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

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2. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
RCOR
?G= -ve - E°= +ve
Kc=Kp
Purple

3. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
They stay the same.
White precipitate
Silvery gray solid - brown - purple

4. What is the catalyst for this reaction Ester + ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
by electrolysis
catalyst=conc H2SO4
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

5. How do you explain trends in atomic properties using Coulomb's Law?
are less dense than water
H+
proton acceptor.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

6. sulfate
Heptane
H2PO4?
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)
SO4²?

7. silver iodide
linear
same KE - but PEice<PEwater
Pale yellow
Evaporation

8. What is the general formula of an alkane?
Nothing
CnH(2n+2)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Products - reactants (except for BDE when it's reactants - products)

9. mercury (I) ion
ROH
Pour liquids using a funnel or down a glass rod
Ppt will NOT form (unsaturated)
Hg2²?

10. Give an example of a dilute strong acid.
T increases exponentially the proportion of molecules with E > Ea
HClO4
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
chemically (ex: with carbon)

11. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
Q=It (time in seconds)
#ligands=charge x2
Concentration

12. What do group I/II metal oxides plus water form?
NH2?
More chaotic (ex: gases made)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
bases

13. What are two allotropes of carbon?
diamond and graphite
Acid rain - dissolves marble buildings/statues and kills trees.
allow for the vapor pressure of water and make sure to level levels
Ksp = 4s³

14. Buffer capacity must contain decent amounts of a ________ ________
blue glass - it filters UV
#ligands=charge x2
Conjugate pair (one must be a weak base or acid)
Hg²?

15. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
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.
Salt + water.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

16. During a titration what is present in the beaker at the equivalence point?
A salt solution.
How grouped results are
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)
Iodine and CO2 (dry ice)

17. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
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
hydroxides (ex: Ba(OH)2)
Iodine and CO2 (dry ice)

18. How do you get the equation for a net electrolysis reaction?
The Faraday or Faraday's constant.
Most are soluble except Ag - Pb
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.
Combine the equations for the half reactions in the non-spontaneous direction

19. What is reflux?
ethers
boiling without losing volatile solvents/reactants
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
The benzene ring (or more correctly the phenyl group - C6H5)

20. acetate
ionic and form hydrogen and hydroxide
Clear
CH3COO?
Ions go through the salt bridge - electrons go through metal wires in the external circuit

21. chlorine
All except for lithium
Greenish-yellow gas
same KE - but PEice<PEwater
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

22. What is the relationship in strength between sigma and pi bonds?
Insoluble (except group 1 ammonium and Ba)
Sigma bonds are stronger than pi bonds
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Mn²? - Cr³? - Cr³

23. Why are noble gases stable?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Group I metals (soft metals) are stored under oil
OH?
C4H10

24. Both Acetic acid and ____________ are also functional isomers.
E=q + w (negative is by system - positive is on system)
strong acids/bases are written as H+ or OH- ions
CO3²?
methyl formate

25. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
zero
Exothermic
RCOOH

26. A Bronsted-Lowry base is...
brown volatile liquid
voltaic: - electrolytic: +
Most INsoluble except group 1 and ammonium
proton acceptor.

27. chlorite
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Read the bottom of the meniscus
proton acceptor.
ClO2?

28. 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.
Orange
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
?G=negative - E° must be positive
A) any range. b) 8-10 c) 4-6

29. carbonates
Pour liquids using a funnel or down a glass rod
Heat a test tube at an angle at the side of the tube (not bottom)
zero-th: decreases - first: constant - second: increases
Insoluble except group 1 and ammonium

30. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
Pale yellow
[A?]/[HA] x 100 or [BH?]/[B] x 100
CrO4²?

31. What do group I/II metal oxides and acids form?
Insoluble except group 1 and ammonium
Soluble
Pale yellow
Salt and water

32. hydroxides
Sulfur
bent
Insoluble (except group 1 ammonium and Ba)
Cr2O7²?

33. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Conjugate pair (one must be a weak base or acid)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
ClO4?
[A?]/[HA] x 100 or [BH?]/[B] x 100

34. What are the signs of ?G and E° for spontaneous reactions?
Tetrahedral
bright yellow
NH2?
?G=negative - E° must be positive

35. What is the charge on a chlorine atom?
H2O + CO2 (it decomposes readily)
Add acid to water so that the acid doesn't boil and spit
zero
Unsaturated - addition (ex: decolorize bromine solution)

36. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Pipette (burette if need repetition)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

37. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
Read the bottom of the meniscus
RCOOR
a-IMFs - b-molecular volume

38. Is the freezing of ice endothermic or exothermic?
T increases exponentially the proportion of molecules with E > Ea
Exothermic
Ksp = 108s5
HClO4

39. What do you do to get rid of most of the solution from a precipitate?
Filtration
Mono; di; tri; tetra; penta; hexa.
SO4²?
Decant

40. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Orange
R=8.31 J/mol/K
water and substances with (s) less dense than

41. What is an Alkyl group?

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42. What is the formula for alkynes?
Heptane
Transition element compounds (except if it has a full or empty d shell)
-Ea/R
CnH2n-2

43. How do you find the pH for a dibasic acid? (H2A)?
left - ppt will form
CN?
Pour liquids using a funnel or down a glass rod
Perform ICE BOX calculation based on K1

44. Nonmetals are good _____ agents. Metals are good _______ agents.
The dilution effect when the solutions mix. M1V1 = M2V2
At half equivalence - pH=pKa
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
benzene has a delocalized pi ring structure

45. How do you clean a buret/pipette for a titration?
E=q + w (negative is by system - positive is on system)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
The Faraday or Faraday's constant.
HClO4

46. dichromate
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Cr2O7²?
?H-kJ - ?S-J - ?G-kJ
Ksp = 108s5

47. How many ligands attach to a central ion in a complex ion?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
#ligands=charge x2
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
ClO3?

48. chromate
CnH2n+1 often designated 'R' ex C3H7 is propyl
CrO4²?
voltaic: - electrolytic: +
No - it depends on the number of ions produced on dissolving.

49. What is the first law of thermodynamics?
S crystal at 0K=0
Insoluble except nitrate and acetate
E=q + w (negative is by system - positive is on system)
0 and 14

50. bromothymol
Ksp = 108s5
CnH2n
Add acid to water so that the acid doesn't boil and spit
blue (BTB)

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AP Chemistry 2

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