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AP Chemistry 2

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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. Color is due to ______ _______ of light.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
It ceases - the circuit is broken.
CO3²?
Selective absorption

2. dichromate (soln + most solids)
?H formation of an element in standard state=0
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
S2O3²?
Orange

3. When combining half equations - what do you do to E° values when multiplying coefficients?
Ksp = 27s4
Salts (ex: CaO + SO2 ? CaSO3)
Nothing
-Ea/R

4. 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.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
A) any range. b) 8-10 c) 4-6
Most are soluble except Ag - Pb

5. What is the test for hydrogen?
lighted splint (positive result=pop)
ClO3?
Ksp = 4s³
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

6. What is the general formula for alkyl halides?
It ceases - the circuit is broken.
bright yellow
fractional distillation
RX

7. Is a graduated cylinder or beaker more accurate?
non-metal oxides and hydrides are covalently bonded and are acidic.
Glowing splint (positive result=relights)
fractional distillation
Graduated cylinder

8. Why are i factors (Van't Hoff factors) often less than ideal?
A salt solution.
lighted splint (positive result=pop)
ion pairing
The Faraday or Faraday's constant.

9. What is the basic structure of an optical isomer?
chemically (ex: with carbon)
Only temperature
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Acids; HCOOCH3 is an ester

10. What causes the dramatic effect of T on rate?
bent
CrO4²?
T increases exponentially the proportion of molecules with E > Ea
Group 1 hydroxides (ex: NaOH)

11. What is the general formula for an alcohol?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Synthetic condensation polymer (aka a polyamide)
ROH
Both electrons come from the same atom (just as good as a regular bond)

12. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
Orange
ClO?
Ksp = 27s4

13. If Q > Ksp - then system shifts _______ and ppt ______
All except for lithium
left - ppt will form
RNH2
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

14. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
zero
RX
0 and 14

15. Ions are not ______.
atoms
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Disulfur dichloride
basic

16. acetate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
CH3COO?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
strong acids/bases are written as H+ or OH- ions

17. How do you compute % dissociation?
Pipette (burette if need repetition)
[A?]/[HA] x 100 or [BH?]/[B] x 100
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Soluble

18. group 1 ions/compounds
Anode - oxygen. Cathode - hydrogen
Exothermic (?H for ANY sa/sb = -57kJ/mol)
CO2 and H2O
Soluble

19. How do you find the pH for a dibasic acid? (H2A)?
Cr2O7²?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Perform ICE BOX calculation based on K1
Time?¹ - (ex. s?¹ - hr?¹ - etc)

20. A geometric (or cis-trans) isomer exists due to.....
+4-covalent - +2-ionic
it's lower and occurs over less sharp a range
Ionic compounds
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

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

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22. carbonate
Insoluble except nitrate and acetate
CO3²?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
it reacts by substitution NOT addition

23. How do you identify which is oxidized or otherwise?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

24. Alcohols and _______ are FG isomers
do not change
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
ethers
CH3COO?

25. What is H2CO3 (carbonate acid) usually written as?
Ksp = s²
But S° of element is not zero (except at 0K)
MnO4?
H2O + CO2 (it decomposes readily)

26. How does the melting point of a mixture compare to the MP of a pure substance?
More chaotic (ex: gases made)
it is lower and occurs over less sharp a range
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
left - ppt will form

27. During a titration what is present in the beaker at the equivalence point?
Combine the equations for the half reactions in the non-spontaneous direction
#ligands=charge x2
blue glass - it filters UV
A salt solution.

28. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Transition element compounds (except if it has a full or empty d shell)
Greenish-yellow gas
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

29. Why are noble gases stable?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Glowing splint (positive result=relights)
benzene has a delocalized pi ring structure

30. Name 2 ways in which you can create a buffer?
Silvery gray solid - brown - purple
Hg²?
no - they're written undissociated (HAaq)
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)

31. How many ligands attach to a central ion in a complex ion?
R=8.31 J/mol/K
#ligands=charge x2
A salt solution.
Orange

32. ________ are Lewis bases - because they can donate a lone pair of electrons.
yellow
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)
OH- and NH3
water and substances with (s) less dense than

33. What are the signs of ?G and E° for spontaneous reactions?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
are less dense than water
?G=negative - E° must be positive
Current - time and charge on ion (moles of e used in half cell reaction)

34. bromothymol
blue (BTB)
White precipitate
RCOOH
chemically (ex: with carbon)

35. What do you do to get rid of most of the solution from a precipitate?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
RNH2
Decant
brown volatile liquid

36. What do group I/II metal oxides and acids form?
diamond and graphite
Exothermic
?H formation of an element in standard state=0
Salt and water

37. hydroxides
red - green - blue
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Insoluble (except group 1 ammonium and Ba)
CnH2n+1 often designated 'R' ex C3H7 is propyl

38. If a weak acid is diluted more - what happens to its % dissociation value?
Decant
CO (poisonous)
Kc=Kp
Increases.

39. What are the common strong bases?
Kc=Kp
Insoluble except group 1 and ammonium
E=q + w (negative is by system - positive is on system)
Group 1 hydroxides (ex: NaOH)

40. How do you heat a test tube?
They stay the same.
Heat a test tube at an angle at the side of the tube (not bottom)
RCOOH
no - they're written undissociated (HAaq)

41. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
Clear
lighted splint (positive result=pop)
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.

42. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
K1 x K2
different forms of the same element
Distillation

43. halides
?G=negative - E° must be positive
Most INsoluble except group 1 and ammonium
Most are soluble except Ag - Pb
Making sigma bonds and holding lone pairs

44. sulfate
SO4²?
Pipette (burette if need repetition)
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.

45. Do anions flow to the cathode or anode?
CnH2n-2
Group 1 hydroxides (ex: NaOH)
Anode
?G=negative - E° must be positive

46. Do you use J or kJ for ?H - ?S - and ?G?
bases
?H-kJ - ?S-J - ?G-kJ
Synthesis - separation and purification of the product and its identification.
Insoluble

47. chlorate
ClO3?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Insoluble except group 1 and ammonium

48. Both Acetic acid and ____________ are also functional isomers.
Soluble
Disulfur dichloride
Initiation energy (NOT Ea)
methyl formate

49. chromate ion (soln + most solids)
Saturated - Substitution (which requires more radical conditions)
water and substances with (s) less dense than
voltaic: - electrolytic: +
yellow

50. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
Insoluble (except group 1 ammonium and Ba)
Distillation
an oxidized and reduced substance

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AP Chemistry 2

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