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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. Acid plus base make?
Pale yellow
Salt + water.
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
0.10M HCl (more ions)

2. hypochlorite
A salt solution.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
The one with most oxygen atoms (highest oxidation number)
ClO?

3. phosphates
atoms
Most INsoluble except group 1 and ammonium
CN?
Purple

4. What is the general formula for an amine?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
boiling without losing volatile solvents/reactants
RNH2
Perform ICE BOX calculation based on K1

5. The oxidation # for acid base reactions...
[A?]/[HA] x 100 or [BH?]/[B] x 100
small size and high charge
The Faraday or Faraday's constant.
do not change

6. What is the charge on a chlorine atom?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
strong acids/bases are written as H+ or OH- ions
zero
bright yellow

7. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Conjugate pair (one must be a weak base or acid)
The one with most oxygen atoms (highest oxidation number)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

8. What do group I/II metal oxides plus water form?
Ppt will NOT form (unsaturated)
fruit - fish - bases
bases
Increases.

9. What apparatus do you use to separate 2 immiscible liquids?
voltaic: - electrolytic: +
Separating funnel
Soluble except Ag - Pb - Ca - Sr Ba)
basic

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

11. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
CO (poisonous)
are less dense than water
yellow
[A?]/[HA] x 100 or [BH?]/[B] x 100

12. chlorine
NO3?
Soluble
Mono; di; tri; tetra; penta; hexa.
Greenish-yellow gas

13. What is the second law of thermodynamics?
How grouped results are
-Ea/R
Suniverse increases for spontaneous processes
Filtration

14. iodine - iodine solution - iodine vapor
No - it depends on the number of ions produced on dissolving.
a-IMFs - b-molecular volume
lighted splint (positive result=pop)
Silvery gray solid - brown - purple

15. When a cell is 'flat' What is its voltage?
are less dense than water
Identity and purity (impure compounds usually have broad & low melting points)
zero
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

16. How are primary alcohols turned into acids?
0.10M HCl (more ions)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

17. Why are i factors (Van't Hoff factors) often less than ideal?
But S° of element is not zero (except at 0K)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
ion pairing

18. How do you explain trends in atomic properties using Coulomb's Law?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
CnH2n+1 often designated 'R' ex C3H7 is propyl
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Graduated cylinder

19. How many ligands attach to a central ion in a complex ion?
a-IMFs - b-molecular volume
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)
diamond and graphite
#ligands=charge x2

20. What is the conjugate acid of H2PO4?
H3PO4
Insoluble
More chaotic (ex: gases made)
Unsaturated - addition (ex: decolorize bromine solution)

21. Ions are not ______.
Soluble
Evaporation
atoms
Silvery gray solid - brown - purple

22. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
Separating funnel
Group I metals (soft metals) are stored under oil
do not change

23. What is the pH of 1.0M HCl? 1M NaOH?
CnH2n
0 and 14
CnH2n+1 often designated 'R' ex C3H7 is propyl
A salt solution.

24. hydroxide
OH?
Transition element compounds (except if it has a full or empty d shell)
NH4?
Exothermic

25. What is the test for hydrogen?
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)
Heat a test tube at an angle at the side of the tube (not bottom)
lighted splint (positive result=pop)
Hg2²?

26. What is accuracy?
O2 needs 4F/mol H2 needs 2F/mol
No - it depends on the number of ions produced on dissolving.
How close results are to the accepted value
are less dense than water

27. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
No - it depends on the number of ions produced on dissolving.
Ionic compounds
CrO4²?
CO2 and H2O

28. Where are group I metals stored?
zero-th: decreases - first: constant - second: increases
chemically (ex: with carbon)
Group I metals (soft metals) are stored under oil
CN?

29. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
H3PO4
zero
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
-Ea/R

30. What are amphoteric oxides?
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?)
bent
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
10?8

31. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Filtration
voltaic: + electrolytic: -
Mono; di; tri; tetra; penta; hexa.
do not change

32. Aromatic compounds contain what?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
ionic and form hydrogen and hydroxide
red - green - blue
The benzene ring (or more correctly the phenyl group - C6H5)

33. 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
Only temperature
zero
K1 x K2

34. What is the catalyst for this reaction Ester + ?
P2O5
are less dense than water
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
catalyst=conc H2SO4

35. What are hybrid orbitals used for?
Pour liquids using a funnel or down a glass rod
Making sigma bonds and holding lone pairs
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Acid rain - dissolves marble buildings/statues and kills trees.

36. What is the general formula for an ether?
T increases exponentially the proportion of molecules with E > Ea
Kc=Kp
An active metal.
ROR

37. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
benzene has a delocalized pi ring structure
bent
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

38. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
water and substances with (s) less dense than
C2O4²?
The dilution effect when the solutions mix. M1V1 = M2V2

39. What element is used to vulcanize rubber?
benzene is less reactive than alkenes
Cu3(PO4)2
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Sulfur

40. What is reflux?
boiling without losing volatile solvents/reactants
q=mc?T q=mL (or n x ?h)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
non-metal oxides and hydrides are covalently bonded and are acidic.

41. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
Separating funnel
-Ea/R
a-IMFs - b-molecular volume

42. sulfates
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Soluble except Ag - Pb - Ca - Sr Ba)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Acids; HCOOCH3 is an ester

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

44. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Selective absorption
At half equivalence - pH=pKa
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
different forms of the same element

45. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Eudiometer
Ksp = s²
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
SO4²?

46. How do you get the equation for a net electrolysis reaction?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Combine the equations for the half reactions in the non-spontaneous direction
are less dense than water
Silvery gray solid - brown - purple

47. What do group I/II metal oxides and acids form?
Selective absorption
Salt and water
OH?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

48. How do you dilute an acid?

49. If Q > Ksp - then system shifts _______ and ppt ______
MnO4?
left - ppt will form
Read the bottom of the meniscus
Insoluble except nitrate and acetate

50. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
CnH2n
Ksp = 4s³
ROR
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.