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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. How does half life change for zero-th order - first order - and second order processes?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
zero-th: decreases - first: constant - second: increases
C2O4²?
H3PO4

2. What is the formula for percent error?
OH- and NH3
|experimental - accepted|/accepted X 100
Greenish-yellow gas
Insoluble

3. What do acids plus active metals form?
Soluble
Ions go through the salt bridge - electrons go through metal wires in the external circuit
?G=negative - E° must be positive
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

4. What do metal oxides plus acids form?
it is lower and occurs over less sharp a range
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
NO3?
Salt + water

5. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
CnH2n
acids
Mn²? - Cr³? - Cr³

6. hydroxides
zero
basic
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Insoluble (except group 1 ammonium and Ba)

7. What is the general formula for an acid?
Nothing
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
blue glass - it filters UV
RCOOH

8. What is the test for hydrogen?
But S° of element is not zero (except at 0K)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
lighted splint (positive result=pop)
Both electrons come from the same atom (just as good as a regular bond)

9. What is the general formula for an amine?
RNH2
Sulfur
Suniverse increases for spontaneous processes
Identity and purity (impure compounds usually have broad & low melting points)

10. What is the general formula for a ketone?
ClO4?
At half equivalence - pH=pKa
RCOR
Glowing splint (positive result=relights)

11. permanganate
Ksp = s²
basic
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
MnO4?

12. Alkanes are _________ and react by _________
Identity and purity (impure compounds usually have broad & low melting points)
Heat a test tube at an angle at the side of the tube (not bottom)
Saturated - Substitution (which requires more radical conditions)
Greenish-yellow gas

13. What is the basic structure of an optical isomer?
methyl formate
Insoluble except for nitrate and acetate
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

14. silver compounds
White precipitate
Insoluble except for nitrate and acetate
#ligands=charge x2
linear

15. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
Increases down group 1 decreases down group 17
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Silvery gray solid - brown - purple

16. Esterification is...
The one with most oxygen atoms (highest oxidation number)
acid + alcohol
Insoluble except for nitrate and acetate
The Faraday or Faraday's constant.

17. What process do you use to obtain a solvent from a solution?
O2 needs 4F/mol H2 needs 2F/mol
Distillation
?G= -ve - E°= +ve
K2

18. How do you find the pH for a dibasic acid? (H2A)?
Conjugate pair (one must be a weak base or acid)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
They stay the same.
Perform ICE BOX calculation based on K1

19. Does reactivity increase/decrease going down group 1 and group 17?
allow for the vapor pressure of water and make sure to level levels
brown volatile liquid
Increases down group 1 decreases down group 17
Anode - oxygen. Cathode - hydrogen

20. What do you do to get rid of most of the solution from a precipitate?
MnO4?
Sulfur
0 and 14
Decant

21. What is the conjugate acid of H2PO4?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Nothing
H3PO4
RNH2

22. What are two substances that sublime at 1 atm when heated?
RCOOR
Iodine and CO2 (dry ice)
benzene is less reactive than alkenes
0.10M HCl (more ions)

23. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
by electrolysis
Insoluble except group 1 and ammonium
brown volatile liquid
10?8

24. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
by electrolysis
Heat a test tube at an angle at the side of the tube (not bottom)
ethers

25. 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
Iodine and CO2 (dry ice)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
How close results are to the accepted value

26. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Cr2O7²?
no - they're written undissociated (HAaq)
Disulfur dichloride
H+

27. If a free element is involved - what type of reaction must be involved?
Salts (ex: CaO + SO2 ? CaSO3)
redox reaction
The one with most oxygen atoms (highest oxidation number)
same KE - but PEice<PEwater

28. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
OH?
OH- and NH3
Ksp = 4s³
Conjugate pair (one must be a weak base or acid)

29. chromate
An active metal.
red - green - blue
CrO4²?
allow for the vapor pressure of water and make sure to level levels

30. When is ?G zero?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
blue
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
The dilution effect when the solutions mix. M1V1 = M2V2

31. What is the general formula for alkyl halides?
Check for air bubbles in the buret and remove the buret funnel from the buret
RX
R=8.31 J/mol/K
No - it depends on the number of ions produced on dissolving.

32. iodine - iodine solution - iodine vapor
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
left - ppt will form
Silvery gray solid - brown - purple
The one with most oxygen atoms (highest oxidation number)

33. What are hybrid orbitals used for?
#ligands=charge x2
Making sigma bonds and holding lone pairs
zero
Mn²? - Cr³? - Cr³

34. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
Group 1 hydroxides (ex: NaOH)
Most INsoluble except group 1 and ammonium
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

35. Alcohols and _______ are FG isomers
Iodine and CO2 (dry ice)
ethers
P2O5
Glowing splint (positive result=relights)

36. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
It ceases - the circuit is broken.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
?H formation of an element in standard state=0

37. Is a graduated cylinder or beaker more accurate?
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.
CnH2n-2
Graduated cylinder
Ions go through the salt bridge - electrons go through metal wires in the external circuit

38. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Initiation energy (NOT Ea)
No - it depends on the number of ions produced on dissolving.
0 and 14
Clear

39. lead iodide
ROH
Decant
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
bright yellow

40. nitrate
NO3?
Iodine and CO2 (dry ice)
a-IMFs - b-molecular volume
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)

41. Nonmetals are good _____ agents. Metals are good _______ agents.
They stay the same.
metal oxides and hydrides are ionically bonded and basic
Disulfur dichloride
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

42. 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)
CnH2n+2
RX
Current - time and charge on ion (moles of e used in half cell reaction)

43. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
The dilution effect when the solutions mix. M1V1 = M2V2
10?8

44. silver iodide
But S° of element is not zero (except at 0K)
CO (poisonous)
ion pairing
Pale yellow

45. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
atoms
Soluble except Ag - Pb - Ca - Sr Ba)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

46. Acids + Carbonates (bicarbonates) make?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Hg²?

47. How do you get the equation for a net electrolysis reaction?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
a-IMFs - b-molecular volume
same KE - but PEice<PEwater
Combine the equations for the half reactions in the non-spontaneous direction

48. carbonates
Purple
linear
Insoluble except group 1 and ammonium
Decant

49. What is the relationship in strength between sigma and pi bonds?
blue
MnO4?
Sigma bonds are stronger than pi bonds
More chaotic (ex: gases made)

50. What are isotopes?
Molecules with the same molecular formulas - but different structural formulas
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Acids; HCOOCH3 is an ester
ClO4?

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AP Chemistry 2

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