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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.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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 range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
A) any range. b) 8-10 c) 4-6
same KE - but PEice<PEwater
C4H10
Synthesis - separation and purification of the product and its identification.

2. What reacts with an acid to create hydrogen gas?
boiling without losing volatile solvents/reactants
An active metal.
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
same KE - but PEice<PEwater

3. Aromatic compounds contain what?
The benzene ring (or more correctly the phenyl group - C6H5)
SO4²?
RCOR
#ligands=charge x2

4. nitrates
q=mc?T q=mL (or n x ?h)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Soluble
They stay the same.

5. Where are group I metals stored?
Group I metals (soft metals) are stored under oil
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.
zero
Current - time and charge on ion (moles of e used in half cell reaction)

6. If Q < Ksp a ppt ______
It ceases - the circuit is broken.
Ppt will NOT form (unsaturated)
Acid rain - dissolves marble buildings/statues and kills trees.
K1 x K2

7. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
it's lower and occurs over less sharp a range
MnO4?
Synthetic condensation polymer (aka a polyamide)

8. What type of compounds do metals/non metals form?
Identity and purity (impure compounds usually have broad & low melting points)
Ionic compounds
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
No - it depends on the number of ions produced on dissolving.

9. When the salt bridge is removed what happens to the cell reaction?
Acidified
HClO4
It ceases - the circuit is broken.
Selective absorption

10. barium sulfate
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
C2O4²?
White precipitate
P2O5

11. What apparatus do you use to pour liquids?
Pour liquids using a funnel or down a glass rod
At half equivalence - pH=pKa
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
#ligands=charge x2

12. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
Iodine and CO2 (dry ice)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Synthesis - separation and purification of the product and its identification.

13. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
red - green - blue
Big K=kf/kr

14. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
They stay the same.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
bases

15. iodine - iodine solution - iodine vapor
zero
No - it depends on the number of ions produced on dissolving.
metal oxides and hydrides are ionically bonded and basic
Silvery gray solid - brown - purple

16. What do group I/II metal oxides plus water form?
ClO2?
CnH2n+1 often designated 'R' ex C3H7 is propyl
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
bases

17. silver compounds
Clear
Insoluble except for nitrate and acetate
bright yellow
Ksp = 4s³

18. What is the formula of butane?
OH?
bent
benzene is less reactive than alkenes
C4H10

19. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Eudiometer
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
Soluble

20. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
proton acceptor.
catalyst=conc H2SO4
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

21. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Salt and water
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
q=mc?T q=mL (or n x ?h)
Current - time and charge on ion (moles of e used in half cell reaction)

22. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Selective absorption
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
same KE - but PEice<PEwater
No - NH3 and HCl gases are extremely soluble

23. When a cell is 'flat' What is its voltage?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
zero
E=q + w (negative is by system - positive is on system)
The compound with the lowest Ksp value.

24. 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
Big K=kf/kr
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
RCOOR

25. What shape is methane?
methyl formate
Tetrahedral
Concentration
Ions go through the salt bridge - electrons go through metal wires in the external circuit

26. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
Hg²?
Insoluble except group 1 and ammonium
boiling without losing volatile solvents/reactants

27. What things should you remember to do when collecting gas over water?
ROH
Greenish-yellow gas
it reacts by substitution NOT addition
allow for the vapor pressure of water and make sure to level levels

28. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
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)
Graduated cylinder
No - it depends on the number of ions produced on dissolving.
|experimental - accepted|/accepted X 100

29. What is the general formula for an ester?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
RCOOR
Purple
H+

30. Does Kw increase or decrease with T? Why?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
|experimental - accepted|/accepted X 100
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
are less dense than water

31. mercury (I) ion
Hg2²?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
CnH(2n+2)
Insoluble except for nitrate and acetate

32. What is the formula for alkynes?
Pale purple - (orange)-yellow - red - blue - green.
CnH2n-2
Group 1 hydroxides (ex: NaOH)
S crystal at 0K=0

33. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Purple
non-metal oxides and hydrides are covalently bonded and are acidic.

34. What shape is water?
CO2 and H2O
Acids; HCOOCH3 is an ester
It ceases - the circuit is broken.
bent

35. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
it is lower and occurs over less sharp a range
?H-kJ - ?S-J - ?G-kJ
Products - reactants (except for BDE when it's reactants - products)

36. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
no - they're written undissociated (HAaq)
Both electrons come from the same atom (just as good as a regular bond)
HClO4

37. What kind of bonding structure does benzene have?
C4H10
Soluble except Ag - Pb - Ca - Sr Ba)
benzene has a delocalized pi ring structure
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

38. Give an example of a dilute strong acid.
NO3?
[A?]/[HA] x 100 or [BH?]/[B] x 100
HClO4
fractional distillation

39. Does Benzene react by addition or substitution?
catalyst=conc H2SO4
A salt solution.
A) any range. b) 8-10 c) 4-6
it reacts by substitution NOT addition

40. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
RCOOR
#ligands=charge x2
RCOOH

41. How are primary alcohols turned into acids?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
R=8.31 J/mol/K
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

42. What is the test for hydrogen?
lighted splint (positive result=pop)
H2O + CO2 (it decomposes readily)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
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.

43. What do metal oxides plus acids form?
H2PO4?
yellow
Salt + water
benzene is less reactive than alkenes

44. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Only temperature
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
But S° of element is not zero (except at 0K)
voltaic: - electrolytic: +

45. Name some properties of Group 17
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Increases down group 1 decreases down group 17
RCOOR
How grouped results are

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

47. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
0 and 14
acid + alcohol
Add acid to water so that the acid doesn't boil and spit

48. What do acids plus active metals form?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Nothing
Heat a test tube at an angle at the side of the tube (not bottom)

49. What process do you use to obtain a solvent from a solution?
Graduated cylinder
Distillation
CH3COO?
RX

50. What should you check for before you begin titrating?
#ligands=charge x2
CO (poisonous)
Check for air bubbles in the buret and remove the buret funnel from the buret
Iodine and CO2 (dry ice)