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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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 equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
P2O5
The compound with the lowest Ksp value.
Ksp = 27s4

2. What should you check for before you begin titrating?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
allow for the vapor pressure of water and make sure to level levels
Check for air bubbles in the buret and remove the buret funnel from the buret
bright yellow

3. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Increases.
Big K=kf/kr
Ksp = 108s5
Anode - oxygen. Cathode - hydrogen

4. Which alkali metals float on water?
?H-kJ - ?S-J - ?G-kJ
Soluble except Ag - Pb - Ca - Sr Ba)
K2
All except for lithium

5. What is Big K in terms of kf and kr?
RCOR
Big K=kf/kr
Pour liquids using a funnel or down a glass rod
it reacts by substitution NOT addition

6. What is the general formula for an aldehyde?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
H2O + CO2 (it decomposes readily)
Disulfur dichloride
RCHO (carbonyl at end)

7. What shape is water?
CnH(2n+2)
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)
CN?
bent

8. What is HCOOCH3?
But S° of element is not zero (except at 0K)
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
+4-covalent - +2-ionic
Acids; HCOOCH3 is an ester

9. A Bronsted-Lowry base is...
A) any range. b) 8-10 c) 4-6
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
proton acceptor.
R=8.31 J/mol/K

10. Color is due to ______ _______ of light.
same KE - but PEice<PEwater
At half equivalence - pH=pKa
All except for lithium
Selective absorption

11. Give an example of a dilute strong acid.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
NH2?
Pale purple - (orange)-yellow - red - blue - green.
HClO4

12. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
H2O + CO2 (it decomposes readily)
Distillation
Ionic compounds

13. How are primary alcohols turned into acids?
Mono; di; tri; tetra; penta; hexa.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
ROH
K2

14. nitrate
NO3?
fruit - fish - bases
An active metal.
allow for the vapor pressure of water and make sure to level levels

15. Is a graduated cylinder or beaker more accurate?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
ClO?
no - they're written undissociated (HAaq)
Graduated cylinder

16. Can you collect soluble gases over water?
S crystal at 0K=0
Decant
CnH2n
No - NH3 and HCl gases are extremely soluble

17. What is the test for hydrogen?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
lighted splint (positive result=pop)
bent
?G= -ve - E°= +ve

18. What is H2CO3 (carbonate acid) usually written as?
lighted splint (positive result=pop)
Cu3(PO4)2
H2O + CO2 (it decomposes readily)
Time?¹ - (ex. s?¹ - hr?¹ - etc)

19. When combining half equations - what do you do to E° values when multiplying coefficients?
RCOOR
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Nothing

20. What is the first law of thermodynamics?
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)
E=q + w (negative is by system - positive is on system)
?H formation of an element in standard state=0
Distillation

21. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
Molecules with the same molecular formulas - but different structural formulas
ROR
Check for air bubbles in the buret and remove the buret funnel from the buret

22. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Kc=Kp
it's lower and occurs over less sharp a range
RCHO (carbonyl at end)
acid + alcohol

23. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Insoluble
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
The dilution effect when the solutions mix. M1V1 = M2V2
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

24. How are strong ones written?
it is lower and occurs over less sharp a range
strong acids/bases are written as H+ or OH- ions
Decant
White precipitate

25. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Current - time and charge on ion (moles of e used in half cell reaction)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
zero
no - they're written undissociated (HAaq)

26. What is the third law of thermodynamics?
CN?
Unsaturated - addition (ex: decolorize bromine solution)
Cu3(PO4)2
S crystal at 0K=0

27. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Insoluble (except group 1 ammonium and Ba)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Clear

28. What do hydrocarbons form when they burn in air (oxygen)?
Decant
CO2 and H2O
NO3?
Pale purple - (orange)-yellow - red - blue - green.

29. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Q=It (time in seconds)
Soluble

30. Acid plus base make?
Selective absorption
Salt + water.
An active metal.
Most INsoluble except group 1 and ammonium

31. lead compounds
Insoluble except nitrate and acetate
'non-active' metals such as Cu - Ag - Au - Pt - etc.
RNH2
E=q + w (negative is by system - positive is on system)

32. What element is used to vulcanize rubber?
Unsaturated - addition (ex: decolorize bromine solution)
Current - time and charge on ion (moles of e used in half cell reaction)
Transition element compounds (except if it has a full or empty d shell)
Sulfur

33. hypochlorite
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
RCOOH
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
ClO?

34. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Purple
Saturated - Substitution (which requires more radical conditions)
are less dense than water

35. bromothymol
Big K=kf/kr
blue (BTB)
K2
Insoluble (except group 1 ammonium and Ba)

36. How do you get Ecell for spontaneous reactions?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
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.
Distillation
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

37. What is the formula for alkenes?
CnH2n
#ligands=charge x2
Hg²?
Synthesis - separation and purification of the product and its identification.

38. What things should you remember to do when collecting gas over water?
Decant
allow for the vapor pressure of water and make sure to level levels
Both electrons come from the same atom (just as good as a regular bond)
Iodine and CO2 (dry ice)

39. What is the formula for alkanes?
RX
Salts (ex: CaO + SO2 ? CaSO3)
Soluble
CnH2n+2

40. Alkenes are ________ and react by __________
Disulfur dichloride
Unsaturated - addition (ex: decolorize bromine solution)
Conjugate pair (one must be a weak base or acid)
Products - reactants (except for BDE when it's reactants - products)

41. What are the signs of ?G and E° for spontaneous reactions?
The dilution effect when the solutions mix. M1V1 = M2V2
?G=negative - E° must be positive
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Combine the equations for the half reactions in the non-spontaneous direction

42. What is reflux?
CO3²?
it is lower and occurs over less sharp a range
ClO3?
boiling without losing volatile solvents/reactants

43. What do metal oxides plus acids form?
Salt + water
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Transition element compounds (except if it has a full or empty d shell)

44. What is the pH of 1.0M HCl? 1M NaOH?
different forms of the same element
How grouped results are
Mn²? - Cr³? - Cr³
0 and 14

45. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
The dilution effect when the solutions mix. M1V1 = M2V2
How close results are to the accepted value
-Ea/R

46. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Iodine and CO2 (dry ice)
allow for the vapor pressure of water and make sure to level levels
No - it depends on the number of ions produced on dissolving.

47. What do the 'a' and 'b' in Van Der Waal's equation allow for?
no - they're written undissociated (HAaq)
ion pairing
a-IMFs - b-molecular volume
NH2?

48. What is the difference between equivalence point and end point of a titration.
A salt solution.
Hg2²?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
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

49. halides
T increases exponentially the proportion of molecules with E > Ea
Most are soluble except Ag - Pb
No - it depends on the number of ions produced on dissolving.
Soluble

50. What do you use to look at burning magnesium? why?
Salts (ex: CaO + SO2 ? CaSO3)
Iodine and CO2 (dry ice)
Only temperature
blue glass - it filters UV