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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 do you need to make a polymer?
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)
Decant
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

2. chromate
CrO4²?
CnH2n-2
Pipette (burette if need repetition)
Pour liquids using a funnel or down a glass rod

3. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
Anode
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
R=8.31 J/mol/K

4. What is the name of S2Cl2? (Know how to name others like this - too)
allow for the vapor pressure of water and make sure to level levels
Pour liquids using a funnel or down a glass rod
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Disulfur dichloride

5. 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
CO (poisonous)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
a-IMFs - b-molecular volume

6. How do you get the equation for a net electrolysis reaction?
RNH2
Tetrahedral
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Combine the equations for the half reactions in the non-spontaneous direction

7. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
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)
Pipette (burette if need repetition)

8. What is the formula for alkenes?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
10?8
CnH2n
CN?

9. If Q > Ksp - then system shifts _______ and ppt ______
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.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
left - ppt will form

10. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
A salt solution.
[A?]/[HA] x 100 or [BH?]/[B] x 100
Mono; di; tri; tetra; penta; hexa.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

11. perchlorate
water and substances with (s) less dense than
The benzene ring (or more correctly the phenyl group - C6H5)
Group I metals (soft metals) are stored under oil
ClO4?

12. phosphates
Mn²? - Cr³? - Cr³
Most INsoluble except group 1 and ammonium
Unsaturated - addition (ex: decolorize bromine solution)
proton donor base

13. What is HCOOCH3?
Acids; HCOOCH3 is an ester
More chaotic (ex: gases made)
Tetrahedral
ion pairing

14. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
same KE - but PEice<PEwater
yellow
zero

15. What should you check for before you begin titrating?
At half equivalence - pH=pKa
Big K=kf/kr
Acid rain - dissolves marble buildings/statues and kills trees.
Check for air bubbles in the buret and remove the buret funnel from the buret

16. What type of polymer is nylon?
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.
Synthetic condensation polymer (aka a polyamide)
Silvery gray solid - brown - purple
Conjugate pair (one must be a weak base or acid)

17. Why are i factors (Van't Hoff factors) often less than ideal?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Soluble
diamond and graphite
ion pairing

18. What is the formula for obtaining charge flowing in a cell?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Q=It (time in seconds)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
benzene has a delocalized pi ring structure

19. How do you identify which is oxidized or otherwise?
Big K=kf/kr
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Salts (ex: CaO + SO2 ? CaSO3)
H+

20. What are allotropes?
voltaic: - electrolytic: +
Suniverse increases for spontaneous processes
different forms of the same element
small size and high charge

21. What do the 'a' and 'b' in Van Der Waal's equation allow for?
CN?
a-IMFs - b-molecular volume
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
redox reaction

22. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Glowing splint (positive result=relights)
Ionic compounds
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.

23. During a titration what is present in the beaker at the equivalence point?
different forms of the same element
A salt solution.
chemically (ex: with carbon)
Acid rain - dissolves marble buildings/statues and kills trees.

24. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
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)
Salt and water
P2O5
CH3COO?

25. acetates
Soluble
Insoluble except group 1 and ammonium
hydroxides (ex: Ba(OH)2)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

26. What are the signs of ?G and E° for spontaneous reactions?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
?G=negative - E° must be positive
q=mc?T q=mL (or n x ?h)

27. An amphiprotic (amphoteric) species is...
RCOR
blue (BTB)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Read the bottom of the meniscus

28. Alkenes are ________ and react by __________
C2O4²?
Ksp = 27s4
Unsaturated - addition (ex: decolorize bromine solution)
Exothermic

29. 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.
Read the bottom of the meniscus
A) any range. b) 8-10 c) 4-6
An active metal.
NH2?

30. Is the standard entropy (S°) of an element zero?
Acid rain - dissolves marble buildings/statues and kills trees.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
by electrolysis
But S° of element is not zero (except at 0K)

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

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32. 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
bright yellow
allow for the vapor pressure of water and make sure to level levels
ROH

33. How many faradays of electric charge do you need to produce one mole of O2? H2?
bright yellow
O2 needs 4F/mol H2 needs 2F/mol
Hg²?
All single: sp³ - one double: sp² - two doubles: sp - one triple: sp - two single and two lone pairs: sp³ - three single and one lone pair: sp³

34. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
The benzene ring (or more correctly the phenyl group - C6H5)
Salt and water
acid + alcohol

35. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Mono; di; tri; tetra; penta; hexa.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Identity and purity (impure compounds usually have broad & low melting points)

36. copper sulfate
CN?
H3PO4
boiling without losing volatile solvents/reactants
blue

37. Where are group I metals stored?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Group I metals (soft metals) are stored under oil
Greenish-yellow gas
H+

38. Name 2 ways in which you can create a buffer?
Trigonal pyramidal
CO3²?
K1 x K2
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)

39. Is the freezing of ice endothermic or exothermic?
Glowing splint (positive result=relights)
Exothermic
Iodine and CO2 (dry ice)
How grouped results are

40. carbonates
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.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Insoluble except group 1 and ammonium
blue

41. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Salt + water
Insoluble
Big K=kf/kr

42. Is the ?H formation of an element in standard state zero?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
?H formation of an element in standard state=0
do not change
Increases down group 1 decreases down group 17

43. Esterification is...
Cr2O7²?
P2O5
ns² electrons (first in-first out)
acid + alcohol

44. What is the general formula for an alcohol?
Cr2O7²?
Insoluble
ROH
No - it depends on the number of ions produced on dissolving.

45. What are the common strong bases?
|experimental - accepted|/accepted X 100
redox reaction
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Group 1 hydroxides (ex: NaOH)

46. What word is a clue for a redox reaction?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Acidified
?H-kJ - ?S-J - ?G-kJ

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

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48. When is ?G zero?
C2O4²?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Mn²? - Cr³? - Cr³
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

49. What is a coordinate covalent bond?
Suniverse increases for spontaneous processes
Both electrons come from the same atom (just as good as a regular bond)
water and substances with (s) less dense than
Insoluble

50. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
#ligands=charge x2
boiling without losing volatile solvents/reactants
RCOOH