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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. chlorine
Greenish-yellow gas
Anode - oxygen. Cathode - hydrogen
boiling without losing volatile solvents/reactants
ROR

2. What things should you remember to do when collecting gas over water?
Cu3(PO4)2
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
allow for the vapor pressure of water and make sure to level levels
T increases exponentially the proportion of molecules with E > Ea

3. How do you clean a buret/pipette for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
CnH(2n+2)
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)

4. silver iodide
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
At half equivalence - pH=pKa
Pale yellow
Monomer + monomer = polymer product + a simple molecule such as water or HCl

5. Esterification is...
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
The one with most oxygen atoms (highest oxidation number)
acid + alcohol
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)

6. What two types of substances are present in all redox reactions?
allow for the vapor pressure of water and make sure to level levels
Reduction always takes place at the cathode (RED CAT) In both types of cell!
zero
an oxidized and reduced substance

7. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
C4H10
Current - time and charge on ion (moles of e used in half cell reaction)
Mn²? - Cr³? - Cr³

8. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
Purple
Increases.
linear

9. mercury (II) ion
Hg²?
metal oxides and hydrides are ionically bonded and basic
Pipette (burette if need repetition)
bent

10. What two compounds are great oxidizing agents?

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11. What is the conjugate acid of H2PO4?
catalyst=conc H2SO4
H3PO4
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
voltaic: - electrolytic: +

12. What is the formula of butane?
Tetrahedral
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
strong acids/bases are written as H+ or OH- ions
C4H10

13. What is H2CO3 (carbonate acid) usually written as?
fractional distillation
Cu3(PO4)2
Monomer + monomer = polymer product + a simple molecule such as water or HCl
H2O + CO2 (it decomposes readily)

14. When combining half equations - what do you do to E° values when multiplying coefficients?
RCOOR
Nothing
boiling without losing volatile solvents/reactants
Graduated cylinder

15. chlorate
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
ClO3?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Salts (ex: CaO + SO2 ? CaSO3)

16. What is the formula for alkynes?
K2
Increases.
same KE - but PEice<PEwater
CnH2n-2

17. What steps do organic labs consist of?
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 group 1 and ammonium
Synthesis - separation and purification of the product and its identification.
White precipitate

18. phosphates
Synthetic condensation polymer (aka a polyamide)
Soluble
zero
Most INsoluble except group 1 and ammonium

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

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20. Acid plus base make?
Salt + water.
proton donor base
Synthesis - separation and purification of the product and its identification.
Greenish-yellow gas

21. nitrate
CO2 and H2O
#ligands=charge x2
NO3?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

22. perchlorate
ClO4?
Selective absorption
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Products - reactants (except for BDE when it's reactants - products)

23. What is the formula for percent error?
Trigonal pyramidal
|experimental - accepted|/accepted X 100
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.
do not change

24. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Mn²? - Cr³? - Cr³
benzene has a delocalized pi ring structure
Concentration

25. What is Big K in terms of kf and kr?
Ppt will NOT form (unsaturated)
RX
it reacts by substitution NOT addition
Big K=kf/kr

26. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
K1 x K2
H2O + CO2 (it decomposes readily)
a-IMFs - b-molecular volume

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

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28. What reacts with an acid to create hydrogen gas?
An active metal.
Mn²? - Cr³? - Cr³
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
CO (poisonous)

29. What are hybrid orbitals used for?
NH4?
Saturated - Substitution (which requires more radical conditions)
Making sigma bonds and holding lone pairs
Suniverse increases for spontaneous processes

30. Give an example of a dilute strong acid.
H2PO4?
HClO4
do not change
10?8

31. What is the general formula for an acid?
0.10M HCl (more ions)
Making sigma bonds and holding lone pairs
RCOOH
RNH2

32. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
They stay the same.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
redox reaction
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

33. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
Increases.
The benzene ring (or more correctly the phenyl group - C6H5)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

34. What process do you use to separate two liquids with different boiling points?
Sulfur
Anode - oxygen. Cathode - hydrogen
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
fractional distillation

35. What is the test for oxygen?
benzene has a delocalized pi ring structure
Group I metals (soft metals) are stored under oil
bent
Glowing splint (positive result=relights)

36. dichromate (soln + most solids)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Orange
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

37. What does a short - sharp melting point indicate?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
H2O + CO2 (it decomposes readily)
Identity and purity (impure compounds usually have broad & low melting points)

38. How are more active metals reduced?
by electrolysis
Soluble
Add acid to water so that the acid doesn't boil and spit
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

39. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
The compound with the lowest Ksp value.
Ksp = 4s³

40. What is the relationship in strength between sigma and pi bonds?
Clear
Graduated cylinder
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Sigma bonds are stronger than pi bonds

41. What is the general formula for a ketone?
RCOR
How close results are to the accepted value
Ksp = 27s4
H2O + CO2 (it decomposes readily)

42. Generally - which oxy acid is strongest?
NO3?
Ionic compounds
Tetrahedral
The one with most oxygen atoms (highest oxidation number)

43. What is the general formula for alkyl halides?
benzene is less reactive than alkenes
lighted splint (positive result=pop)
CO (poisonous)
RX

44. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
T increases exponentially the proportion of molecules with E > Ea
Group I metals (soft metals) are stored under oil
K1 x K2
Monomer + monomer = polymer product + a simple molecule such as water or HCl

45. What type of metals don't react with water or acids to form H2?

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46. What shape is carbon dioxide?
linear
Conjugate pair (one must be a weak base or acid)
Greenish-yellow gas
ion pairing

47. bromine
brown volatile liquid
Sulfur
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Mono; di; tri; tetra; penta; hexa.

48. halides
Most are soluble except Ag - Pb
Combine the equations for the half reactions in the non-spontaneous direction
Glowing splint (positive result=relights)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

49. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Pour liquids using a funnel or down a glass rod
ClO3?
a-IMFs - b-molecular volume
Ksp = s²

50. What is the third law of thermodynamics?
Kc=Kp
S crystal at 0K=0
Soluble
catalyst=conc H2SO4

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AP Chemistry 2

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