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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. Acidic gases like SO2 in the atmosphere cause what environmental problems?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Acid rain - dissolves marble buildings/statues and kills trees.
do not change
Salts (ex: CaO + SO2 ? CaSO3)

2. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Heptane
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

3. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
ionic and form hydrogen and hydroxide
P2O5
Acidified
RCOR

4. ________ are Lewis bases - because they can donate a lone pair of electrons.
ClO4?
same KE - but PEice<PEwater
blue glass - it filters UV
OH- and NH3

5. dichromate
Cr2O7²?
acid + alcohol
?H formation of an element in standard state=0
Time?¹ - (ex. s?¹ - hr?¹ - etc)

6. Is the ?H formation of an element in standard state zero?
different forms of the same element
?H formation of an element in standard state=0
atoms
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

7. hypochlorite
Suniverse increases for spontaneous processes
ethers
?H-kJ - ?S-J - ?G-kJ
ClO?

8. chromate ion (soln + most solids)
Group I metals (soft metals) are stored under oil
yellow
OH- and NH3
?H-kJ - ?S-J - ?G-kJ

9. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
The Faraday or Faraday's constant.
K2
Ksp = 4s³
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

10. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
E=q + w (negative is by system - positive is on system)
Pale yellow
same KE - but PEice<PEwater
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

11. If a free element is involved - what type of reaction must be involved?
redox reaction
fruit - fish - bases
CO2 and H2O
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.

12. Name six characteristics of transition elements (or their compounds)
voltaic: + electrolytic: -
blue
a-IMFs - b-molecular volume
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)

13. What type of polymer is nylon?
proton donor base
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)
Clear
Synthetic condensation polymer (aka a polyamide)

14. What do group I/II metal oxides and acids form?
it reacts by substitution NOT addition
Most INsoluble except group 1 and ammonium
Salt and water
10?8

15. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Add acid to water so that the acid doesn't boil and spit
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Anode - oxygen. Cathode - hydrogen
Acid rain - dissolves marble buildings/statues and kills trees.

16. Which would cause the bulb in a conductivity apparatus to be brightest?
Tetrahedral
ClO3?
An active metal.
0.10M HCl (more ions)

17. What is a coordinate covalent bond?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Filtration
Both electrons come from the same atom (just as good as a regular bond)
proton acceptor.

18. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
T increases exponentially the proportion of molecules with E > Ea
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
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)

19. What is the formula for percent yield?
a-IMFs - b-molecular volume
Experimental mass/theoretical mass X 100
zero
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

20. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
metal oxides and hydrides are ionically bonded and basic
benzene is less reactive than alkenes
Sigma bonds are stronger than pi bonds

21. What shape is ammonia?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
voltaic: + electrolytic: -
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
Trigonal pyramidal

22. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
An active metal.
Ksp = s²
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

23. Which value of R do you use for all energy and kinetics calculations?
benzene has a delocalized pi ring structure
zero-th: decreases - first: constant - second: increases
R=8.31 J/mol/K
Insoluble except for nitrate and acetate

24. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Concentration
zero

25. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
boiling without losing volatile solvents/reactants
benzene is less reactive than alkenes
Most are soluble except Ag - Pb

26. What does saturated mean? Unsaturated?
CnH2n-2
-Ea/R
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
q=mc?T q=mL (or n x ?h)

27. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
Mn²? - Cr³? - Cr³
Anode - oxygen. Cathode - hydrogen
|experimental - accepted|/accepted X 100

28. How does half life change for zero-th order - first order - and second order processes?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
zero-th: decreases - first: constant - second: increases
CnH2n
Salt + water

29. 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.
P2O5
Most are soluble except Ag - Pb
Ksp = 27s4

30. What process do you use to separate two liquids with different boiling points?
fractional distillation
Filtration
Add acid to water so that the acid doesn't boil and spit
CnH2n

31. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
ClO4?
T increases exponentially the proportion of molecules with E > Ea
CnH2n+1 often designated 'R' ex C3H7 is propyl
Kc=Kp

32. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Only temperature
T increases exponentially the proportion of molecules with E > Ea
ionic and form hydrogen and hydroxide

33. Alkenes are ________ and react by __________
At half equivalence - pH=pKa
ion pairing
blue glass - it filters UV
Unsaturated - addition (ex: decolorize bromine solution)

34. Color is due to ______ _______ of light.
Selective absorption
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
OH?
Hg²?

35. Acid plus base make?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Salt + water.
CnH(2n+2)
Big K=kf/kr

36. chlorite
Most are soluble except Ag - Pb
ClO2?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Soluble

37. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
R=8.31 J/mol/K
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

38. What do you use to look at burning magnesium? why?
Anode - oxygen. Cathode - hydrogen
White precipitate
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
blue glass - it filters UV

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

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40. Where are group I metals stored?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Trigonal pyramidal
Group I metals (soft metals) are stored under oil

41. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
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.
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

42. Both Acetic acid and ____________ are also functional isomers.
methyl formate
SO4²?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Iodine and CO2 (dry ice)

43. What do you do to get rid of most of the solution from a precipitate?
it's lower and occurs over less sharp a range
CO (poisonous)
Decant
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

44. Can you collect soluble gases over water?
Disulfur dichloride
H2PO4?
Most INsoluble except group 1 and ammonium
No - NH3 and HCl gases are extremely soluble

45. What word is a clue for a redox reaction?
Products - reactants (except for BDE when it's reactants - products)
Acidified
Greenish-yellow gas
proton acceptor.

46. hydroxide
Identity and purity (impure compounds usually have broad & low melting points)
OH?
Separating funnel
The Faraday or Faraday's constant.

47. What is the catalyst for this reaction Ester + ?
chemically (ex: with carbon)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
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.
catalyst=conc H2SO4

48. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Most INsoluble except group 1 and ammonium
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
The one with most oxygen atoms (highest oxidation number)
CnH(2n+2)

49. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
CnH2n+2
Insoluble except group 1 and ammonium
A) any range. b) 8-10 c) 4-6
Hg2²?

50. What do metal oxides plus non- metal oxides form?
Greenish-yellow gas
methyl formate
Salts (ex: CaO + SO2 ? CaSO3)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).