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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 changes Keq?
Only temperature
Salt + water
Graduated cylinder
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

2. What is the general formula for an aldehyde?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
diamond and graphite
S crystal at 0K=0
RCHO (carbonyl at end)

3. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Unsaturated - addition (ex: decolorize bromine solution)
Increases.
RCOR

4. What do hydrocarbons form when they burn in air (oxygen)?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CO2 and H2O
hydroxides (ex: Ba(OH)2)
linear

5. What apparatus do you use to separate 2 immiscible liquids?
left - ppt will form
Separating funnel
Ksp = 108s5
zero

6. What shape is methane?
Conjugate pair (one must be a weak base or acid)
CnH2n+2
brown volatile liquid
Tetrahedral

7. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
[A?]/[HA] x 100 or [BH?]/[B] x 100
Concentration
Ksp = 27s4

8. Acidic gases like SO2 in the atmosphere cause what environmental problems?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Salt + water
fractional distillation
Acid rain - dissolves marble buildings/statues and kills trees.

9. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
zero
RCOOH
K1 x K2

10. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
They stay the same.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
H3PO4
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

11. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
The benzene ring (or more correctly the phenyl group - C6H5)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
OH- and NH3
Mn²? - Cr³? - Cr³

12. What part of a liquid do you look at to measure its volume?
How grouped results are
small size and high charge
Read the bottom of the meniscus
Both electrons come from the same atom (just as good as a regular bond)

13. 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
ClO?
[A?]/[HA] x 100 or [BH?]/[B] x 100
blue

14. BaSO4
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
water and substances with (s) less dense than
are less dense than water
Insoluble

15. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
CO3²?
Only temperature
#ligands=charge x2

16. How do you find the pH for a dibasic acid? (H2A)?
Perform ICE BOX calculation based on K1
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
CO3²?
acids

17. Are weak acids (and bases) written dissociated?

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18. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
Sigma bonds are stronger than pi bonds
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

19. What are the common strong bases?
same KE - but PEice<PEwater
Synthesis - separation and purification of the product and its identification.
Group 1 hydroxides (ex: NaOH)
lighted splint (positive result=pop)

20. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Anode - oxygen. Cathode - hydrogen
0.10M HCl (more ions)
CO (poisonous)
All except for lithium

21. What is the formula for alkenes?
CnH2n
Pale yellow
The one with most oxygen atoms (highest oxidation number)
do not change

22. What steps do organic labs consist of?
zero
H2PO4?
ion pairing
Synthesis - separation and purification of the product and its identification.

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

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24. What are the formulas for q?
Orange
q=mc?T q=mL (or n x ?h)
CN?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

25. Where are group I metals stored?
Group I metals (soft metals) are stored under oil
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
A) any range. b) 8-10 c) 4-6
catalyst=conc H2SO4

26. What things should you remember to do when collecting gas over water?
At half equivalence - pH=pKa
allow for the vapor pressure of water and make sure to level levels
OH- and NH3
Salt + water

27. What is an Alkyl group?

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28. What word is a clue for a redox reaction?
Acidified
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.
CN?
Clear

29. What do nonmetal oxides plus water form?
acids
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
zero
NH4?

30. Is the freezing of ice endothermic or exothermic?
ion pairing
H+
Exothermic
Both electrons come from the same atom (just as good as a regular bond)

31. chromate ion (soln + most solids)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
bases
yellow
ClO3?

32. What is the formula for alkanes?
CnH2n+2
Insoluble
hydroxides (ex: Ba(OH)2)
different forms of the same element

33. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
An active metal.
P2O5
PO4³?

34. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
R=8.31 J/mol/K
fruit - fish - bases
Read the bottom of the meniscus

35. Name some properties of Group 17
Mono; di; tri; tetra; penta; hexa.
CnH2n-2
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
different forms of the same element

36. ammonium
Silvery gray solid - brown - purple
CnH2n+1 often designated 'R' ex C3H7 is propyl
#ligands=charge x2
NH4?

37. What is the basic structure of an optical isomer?
The Faraday or Faraday's constant.
voltaic: - electrolytic: +
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
ROR

38. copper sulfate
Soluble
C4H10
Iodine and CO2 (dry ice)
blue

39. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
same KE - but PEice<PEwater
OH?
Monomer + monomer = polymer product + a simple molecule such as water or HCl

40. What is the slope of the graph of lnk vs. 1/T?
H3PO4
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
-Ea/R
How grouped results are

41. What does a short - sharp melting point indicate?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Identity and purity (impure compounds usually have broad & low melting points)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Heat a test tube at an angle at the side of the tube (not bottom)

42. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
CnH(2n+2)
water and substances with (s) less dense than
atoms

43. How do you get the equation for a net electrolysis reaction?
How close results are to the accepted value
it is lower and occurs over less sharp a range
Clear
Combine the equations for the half reactions in the non-spontaneous direction

44. Colorless doesn't mean ______
voltaic: - electrolytic: +
Purple
Synthesis - separation and purification of the product and its identification.
Clear

45. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Products - reactants (except for BDE when it's reactants - products)
Synthetic condensation polymer (aka a polyamide)

46. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Insoluble except for nitrate and acetate
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
H3PO4

47. Is a graduated cylinder or beaker more accurate?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Graduated cylinder
Nothing

48. How does group 1 metals' density compare to water's?
The Faraday or Faraday's constant.
redox reaction
are less dense than water
+4-covalent - +2-ionic

49. A geometric (or cis-trans) isomer exists due to.....
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
CO (poisonous)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

50. What are amphoteric oxides?
Initiation energy (NOT Ea)
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?)
Disulfur dichloride
Glacial acetic acid