Kc=Kp
Acids; HCOOCH3 is an ester

19. What are the common strong bases?
ClO?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Group 1 hydroxides (ex: NaOH)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

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

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21. What is the name of S2Cl2? (Know how to name others like this - too)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Disulfur dichloride
fruit - fish - bases
Sulfur

22. Esterification is...
acid + alcohol
Only temperature
Filtration
Current - time and charge on ion (moles of e used in half cell reaction)

23. oxalate
water and substances with (s) less dense than
Increases down group 1 decreases down group 17
C2O4²?
blue

24. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
zero
Purple
No - it depends on the number of ions produced on dissolving.

25. Acids + Carbonates (bicarbonates) make?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Ppt will NOT form (unsaturated)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

26. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
H2PO4?
How grouped results are
Mn²? - Cr³? - Cr³
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

27. What does the solubility of organic compounds depend on?
Most INsoluble except group 1 and ammonium
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Soluble except Ag - Pb - Ca - Sr Ba)
H2PO4?

28. What do nonmetal oxides plus water form?
#ligands=charge x2
Clear
acids
a-IMFs - b-molecular volume

29. What do you need to make a polymer?
Salt + water.
lighted splint (positive result=pop)
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)

30. During a titration what is present in the beaker at the equivalence point?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
ns² electrons (first in-first out)
S crystal at 0K=0
A salt solution.

31. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Pale purple - (orange)-yellow - red - blue - green.
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
allow for the vapor pressure of water and make sure to level levels

32. ammonium/ammonium compounds
Experimental mass/theoretical mass X 100
Separating funnel
Soluble
Insoluble (except group 1 ammonium and Ba)

33. What do you do to get rid of most of the solution from a precipitate?
Decant
RCOOH
[A?]/[HA] x 100 or [BH?]/[B] x 100
Distillation

34. The oxidation # for acid base reactions...
proton acceptor.
benzene has a delocalized pi ring structure
it is lower and occurs over less sharp a range
do not change

35. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
red - green - blue
water and substances with (s) less dense than
yellow
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

36. What is the relationship in strength between sigma and pi bonds?
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?)
Sigma bonds are stronger than pi bonds
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
?H formation of an element in standard state=0

37. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
zero
Acid rain - dissolves marble buildings/statues and kills trees.
do not change

38. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Synthetic condensation polymer (aka a polyamide)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Current - time and charge on ion (moles of e used in half cell reaction)
RNH2

39. nitrate
Perform ICE BOX calculation based on K1
NO3?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Silvery gray solid - brown - purple

40. What is H2CO3 (carbonate acid) usually written as?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
NO3?
H2O + CO2 (it decomposes readily)
More chaotic (ex: gases made)

41. acetate
CH3COO?
T increases exponentially the proportion of molecules with E > Ea
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
ion pairing

42. What is the conjugate acid of H2PO4?
A salt solution.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
H3PO4
White precipitate

43. What is the general formula for an ether?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
zero
ROR
All except for lithium

44. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
O2 needs 4F/mol H2 needs 2F/mol
Ionic compounds
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

45. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
a-IMFs - b-molecular volume
Soluble
H+
Silvery gray solid - brown - purple

46. How do you get Ecell for spontaneous reactions?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Purple
Unsaturated - addition (ex: decolorize bromine solution)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

47. iodine - iodine solution - iodine vapor
At half equivalence - pH=pKa
Silvery gray solid - brown - purple
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.
Pour liquids using a funnel or down a glass rod

48. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Add acid to water so that the acid doesn't boil and spit
Purple
K2
a-IMFs - b-molecular volume

49. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
ethers
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

50. What shape is carbon dioxide?
ethers
Hg2²?
Orange
linear