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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. What is the catalyst for this reaction Ester + ?
no - they're written undissociated (HAaq)
catalyst=conc H2SO4
Ksp = s²
Increases down group 1 decreases down group 17

2. What is accuracy?
Exothermic
Current - time and charge on ion (moles of e used in half cell reaction)
Experimental mass/theoretical mass X 100
How close results are to the accepted value

3. When is ?G zero?
Hg²?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
RX
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

4. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
White precipitate
Time?¹ - (ex. s?¹ - hr?¹ - etc)
K2

5. What complex ion does ammonia form with silver? copper? cadmium? zinc?
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.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

6. What is the slope of the graph of lnk vs. 1/T?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
CnH2n+1 often designated 'R' ex C3H7 is propyl
Tetrahedral
-Ea/R

7. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
q=mc?T q=mL (or n x ?h)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
water and substances with (s) less dense than

8. halides
More chaotic (ex: gases made)
Add acid to water so that the acid doesn't boil and spit
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
Most are soluble except Ag - Pb

9. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
How grouped results are
Soluble
Pour liquids using a funnel or down a glass rod

10. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
C2O4²?
O2 needs 4F/mol H2 needs 2F/mol
They stay the same.
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

11. What are two substances that sublime at 1 atm when heated?
no - they're written undissociated (HAaq)
it reacts by substitution NOT addition
Iodine and CO2 (dry ice)
The dilution effect when the solutions mix. M1V1 = M2V2

12. lead iodide
bright yellow
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Soluble except Ag - Pb - Ca - Sr Ba)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

13. What value of R do you use for thermo calculations? gas calculations?
-Ea/R
The compound with the lowest Ksp value.
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

14. What is a coordinate covalent bond?
metal oxides and hydrides are ionically bonded and basic
ClO2?
Both electrons come from the same atom (just as good as a regular bond)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

15. What electrons are lost/gained first in transition element ions?
Check for air bubbles in the buret and remove the buret funnel from the buret
RX
atoms
ns² electrons (first in-first out)

16. What are hybrid orbitals used for?
Insoluble except nitrate and acetate
Making sigma bonds and holding lone pairs
Time?¹ - (ex. s?¹ - hr?¹ - etc)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

17. chlorate
ClO3?
H2O + CO2 (it decomposes readily)
allow for the vapor pressure of water and make sure to level levels
Unsaturated - addition (ex: decolorize bromine solution)

18. If Q < Ksp a ppt ______
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Ppt will NOT form (unsaturated)
Distillation
Ksp = 4s³

19. What shape is carbon dioxide?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
linear
fractional distillation
Cu3(PO4)2

20. How can metals like iron and zinc be reduced?
CnH(2n+2)
acid + alcohol
-Ea/R
chemically (ex: with carbon)

21. What is a dipeptide? polypeptide? protein?
Ksp = 27s4
lighted splint (positive result=pop)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

22. What type of polymer is nylon?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
S crystal at 0K=0
Synthetic condensation polymer (aka a polyamide)
Salt and water

23. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
CrO4²?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
RCHO (carbonyl at end)

24. What is the general formula for an alcohol?
A salt solution.
Heat a test tube at an angle at the side of the tube (not bottom)
Graduated cylinder
ROH

25. What is the test for oxygen?
Only temperature
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
OH?
Glowing splint (positive result=relights)

26. What process do you use to obtain the solute from a solution?
Exothermic
Evaporation
it's lower and occurs over less sharp a range
proton donor base

27. What is the third law of thermodynamics?
S crystal at 0K=0
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Group I metals (soft metals) are stored under oil
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

28. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Insoluble except nitrate and acetate
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
benzene is less reactive than alkenes
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

29. lead compounds
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)
Saturated - Substitution (which requires more radical conditions)
Sigma bonds are stronger than pi bonds
Insoluble except nitrate and acetate

30. Ions are not ______.
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
Unsaturated - addition (ex: decolorize bromine solution)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
atoms

31. What two compounds are great oxidizing agents?

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32. chlorine
Evaporation
ionic and form hydrogen and hydroxide
Ksp = s²
Greenish-yellow gas

33. What do you use to look at burning magnesium? why?
Sulfur
blue glass - it filters UV
blue
voltaic: + electrolytic: -

34. primary colors
Synthetic condensation polymer (aka a polyamide)
red - green - blue
by electrolysis
a-IMFs - b-molecular volume

35. Alkanes are _________ and react by _________
Nothing
CO2 and H2O
Saturated - Substitution (which requires more radical conditions)
ClO3?

36. Acid plus base make?
?H formation of an element in standard state=0
All except for lithium
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Salt + water.

37. What do group I/II metal oxides plus water form?
ROR
bases
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
it is lower and occurs over less sharp a range

38. Where are group I metals stored?
Check for air bubbles in the buret and remove the buret funnel from the buret
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Group I metals (soft metals) are stored under oil
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

39. carbonate
Insoluble
Filtration
CO3²?
Ksp = s²

40. What process do you use to obtain a solvent from a solution?
How grouped results are
O2 needs 4F/mol H2 needs 2F/mol
Distillation
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

41. What is precision?
CN?
How grouped results are
C2O4²?
Insoluble except nitrate and acetate

42. What do ions and electrons travel through in a voltaic/electrolytic cell?
K2
Salt and water
Check for air bubbles in the buret and remove the buret funnel from the buret
Ions go through the salt bridge - electrons go through metal wires in the external circuit

43. chromate
?G=negative - E° must be positive
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
CrO4²?
RCOR

44. Both Acetic acid and ____________ are also functional isomers.
blue (BTB)
Disulfur dichloride
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)
methyl formate

45. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
S2O3²?
Sigma bonds are stronger than pi bonds
SO4²?

46. Neutralization is an ________ reaction.
CO2 and H2O
Glowing splint (positive result=relights)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

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

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48. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
NH4?
H2PO4?
Soluble except Ag - Pb - Ca - Sr Ba)

49. bromothymol
Silvery gray solid - brown - purple
Increases down group 1 decreases down group 17
blue (BTB)
Group I metals (soft metals) are stored under oil

50. How does benzene compare in reactivity to alkenes?
Making sigma bonds and holding lone pairs
benzene is less reactive than alkenes
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
do not change