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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. Why are i factors (Van't Hoff factors) often less than ideal?
PO4³?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
ion pairing
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

2. Does reactivity increase/decrease going down group 1 and group 17?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
zero
Ksp = 4s³
Increases down group 1 decreases down group 17

3. What is the general formula for an alcohol?
ROH
S crystal at 0K=0
fractional distillation
metal oxides and hydrides are ionically bonded and basic

4. What does saturated mean? Unsaturated?
Synthesis - separation and purification of the product and its identification.
Ionic compounds
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
C4H10

5. What is the sign of the anode in voltaic cells? in electrolytic cells?
HClO4
voltaic: - electrolytic: +
Saturated - Substitution (which requires more radical conditions)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

6. cyanide
ion pairing
Saturated - Substitution (which requires more radical conditions)
A) any range. b) 8-10 c) 4-6
CN?

7. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
K1 x K2
CnH2n+2
Pale purple - (orange)-yellow - red - blue - green.
Insoluble except group 1 and ammonium

8. What do you use for an acid spill? base spill?
Insoluble
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

9. dihydrogen phosphate
H2PO4?
C4H10
blue
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)

10. chlorite
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Cr2O7²?
Silvery gray solid - brown - purple
ClO2?

11. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
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)
It ceases - the circuit is broken.
-Ea/R

12. acetates
RCOOR
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Soluble
Products - reactants (except for BDE when it's reactants - products)

13. What measuring device would you use for very small volumes of liquids?
acids
Pipette (burette if need repetition)
Increases down group 1 decreases down group 17
Group 1 hydroxides (ex: NaOH)

14. Why are i factors (Van't Hoff factors) often less than ideal?
ROH
ion pairing
Most INsoluble except group 1 and ammonium
Combine the equations for the half reactions in the non-spontaneous direction

15. What device would you use to measure a volume of gas?
Eudiometer
Both electrons come from the same atom (just as good as a regular bond)
proton acceptor.
Insoluble (except group 1 ammonium and Ba)

16. What are the signs of ?G and E° for spontaneous reactions?
?G=negative - E° must be positive
Perform ICE BOX calculation based on K1
K2
Iodine and CO2 (dry ice)

17. What process do you use to obtain the precipitate from a solution?
Filtration
C2O4²?
Ppt will NOT form (unsaturated)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

18. When driving off water from a hydrate - how do you tell you're done?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
benzene has a delocalized pi ring structure
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
ClO?

19. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
small size and high charge
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
blue (BTB)

20. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
ClO3?
ClO2?
Clear

21. What element is used to vulcanize rubber?
Sulfur
OH- and NH3
redox reaction
C4H10

22. If Q > Ksp - then system shifts _______ and ppt ______
CN?
zero
Increases down group 1 decreases down group 17
left - ppt will form

23. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
allow for the vapor pressure of water and make sure to level levels
RCHO (carbonyl at end)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
No - it depends on the number of ions produced on dissolving.

24. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
blue glass - it filters UV
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
The one with most oxygen atoms (highest oxidation number)

25. What reacts with an acid to create hydrogen gas?
bright yellow
water and substances with (s) less dense than
An active metal.
boiling without losing volatile solvents/reactants

26. carbonates
Unsaturated - addition (ex: decolorize bromine solution)
S crystal at 0K=0
0 and 14
Insoluble except group 1 and ammonium

27. hydroxides
same KE - but PEice<PEwater
benzene has a delocalized pi ring structure
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Insoluble (except group 1 ammonium and Ba)

28. Aromatic compounds contain what?
ROR
?H-kJ - ?S-J - ?G-kJ
Soluble
The benzene ring (or more correctly the phenyl group - C6H5)

29. What do you need to make a polymer?
Salt + water
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)
NH2?
Ksp = 4s³

30. What is the relationship in strength between sigma and pi bonds?
O2 needs 4F/mol H2 needs 2F/mol
ionic and form hydrogen and hydroxide
Mono; di; tri; tetra; penta; hexa.
Sigma bonds are stronger than pi bonds

31. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
A salt solution.
K1 x K2
Mn²? - Cr³? - Cr³
voltaic: - electrolytic: +

32. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
0.10M HCl (more ions)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
same KE - but PEice<PEwater
acids

33. What are two substances that sublime at 1 atm when heated?
Insoluble except group 1 and ammonium
Iodine and CO2 (dry ice)
No - it depends on the number of ions produced on dissolving.
fractional distillation

34. Both Acetic acid and ____________ are also functional isomers.
Heat a test tube at an angle at the side of the tube (not bottom)
E=q + w (negative is by system - positive is on system)
Graduated cylinder
methyl formate

35. What is the catalyst for this reaction Ester + ?
ion pairing
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
catalyst=conc H2SO4
boiling without losing volatile solvents/reactants

36. What is a coordinate covalent bond?
allow for the vapor pressure of water and make sure to level levels
Both electrons come from the same atom (just as good as a regular bond)
methyl formate
Greenish-yellow gas

37. What process do you use to obtain a solvent from a solution?
same KE - but PEice<PEwater
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Distillation
blue (BTB)

38. acetate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
zero
CH3COO?
Ionic compounds

39. Give an example of a dilute strong acid.
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
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
HClO4
CnH2n+2

40. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Ppt will NOT form (unsaturated)
same KE - but PEice<PEwater
Acid rain - dissolves marble buildings/statues and kills trees.
Salt and water

41. carbonate
Ionic compounds
CO3²?
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
Heat a test tube at an angle at the side of the tube (not bottom)

42. What do metal oxides plus acids form?
red - green - blue
Salt + water
O2 needs 4F/mol H2 needs 2F/mol
CN?

43. A Bronsted-Lowry base is...
Reduction always takes place at the cathode (RED CAT) In both types of cell!
proton acceptor.
C4H10
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

44. What is Big K in terms of kf and kr?
proton donor base
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Big K=kf/kr
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

45. What is the second law of thermodynamics?
basic
Suniverse increases for spontaneous processes
No - it depends on the number of ions produced on dissolving.
0 and 14

46. bromine
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
blue glass - it filters UV
brown volatile liquid
Molecules with the same molecular formulas - but different structural formulas

47. What does the solubility of organic compounds depend on?
allow for the vapor pressure of water and make sure to level levels
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
ionic and form hydrogen and hydroxide

48. Name 2 ways in which you can create a buffer?
Perform ICE BOX calculation based on K1
Mono; di; tri; tetra; penta; hexa.
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)
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)

49. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
acids
Perform ICE BOX calculation based on K1
no - they're written undissociated (HAaq)
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

50. What is the formula of butane?
C4H10
P2O5
zero
zero-th: decreases - first: constant - second: increases