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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.
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1. dichromate (soln + most solids)
Orange
Salt and water
linear
CnH(2n+2)

2. perchlorate
?G= -ve - E°= +ve
Clear
ClO4?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

3. oxalate
How grouped results are
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
C2O4²?

4. How do you find the pH for a dibasic acid? (H2A)?
Insoluble except for nitrate and acetate
left - ppt will form
Perform ICE BOX calculation based on K1
blue glass - it filters UV

5. How does half life change for zero-th order - first order - and second order processes?
allow for the vapor pressure of water and make sure to level levels
The benzene ring (or more correctly the phenyl group - C6H5)
zero-th: decreases - first: constant - second: increases
Sigma bonds are stronger than pi bonds

6. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
CO3²?
Pale purple - (orange)-yellow - red - blue - green.
proton acceptor.
They stay the same.

7. What is accuracy?
How close results are to the accepted value
voltaic: - electrolytic: +
Ionic compounds
Silvery gray solid - brown - purple

8. acetate
ClO2?
NH4?
CH3COO?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

9. Aromatic compounds contain what?
The benzene ring (or more correctly the phenyl group - C6H5)
bases
Suniverse increases for spontaneous processes
Initiation energy (NOT Ea)

10. acetates
No - NH3 and HCl gases are extremely soluble
Soluble
voltaic: - electrolytic: +
Disulfur dichloride

11. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
voltaic: - electrolytic: +
Check for air bubbles in the buret and remove the buret funnel from the buret
water and substances with (s) less dense than
T increases exponentially the proportion of molecules with E > Ea

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

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13. Color (absorbance) is proportional to ________
Concentration
The benzene ring (or more correctly the phenyl group - C6H5)
Insoluble
q=mc?T q=mL (or n x ?h)

14. What do hydrocarbons form when they burn in air (oxygen)?
Salt + water
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
E=q + w (negative is by system - positive is on system)
CO2 and H2O

15. How many normal boiling points and boiling points are there?

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16. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Initiation energy (NOT Ea)
allow for the vapor pressure of water and make sure to level levels

17. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
PO4³?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
redox reaction

18. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
strong acids/bases are written as H+ or OH- ions
More chaotic (ex: gases made)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

19. What process do you use to obtain the solute from a solution?
Saturated - Substitution (which requires more radical conditions)
Big K=kf/kr
benzene has a delocalized pi ring structure
Evaporation

20. How are metal oxides and hydrides bonded? are they acidic or basic?
[A?]/[HA] x 100 or [BH?]/[B] x 100
ClO3?
metal oxides and hydrides are ionically bonded and basic
Insoluble

21. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
bright yellow
ion pairing
CnH2n+1 often designated 'R' ex C3H7 is propyl

22. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
proton acceptor.
Read the bottom of the meniscus
Suniverse increases for spontaneous processes

23. phosphate
Acidified
Monomer + monomer = polymer product + a simple molecule such as water or HCl
CnH2n+1 often designated 'R' ex C3H7 is propyl
PO4³?

24. How are strong ones written?
RNH2
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
strong acids/bases are written as H+ or OH- ions
CnH2n+2

25. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
Only temperature
Soluble
10?8
?H-kJ - ?S-J - ?G-kJ

26. What are two allotropes of carbon?
diamond and graphite
Tetrahedral
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Nothing

27. Ca - Sr - Ba
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
hydroxides (ex: Ba(OH)2)
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.
The dilution effect when the solutions mix. M1V1 = M2V2

28. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
The dilution effect when the solutions mix. M1V1 = M2V2
Concentration

29. Generally - which oxy acid is strongest?
The benzene ring (or more correctly the phenyl group - C6H5)
The one with most oxygen atoms (highest oxidation number)
Soluble except Ag - Pb - Ca - Sr Ba)
The dilution effect when the solutions mix. M1V1 = M2V2

30. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Perform ICE BOX calculation based on K1
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Group 1 hydroxides (ex: NaOH)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

31. What is a coordinate covalent bond?
left - ppt will form
Both electrons come from the same atom (just as good as a regular bond)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

32. Does Kw increase or decrease with T? Why?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Silvery gray solid - brown - purple
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
0 and 14

33. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
methyl formate
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)
RCOR
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

34. What is reflux?
Filtration
Only temperature
Increases.
boiling without losing volatile solvents/reactants

35. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Ppt will NOT form (unsaturated)
Graduated cylinder
bases

36. halides
same KE - but PEice<PEwater
H+
Most are soluble except Ag - Pb
zero

37. hydroxides
T increases exponentially the proportion of molecules with E > Ea
H+
Insoluble (except group 1 ammonium and Ba)
Soluble

38. What two compounds are great oxidizing agents?

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39. How do you explain trends in atomic properties using Coulomb's Law?
A salt solution.
They stay the same.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
CnH2n+1 often designated 'R' ex C3H7 is propyl

40. What are the signs of ?G and E° for spontaneous reactions?
ionic and form hydrogen and hydroxide
More chaotic (ex: gases made)
Ksp = 4s³
?G=negative - E° must be positive

41. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
The benzene ring (or more correctly the phenyl group - C6H5)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Most are soluble except Ag - Pb

42. What is the pH of 1.0M HCl? 1M NaOH?
Group 1 hydroxides (ex: NaOH)
Identity and purity (impure compounds usually have broad & low melting points)
0 and 14
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

43. Is the ?H formation of an element in standard state zero?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Heptane
CO3²?
?H formation of an element in standard state=0

44. What steps do organic labs consist of?
Soluble except Ag - Pb - Ca - Sr Ba)
No - it depends on the number of ions produced on dissolving.
Synthesis - separation and purification of the product and its identification.
Soluble

45. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
do not change
Unsaturated - addition (ex: decolorize bromine solution)
More chaotic (ex: gases made)

46. What two types of substances are present in all redox reactions?
Synthetic condensation polymer (aka a polyamide)
ClO?
an oxidized and reduced substance
Read the bottom of the meniscus

47. If Q < Ksp a ppt ______
do not change
Ppt will NOT form (unsaturated)
How close results are to the accepted value
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

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

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49. phosphates
CN?
Acidified
Most INsoluble except group 1 and ammonium
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

50. What is the conjugate base of NH3?
CnH2n+2
basic
NH2?
ionic and form hydrogen and hydroxide

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AP Chemistry 2

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