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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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. Give an example of a concentrated weak acid.
Glacial acetic acid
small size and high charge
Initiation energy (NOT Ea)
methyl formate

2. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
P2O5
Initiation energy (NOT Ea)
CO (poisonous)
zero

3. What value of R do you use for thermo calculations? gas calculations?
No - it depends on the number of ions produced on dissolving.
Unsaturated - addition (ex: decolorize bromine solution)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
?H formation of an element in standard state=0

4. How do you find the pH for a dibasic acid? (H2A)?
ClO4?
Sigma bonds are stronger than pi bonds
Perform ICE BOX calculation based on K1
allow for the vapor pressure of water and make sure to level levels

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

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6. What apparatus do you use to separate 2 immiscible liquids?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Separating funnel
Hg²?
hydroxides (ex: Ba(OH)2)

7. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
non-metal oxides and hydrides are covalently bonded and are acidic.
Soluble
Q=It (time in seconds)

8. What should you check for before you begin titrating?
Kc=Kp
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Check for air bubbles in the buret and remove the buret funnel from the buret
H2PO4?

9. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
no - they're written undissociated (HAaq)
Ksp = 108s5
non-metal oxides and hydrides are covalently bonded and are acidic.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

10. What are two substances that sublime at 1 atm when heated?
Salt and water
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Iodine and CO2 (dry ice)
Acids; HCOOCH3 is an ester

11. What is the formula for percent error?
basic
The dilution effect when the solutions mix. M1V1 = M2V2
|experimental - accepted|/accepted X 100
acids

12. Both Acetic acid and ____________ are also functional isomers.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
methyl formate
allow for the vapor pressure of water and make sure to level levels
Combine the equations for the half reactions in the non-spontaneous direction

13. The oxidation # for acid base reactions...
No - NH3 and HCl gases are extremely soluble
do not change
0 and 14
bright yellow

14. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
C4H10
MnO4?
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)

15. chlorite
ClO2?
brown volatile liquid
zero
bright yellow

16. What is the difference between equivalence point and end point of a titration.
Soluble
different forms of the same element
bright yellow
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

17. What is the general formula for an ester?
How close results are to the accepted value
Only temperature
RCOOR
Pale yellow

18. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
left - ppt will form
diamond and graphite
No - it depends on the number of ions produced on dissolving.

19. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
NO3?
Read the bottom of the meniscus
Nothing

20. hydroxides
Nothing
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Current - time and charge on ion (moles of e used in half cell reaction)
Insoluble (except group 1 ammonium and Ba)

21. Where are group I metals stored?
brown volatile liquid
NO3?
Group I metals (soft metals) are stored under oil
The one with most oxygen atoms (highest oxidation number)

22. How do you identify which is oxidized or otherwise?
no - they're written undissociated (HAaq)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
acid + alcohol
Current - time and charge on ion (moles of e used in half cell reaction)

23. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
zero-th: decreases - first: constant - second: increases
|experimental - accepted|/accepted X 100

24. Colorless doesn't mean ______
Clear
They stay the same.
a-IMFs - b-molecular volume
C4H10

25. acetates
Soluble
Conjugate pair (one must be a weak base or acid)
it's lower and occurs over less sharp a range
Exothermic (?H for ANY sa/sb = -57kJ/mol)

26. What are allotropes?
Cr2O7²?
different forms of the same element
hydroxides (ex: Ba(OH)2)
catalyst=conc H2SO4

27. What does a short - sharp melting point indicate?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Identity and purity (impure compounds usually have broad & low melting points)
Transition element compounds (except if it has a full or empty d shell)
The compound with the lowest Ksp value.

28. What is the energy you must put into a reaction to make it start called?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
boiling without losing volatile solvents/reactants
Initiation energy (NOT Ea)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

29. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
10?8
Experimental mass/theoretical mass X 100

30. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Disulfur dichloride
redox reaction
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
The benzene ring (or more correctly the phenyl group - C6H5)

31. bromothymol
The dilution effect when the solutions mix. M1V1 = M2V2
+4-covalent - +2-ionic
K2
blue (BTB)

32. At what point during titration do you have the perfect buffer - and what is the pH at this point?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
At half equivalence - pH=pKa
ROR
No - NH3 and HCl gases are extremely soluble

33. What is the formula for alkanes?
benzene is less reactive than alkenes
CnH2n+2
#ligands=charge x2
E=q + w (negative is by system - positive is on system)

34. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Salt + water
S crystal at 0K=0

35. What do you do to get rid of most of the solution from a precipitate?
chemically (ex: with carbon)
Decant
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)
10?8

36. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
proton donor base
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
methyl formate
RCHO (carbonyl at end)

37. What are two substances that sublime at 1 atm when heated?
it's lower and occurs over less sharp a range
?H-kJ - ?S-J - ?G-kJ
Iodine and CO2 (dry ice)
same KE - but PEice<PEwater

38. chlorine
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Greenish-yellow gas
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

39. carbonate
Heat a test tube at an angle at the side of the tube (not bottom)
Anode
CO3²?
H+

40. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Ksp = s²
CO3²?
different forms of the same element
do not change

41. What is the sign of the anode in voltaic cells? in electrolytic cells?
?H formation of an element in standard state=0
Insoluble except nitrate and acetate
Ppt will NOT form (unsaturated)
voltaic: - electrolytic: +

42. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
ionic and form hydrogen and hydroxide
proton donor base
Mn²? - Cr³? - Cr³
allow for the vapor pressure of water and make sure to level levels

43. What is the first law of thermodynamics?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
blue
Most INsoluble except group 1 and ammonium
E=q + w (negative is by system - positive is on system)

44. What device would you use to measure a volume of gas?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Separating funnel
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Eudiometer

45. Why are noble gases stable?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Evaporation
#ligands=charge x2

46. Is a graduated cylinder or beaker more accurate?
Insoluble (except group 1 ammonium and Ba)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Graduated cylinder
Time?¹ - (ex. s?¹ - hr?¹ - etc)

47. What are the signs of ?G and E° for spontaneous reactions?
atoms
Ions go through the salt bridge - electrons go through metal wires in the external circuit
?G=negative - E° must be positive
Most are soluble except Ag - Pb

48. Do anions flow to the cathode or anode?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
ROR
Anode
Salt and water

49. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Pale purple - (orange)-yellow - red - blue - green.
voltaic: + electrolytic: -
The dilution effect when the solutions mix. M1V1 = M2V2
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.

50. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
different forms of the same element
RCOR
Kc=Kp
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble