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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. What measuring device would you use for very small volumes of liquids?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
10?8
Pipette (burette if need repetition)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

2. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Soluble
methyl formate
CrO4²?
water and substances with (s) less dense than

3. What type of compounds do Group 14 form?
+4-covalent - +2-ionic
K2
Perform ICE BOX calculation based on K1
Nothing

4. If Q > Ksp - then system shifts _______ and ppt ______
basic
O2 needs 4F/mol H2 needs 2F/mol
it is lower and occurs over less sharp a range
left - ppt will form

5. potassium permanganate
Group 1 hydroxides (ex: NaOH)
diamond and graphite
Purple
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

6. What is the formula for alkanes?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
CnH2n+2
MnO4?
No - NH3 and HCl gases are extremely soluble

7. What are hybrid orbitals used for?
redox reaction
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Making sigma bonds and holding lone pairs

8. How are strong ones written?
red - green - blue
strong acids/bases are written as H+ or OH- ions
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

9. Colorless doesn't mean ______
Clear
ClO2?
lighted splint (positive result=pop)
Read the bottom of the meniscus

10. What type of polymer is nylon?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Synthetic condensation polymer (aka a polyamide)
ion pairing
Insoluble (except group 1 ammonium and Ba)

11. Name six characteristics of transition elements (or their compounds)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
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)
OH?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

12. mercury (II) ion
Hg²?
diamond and graphite
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Check for air bubbles in the buret and remove the buret funnel from the buret

13. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
CnH2n+2
-Ea/R
water and substances with (s) less dense than
Glacial acetic acid

14. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
Big K=kf/kr
red - green - blue
q=mc?T q=mL (or n x ?h)

15. How are primary alcohols turned into acids?
No - NH3 and HCl gases are extremely soluble
All except for lithium
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Pipette (burette if need repetition)

16. What do you use to look at burning magnesium? why?
ion pairing
Molecules with the same molecular formulas - but different structural formulas
diamond and graphite
blue glass - it filters UV

17. Ca - Sr - Ba
K1 x K2
hydroxides (ex: Ba(OH)2)
catalyst=conc H2SO4
Pipette (burette if need repetition)

18. When driving off water from a hydrate - how do you tell you're done?
?G= -ve - E°= +ve
Pour liquids using a funnel or down a glass rod
chemically (ex: with carbon)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

19. copper sulfate
Ppt will NOT form (unsaturated)
blue
How grouped results are
ns² electrons (first in-first out)

20. dichromate (soln + most solids)
left - ppt will form
Orange
Suniverse increases for spontaneous processes
Both electrons come from the same atom (just as good as a regular bond)

21. What are the prefixes for the naming of binary molecular compound formulas (up to six)
fractional distillation
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Mono; di; tri; tetra; penta; hexa.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

22. ammonium
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
NH4?
Pipette (burette if need repetition)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

23. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
CO (poisonous)
Mn²? - Cr³? - Cr³

24. What things should you remember to do when collecting gas over water?
Anode - oxygen. Cathode - hydrogen
zero
allow for the vapor pressure of water and make sure to level levels
methyl formate

25. What is the general formula for an aldehyde?
C4H10
E=q + w (negative is by system - positive is on system)
Sulfur
RCHO (carbonyl at end)

26. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Soluble
Trigonal pyramidal
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Ppt will NOT form (unsaturated)

27. An amphiprotic (amphoteric) species is...
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
#ligands=charge x2
ClO2?

28. What element is used to vulcanize rubber?
NH2?
Orange
Mono; di; tri; tetra; penta; hexa.
Sulfur

29. halides
redox reaction
Most are soluble except Ag - Pb
Check for air bubbles in the buret and remove the buret funnel from the buret
acid + alcohol

30. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
?H formation of an element in standard state=0
Insoluble except nitrate and acetate
Most INsoluble except group 1 and ammonium
same KE - but PEice<PEwater

31. What is the general formula for an ether?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
ROR
?H formation of an element in standard state=0
water and substances with (s) less dense than

32. What is the conjugate acid of H2PO4?
Nothing
basic
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
H3PO4

33. What is accuracy?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Read the bottom of the meniscus
How close results are to the accepted value
zero

34. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Read the bottom of the meniscus
RCOOH
water and substances with (s) less dense than

35. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
a-IMFs - b-molecular volume
RCOOH
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.

36. Can you collect soluble gases over water?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
No - NH3 and HCl gases are extremely soluble
Group I metals (soft metals) are stored under oil
CN?

37. What is the general formula for an amine?
voltaic: + electrolytic: -
RNH2
brown volatile liquid
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

38. Does Kw increase or decrease with T? Why?
An active metal.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
an oxidized and reduced substance
fruit - fish - bases

39. How are metal oxides and hydrides bonded? are they acidic or basic?
bright yellow
same KE - but PEice<PEwater
metal oxides and hydrides are ionically bonded and basic
OH- and NH3

40. Color (absorbance) is proportional to ________
0.10M HCl (more ions)
MnO4?
Soluble
Concentration

41. What is the conjugate base of NH3?
-Ea/R
E=q + w (negative is by system - positive is on system)
Evaporation
NH2?

42. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
Anode - oxygen. Cathode - hydrogen
Reduction always takes place at the cathode (RED CAT) In both types of cell!
MnO4?

43. ________ are Lewis bases - because they can donate a lone pair of electrons.
RNH2
Most are soluble except Ag - Pb
Insoluble except nitrate and acetate
OH- and NH3

44. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Most INsoluble except group 1 and ammonium
HClO4
Insoluble except nitrate and acetate

45. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
A salt solution.
no - they're written undissociated (HAaq)
linear
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

46. When the salt bridge is removed what happens to the cell reaction?
Soluble except Ag - Pb - Ca - Sr Ba)
Heat a test tube at an angle at the side of the tube (not bottom)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
It ceases - the circuit is broken.

47. Which would cause the bulb in a conductivity apparatus to be brightest?
0 and 14
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)
0.10M HCl (more ions)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

48. What is a coordinate covalent bond?
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
Both electrons come from the same atom (just as good as a regular bond)
Cr2O7²?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

49. What is the difference between equivalence point and end point of a titration.
yellow
Eudiometer
Ksp = s²
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

50. What is H2CO3 (carbonate acid) usually written as?
left - ppt will form
H2O + CO2 (it decomposes readily)
diamond and graphite
blue glass - it filters UV

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AP Chemistry 2

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