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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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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. How do you explain trends in atomic properties using Coulomb's Law?
RNH2
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Heptane
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

2. Alkenes are ________ and react by __________
Pale yellow
Unsaturated - addition (ex: decolorize bromine solution)
a-IMFs - b-molecular volume
Concentration

3. Name six characteristics of transition elements (or their compounds)
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)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Ions go through the salt bridge - electrons go through metal wires in the external circuit
metal oxides and hydrides are ionically bonded and basic

4. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
But S° of element is not zero (except at 0K)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
H+
methyl formate

5. Is the freezing of ice endothermic or exothermic?
Exothermic
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
PO4³?
Ksp = s²

6. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
boiling without losing volatile solvents/reactants
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
Insoluble except group 1 and ammonium
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

7. perchlorate
C2O4²?
a-IMFs - b-molecular volume
ClO4?
ion pairing

8. cyanide
Insoluble except for nitrate and acetate
Acid rain - dissolves marble buildings/statues and kills trees.
CN?
Heat a test tube at an angle at the side of the tube (not bottom)

9. thiosulfate
S2O3²?
RX
Graduated cylinder
it reacts by substitution NOT addition

10. What is the general formula for an alcohol?
-Ea/R
Nothing
ROH
CrO4²?

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

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12. What are the names and formulas of the 6 strong acids?
CH3COO?
S crystal at 0K=0
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Combine the equations for the half reactions in the non-spontaneous direction

13. mercury (I) ion
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
ethers
Pale yellow
Hg2²?

14. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
Conjugate pair (one must be a weak base or acid)
Distillation
RCHO (carbonyl at end)

15. Buffer capacity must contain decent amounts of a ________ ________
allow for the vapor pressure of water and make sure to level levels
brown volatile liquid
catalyst=conc H2SO4
Conjugate pair (one must be a weak base or acid)

16. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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17. What do the 'a' and 'b' in Van Der Waal's equation allow for?
catalyst=conc H2SO4
H2O + CO2 (it decomposes readily)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
a-IMFs - b-molecular volume

18. Give an example of a dilute strong acid.
?H-kJ - ?S-J - ?G-kJ
HClO4
Silvery gray solid - brown - purple
They decrease (or could be the same if the solid has ONLY JUST disappeared)

19. What is the general formula for an acid?
RCOOH
H+
methyl formate
Conjugate pair (one must be a weak base or acid)

20. hydroxides
proton acceptor.
Insoluble (except group 1 ammonium and Ba)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Synthetic condensation polymer (aka a polyamide)

21. ________ are Lewis bases - because they can donate a lone pair of electrons.
OH- and NH3
Iodine and CO2 (dry ice)
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
Saturated - Substitution (which requires more radical conditions)

22. What is the name of S2Cl2? (Know how to name others like this - too)
Mono; di; tri; tetra; penta; hexa.
small size and high charge
Disulfur dichloride
Perform ICE BOX calculation based on K1

23. How do you dilute an acid?

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24. What is the formula for alkanes?
redox reaction
0.10M HCl (more ions)
CnH2n+2
Pipette (burette if need repetition)

25. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Sigma bonds are stronger than pi bonds
PO4³?
Ppt will NOT form (unsaturated)
At half equivalence - pH=pKa

26. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Silvery gray solid - brown - purple
ClO2?
brown volatile liquid

27. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Pale yellow
neutralization: high K - H2O product dissociation: low K - H2O reactant
H3PO4
zero

28. Ions are not ______.
K1 x K2
zero
atoms
SO4²?

29. Alcohols and _______ are FG isomers
Cr2O7²?
Big K=kf/kr
Iodine and CO2 (dry ice)
ethers

30. What is the general formula for an ester?
RCOOR
Separating funnel
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)
The one with most oxygen atoms (highest oxidation number)

31. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
Salt and water
It ceases - the circuit is broken.
lighted splint (positive result=pop)
A) any range. b) 8-10 c) 4-6

32. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
basic
Increases.
Concentration

33. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
yellow
a-IMFs - b-molecular volume
basic

34. dihydrogen phosphate
ROH
H2PO4?
by electrolysis
S2O3²?

35. Esterification is...
E=q + w (negative is by system - positive is on system)
Filtration
The one with most oxygen atoms (highest oxidation number)
acid + alcohol

36. Acids + Carbonates (bicarbonates) make?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Silvery gray solid - brown - purple
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
by electrolysis

37. What are allotropes?
CnH2n
Mono; di; tri; tetra; penta; hexa.
different forms of the same element
H2O + CO2 (it decomposes readily)

38. What type of compounds do Group 14 form?
chemically (ex: with carbon)
The one with most oxygen atoms (highest oxidation number)
+4-covalent - +2-ionic
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

39. What is the difference between equivalence point and end point of a titration.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
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
Nothing
Both electrons come from the same atom (just as good as a regular bond)

40. What do metal oxides plus acids form?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Glacial acetic acid
Salt + water
10?8

41. What do group I/II metal oxides and acids form?
Salt and water
It ceases - the circuit is broken.
hydroxides (ex: Ba(OH)2)
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

42. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
No - it depends on the number of ions produced on dissolving.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
left - ppt will form

43. oxalate
Unsaturated - addition (ex: decolorize bromine solution)
Ksp = 4s³
Salt + water
C2O4²?

44. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Glacial acetic acid
Ions go through the salt bridge - electrons go through metal wires in the external circuit
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
non-metal oxides and hydrides are covalently bonded and are acidic.

45. acetate
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)
Separating funnel
CH3COO?
[A?]/[HA] x 100 or [BH?]/[B] x 100

46. phosphate
bent
Ksp = 27s4
?G=negative - E° must be positive
PO4³?

47. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
red - green - blue
Sulfur
Acid rain - dissolves marble buildings/statues and kills trees.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

48. Nonmetals are good _____ agents. Metals are good _______ agents.
fruit - fish - bases
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Acids; HCOOCH3 is an ester
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

49. What are the signs of ?G and E° for spontaneous reactions?
catalyst=conc H2SO4
Add acid to water so that the acid doesn't boil and spit
?G=negative - E° must be positive
a-IMFs - b-molecular volume

50. What is the general formula of an alkane?
O2 needs 4F/mol H2 needs 2F/mol
At half equivalence - pH=pKa
CnH(2n+2)
Most INsoluble except group 1 and ammonium

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AP Chemistry 2

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