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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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This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.

1. What type of compounds do Group 14 form?
Pale yellow
+4-covalent - +2-ionic
Monomer + monomer = polymer product + a simple molecule such as water or HCl
RNH2

2. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
lighted splint (positive result=pop)
non-metal oxides and hydrides are covalently bonded and are acidic.
zero
They stay the same.

3. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
neutralization: high K - H2O product dissociation: low K - H2O reactant
?G=negative - E° must be positive

4. What are the products of the reaction between group 1 metals and water?

5. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
E=q + w (negative is by system - positive is on system)
CnH2n+2
SO4²?

6. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
They stay the same.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
0.10M HCl (more ions)
Mn²? - Cr³? - Cr³

7. barium sulfate
Pipette (burette if need repetition)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Ksp = s²
White precipitate

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

9. How does group 1 metals' density compare to water's?
It ceases - the circuit is broken.
Group I metals (soft metals) are stored under oil
are less dense than water
Add acid to water so that the acid doesn't boil and spit

10. ammonium/ammonium compounds
benzene has a delocalized pi ring structure
Soluble
zero
fractional distillation

11. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
strong acids/bases are written as H+ or OH- ions
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
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)

12. What does the solubility of organic compounds depend on?
RCHO (carbonyl at end)
metal oxides and hydrides are ionically bonded and basic
redox reaction
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

13. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
The dilution effect when the solutions mix. M1V1 = M2V2
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Ksp = 4s³
H+

14. What do the 'a' and 'b' in Van Der Waal's equation allow for?
an oxidized and reduced substance
brown volatile liquid
a-IMFs - b-molecular volume
[A?]/[HA] x 100 or [BH?]/[B] x 100

15. What measuring device would you use for very small volumes of liquids?
MnO4?
SO4²?
Heptane
Pipette (burette if need repetition)

16. When is ?G zero?
The dilution effect when the solutions mix. M1V1 = M2V2
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
it is lower and occurs over less sharp a range
blue glass - it filters UV

17. mercury (I) ion
Hg2²?
S crystal at 0K=0
Ksp = 4s³
Pour liquids using a funnel or down a glass rod

18. How do you find the pH for a dibasic acid? (H2A)?
K1 x K2
allow for the vapor pressure of water and make sure to level levels
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Perform ICE BOX calculation based on K1

19. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
Suniverse increases for spontaneous processes
Exothermic (?H for ANY sa/sb = -57kJ/mol)
The compound with the lowest Ksp value.
ion pairing

20. What is an Alkyl group?

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

22. What is a dipeptide? polypeptide? protein?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
?G= -ve - E°= +ve
blue (BTB)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

23. chlorate
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
ClO3?
MnO4?
They stay the same.

24. What value of R do you use for thermo calculations? gas calculations?
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.
Ksp = s²
O2 needs 4F/mol H2 needs 2F/mol
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

25. What is the formula for alkenes?
CnH2n
Cu3(PO4)2
10?8
proton donor base

26. lead iodide
zero
MnO4?
bright yellow
The one with most oxygen atoms (highest oxidation number)

27. What steps do organic labs consist of?
CN?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
T increases exponentially the proportion of molecules with E > Ea
Synthesis - separation and purification of the product and its identification.

28. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
a-IMFs - b-molecular volume
Acidified
basic
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

29. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
ClO2?
Iodine and CO2 (dry ice)
Saturated - Substitution (which requires more radical conditions)

30. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
CnH2n
Most INsoluble except group 1 and ammonium
Concentration

31. acetate
boiling without losing volatile solvents/reactants
Insoluble except group 1 and ammonium
CH3COO?
K2

32. Esterification is...
allow for the vapor pressure of water and make sure to level levels
S crystal at 0K=0
acid + alcohol
-Ea/R

33. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
zero
Group I metals (soft metals) are stored under oil
CO3²?
same KE - but PEice<PEwater

34. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
do not change
Products - reactants (except for BDE when it's reactants - products)
K1 x K2

35. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
no - they're written undissociated (HAaq)
Heptane
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

36. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Pale purple - (orange)-yellow - red - blue - green.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
zero
Filtration

37. How does the melting point of a mixture compare to the MP of a pure substance?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
acid + alcohol
proton donor base
it is lower and occurs over less sharp a range

38. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
catalyst=conc H2SO4
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Pipette (burette if need repetition)

39. What do group I/II metal oxides and acids form?
Insoluble (except group 1 ammonium and Ba)
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
CN?
Salt and water

40. What is the basic structure of an optical isomer?
RNH2
The one with most oxygen atoms (highest oxidation number)
hydroxides (ex: Ba(OH)2)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

41. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Most are soluble except Ag - Pb
RX
CnH2n+1 often designated 'R' ex C3H7 is propyl
neutralization: high K - H2O product dissociation: low K - H2O reactant

42. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Suniverse increases for spontaneous processes
No - it depends on the number of ions produced on dissolving.
voltaic: + electrolytic: -
RCOOH

43. Which alkali metals float on water?
Only temperature
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
All except for lithium
ClO4?

44. dihydrogen phosphate
H2PO4?
Only temperature
CrO4²?
Soluble except Ag - Pb - Ca - Sr Ba)

45. What are the signs for ?G and E° for spontaneous reactions?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
same KE - but PEice<PEwater
?G= -ve - E°= +ve
The one with most oxygen atoms (highest oxidation number)

46. What is the general formula for an amine?
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.
RNH2
neutralization: high K - H2O product dissociation: low K - H2O reactant
Big K=kf/kr

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

48. What equipment do you need for a titration?
#ligands=charge x2
+4-covalent - +2-ionic
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Cu3(PO4)2

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

50. When a cell is 'flat' What is its voltage?
zero
CnH2n-2
#ligands=charge x2
Pour liquids using a funnel or down a glass rod