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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. The oxidation # for acid base reactions...
E=q + w (negative is by system - positive is on system)
Ksp = 108s5
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
do not change

2. How do you compute % dissociation?
Both electrons come from the same atom (just as good as a regular bond)
[A?]/[HA] x 100 or [BH?]/[B] x 100
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

3. When is ?G zero?
Soluble
voltaic: + electrolytic: -
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

4. What steps do organic labs consist of?
Synthesis - separation and purification of the product and its identification.
CO3²?
The compound with the lowest Ksp value.
Greenish-yellow gas

5. Are weak acids (and bases) written dissociated?

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6. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
hydroxides (ex: Ba(OH)2)
The one with most oxygen atoms (highest oxidation number)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

7. What is the charge on a chlorine atom?
zero
RCOOR
Concentration
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

8. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
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)
Current - time and charge on ion (moles of e used in half cell reaction)
Exothermic

9. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Insoluble except group 1 and ammonium
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
neutralization: high K - H2O product dissociation: low K - H2O reactant

10. A Bronsted-Lowry acid is...
White precipitate
proton donor base
zero-th: decreases - first: constant - second: increases
-Ea/R

11. Nonmetals are good _____ agents. Metals are good _______ agents.
lighted splint (positive result=pop)
Combine the equations for the half reactions in the non-spontaneous direction
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
ion pairing

12. What is the formula for alkynes?
yellow
CnH2n-2
bent
Most are soluble except Ag - Pb

13. For a dibasic acid (H2A) - [A²?]= ____ ?
Insoluble
HClO4
K2
Experimental mass/theoretical mass X 100

14. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
redox reaction
blue (BTB)
P2O5
-Ea/R

15. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Saturated - Substitution (which requires more radical conditions)
Identity and purity (impure compounds usually have broad & low melting points)
Ksp = 108s5
a-IMFs - b-molecular volume

16. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
They stay the same.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
strong acids/bases are written as H+ or OH- ions

17. Alkenes are ________ and react by __________
Distillation
No - it depends on the number of ions produced on dissolving.
Unsaturated - addition (ex: decolorize bromine solution)
Initiation energy (NOT Ea)

18. What do you use to look at burning magnesium? why?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
blue glass - it filters UV
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
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.

19. What two compounds are great oxidizing agents?

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20. dichromate
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Increases down group 1 decreases down group 17
Cr2O7²?
voltaic: - electrolytic: +

21. What is the difference between equivalence point and end point of a titration.
Graduated cylinder
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
H2O + CO2 (it decomposes readily)
Q=It (time in seconds)

22. What are the signs of ?G and E° for spontaneous reactions?
Most are soluble except Ag - Pb
?G=negative - E° must be positive
Q=It (time in seconds)
CnH2n

23. bromine
brown volatile liquid
CnH2n+1 often designated 'R' ex C3H7 is propyl
Perform ICE BOX calculation based on K1
Orange

24. What is the formula of butane?
CnH2n
How grouped results are
C4H10
zero

25. Which alkali metals float on water?
All except for lithium
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)
do not change
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

26. 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?
The compound with the lowest Ksp value.
Making sigma bonds and holding lone pairs
Nothing
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

27. Which value of R do you use for all energy and kinetics calculations?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
R=8.31 J/mol/K
Greenish-yellow gas
same KE - but PEice<PEwater

28. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
K1 x K2
do not change
P2O5
Soluble

29. Color is due to ______ _______ of light.
Selective absorption
proton donor base
small size and high charge
R=8.31 J/mol/K

30. At what point during titration do you have the perfect buffer - and what is the pH at this point?
It ceases - the circuit is broken.
Concentration
At half equivalence - pH=pKa
ClO?

31. What shape is methane?
Tetrahedral
0 and 14
Iodine and CO2 (dry ice)
voltaic: + electrolytic: -

32. When the salt bridge is removed what happens to the cell reaction?
?G= -ve - E°= +ve
It ceases - the circuit is broken.
metal oxides and hydrides are ionically bonded and basic
blue (BTB)

33. Give an example of a dilute strong acid.
E=q + w (negative is by system - positive is on system)
Big K=kf/kr
HClO4
O2 needs 4F/mol H2 needs 2F/mol

34. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Soluble except Ag - Pb - Ca - Sr Ba)
Most are soluble except Ag - Pb
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
0 and 14

35. carbonates
Insoluble except group 1 and ammonium
Perform ICE BOX calculation based on K1
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
ns² electrons (first in-first out)

36. mercury (II) ion
H3PO4
Hg²?
|experimental - accepted|/accepted X 100
E=q + w (negative is by system - positive is on system)

37. Color (absorbance) is proportional to ________
Experimental mass/theoretical mass X 100
benzene is less reactive than alkenes
Concentration
Transition element compounds (except if it has a full or empty d shell)

38. What are isotopes?
Ionic compounds
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
same KE - but PEice<PEwater
Cu3(PO4)2

39. What is the formula for summation?

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40. What type of polymer is nylon?
CO2 and H2O
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Synthetic condensation polymer (aka a polyamide)
Ppt will NOT form (unsaturated)

41. Ions are not ______.
proton donor base
H2PO4?
Soluble
atoms

42. Does reactivity increase/decrease going down group 1 and group 17?
bases
Increases down group 1 decreases down group 17
a-IMFs - b-molecular volume
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

43. Name some properties of Group 17
?H formation of an element in standard state=0
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
|experimental - accepted|/accepted X 100
ionic and form hydrogen and hydroxide

44. What value of R do you use for thermo calculations? gas calculations?
CnH(2n+2)
Greenish-yellow gas
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

45. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
-Ea/R
The dilution effect when the solutions mix. M1V1 = M2V2
They stay the same.
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

46. nitrate
#ligands=charge x2
Pour liquids using a funnel or down a glass rod
0.10M HCl (more ions)
NO3?

47. What is an Alkyl group?

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48. What is the catalyst for this reaction Ester + ?
proton acceptor.
voltaic: + electrolytic: -
Ppt will NOT form (unsaturated)
catalyst=conc H2SO4

49. What is the formula for alkanes?
CnH2n+2
small size and high charge
NH4?
Acids; HCOOCH3 is an ester

50. Esterification is...
acid + alcohol
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
water and substances with (s) less dense than
a-IMFs - b-molecular volume