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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. When combining half equations - what do you do to E° values when multiplying coefficients?
Concentration
Sulfur
Nothing
C2O4²?

2. What are the units of the first order rate constant?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
red - green - blue
Time?¹ - (ex. s?¹ - hr?¹ - etc)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

3. potassium permanganate
CO (poisonous)
acids
But S° of element is not zero (except at 0K)
Purple

4. When driving off water from a hydrate - how do you tell you're done?
Pour liquids using a funnel or down a glass rod
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Cr2O7²?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

5. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Graduated cylinder
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

6. What is the third law of thermodynamics?
T increases exponentially the proportion of molecules with E > Ea
S crystal at 0K=0
Products - reactants (except for BDE when it's reactants - products)
H2O + CO2 (it decomposes readily)

7. Nonmetals are good _____ agents. Metals are good _______ agents.
by electrolysis
look for changes in oxidation # - the one that goes up is oxidized and is the RA
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
chemically (ex: with carbon)

8. If a free element is involved - what type of reaction must be involved?
Ionic compounds
RNH2
redox reaction
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

9. What things should you remember to do when collecting gas over water?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
allow for the vapor pressure of water and make sure to level levels
Insoluble except for nitrate and acetate
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

10. What are isomers?
q=mc?T q=mL (or n x ?h)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Molecules with the same molecular formulas - but different structural formulas
'non-active' metals such as Cu - Ag - Au - Pt - etc.

11. The oxidation # for acid base reactions...
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
do not change
0.10M HCl (more ions)
Distillation

12. When the salt bridge is removed what happens to the cell reaction?
Concentration
It ceases - the circuit is broken.
S crystal at 0K=0
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

13. What is an Alkyl group?

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14. What are the common strong bases?
Group 1 hydroxides (ex: NaOH)
Decant
Increases down group 1 decreases down group 17
C2O4²?

15. What is the general formula for an ester?
RCOOR
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.
ClO3?
blue (BTB)

16. dichromate
Cr2O7²?
atoms
allow for the vapor pressure of water and make sure to level levels
?H formation of an element in standard state=0

17. phosphates
Disulfur dichloride
Cu3(PO4)2
Evaporation
Most INsoluble except group 1 and ammonium

18. What process do you use to obtain the solute from a solution?
?H formation of an element in standard state=0
'non-active' metals such as Cu - Ag - Au - Pt - etc.
+4-covalent - +2-ionic
Evaporation

19. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
do not change
Soluble
RX
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.

20. How do you heat a test tube?
Insoluble except for nitrate and acetate
zero
E=q + w (negative is by system - positive is on system)
Heat a test tube at an angle at the side of the tube (not bottom)

21. What type of polymer is nylon?
zero
Pale yellow
Cr2O7²?
Synthetic condensation polymer (aka a polyamide)

22. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Current - time and charge on ion (moles of e used in half cell reaction)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
The compound with the lowest Ksp value.
Acid rain - dissolves marble buildings/statues and kills trees.

23. Esters smell like _______ and amines smell like _______ and are ______.
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
strong acids/bases are written as H+ or OH- ions
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)
fruit - fish - bases

24. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Salt and water
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

25. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
But S° of element is not zero (except at 0K)
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

26. What are hybrid orbitals used for?
ROH
Making sigma bonds and holding lone pairs
Pour liquids using a funnel or down a glass rod
fruit - fish - bases

27. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
benzene has a delocalized pi ring structure
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
water and substances with (s) less dense than
Big K=kf/kr

28. What changes Keq?
Only temperature
Insoluble except nitrate and acetate
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
a-IMFs - b-molecular volume

29. Ions are not ______.
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
10?8
blue
atoms

30. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
CO (poisonous)
an oxidized and reduced substance
Synthetic condensation polymer (aka a polyamide)

31. What two compounds are great oxidizing agents?

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32. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
A) any range. b) 8-10 c) 4-6
ClO3?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
do not change

33. halides
Most are soluble except Ag - Pb
NH4?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Most INsoluble except group 1 and ammonium

34. What is the formula for obtaining charge flowing in a cell?
The dilution effect when the solutions mix. M1V1 = M2V2
Selective absorption
Q=It (time in seconds)
red - green - blue

35. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
Distillation
voltaic: + electrolytic: -
ion pairing

36. What are amphoteric oxides?
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
Group I metals (soft metals) are stored under oil
Kc=Kp
Soluble

37. What type of compounds are almost always colored?
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.
More chaotic (ex: gases made)
Transition element compounds (except if it has a full or empty d shell)
[A?]/[HA] x 100 or [BH?]/[B] x 100

38. What reacts with an acid to create hydrogen gas?
do not change
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Hg2²?
An active metal.

39. What are allotropes?
[A?]/[HA] x 100 or [BH?]/[B] x 100
RCOR
different forms of the same element
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

40. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
an oxidized and reduced substance
Silvery gray solid - brown - purple
same KE - but PEice<PEwater
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

41. silver iodide
HClO4
Pale yellow
zero
Hg²?

42. What do ions and electrons travel through in a voltaic/electrolytic cell?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Ions go through the salt bridge - electrons go through metal wires in the external circuit
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

43. What process do you use to obtain the precipitate from a solution?
Filtration
|experimental - accepted|/accepted X 100
Heptane
redox reaction

44. nitrate
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
NO3?
?H-kJ - ?S-J - ?G-kJ
S crystal at 0K=0

45. Does Kw increase or decrease with T? Why?
OH- and NH3
Group I metals (soft metals) are stored under oil
ROR
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

46. Name six characteristics of transition elements (or their compounds)
ns² electrons (first in-first out)
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)
bent
boiling without losing volatile solvents/reactants

47. What is H2CO3 (carbonate acid) usually written as?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
P2O5
H2O + CO2 (it decomposes readily)
fractional distillation

48. What do you use to look at burning magnesium? why?
blue glass - it filters UV
CnH2n
CN?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

49. What are the products of the reaction between group 1 metals and water?

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50. Why are i factors (Van't Hoff factors) often less than ideal?
At half equivalence - pH=pKa
proton donor base
ion pairing
Pipette (burette if need repetition)

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AP Chemistry 2

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