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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. When can supercooling occur? What does it look like on a cooling curve?

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2. Why are i factors (Van't Hoff factors) often less than ideal?
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.
-Ea/R
Silvery gray solid - brown - purple
ion pairing

3. Is the standard entropy (S°) of an element zero?
benzene has a delocalized pi ring structure
Anode
But S° of element is not zero (except at 0K)
Eudiometer

4. How do you find the pH for a dibasic acid? (H2A)?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
The one with most oxygen atoms (highest oxidation number)
Perform ICE BOX calculation based on K1
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

5. What do you do to get rid of most of the solution from a precipitate?
proton donor base
do not change
Decant
no - they're written undissociated (HAaq)

6. hypochlorite
non-metal oxides and hydrides are covalently bonded and are acidic.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Kc=Kp
ClO?

7. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
RCOR
Separating funnel

8. What shape is water?
Greenish-yellow gas
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
bent

9. 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
zero-th: decreases - first: constant - second: increases
NH4?
Purple

10. acetate
How grouped results are
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)
CH3COO?
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

11. What is the third law of thermodynamics?
?H-kJ - ?S-J - ?G-kJ
fractional distillation
S crystal at 0K=0
same KE - but PEice<PEwater

12. copper sulfate
blue
Both electrons come from the same atom (just as good as a regular bond)
Kc=Kp
+4-covalent - +2-ionic

13. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Eudiometer
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
The one with most oxygen atoms (highest oxidation number)

14. 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?)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

15. What does a short - sharp melting point indicate?
zero
Identity and purity (impure compounds usually have broad & low melting points)
C2O4²?
small size and high charge

16. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
How close results are to the accepted value
H3PO4
Current - time and charge on ion (moles of e used in half cell reaction)

17. What do group I/II metal oxides and acids form?
The one with most oxygen atoms (highest oxidation number)
water and substances with (s) less dense than
Salt and water
an oxidized and reduced substance

18. What type of polymer is nylon?
Ksp = 4s³
Synthetic condensation polymer (aka a polyamide)
All single: sp³ - one double: sp² - two doubles: sp - one triple: sp - two single and two lone pairs: sp³ - three single and one lone pair: sp³
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

19. How do you identify which is oxidized or otherwise?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
CnH2n-2
Ionic compounds

20. How are primary alcohols turned into acids?
Check for air bubbles in the buret and remove the buret funnel from the buret
an oxidized and reduced substance
Eudiometer
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

21. Alkenes are ________ and react by __________
Mn²? - Cr³? - Cr³
Unsaturated - addition (ex: decolorize bromine solution)
Salt + water.
Identity and purity (impure compounds usually have broad & low melting points)

22. barium sulfate
Insoluble (except group 1 ammonium and Ba)
White precipitate
Read the bottom of the meniscus
methyl formate

23. What is the formula for obtaining charge flowing in a cell?
Graduated cylinder
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Q=It (time in seconds)

24. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
acid + alcohol
The benzene ring (or more correctly the phenyl group - C6H5)
Concentration
H+

25. What apparatus do you use to separate 2 immiscible liquids?
same KE - but PEice<PEwater
voltaic: + electrolytic: -
All except for lithium
Separating funnel

26. How many ligands attach to a central ion in a complex ion?
Glowing splint (positive result=relights)
Orange
#ligands=charge x2
ClO4?

27. dihydrogen phosphate
H2PO4?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Distillation

28. Why are noble gases stable?
Cu3(PO4)2
Big K=kf/kr
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
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

29. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
Most INsoluble except group 1 and ammonium
Tetrahedral
Combine the equations for the half reactions in the non-spontaneous direction

30. What changes Keq?
Soluble
Only temperature
Initiation energy (NOT Ea)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

31. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
Filtration
Heat a test tube at an angle at the side of the tube (not bottom)
?H formation of an element in standard state=0

32. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
But S° of element is not zero (except at 0K)
The compound with the lowest Ksp value.
RX

33. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
blue
acid + alcohol

34. Name some properties of Group 17
Nothing
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
H2O + CO2 (it decomposes readily)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

35. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
metal oxides and hydrides are ionically bonded and basic
Nothing

36. The definition of acidic basic and neutral aqueous solutions is:
Anode
At half equivalence - pH=pKa
Suniverse increases for spontaneous processes
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

37. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Sigma bonds are stronger than pi bonds
E=q + w (negative is by system - positive is on system)
red - green - blue

38. What is precision?
How grouped results are
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
OH- and NH3
RNH2

39. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
Greenish-yellow gas
Cu3(PO4)2
linear

40. What word is a clue for a redox reaction?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
bent
Acidified
Soluble

41. What are two substances that sublime at 1 atm when heated?
CN?
Iodine and CO2 (dry ice)
More chaotic (ex: gases made)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

42. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
No - it depends on the number of ions produced on dissolving.
CH3COO?
Sulfur

43. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
do not change
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

44. Which of the rates changes more when temperature is increased?
Decant
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Evaporation

45. How does the melting point of a mixture compare to the MP of a pure substance?

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46. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Anode - oxygen. Cathode - hydrogen
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
red - green - blue
Exothermic (?H for ANY sa/sb = -57kJ/mol)

47. What is the general formula for a ketone?
ClO4?
ns² electrons (first in-first out)
RCOR
They stay the same.

48. What do nonmetal oxides plus water form?
The dilution effect when the solutions mix. M1V1 = M2V2
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
voltaic: + electrolytic: -
acids

49. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
A) any range. b) 8-10 c) 4-6
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

50. Esters smell like _______ and amines smell like _______ and are ______.
Glowing splint (positive result=relights)
Salt and water
blue
fruit - fish - bases

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AP Chemistry 2

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