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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 is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Pipette (burette if need repetition)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Time?¹ - (ex. s?¹ - hr?¹ - etc)

2. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
MnO4?
basic
benzene is less reactive than alkenes
voltaic: + electrolytic: -

3. What complex ion does ammonia form with silver? copper? cadmium? zinc?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
proton donor base
redox reaction

4. Metal hydrides are _____ and form _______ and _______ when added to water
ClO3?
C2O4²?
Insoluble except for nitrate and acetate
ionic and form hydrogen and hydroxide

5. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
RCOR
same KE - but PEice<PEwater
Separating funnel
H+

6. What process do you use to separate two liquids with different boiling points?
brown volatile liquid
No - NH3 and HCl gases are extremely soluble
fractional distillation
water and substances with (s) less dense than

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

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8. When a cell is 'flat' What is its voltage?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
zero
CN?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

9. What apparatus do you use to pour liquids?
C4H10
Pour liquids using a funnel or down a glass rod
Add acid to water so that the acid doesn't boil and spit
It ceases - the circuit is broken.

10. Where are group I metals stored?
Group I metals (soft metals) are stored under oil
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
PO4³?

11. What is the energy you must put into a reaction to make it start called?
no - they're written undissociated (HAaq)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Initiation energy (NOT Ea)
Filtration

12. chromate ion (soln + most solids)
Clear
basic
yellow
But S° of element is not zero (except at 0K)

13. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
ClO2?
A salt solution.
look for changes in oxidation # - the one that goes up is oxidized and is the RA
do not change

14. nitrate
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Making sigma bonds and holding lone pairs
NO3?
ClO4?

15. potassium permanganate
Salt and water
Purple
H3PO4
S crystal at 0K=0

16. lead compounds
water and substances with (s) less dense than
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
it is lower and occurs over less sharp a range
Insoluble except nitrate and acetate

17. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Decant
0 and 14
a-IMFs - b-molecular volume

18. What is the general formula for alkyl halides?
bright yellow
it's lower and occurs over less sharp a range
RX
Identity and purity (impure compounds usually have broad & low melting points)

19. How do you find the pH for a dibasic acid? (H2A)?
Perform ICE BOX calculation based on K1
Reduction always takes place at the cathode (RED CAT) In both types of cell!
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

20. Nonmetals are good _____ agents. Metals are good _______ agents.
CO3²?
Cr2O7²?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Most are soluble except Ag - Pb

21. 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.
PO4³?
bases
Group I metals (soft metals) are stored under oil

22. Which value of R do you use for all energy and kinetics calculations?
Unsaturated - addition (ex: decolorize bromine solution)
Making sigma bonds and holding lone pairs
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
R=8.31 J/mol/K

23. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
bases
Add acid to water so that the acid doesn't boil and spit
They stay the same.
K1 x K2

24. hypochlorite
benzene is less reactive than alkenes
ClO?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

25. Which alkali metals float on water?
H+
by electrolysis
All except for lithium
it's lower and occurs over less sharp a range

26. What type of compounds do Group 14 form?
C4H10
+4-covalent - +2-ionic
How grouped results are
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

27. How do you dilute an acid?

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28. hydroxide
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
CrO4²?
OH?

29. How does group 1 metals' density compare to water's?
0 and 14
are less dense than water
a-IMFs - b-molecular volume
Monomer + monomer = polymer product + a simple molecule such as water or HCl

30. 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?]
lighted splint (positive result=pop)
ns² electrons (first in-first out)
[A?]/[HA] x 100 or [BH?]/[B] x 100

31. What is reflux?
boiling without losing volatile solvents/reactants
Only temperature
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
zero

32. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
The Faraday or Faraday's constant.
Pale yellow
atoms
zero

33. How are strong ones written?
ClO?
voltaic: - electrolytic: +
strong acids/bases are written as H+ or OH- ions
methyl formate

34. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
hydroxides (ex: Ba(OH)2)
K2
bent

35. Do you use J or kJ for ?H - ?S - and ?G?
CH3COO?
CO3²?
?H-kJ - ?S-J - ?G-kJ
Unsaturated - addition (ex: decolorize bromine solution)

36. During a titration what is present in the beaker at the equivalence point?
No - it depends on the number of ions produced on dissolving.
C4H10
A salt solution.
benzene has a delocalized pi ring structure

37. What are hybrid orbitals used for?
Suniverse increases for spontaneous processes
Making sigma bonds and holding lone pairs
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

38. chlorate
Heat a test tube at an angle at the side of the tube (not bottom)
ethers
?G= -ve - E°= +ve
ClO3?

39. Does Benzene react by addition or substitution?
P2O5
CO3²?
Salts (ex: CaO + SO2 ? CaSO3)
it reacts by substitution NOT addition

40. How are non-metal oxides and hydrides bonded? are they acidic or basic?
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
non-metal oxides and hydrides are covalently bonded and are acidic.
CrO4²?
Acid rain - dissolves marble buildings/statues and kills trees.

41. lead iodide
NH4?
bright yellow
Disulfur dichloride
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

42. What process do you use to obtain the precipitate from a solution?
Group I metals (soft metals) are stored under oil
Soluble
strong acids/bases are written as H+ or OH- ions
Filtration

43. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
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.
diamond and graphite
No - it depends on the number of ions produced on dissolving.
H2O + CO2 (it decomposes readily)

44. What does saturated mean? Unsaturated?
CnH2n-2
Insoluble except nitrate and acetate
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
K1 x K2

45. How do you explain trends in atomic properties using Coulomb's Law?
10?8
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
do not change
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

46. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
bright yellow
Ksp = 108s5
White precipitate

47. acetates
CnH2n+2
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
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Soluble

48. bromine
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
brown volatile liquid
zero
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

49. What is the word equation for addition polymerisation?
do not change
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
CnH2n
ClO?

50. What is the third law of thermodynamics?
PO4³?
no - they're written undissociated (HAaq)
S crystal at 0K=0
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

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AP Chemistry 2

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