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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. Lattice energy is high for ions with _____ size and _____ charge
Heat a test tube at an angle at the side of the tube (not bottom)
small size and high charge
CnH(2n+2)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

2. What equipment do you need for a titration?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
no - they're written undissociated (HAaq)

3. What is the general formula for an ester?
zero-th: decreases - first: constant - second: increases
RCOOR
hydroxides (ex: Ba(OH)2)
NH4?

4. nitrates
Soluble
CnH(2n+2)
Making sigma bonds and holding lone pairs
water and substances with (s) less dense than

5. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
CO2 and H2O
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
CO3²?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

6. If Q < Ksp a ppt ______
Soluble
C4H10
Ppt will NOT form (unsaturated)
Distillation

7. What is precision?
Big K=kf/kr
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Filtration
How grouped results are

8. Buffer capacity must contain decent amounts of a ________ ________
Salt + water
T increases exponentially the proportion of molecules with E > Ea
Conjugate pair (one must be a weak base or acid)
10?8

9. Colorless doesn't mean ______
Clear
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)
Initiation energy (NOT Ea)
Hg²?

10. What is the conjugate acid of H2PO4?
bases
H3PO4
They decrease (or could be the same if the solid has ONLY JUST disappeared)
?G=negative - E° must be positive

11. Metal hydrides are _____ and form _______ and _______ when added to water
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Sigma bonds are stronger than pi bonds
ionic and form hydrogen and hydroxide
boiling without losing volatile solvents/reactants

12. What is the test for oxygen?
Pale purple - (orange)-yellow - red - blue - green.
How close results are to the accepted value
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Glowing splint (positive result=relights)

13. What is H2CO3 (carbonate acid) usually written as?
Mn²? - Cr³? - Cr³
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
H2O + CO2 (it decomposes readily)
Synthesis - separation and purification of the product and its identification.

14. dihydrogen phosphate
Iodine and CO2 (dry ice)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Acids; HCOOCH3 is an ester
H2PO4?

15. Is a graduated cylinder or beaker more accurate?
C4H10
Insoluble except nitrate and acetate
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Graduated cylinder

16. hydroxide
An active metal.
OH?
lighted splint (positive result=pop)
basic

17. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Experimental mass/theoretical mass X 100
a-IMFs - b-molecular volume
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
water and substances with (s) less dense than

18. For a dibasic acid (H2A) - [A²?]= ____ ?
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
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.
K2
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

19. Acids + Carbonates (bicarbonates) make?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
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
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

20. What should you check for before you begin titrating?
Group I metals (soft metals) are stored under oil
An active metal.
Check for air bubbles in the buret and remove the buret funnel from the buret
it is lower and occurs over less sharp a range

21. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
Both electrons come from the same atom (just as good as a regular bond)
Acidified
Tetrahedral

22. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
RCOR
Insoluble
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

23. If Q > Ksp - then system shifts _______ and ppt ______
Concentration
The benzene ring (or more correctly the phenyl group - C6H5)
left - ppt will form
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)

24. If ?S is positive - are the products more or less chaotic than the reactants?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
More chaotic (ex: gases made)
Unsaturated - addition (ex: decolorize bromine solution)
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.

25. What is the formula of butane?
C4H10
proton donor base
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Concentration

26. What are the signs for ?G and E° for spontaneous reactions?
Orange
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
RCOR
?G= -ve - E°= +ve

27. What is the conjugate base of NH3?
allow for the vapor pressure of water and make sure to level levels
NH2?
CrO4²?
H3PO4

28. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
bases
strong acids/bases are written as H+ or OH- ions
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

29. At what point during titration do you have the perfect buffer - and what is the pH at this point?
hydroxides (ex: Ba(OH)2)
CH3COO?
At half equivalence - pH=pKa
Both electrons come from the same atom (just as good as a regular bond)

30. Color (absorbance) is proportional to ________
same KE - but PEice<PEwater
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
?H-kJ - ?S-J - ?G-kJ
Concentration

31. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
it is lower and occurs over less sharp a range
proton donor base
Ksp = s²
0.10M HCl (more ions)

32. What complex ion does ammonia form with silver? copper? cadmium? zinc?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
RCOOR
Iodine and CO2 (dry ice)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

33. group 1 ions/compounds
10?8
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.
Kc=Kp
Soluble

34. Which value of R do you use for all energy and kinetics calculations?
Pale yellow
R=8.31 J/mol/K
Greenish-yellow gas
Iodine and CO2 (dry ice)

35. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia
10?8
How close results are to the accepted value

36. carbonate
Eudiometer
Ksp = 108s5
CO3²?
The benzene ring (or more correctly the phenyl group - C6H5)

37. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
boiling without losing volatile solvents/reactants
water and substances with (s) less dense than
Ksp = 27s4
ion pairing

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

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39. How does half life change for zero-th order - first order - and second order processes?
HClO4
zero-th: decreases - first: constant - second: increases
Ppt will NOT form (unsaturated)
Pale yellow

40. ammonium/ammonium compounds
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Both electrons come from the same atom (just as good as a regular bond)
Soluble
blue

41. chromate ion (soln + most solids)
water and substances with (s) less dense than
yellow
proton acceptor.
Unsaturated - addition (ex: decolorize bromine solution)

42. What is the general formula of an alkane?
Sigma bonds are stronger than pi bonds
CnH(2n+2)
Ksp = 27s4
Cr2O7²?

43. What apparatus do you use to pour liquids?
Pour liquids using a funnel or down a glass rod
They stay the same.
MnO4?
non-metal oxides and hydrides are covalently bonded and are acidic.

44. 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?
All except for lithium
The compound with the lowest Ksp value.
blue
Acidified

45. What process do you use to obtain the precipitate from a solution?
Ksp = s²
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)
bases
Filtration

46. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
R=8.31 J/mol/K
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
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)

47. Both Acetic acid and ____________ are also functional isomers.
Hg2²?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Soluble except Ag - Pb - Ca - Sr Ba)
methyl formate

48. Does Kw increase or decrease with T? Why?
NH4?
Tetrahedral
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
bright yellow

49. What is the formula of copper (II) phosphate?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
proton donor base
Cu3(PO4)2
Conjugate pair (one must be a weak base or acid)

50. halides
Ksp = 108s5
voltaic: + electrolytic: -
Most are soluble except Ag - Pb
Most INsoluble except group 1 and ammonium