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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. Give an example of a dilute strong acid.
HClO4
SO4²?
Insoluble except group 1 and ammonium
?H-kJ - ?S-J - ?G-kJ

2. What are allotropes?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
different forms of the same element
Exothermic
Insoluble (except group 1 ammonium and Ba)

3. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
do not change
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Filtration
zero

4. What type of compounds do metals/non metals form?
The benzene ring (or more correctly the phenyl group - C6H5)
Ionic compounds
Group 1 hydroxides (ex: NaOH)
Exothermic

5. phosphates
q=mc?T q=mL (or n x ?h)
Most INsoluble except group 1 and ammonium
Reduction always takes place at the cathode (RED CAT) In both types of cell!
ClO4?

6. dihydrogen phosphate
All except for lithium
blue (BTB)
Pale purple - (orange)-yellow - red - blue - green.
H2PO4?

7. How are metal oxides and hydrides bonded? are they acidic or basic?
metal oxides and hydrides are ionically bonded and basic
?G= -ve - E°= +ve
Big K=kf/kr
S2O3²?

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

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9. If a weak acid is diluted more - what happens to its % dissociation value?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
0.10M HCl (more ions)
Increases.
A) any range. b) 8-10 c) 4-6

10. Do you use J or kJ for ?H - ?S - and ?G?
H2O + CO2 (it decomposes readily)
HClO4
ion pairing
?H-kJ - ?S-J - ?G-kJ

11. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
How close results are to the accepted value

12. What complex ion does ammonia form with silver? copper? cadmium? zinc?
bent
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)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
ClO3?

13. mercury (I) ion
Hg2²?
ion pairing
Soluble
diamond and graphite

14. Ions are not ______.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
atoms

15. What word is a clue for a redox reaction?
Acidified
Soluble
The benzene ring (or more correctly the phenyl group - C6H5)
Insoluble except nitrate and acetate

16. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
CnH2n+1 often designated 'R' ex C3H7 is propyl
Anode - oxygen. Cathode - hydrogen
Silvery gray solid - brown - purple

17. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
H2PO4?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Transition element compounds (except if it has a full or empty d shell)

18. When combining half equations - what do you do to E° values when multiplying coefficients?
Nothing
NH4?
bent
Most INsoluble except group 1 and ammonium

19. Ca - Sr - Ba
CnH2n+2
ClO?
hydroxides (ex: Ba(OH)2)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

20. silver compounds
Insoluble except for nitrate and acetate
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
by electrolysis

21. Buffer capacity must contain decent amounts of a ________ ________
Identity and purity (impure compounds usually have broad & low melting points)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Conjugate pair (one must be a weak base or acid)

22. What things should you remember to do when collecting gas over water?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
allow for the vapor pressure of water and make sure to level levels
T increases exponentially the proportion of molecules with E > Ea
?G= -ve - E°= +ve

23. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Making sigma bonds and holding lone pairs
Cu3(PO4)2
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
benzene is less reactive than alkenes

24. hypochlorite
Heat a test tube at an angle at the side of the tube (not bottom)
do not change
CnH2n-2
ClO?

25. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Read the bottom of the meniscus
Salt and water
Reduction always takes place at the cathode (RED CAT) In both types of cell!
zero

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

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27. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
a-IMFs - b-molecular volume
metal oxides and hydrides are ionically bonded and basic
bright yellow
Pale purple - (orange)-yellow - red - blue - green.

28. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
NH4?
C2O4²?
Mn²? - Cr³? - Cr³

29. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
it reacts by substitution NOT addition
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

30. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
acids
acid + alcohol
look for changes in oxidation # - the one that goes up is oxidized and is the RA

31. What are two substances that sublime at 1 atm when heated?
The dilution effect when the solutions mix. M1V1 = M2V2
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Iodine and CO2 (dry ice)

32. What does a short - sharp melting point indicate?
#ligands=charge x2
Identity and purity (impure compounds usually have broad & low melting points)
[A?]/[HA] x 100 or [BH?]/[B] x 100
water and substances with (s) less dense than

33. What are hybrid orbitals used for?
it's lower and occurs over less sharp a range
zero
Making sigma bonds and holding lone pairs
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

34. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
Insoluble
allow for the vapor pressure of water and make sure to level levels
RCHO (carbonyl at end)

35. What is the second law of thermodynamics?
Saturated - Substitution (which requires more radical conditions)
Suniverse increases for spontaneous processes
Cr2O7²?
0.10M HCl (more ions)

36. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
CO (poisonous)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Silvery gray solid - brown - purple

37. mercury (II) ion
Hg2²?
Suniverse increases for spontaneous processes
Making sigma bonds and holding lone pairs
Hg²?

38. If Q < Ksp a ppt ______
zero
Purple
Ppt will NOT form (unsaturated)
-Ea/R

39. bromine
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
brown volatile liquid
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
CO2 and H2O

40. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
small size and high charge
CO (poisonous)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

41. What is the test for oxygen?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Glowing splint (positive result=relights)
H2O + CO2 (it decomposes readily)
ROH

42. What is the formula for percent error?
10?8
|experimental - accepted|/accepted X 100
zero-th: decreases - first: constant - second: increases
?G=negative - E° must be positive

43. thiosulfate
bent
ion pairing
?H formation of an element in standard state=0
S2O3²?

44. What is the difference between equivalence point and end point of a titration.
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
linear
Q=It (time in seconds)
The one with most oxygen atoms (highest oxidation number)

45. permanganate
MnO4?
voltaic: + electrolytic: -
Cu3(PO4)2
OH?

46. What is the general formula for an ester?
RCOOR
it reacts by substitution NOT addition
|experimental - accepted|/accepted X 100
Heptane

47. sulfate
MnO4?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Products - reactants (except for BDE when it's reactants - products)
SO4²?

48. dichromate
bent
Cr2O7²?
by electrolysis
A) any range. b) 8-10 c) 4-6

49. When is ?G zero?
Current - time and charge on ion (moles of e used in half cell reaction)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Purple
atoms

50. dichromate (soln + most solids)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
blue (BTB)
do not change
Orange

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AP Chemistry 2

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