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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. BaSO4
All except for lithium
Acidified
Insoluble
Ksp = 27s4

2. What shape is ammonia?
Trigonal pyramidal
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Evaporation
Conjugate pair (one must be a weak base or acid)

3. What is precision?
brown volatile liquid
neutralization: high K - H2O product dissociation: low K - H2O reactant
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
How grouped results are

4. What is the energy you must put into a reaction to make it start called?
voltaic: + electrolytic: -
Initiation energy (NOT Ea)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
RCHO (carbonyl at end)

5. What are two substances that sublime at 1 atm when heated?
Experimental mass/theoretical mass X 100
Suniverse increases for spontaneous processes
benzene has a delocalized pi ring structure
Iodine and CO2 (dry ice)

6. During a titration what is present in the beaker at the equivalence point?
A salt solution.
Identity and purity (impure compounds usually have broad & low melting points)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

7. What steps do organic labs consist of?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
?G= -ve - E°= +ve
CH3COO?
Synthesis - separation and purification of the product and its identification.

8. What is the third law of thermodynamics?
CnH2n+2
boiling without losing volatile solvents/reactants
S crystal at 0K=0
are less dense than water

9. How are strong ones written?
Anode - oxygen. Cathode - hydrogen
Saturated - Substitution (which requires more radical conditions)
-Ea/R
strong acids/bases are written as H+ or OH- ions

10. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Silvery gray solid - brown - purple
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
acid + alcohol
Acid rain - dissolves marble buildings/statues and kills trees.

11. Acids + Carbonates (bicarbonates) make?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Sulfur
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
ClO2?

12. Both Acetic acid and ____________ are also functional isomers.
CO2 and H2O
small size and high charge
Concentration
methyl formate

13. silver compounds
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Insoluble except for nitrate and acetate
Q=It (time in seconds)
O2 needs 4F/mol H2 needs 2F/mol

14. A Bronsted-Lowry acid is...
RCOOH
a-IMFs - b-molecular volume
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
proton donor base

15. What type of compounds do metals/non metals form?
Nothing
Ionic compounds
ClO?
0 and 14

16. What is the formula for alkanes?
CnH2n+2
RCOR
benzene has a delocalized pi ring structure
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

17. What do hydrocarbons form when they burn in air (oxygen)?
How close results are to the accepted value
Check for air bubbles in the buret and remove the buret funnel from the buret
T increases exponentially the proportion of molecules with E > Ea
CO2 and H2O

18. Why are noble gases stable?
q=mc?T q=mL (or n x ?h)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
non-metal oxides and hydrides are covalently bonded and are acidic.
Kc=Kp

19. permanganate
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
bases
Soluble except Ag - Pb - Ca - Sr Ba)
MnO4?

20. What is the difference between equivalence point and end point of a titration.
an oxidized and reduced substance
R=8.31 J/mol/K
Kc=Kp
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

21. What is the test for oxygen?
The Faraday or Faraday's constant.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
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?)
Glowing splint (positive result=relights)

22. What is the formula for alkynes?
do not change
Increases down group 1 decreases down group 17
CnH2n-2
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

23. How does group 1 metals' density compare to water's?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
CnH2n+1 often designated 'R' ex C3H7 is propyl
are less dense than water
Acidified

24. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
it's lower and occurs over less sharp a range
Synthesis - separation and purification of the product and its identification.
K1 x K2
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

25. What does saturated mean? Unsaturated?
PO4³?
Pale purple - (orange)-yellow - red - blue - green.
Soluble except Ag - Pb - Ca - Sr Ba)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

26. ________ are Lewis bases - because they can donate a lone pair of electrons.
acids
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?)
E=q + w (negative is by system - positive is on system)
OH- and NH3

27. What do you need to make a polymer?
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)
Anode
0 and 14
Current - time and charge on ion (moles of e used in half cell reaction)

28. dihydrogen phosphate
CN?
All except for lithium
Transition element compounds (except if it has a full or empty d shell)
H2PO4?

29. What do group I/II metal oxides plus water form?
Transition element compounds (except if it has a full or empty d shell)
zero
bases
catalyst=conc H2SO4

30. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Mn²? - Cr³? - Cr³
A) any range. b) 8-10 c) 4-6

31. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
an oxidized and reduced substance
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
OH- and NH3

32. A Bronsted-Lowry base is...
redox reaction
Glacial acetic acid
|experimental - accepted|/accepted X 100
proton acceptor.

33. chromate
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
CrO4²?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Acidified

34. hydroxides
Insoluble (except group 1 ammonium and Ba)
bases
methyl formate
RCOOR

35. What process do you use to obtain the solute from a solution?
Insoluble except group 1 and ammonium
Q=It (time in seconds)
Acids; HCOOCH3 is an ester
Evaporation

36. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
It ceases - the circuit is broken.
Increases.
Current - time and charge on ion (moles of e used in half cell reaction)
metal oxides and hydrides are ionically bonded and basic

37. If a free element is involved - what type of reaction must be involved?
redox reaction
CnH2n-2
Glowing splint (positive result=relights)
RNH2

38. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
R=8.31 J/mol/K
blue (BTB)
Check for air bubbles in the buret and remove the buret funnel from the buret

39. How does the melting point of a mixture compare to the MP of a pure substance?
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?)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
it is lower and occurs over less sharp a range
S2O3²?

40. Neutralization is an ________ reaction.
left - ppt will form
allow for the vapor pressure of water and make sure to level levels
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Sulfur

41. Aromatic compounds contain what?
benzene is less reactive than alkenes
Soluble
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
The benzene ring (or more correctly the phenyl group - C6H5)

42. Nonmetals are good _____ agents. Metals are good _______ agents.
No - NH3 and HCl gases are extremely soluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

43. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
RNH2
Ksp = 27s4
Ksp = 108s5
ns² electrons (first in-first out)

44. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Distillation
The Faraday or Faraday's constant.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
water and substances with (s) less dense than

45. What is the general formula for an acid?
Increases.
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Mono; di; tri; tetra; penta; hexa.
RCOOH

46. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Kc=Kp
The dilution effect when the solutions mix. M1V1 = M2V2
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
metal oxides and hydrides are ionically bonded and basic

47. dichromate (soln + most solids)
Orange
The benzene ring (or more correctly the phenyl group - C6H5)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
it's lower and occurs over less sharp a range

48. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
blue (BTB)
10?8
bent
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

49. What complex ion does ammonia form with silver? copper? cadmium? zinc?
But S° of element is not zero (except at 0K)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Hg2²?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

50. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Sulfur
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Insoluble except for nitrate and acetate