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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. acetate
NH2?
Evaporation
CH3COO?
yellow

2. Color (absorbance) is proportional to ________
Both electrons come from the same atom (just as good as a regular bond)
Concentration
The compound with the lowest Ksp value.
They decrease (or could be the same if the solid has ONLY JUST disappeared)

3. Can you collect soluble gases over water?
At half equivalence - pH=pKa
+4-covalent - +2-ionic
No - NH3 and HCl gases are extremely soluble
Silvery gray solid - brown - purple

4. How does group 1 metals' density compare to water's?
S2O3²?
[A?]/[HA] x 100 or [BH?]/[B] x 100
are less dense than 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 -

5. What do hydrocarbons form when they burn in air (oxygen)?
?G= -ve - E°= +ve
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)
CO2 and H2O
basic

6. bromothymol
Cu3(PO4)2
strong acids/bases are written as H+ or OH- ions
Experimental mass/theoretical mass X 100
blue (BTB)

7. One mole of electrons carries 96500Coulombs - what is this quantity called?

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8. Do you use J or kJ for ?H - ?S - and ?G?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
diamond and graphite
?H-kJ - ?S-J - ?G-kJ
Acid rain - dissolves marble buildings/statues and kills trees.

9. What type of polymer is nylon?
Ksp = 108s5
Synthetic condensation polymer (aka a polyamide)
0.10M HCl (more ions)
Salt and water

10. Why are noble gases stable?
Disulfur dichloride
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Both electrons come from the same atom (just as good as a regular bond)
catalyst=conc H2SO4

11. How many ligands attach to a central ion in a complex ion?
K2
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
#ligands=charge x2

12. What is the formula for summation?

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13. Name six characteristics of transition elements (or their compounds)
Increases.
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)
a-IMFs - b-molecular volume
Making sigma bonds and holding lone pairs

14. 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)
benzene is less reactive than alkenes
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
ionic and form hydrogen and hydroxide

15. How are metal oxides and hydrides bonded? are they acidic or basic?
Salt + water.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
metal oxides and hydrides are ionically bonded and basic
?G= -ve - E°= +ve

16. sulfate
SO4²?
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)
?H-kJ - ?S-J - ?G-kJ
MnO4?

17. nitrate
NO3?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
it is lower and occurs over less sharp a range
Insoluble

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

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19. What type of solutions do small - highly charged cations tend to form?
metal oxides and hydrides are ionically bonded and basic
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Anode
boiling without losing volatile solvents/reactants

20. When a cell is 'flat' What is its voltage?
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?)
zero
brown volatile liquid
CnH(2n+2)

21. cyanide
Orange
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
A) any range. b) 8-10 c) 4-6
CN?

22. Give an example of a dilute strong acid.
No - NH3 and HCl gases are extremely soluble
proton donor base
HClO4
brown volatile liquid

23. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Group 1 hydroxides (ex: NaOH)
Suniverse increases for spontaneous processes
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Ksp = 108s5

24. Is a graduated cylinder or beaker more accurate?
linear
Graduated cylinder
?H-kJ - ?S-J - ?G-kJ
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

25. What shape is water?
How grouped results are
bent
SO4²?
0 and 14

26. What is the conjugate acid of H2PO4?
ClO3?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
?G= -ve - E°= +ve
H3PO4

27. For a dibasic acid (H2A) - [A²?]= ____ ?
Hg2²?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
K2
Iodine and CO2 (dry ice)

28. How do you heat a test tube?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Combine the equations for the half reactions in the non-spontaneous direction
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Heat a test tube at an angle at the side of the tube (not bottom)

29. Lattice energy is high for ions with _____ size and _____ charge
methyl formate
P2O5
small size and high charge
ROH

30. lead compounds
Conjugate pair (one must be a weak base or acid)
Insoluble except nitrate and acetate
CnH2n-2
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

31. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Pour liquids using a funnel or down a glass rod
left - ppt will form
H2O + CO2 (it decomposes readily)

32. If ?S is positive - are the products more or less chaotic than the reactants?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
More chaotic (ex: gases made)
Pipette (burette if need repetition)
do not change

33. ________ are Lewis bases - because they can donate a lone pair of electrons.
Heat a test tube at an angle at the side of the tube (not bottom)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Pour liquids using a funnel or down a glass rod
OH- and NH3

34. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Clear
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Group I metals (soft metals) are stored under oil

35. thiosulfate
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
S2O3²?
Exothermic
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.

36. When combining half equations - what do you do to E° values when multiplying coefficients?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Nothing
Orange
q=mc?T q=mL (or n x ?h)

37. What are the units of the first order rate constant?
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)
An active metal.
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Time?¹ - (ex. s?¹ - hr?¹ - etc)

38. How do you clean a buret/pipette for a titration?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
zero
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

39. BaSO4
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Insoluble
MnO4?
The benzene ring (or more correctly the phenyl group - C6H5)

40. What is the third law of thermodynamics?
They stay the same.
?G=negative - E° must be positive
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
S crystal at 0K=0

41. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
Only temperature
H+
Ksp = 108s5

42. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
C2O4²?
small size and high charge
Soluble

43. Metal hydrides are _____ and form _______ and _______ when added to water
diamond and graphite
No - it depends on the number of ions produced on dissolving.
no - they're written undissociated (HAaq)
ionic and form hydrogen and hydroxide

44. What is the second law of thermodynamics?
Sulfur
Suniverse increases for spontaneous processes
linear
Perform ICE BOX calculation based on K1

45. Ca - Sr - Ba
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
hydroxides (ex: Ba(OH)2)
CO2 and H2O
No - NH3 and HCl gases are extremely soluble

46. What causes the dramatic effect of T on rate?
Most are soluble except Ag - Pb
O2 needs 4F/mol H2 needs 2F/mol
lighted splint (positive result=pop)
T increases exponentially the proportion of molecules with E > Ea

47. What changes Keq?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Only temperature
proton donor base

48. What are hybrid orbitals used for?
T increases exponentially the proportion of molecules with E > Ea
Making sigma bonds and holding lone pairs
Combine the equations for the half reactions in the non-spontaneous direction
OH?

49. What apparatus do you use to separate 2 immiscible liquids?
Pale purple - (orange)-yellow - red - blue - green.
Separating funnel
Trigonal pyramidal
H2PO4?

50. If Q < Ksp a ppt ______
ion pairing
Ppt will NOT form (unsaturated)
R=8.31 J/mol/K
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)