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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. acetate
CH3COO?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
acids
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

2. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
Acid rain - dissolves marble buildings/statues and kills trees.
redox reaction
benzene is less reactive than alkenes

3. What is the formula for percent error?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Initiation energy (NOT Ea)
|experimental - accepted|/accepted X 100
The dilution effect when the solutions mix. M1V1 = M2V2

4. What are isomers?
0 and 14
Molecules with the same molecular formulas - but different structural formulas
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
?H formation of an element in standard state=0

5. If Q < Ksp a ppt ______
Hg²?
Ppt will NOT form (unsaturated)
ethers
-Ea/R

6. Alcohols and _______ are FG isomers
OH?
The dilution effect when the solutions mix. M1V1 = M2V2
Ionic compounds
ethers

7. Metal hydrides are _____ and form _______ and _______ when added to water
Pale yellow
Concentration
ionic and form hydrogen and hydroxide
atoms

8. Name six characteristics of transition elements (or their compounds)
blue
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
?H formation of an element in standard state=0
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)

9. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
Current - time and charge on ion (moles of e used in half cell reaction)
allow for the vapor pressure of water and make sure to level levels
q=mc?T q=mL (or n x ?h)

10. carbonate
CO3²?
MnO4?
Group I metals (soft metals) are stored under oil
ionic and form hydrogen and hydroxide

11. What is the general formula for a ketone?
SO4²?
RCOR
C2O4²?
Heat a test tube at an angle at the side of the tube (not bottom)

12. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
R=8.31 J/mol/K
They stay the same.
Filtration
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

13. Buffer capacity must contain decent amounts of a ________ ________
CN?
Identity and purity (impure compounds usually have broad & low melting points)
Kc=Kp
Conjugate pair (one must be a weak base or acid)

14. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
RNH2
proton donor base

15. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
OH?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Group 1 hydroxides (ex: NaOH)
Greenish-yellow gas

16. What is the relationship in strength between sigma and pi bonds?
ClO4?
Pale yellow
Sigma bonds are stronger than pi bonds
Ksp = 27s4

17. bromothymol
RCOOH
blue (BTB)
Ksp = 27s4
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

18. What word is a clue for a redox reaction?
methyl formate
Acidified
Soluble
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

19. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Clear
it reacts by substitution NOT addition
Pale purple - (orange)-yellow - red - blue - green.
CnH2n

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

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21. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
CO2 and H2O
methyl formate
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

22. What is H2CO3 (carbonate acid) usually written as?
Ksp = 27s4
H2O + CO2 (it decomposes readily)
Purple
RCHO (carbonyl at end)

23. potassium permanganate
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?)
Purple
Insoluble (except group 1 ammonium and Ba)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

24. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
non-metal oxides and hydrides are covalently bonded and are acidic.
blue
Increases down group 1 decreases down group 17

25. Name some properties of Group 17
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
Insoluble (except group 1 ammonium and Ba)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

26. What is the conjugate acid of H2PO4?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Pale purple - (orange)-yellow - red - blue - green.
H3PO4
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

27. What are the signs for ?G and E° for spontaneous reactions?
Salt and water
?G= -ve - E°= +ve
RX
Silvery gray solid - brown - purple

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

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

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30. acetates
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Soluble
Purple
Saturated - Substitution (which requires more radical conditions)

31. What is the slope of the graph of lnk vs. 1/T?
bright yellow
allow for the vapor pressure of water and make sure to level levels
?H-kJ - ?S-J - ?G-kJ
-Ea/R

32. What does saturated mean? Unsaturated?
lighted splint (positive result=pop)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Add acid to water so that the acid doesn't boil and spit

33. What is the general formula for an ether?
ROR
NH4?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Perform ICE BOX calculation based on K1

34. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
Soluble except Ag - Pb - Ca - Sr Ba)
Salt + water.
Pipette (burette if need repetition)

35. Name C7H16
blue
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
proton acceptor.
Heptane

36. What things should you remember to do when collecting gas over water?
redox reaction
Hg²?
allow for the vapor pressure of water and make sure to level levels
bright yellow

37. What process do you use to separate two liquids with different boiling points?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Identity and purity (impure compounds usually have broad & low melting points)
fractional distillation
K1 x K2

38. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
CO (poisonous)
zero-th: decreases - first: constant - second: increases
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Reduction always takes place at the cathode (RED CAT) In both types of cell!

39. What is the formula of butane?
?G= -ve - E°= +ve
C4H10
White precipitate
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

40. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Insoluble (except group 1 ammonium and Ba)
-Ea/R
No - it depends on the number of ions produced on dissolving.

41. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
metal oxides and hydrides are ionically bonded and basic
atoms
do not change
Kc=Kp

42. carbonates
benzene has a delocalized pi ring structure
MnO4?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Insoluble except group 1 and ammonium

43. hydroxide
ionic and form hydrogen and hydroxide
E=q + w (negative is by system - positive is on system)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
OH?

44. What is an Alkyl group?

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45. mercury (II) ion
Hg²?
Pale yellow
CnH2n+1 often designated 'R' ex C3H7 is propyl
CrO4²?

46. What shape is carbon dioxide?
linear
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
voltaic: - electrolytic: +
Perform ICE BOX calculation based on K1

47. What do group I/II metal oxides and acids form?
Salt and water
No - it depends on the number of ions produced on dissolving.
Ppt will NOT form (unsaturated)
Ions go through the salt bridge - electrons go through metal wires in the external circuit

48. What measuring device would you use for very small volumes of liquids?
E=q + w (negative is by system - positive is on system)
Pipette (burette if need repetition)
T increases exponentially the proportion of molecules with E > Ea
blue (BTB)

49. dihydrogen phosphate
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?)
H2PO4?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
basic

50. chlorate
Suniverse increases for spontaneous processes
They decrease (or could be the same if the solid has ONLY JUST disappeared)
ClO3?
metal oxides and hydrides are ionically bonded and basic

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AP Chemistry 2

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