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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. Name six characteristics of transition elements (or their compounds)
?G=negative - E° must be positive
acids
Ksp = 108s5
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)

2. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
Acidified
Initiation energy (NOT Ea)
RNH2

3. silver compounds
Insoluble except for nitrate and acetate
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
q=mc?T q=mL (or n x ?h)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

4. What is the formula for alkynes?
Iodine and CO2 (dry ice)
CnH2n-2
Nothing
R=8.31 J/mol/K

5. Alkenes are ________ and react by __________
Cr2O7²?
H2PO4?
acids
Unsaturated - addition (ex: decolorize bromine solution)

6. What are allotropes?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Ksp = 4s³
it reacts by substitution NOT addition
different forms of the same element

7. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Salt + water
Saturated - Substitution (which requires more radical conditions)

8. Ca - Sr - Ba
NO3?
Ksp = 4s³
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
hydroxides (ex: Ba(OH)2)

9. BaSO4
it reacts by substitution NOT addition
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Insoluble
allow for the vapor pressure of water and make sure to level levels

10. What are hybrid orbitals used for?
Salts (ex: CaO + SO2 ? CaSO3)
Clear
Making sigma bonds and holding lone pairs
zero

11. How can metals like iron and zinc be reduced?
P2O5
it is lower and occurs over less sharp a range
chemically (ex: with carbon)
HClO4

12. Acid plus base make?
same KE - but PEice<PEwater
CH3COO?
Anode - oxygen. Cathode - hydrogen
Salt + water.

13. How does group 1 metals' density compare to water's?
The benzene ring (or more correctly the phenyl group - C6H5)
same KE - but PEice<PEwater
Molecules with the same molecular formulas - but different structural formulas
are less dense than water

14. What are isomers?
CnH2n+2
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Molecules with the same molecular formulas - but different structural formulas
0.10M HCl (more ions)

15. What process do you use to obtain the solute from a solution?
metal oxides and hydrides are ionically bonded and basic
Evaporation
They stay the same.
Monomer + monomer = polymer product + a simple molecule such as water or HCl

16. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
?H-kJ - ?S-J - ?G-kJ
C4H10
Soluble

17. potassium permanganate
Purple
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

18. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
NO3?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
A) any range. b) 8-10 c) 4-6

19. What do group I/II metal oxides and acids form?
different forms of the same element
Salt and water
Heat a test tube at an angle at the side of the tube (not bottom)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

20. 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.
C2O4²?
10?8
a-IMFs - b-molecular volume

21. Give an example of a dilute strong acid.
Separating funnel
Making sigma bonds and holding lone pairs
CrO4²?
HClO4

22. A geometric (or cis-trans) isomer exists due to.....
Unsaturated - addition (ex: decolorize bromine solution)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
ClO?

23. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
T increases exponentially the proportion of molecules with E > Ea
zero
Ksp = s²

24. Does Benzene react by addition or substitution?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Ksp = s²
Transition element compounds (except if it has a full or empty d shell)
it reacts by substitution NOT addition

25. How are strong ones written?
H2O + CO2 (it decomposes readily)
strong acids/bases are written as H+ or OH- ions
NH2?
Ionic compounds

26. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
0.10M HCl (more ions)
Pale yellow
same KE - but PEice<PEwater
Cr2O7²?

27. What is the sign of the cathode in voltaic cells? in electrolytic cells?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
voltaic: + electrolytic: -

28. What process do you use to obtain a solvent from a solution?
Acidified
Distillation
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Identity and purity (impure compounds usually have broad & low melting points)

29. When driving off water from a hydrate - how do you tell you're done?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
NH4?
Most are soluble except Ag - Pb
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.

30. How does half life change for zero-th order - first order - and second order processes?
by electrolysis
zero-th: decreases - first: constant - second: increases
Anode
Evaporation

31. What do you need to make a polymer?
?G=negative - E° must be positive
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)
no - they're written undissociated (HAaq)
Add acid to water so that the acid doesn't boil and spit

32. What are the prefixes for the naming of binary molecular compound formulas (up to six)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Mono; di; tri; tetra; penta; hexa.
RCOOR
Selective absorption

33. silver iodide
Pale yellow
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Glowing splint (positive result=relights)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

34. What is the test for oxygen?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Glowing splint (positive result=relights)

35. 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
proton acceptor.
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?)
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.

36. What shape is carbon dioxide?
ROR
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
CN?
linear

37. cyanide
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
CN?
acids
Tetrahedral

38. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
NH4?
Sulfur

39. What do hydrocarbons form when they burn in air (oxygen)?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Filtration
CO2 and H2O
Exothermic

40. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
NO3?
metal oxides and hydrides are ionically bonded and basic
R=8.31 J/mol/K
Kc=Kp

41. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
Initiation energy (NOT Ea)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
small size and high charge

42. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
zero
fruit - fish - bases
ClO2?
K1 x K2

43. When a cell is 'flat' What is its voltage?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Unsaturated - addition (ex: decolorize bromine solution)
do not change
zero

44. What changes Keq?
Selective absorption
Only temperature
a-IMFs - b-molecular volume
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

45. ammonium
NH4?
Soluble
q=mc?T q=mL (or n x ?h)
Increases.

46. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
strong acids/bases are written as H+ or OH- ions
The one with most oxygen atoms (highest oxidation number)
blue

47. An amphiprotic (amphoteric) species is...
Monomer + monomer = polymer product + a simple molecule such as water or HCl
The compound with the lowest Ksp value.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

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

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49. Why are i factors (Van't Hoff factors) often less than ideal?
Current - time and charge on ion (moles of e used in half cell reaction)
ion pairing
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Distillation

50. Acids + Carbonates (bicarbonates) make?
RX
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Suniverse increases for spontaneous processes
CnH2n+2