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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. Do you use J or kJ for ?H - ?S - and ?G?
it is lower and occurs over less sharp a range
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
?H-kJ - ?S-J - ?G-kJ
Current - time and charge on ion (moles of e used in half cell reaction)

2. Lattice energy is high for ions with _____ size and _____ charge
Q=It (time in seconds)
small size and high charge
Insoluble except nitrate and acetate
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

3. What causes the dramatic effect of T on rate?
linear
Exothermic
Increases down group 1 decreases down group 17
T increases exponentially the proportion of molecules with E > Ea

4. How does benzene compare in reactivity to alkenes?
Pale purple - (orange)-yellow - red - blue - green.
Glacial acetic acid
10?8
benzene is less reactive than alkenes

5. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Graduated cylinder
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

6. hydroxides
different forms of the same element
Insoluble (except group 1 ammonium and Ba)
allow for the vapor pressure of water and make sure to level levels
Salt and water

7. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
CH3COO?
Selective absorption
No - NH3 and HCl gases are extremely soluble
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

8. Color is due to ______ _______ of light.
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.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Soluble
Selective absorption

9. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Pipette (burette if need repetition)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
an oxidized and reduced substance

10. Colorless doesn't mean ______
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Clear
S crystal at 0K=0
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

11. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
CnH2n-2
0 and 14
Experimental mass/theoretical mass X 100
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

12. What is the general formula for an ester?
?G= -ve - E°= +ve
RCOOR
Pipette (burette if need repetition)
Eudiometer

13. What is the general formula for an ether?
ROR
ethers
S crystal at 0K=0
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

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

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15. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Transition element compounds (except if it has a full or empty d shell)
-Ea/R
Synthesis - separation and purification of the product and its identification.
They stay the same.

16. Acid plus base make?
P2O5
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Salt + water.
acids

17. How are strong ones written?
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.
q=mc?T q=mL (or n x ?h)
RX
strong acids/bases are written as H+ or OH- ions

18. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
?G=negative - E° must be positive
are less dense than water
ionic and form hydrogen and hydroxide

19. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Identity and purity (impure compounds usually have broad & low melting points)
K2
basic
q=mc?T q=mL (or n x ?h)

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

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21. When driving off water from a hydrate - how do you tell you're done?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Selective absorption
same KE - but PEice<PEwater
Salts (ex: CaO + SO2 ? CaSO3)

22. What is the slope of the graph of lnk vs. 1/T?
bent
look for changes in oxidation # - the one that goes up is oxidized and is the RA
-Ea/R
Pale purple - (orange)-yellow - red - blue - green.

23. What is the formula for obtaining charge flowing in a cell?
The one with most oxygen atoms (highest oxidation number)
Q=It (time in seconds)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
A salt solution.

24. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
E=q + w (negative is by system - positive is on system)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

25. Buffer capacity must contain decent amounts of a ________ ________
C4H10
Conjugate pair (one must be a weak base or acid)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Acidified

26. What element is used to vulcanize rubber?
S crystal at 0K=0
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
ns² electrons (first in-first out)
Sulfur

27. What kind of bonding structure does benzene have?
Group I metals (soft metals) are stored under oil
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
benzene has a delocalized pi ring structure
Q=It (time in seconds)

28. What type of compounds do Group 14 form?
metal oxides and hydrides are ionically bonded and basic
HClO4
+4-covalent - +2-ionic
C4H10

29. acetate
Most are soluble except Ag - Pb
CH3COO?
OH?
Eudiometer

30. What is the formula of copper (II) phosphate?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Cu3(PO4)2
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Salt + water.

31. What are two substances that sublime at 1 atm when heated?
How grouped results are
Iodine and CO2 (dry ice)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Concentration

32. What things should you remember to do when collecting gas over water?
Heat a test tube at an angle at the side of the tube (not bottom)
PO4³?
The Faraday or Faraday's constant.
allow for the vapor pressure of water and make sure to level levels

33. What is the word equation for condensation polymerisation ?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Monomer + monomer = polymer product + a simple molecule such as water or HCl

34. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
diamond and graphite
Tetrahedral
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

35. What two compounds are great oxidizing agents?

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36. What is the test for hydrogen?
Transition element compounds (except if it has a full or empty d shell)
small size and high charge
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)
lighted splint (positive result=pop)

37. acetates
do not change
RX
Anode
Soluble

38. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
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
NH4?
allow for the vapor pressure of water and make sure to level levels

39. What process do you use to separate two liquids with different boiling points?
fractional distillation
MnO4?
R=8.31 J/mol/K
ion pairing

40. phosphate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
blue
ClO?
PO4³?

41. chlorite
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Exothermic
ClO2?
The benzene ring (or more correctly the phenyl group - C6H5)

42. What is HCOOCH3?
Pale yellow
Acids; HCOOCH3 is an ester
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
E=q + w (negative is by system - positive is on system)

43. potassium permanganate
Purple
Insoluble
voltaic: + electrolytic: -
Soluble

44. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
The compound with the lowest Ksp value.
Greenish-yellow gas
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
water and substances with (s) less dense than

45. What is H2CO3 (carbonate acid) usually written as?
Saturated - Substitution (which requires more radical conditions)
Unsaturated - addition (ex: decolorize bromine solution)
Trigonal pyramidal
H2O + CO2 (it decomposes readily)

46. 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)
non-metal oxides and hydrides are covalently bonded and are acidic.
ion pairing
Cu3(PO4)2

47. How many ligands attach to a central ion in a complex ion?
ClO3?
It ceases - the circuit is broken.
#ligands=charge x2
Acidified

48. How do you get Ecell for spontaneous reactions?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
RX
Ksp = 4s³
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

49. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
ClO2?
Ksp = 108s5
Perform ICE BOX calculation based on K1

50. What is a coordinate covalent bond?
The benzene ring (or more correctly the phenyl group - C6H5)
ion pairing
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Both electrons come from the same atom (just as good as a regular bond)

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AP Chemistry 2

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