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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 is the formula for alkenes?
Salts (ex: CaO + SO2 ? CaSO3)
CnH2n
C4H10
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

2. What is the energy you must put into a reaction to make it start called?
H2PO4?
water and substances with (s) less dense than
Initiation energy (NOT Ea)
Evaporation

3. What is the formula of copper (II) phosphate?
Cu3(PO4)2
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)
CH3COO?
It ceases - the circuit is broken.

4. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
H+
fruit - fish - bases
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

5. When is ?G zero?
by electrolysis
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
benzene is less reactive than alkenes
proton donor base

6. Metal hydrides are _____ and form _______ and _______ when added to water
RNH2
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
ionic and form hydrogen and hydroxide
Silvery gray solid - brown - purple

7. Ions are not ______.
atoms
blue
H2PO4?
voltaic: - electrolytic: +

8. What is the general formula for an amine?
NO3?
it reacts by substitution NOT addition
RNH2
RX

9. What effect does increasing the size/surface area of a voltaic cell have on the cell?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
NH4?
0.10M HCl (more ions)

10. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Synthesis - separation and purification of the product and its identification.
Insoluble except nitrate and acetate
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

11. What two compounds are great oxidizing agents?

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12. What is Big K in terms of kf and kr?
water and substances with (s) less dense than
O2 needs 4F/mol H2 needs 2F/mol
Big K=kf/kr
no - they're written undissociated (HAaq)

13. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Disulfur dichloride
benzene is less reactive than alkenes
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

14. How do you heat a test tube?
hydroxides (ex: Ba(OH)2)
an oxidized and reduced substance
Heat a test tube at an angle at the side of the tube (not bottom)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

15. What is a dipeptide? polypeptide? protein?
Heptane
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
ROH
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

16. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
ClO?
Read the bottom of the meniscus

17. What is the sign of the cathode in voltaic cells? in electrolytic cells?
zero
voltaic: + electrolytic: -
non-metal oxides and hydrides are covalently bonded and are acidic.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

18. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
yellow
Experimental mass/theoretical mass X 100
Products - reactants (except for BDE when it's reactants - products)

19. Both Acetic acid and ____________ are also functional isomers.
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
methyl formate
H2O + CO2 (it decomposes readily)
RCOR

20. How does half life change for zero-th order - first order - and second order processes?
Sulfur
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
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)
zero-th: decreases - first: constant - second: increases

21. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
a-IMFs - b-molecular volume
Sigma bonds are stronger than pi bonds
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

22. An amphiprotic (amphoteric) species is...
The dilution effect when the solutions mix. M1V1 = M2V2
O2 needs 4F/mol H2 needs 2F/mol
Decant
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

23. Color is due to ______ _______ of light.
Products - reactants (except for BDE when it's reactants - products)
Hg2²?
Selective absorption
Monomer + monomer = polymer product + a simple molecule such as water or HCl

24. dichromate (soln + most solids)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Acidified
chemically (ex: with carbon)
Orange

25. Why are i factors (Van't Hoff factors) often less than ideal?
Most INsoluble except group 1 and ammonium
ion pairing
Initiation energy (NOT Ea)
CrO4²?

26. Do anions flow to the cathode or anode?
|experimental - accepted|/accepted X 100
bent
Group 1 hydroxides (ex: NaOH)
Anode

27. What is the formula for obtaining charge flowing in a cell?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Transition element compounds (except if it has a full or empty d shell)
Q=It (time in seconds)
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.

28. bromine
brown volatile liquid
RNH2
ROH
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

29. What is the general formula of an alkane?
small size and high charge
CnH(2n+2)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

30. What apparatus do you use to pour liquids?
basic
Kc=Kp
Pour liquids using a funnel or down a glass rod
non-metal oxides and hydrides are covalently bonded and are acidic.

31. 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?
CO2 and H2O
They decrease (or could be the same if the solid has ONLY JUST disappeared)
ethers

32. sulfate
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
SO4²?
atoms
voltaic: + electrolytic: -

33. How do you compute % dissociation?
Iodine and CO2 (dry ice)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Most INsoluble except group 1 and ammonium
left - ppt will form

34. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
S crystal at 0K=0
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Salt and water

35. Which alkali metals float on water?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
blue
do not change
All except for lithium

36. What is the difference between equivalence point and end point of a titration.
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
acids
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Graduated cylinder

37. What is the word equation for addition polymerisation?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
atoms
Disulfur dichloride

38. What is the general formula for alkyl halides?
bright yellow
RX
Silvery gray solid - brown - purple
Perform ICE BOX calculation based on K1

39. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
CO (poisonous)
|experimental - accepted|/accepted X 100
+4-covalent - +2-ionic
Group 1 hydroxides (ex: NaOH)

40. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Ppt will NOT form (unsaturated)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Insoluble except nitrate and acetate

41. What is the general formula for an acid?
The dilution effect when the solutions mix. M1V1 = M2V2
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
RCOOH
CnH(2n+2)

42. Do you use J or kJ for ?H - ?S - and ?G?
red - green - blue
fractional distillation
?H-kJ - ?S-J - ?G-kJ
Add acid to water so that the acid doesn't boil and spit

43. What process do you use to obtain a solvent from a solution?
Distillation
ClO2?
Salt + water.
q=mc?T q=mL (or n x ?h)

44. When combining half equations - what do you do to E° values when multiplying coefficients?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
zero-th: decreases - first: constant - second: increases
Saturated - Substitution (which requires more radical conditions)
Nothing

45. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
White precipitate
it is lower and occurs over less sharp a range
They decrease (or could be the same if the solid has ONLY JUST disappeared)
strong acids/bases are written as H+ or OH- ions

46. What is the formula for percent error?
brown volatile liquid
O2 needs 4F/mol H2 needs 2F/mol
#ligands=charge x2
|experimental - accepted|/accepted X 100

47. Buffer capacity must contain decent amounts of a ________ ________
CO (poisonous)
Q=It (time in seconds)
Current - time and charge on ion (moles of e used in half cell reaction)
Conjugate pair (one must be a weak base or acid)

48. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Salt and water
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
it's lower and occurs over less sharp a range
Experimental mass/theoretical mass X 100

49. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
neutralization: high K - H2O product dissociation: low K - H2O reactant
blue glass - it filters UV
Ksp = 4s³
-Ea/R

50. Alkanes are _________ and react by _________
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Silvery gray solid - brown - purple
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Saturated - Substitution (which requires more radical conditions)