Test your basic knowledge |

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 causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
acid + alcohol
Insoluble
H+

2. carbonate
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
CO3²?
Acidified
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

3. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
RCOOR
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.
Hg²?

4. Give an example of a dilute strong acid.
HClO4
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

5. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Products - reactants (except for BDE when it's reactants - products)
H2O + CO2 (it decomposes readily)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
CnH2n+2

6. Which alkali metals float on water?
All except for lithium
Increases down group 1 decreases down group 17
Unsaturated - addition (ex: decolorize bromine solution)
Kc=Kp

7. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
proton donor base
Perform ICE BOX calculation based on K1
yellow

8. What part of a liquid do you look at to measure its volume?
water and substances with (s) less dense than
Read the bottom of the meniscus
ClO3?
NH4?

9. silver iodide
Graduated cylinder
T increases exponentially the proportion of molecules with E > Ea
Pale yellow
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

10. What is the sign of the anode in voltaic cells? in electrolytic cells?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
voltaic: - electrolytic: +
Insoluble except for nitrate and acetate
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

11. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
Add acid to water so that the acid doesn't boil and spit
ionic and form hydrogen and hydroxide
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

12. What is the test for oxygen?
red - green - blue
A salt solution.
Add acid to water so that the acid doesn't boil and spit
Glowing splint (positive result=relights)

13. What is a coordinate covalent bond?
it is lower and occurs over less sharp a range
OH?
Both electrons come from the same atom (just as good as a regular bond)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

14. sulfate
diamond and graphite
SO4²?
O2 needs 4F/mol H2 needs 2F/mol
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

16. What complex ion does ammonia form with silver? copper? cadmium? zinc?
zero
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
The compound with the lowest Ksp value.
0.10M HCl (more ions)

17. What is an Alkyl group?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

18. A geometric (or cis-trans) isomer exists due to.....
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

19. chromate ion (soln + most solids)
do not change
ClO4?
Ksp = 27s4
yellow

20. What type of compounds are almost always colored?
How grouped results are
Transition element compounds (except if it has a full or empty d shell)
Insoluble (except group 1 ammonium and Ba)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

21. nitrates
CnH2n
Soluble
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
linear

22. Name six characteristics of transition elements (or their compounds)
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)
benzene has a delocalized pi ring structure
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Sigma bonds are stronger than pi bonds

23. What is the catalyst for this reaction Ester + ?
catalyst=conc H2SO4
a-IMFs - b-molecular volume
All except for lithium
neutralization: high K - H2O product dissociation: low K - H2O reactant

24. How do you heat a test tube?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Heat a test tube at an angle at the side of the tube (not bottom)
chemically (ex: with carbon)
HClO4

25. What two types of substances are present in all redox reactions?
left - ppt will form
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
an oxidized and reduced substance
Add acid to water so that the acid doesn't boil and spit

26. What is the first law of thermodynamics?
benzene is less reactive than alkenes
E=q + w (negative is by system - positive is on system)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
same KE - but PEice<PEwater

27. What do group I/II metal oxides and acids form?
RCOR
same KE - but PEice<PEwater
White precipitate
Salt and water

28. What word is a clue for a redox reaction?
NH2?
no - they're written undissociated (HAaq)
Acidified
Soluble

29. What is reflux?
boiling without losing volatile solvents/reactants
H2PO4?
PO4³?
ROR

30. Is the standard entropy (S°) of an element zero?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
+4-covalent - +2-ionic
But S° of element is not zero (except at 0K)
yellow

31. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
H2O + CO2 (it decomposes readily)
Unsaturated - addition (ex: decolorize bromine solution)
Ksp = s²
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

32. What changes Keq?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Synthetic condensation polymer (aka a polyamide)
ethers
Only temperature

33. When driving off water from a hydrate - how do you tell you're done?
Decant
?H formation of an element in standard state=0
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

34. Which would cause the bulb in a conductivity apparatus to be brightest?
atoms
0.10M HCl (more ions)
Group I metals (soft metals) are stored under oil
Graduated cylinder

35. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
?H formation of an element in standard state=0
|experimental - accepted|/accepted X 100
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

36. What is a dipeptide? polypeptide? protein?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
allow for the vapor pressure of water and make sure to level levels
Perform ICE BOX calculation based on K1
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

37. How are primary alcohols turned into acids?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
CnH2n-2
Separating funnel

38. What is the formula for percent yield?
fruit - fish - bases
Experimental mass/theoretical mass X 100
Saturated - Substitution (which requires more radical conditions)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

39. How many normal boiling points and boiling points are there?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

40. What is the general formula for an alcohol?
basic
K2
Hg2²?
ROH

41. dihydrogen phosphate
RCOOR
H2PO4?
Big K=kf/kr
blue

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

43. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
#ligands=charge x2
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
RX
Concentration

44. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Big K=kf/kr
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
E=q + w (negative is by system - positive is on system)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

45. How are more active metals reduced?
Q=It (time in seconds)
CO (poisonous)
by electrolysis
They decrease (or could be the same if the solid has ONLY JUST disappeared)

46. For a dibasic acid (H2A) - [A²?]= ____ ?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
zero
Conjugate pair (one must be a weak base or acid)
K2

47. What are two substances that sublime at 1 atm when heated?
red - green - blue
Iodine and CO2 (dry ice)
OH?
Molecules with the same molecular formulas - but different structural formulas

48. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
CO (poisonous)
Acids; HCOOCH3 is an ester
Ksp = 27s4
voltaic: + electrolytic: -

49. acetate
NH2?
Iodine and CO2 (dry ice)
RNH2
CH3COO?

50. Where are group I metals stored?
?G= -ve - E°= +ve
Experimental mass/theoretical mass X 100
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Group I metals (soft metals) are stored under oil