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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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 is a dipeptide? polypeptide? protein?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Iodine and CO2 (dry ice)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

2. What shape is carbon dioxide?
by electrolysis
Hg²?
linear
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)

3. What is the test for oxygen?
Glowing splint (positive result=relights)
hydroxides (ex: Ba(OH)2)
A salt solution.
Salt and water

4. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
water and substances with (s) less dense than
No - it depends on the number of ions produced on dissolving.
RCOOH
More chaotic (ex: gases made)

5. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
Mn²? - Cr³? - Cr³
Combine the equations for the half reactions in the non-spontaneous direction
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

6. How are more active metals reduced?
Mono; di; tri; tetra; penta; hexa.
Ksp = 27s4
water and substances with (s) less dense than
by electrolysis

7. Is a graduated cylinder or beaker more accurate?
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.
Graduated cylinder
Iodine and CO2 (dry ice)
linear

8. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
A) any range. b) 8-10 c) 4-6
?H formation of an element in standard state=0
|experimental - accepted|/accepted X 100
Distillation

9. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Ksp = 27s4
same KE - but PEice<PEwater
catalyst=conc H2SO4
red - green - blue

10. What apparatus do you use to separate 2 immiscible liquids?
CH3COO?
Separating funnel
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
blue

11. Does Kw increase or decrease with T? Why?
lighted splint (positive result=pop)
CnH(2n+2)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
an oxidized and reduced substance

12. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Group 1 hydroxides (ex: NaOH)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
K1 x K2
basic

13. chromate ion (soln + most solids)
yellow
Decant
same KE - but PEice<PEwater
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

14. Esterification is...
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Salt + water.
red - green - blue
acid + alcohol

15. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Increases down group 1 decreases down group 17
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

16. permanganate
methyl formate
Eudiometer
MnO4?
RCOR

17. copper sulfate
blue
Hg2²?
Pour liquids using a funnel or down a glass rod
acid + alcohol

18. When is ?G zero?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
At half equivalence - pH=pKa
No - it depends on the number of ions produced on dissolving.

19. What is HCOOCH3?
CN?
PO4³?
-Ea/R
Acids; HCOOCH3 is an ester

20. iodine - iodine solution - iodine vapor
non-metal oxides and hydrides are covalently bonded and are acidic.
Silvery gray solid - brown - purple
Mn²? - Cr³? - Cr³
CnH2n

21. What process do you use to obtain a solvent from a solution?
Soluble
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Distillation
water and substances with (s) less dense than

22. What are two substances that sublime at 1 atm when heated?
#ligands=charge x2
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Iodine and CO2 (dry ice)

23. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
water and substances with (s) less dense than
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.
strong acids/bases are written as H+ or OH- ions

24. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
C2O4²?
Iodine and CO2 (dry ice)

25. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
do not change
Insoluble (except group 1 ammonium and Ba)
Saturated - Substitution (which requires more radical conditions)
Insoluble except group 1 and ammonium

26. What is the formula of butane?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
C4H10
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

27. What shape is methane?
Tetrahedral
Glacial acetic acid
ClO2?
Making sigma bonds and holding lone pairs

28. What is reflux?
boiling without losing volatile solvents/reactants
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Identity and purity (impure compounds usually have broad & low melting points)
H2O + CO2 (it decomposes readily)

29. The definition of acidic basic and neutral aqueous solutions is:
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
ROH

30. What is accuracy?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
How close results are to the accepted value
water and substances with (s) less dense than
no - they're written undissociated (HAaq)

31. What is the general formula of an alkane?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
CrO4²?
bases
CnH(2n+2)

32. If a weak acid is diluted more - what happens to its % dissociation value?
ethers
Increases.
fruit - fish - bases
CH3COO?

33. What causes the dramatic effect of T on rate?
boiling without losing volatile solvents/reactants
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Reduction always takes place at the cathode (RED CAT) In both types of cell!
T increases exponentially the proportion of molecules with E > Ea

34. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
+4-covalent - +2-ionic
blue (BTB)
Ppt will NOT form (unsaturated)

35. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
fractional distillation
Ksp = 4s³
NO3?
acids

36. What reacts with an acid to create hydrogen gas?
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?)
An active metal.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
NO3?

37. Which value of R do you use for all energy and kinetics calculations?
?H-kJ - ?S-J - ?G-kJ
CnH2n-2
R=8.31 J/mol/K
Heptane

38. What type of compounds do metals/non metals form?
Products - reactants (except for BDE when it's reactants - products)
Ionic compounds
Ions go through the salt bridge - electrons go through metal wires in the external circuit
atoms

39. potassium permanganate
?H formation of an element in standard state=0
Insoluble except for nitrate and acetate
Purple
CnH2n+2

40. What do metal oxides plus acids form?
Glacial acetic acid
CnH2n
Salt + water
Hg2²?

41. A Bronsted-Lowry acid is...
Insoluble except nitrate and acetate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Ionic compounds
proton donor base

42. How does benzene compare in reactivity to alkenes?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
CnH2n
The dilution effect when the solutions mix. M1V1 = M2V2
benzene is less reactive than alkenes

43. What are the names and formulas of the 6 strong acids?
CnH2n
Pour liquids using a funnel or down a glass rod
benzene is less reactive than alkenes
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

44. ammonium/ammonium compounds
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
ionic and form hydrogen and hydroxide
Soluble
Insoluble except group 1 and ammonium

45. acetate
it reacts by substitution NOT addition
Eudiometer
Add acid to water so that the acid doesn't boil and spit
CH3COO?

46. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Sigma bonds are stronger than pi bonds
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Synthetic condensation polymer (aka a polyamide)
Acids; HCOOCH3 is an ester

47. Is the ?H formation of an element in standard state zero?
brown volatile liquid
CnH2n-2
PO4³?
?H formation of an element in standard state=0

48. What are allotropes?
Products - reactants (except for BDE when it's reactants - products)
different forms of the same element
RCHO (carbonyl at end)
ion pairing

49. Why are noble gases stable?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
H3PO4
fractional distillation

50. What apparatus do you use to pour liquids?
The one with most oxygen atoms (highest oxidation number)
Pour liquids using a funnel or down a glass rod
Pale purple - (orange)-yellow - red - blue - green.
NH2?