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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. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
?G=negative - E° must be positive
Evaporation
same KE - but PEice<PEwater

2. 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.
Silvery gray solid - brown - purple
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
A) any range. b) 8-10 c) 4-6
catalyst=conc H2SO4

3. chlorate
A) any range. b) 8-10 c) 4-6
strong acids/bases are written as H+ or OH- ions
Making sigma bonds and holding lone pairs
ClO3?

4. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
CO3²?
Heptane
Anode - oxygen. Cathode - hydrogen
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

5. What changes Keq?
Cr2O7²?
Only temperature
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
O2 needs 4F/mol H2 needs 2F/mol

6. carbonate
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Filtration
CO3²?
voltaic: + electrolytic: -

7. What is the second law of thermodynamics?
|experimental - accepted|/accepted X 100
SO4²?
Suniverse increases for spontaneous processes
ClO?

8. What two compounds are great oxidizing agents?

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

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10. Is a graduated cylinder or beaker more accurate?
The one with most oxygen atoms (highest oxidation number)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
H+
Graduated cylinder

11. How are metal oxides and hydrides bonded? are they acidic or basic?
Trigonal pyramidal
metal oxides and hydrides are ionically bonded and basic
linear
CnH2n+2

12. halides
voltaic: - electrolytic: +
Most are soluble except Ag - Pb
Experimental mass/theoretical mass X 100
same KE - but PEice<PEwater

13. phosphates
Most INsoluble except group 1 and ammonium
ROR
+4-covalent - +2-ionic
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

14. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
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
Synthetic condensation polymer (aka a polyamide)
Most are soluble except Ag - Pb
neutralization: high K - H2O product dissociation: low K - H2O reactant

15. 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?
CO2 and H2O
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
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

16. lead iodide
Suniverse increases for spontaneous processes
same KE - but PEice<PEwater
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)
bright yellow

17. What device would you use to measure a volume of gas?
Soluble
Current - time and charge on ion (moles of e used in half cell reaction)
Eudiometer
Read the bottom of the meniscus

18. cyanide
S2O3²?
CN?
neutralization: high K - H2O product dissociation: low K - H2O reactant
H+

19. What complex ion does ammonia form with silver? copper? cadmium? zinc?
ClO4?
allow for the vapor pressure of water and make sure to level levels
RNH2
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

20. When a cell is 'flat' What is its voltage?
C2O4²?
zero
Clear
Silvery gray solid - brown - purple

21. 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
Pale purple - (orange)-yellow - red - blue - green.
Salt + water.
P2O5

22. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
water and substances with (s) less dense than
Q=It (time in seconds)

23. Give an example of a concentrated weak acid.
Concentration
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Insoluble except for nitrate and acetate
Glacial acetic acid

24. What type of compounds do Group 14 form?
Soluble except Ag - Pb - Ca - Sr Ba)
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?)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
+4-covalent - +2-ionic

25. Does Benzene react by addition or substitution?
Ksp = 4s³
Selective absorption
Insoluble except nitrate and acetate
it reacts by substitution NOT addition

26. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Trigonal pyramidal
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
The dilution effect when the solutions mix. M1V1 = M2V2

27. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
ion pairing
Only temperature

28. acetates
Monomer + monomer = polymer product + a simple molecule such as water or HCl
catalyst=conc H2SO4
Soluble
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

29. How do you clean a buret/pipette for a titration?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
White precipitate
Read the bottom of the meniscus

30. What is the formula of copper (II) phosphate?
zero-th: decreases - first: constant - second: increases
allow for the vapor pressure of water and make sure to level levels
Group I metals (soft metals) are stored under oil
Cu3(PO4)2

31. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Separating funnel
catalyst=conc H2SO4
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

32. nitrates
Soluble
H2PO4?
hydroxides (ex: Ba(OH)2)
?H formation of an element in standard state=0

33. What is the formula for percent error?
Silvery gray solid - brown - purple
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
|experimental - accepted|/accepted X 100
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

34. What is the general formula for an ether?
ROR
An active metal.
Ppt will NOT form (unsaturated)
O2 needs 4F/mol H2 needs 2F/mol

35. What shape is methane?
#ligands=charge x2
boiling without losing volatile solvents/reactants
Transition element compounds (except if it has a full or empty d shell)
Tetrahedral

36. One mole of electrons carries 96500Coulombs - what is this quantity called?

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37. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
ClO?
Soluble

38. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
bright yellow
How grouped results are
MnO4?

39. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Insoluble
All except for lithium

40. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
CO (poisonous)
A salt solution.
Salts (ex: CaO + SO2 ? CaSO3)

41. If a free element is involved - what type of reaction must be involved?
proton donor base
redox reaction
-Ea/R
S crystal at 0K=0

42. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Exothermic
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
?H formation of an element in standard state=0
a-IMFs - b-molecular volume

43. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Experimental mass/theoretical mass X 100
K2
basic
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

44. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
atoms
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Molecules with the same molecular formulas - but different structural formulas
Cr2O7²?

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

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46. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
it reacts by substitution NOT addition
Clear
Reduction always takes place at the cathode (RED CAT) In both types of cell!

47. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
different forms of the same element
a-IMFs - b-molecular volume
Salt + water

48. What is H2CO3 (carbonate acid) usually written as?
Acid rain - dissolves marble buildings/statues and kills trees.
Soluble except Ag - Pb - Ca - Sr Ba)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
H2O + CO2 (it decomposes readily)

49. What is the test for hydrogen?
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
ClO?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
lighted splint (positive result=pop)

50. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Most INsoluble except group 1 and ammonium
No - NH3 and HCl gases are extremely soluble
Transition element compounds (except if it has a full or empty d shell)