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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 process do you use to separate two liquids with different boiling points?
Check for air bubbles in the buret and remove the buret funnel from the buret
fractional distillation
Salt and water
Ppt will NOT form (unsaturated)

2. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
it is lower and occurs over less sharp a range
Ksp = 108s5
same KE - but PEice<PEwater

3. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
same KE - but PEice<PEwater
RCOR
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

4. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Current - time and charge on ion (moles of e used in half cell reaction)
Ppt will NOT form (unsaturated)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

5. Is the freezing of ice endothermic or exothermic?
Heat a test tube at an angle at the side of the tube (not bottom)
q=mc?T q=mL (or n x ?h)
Exothermic
A salt solution.

6. If a free element is involved - what type of reaction must be involved?
a-IMFs - b-molecular volume
redox reaction
RCOOR
no - they're written undissociated (HAaq)

7. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
ns² electrons (first in-first out)
Group 1 hydroxides (ex: NaOH)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Soluble

8. What is the difference between equivalence point and end point of a titration.
Q=It (time in seconds)
ionic and form hydrogen and hydroxide
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
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

9. silver compounds
10?8
Insoluble except for nitrate and acetate
Soluble
Mono; di; tri; tetra; penta; hexa.

10. A Bronsted-Lowry acid is...
Soluble
proton donor base
R=8.31 J/mol/K
ClO?

11. What part of a liquid do you look at to measure its volume?
Soluble except Ag - Pb - Ca - Sr Ba)
An active metal.
Read the bottom of the meniscus
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

12. What is the word equation for condensation polymerisation ?
?G=negative - E° must be positive
lighted splint (positive result=pop)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Eudiometer

13. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
voltaic: + electrolytic: -
Ksp = 27s4
[A?]/[HA] x 100 or [BH?]/[B] x 100
do not change

14. What apparatus do you use to pour liquids?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
ionic and form hydrogen and hydroxide
neutralization: high K - H2O product dissociation: low K - H2O reactant
Pour liquids using a funnel or down a glass rod

15. What type of compounds do metals/non metals form?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
neutralization: high K - H2O product dissociation: low K - H2O reactant
Ionic compounds
Concentration

16. How are primary alcohols turned into acids?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
ionic and form hydrogen and hydroxide
Unsaturated - addition (ex: decolorize bromine solution)

17. carbonate
Sulfur
fruit - fish - bases
'non-active' metals such as Cu - Ag - Au - Pt - etc.
CO3²?

18. What are the signs for ?G and E° for spontaneous reactions?
hydroxides (ex: Ba(OH)2)
Most are soluble except Ag - Pb
But S° of element is not zero (except at 0K)
?G= -ve - E°= +ve

19. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Unsaturated - addition (ex: decolorize bromine solution)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
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
Transition element compounds (except if it has a full or empty d shell)

20. How does half life change for zero-th order - first order - and second order processes?
Distillation
zero-th: decreases - first: constant - second: increases
diamond and graphite
?H formation of an element in standard state=0

21. halides
Group 1 hydroxides (ex: NaOH)
Decant
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
Most are soluble except Ag - Pb

22. group 1 ions/compounds
Soluble
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
No - NH3 and HCl gases are extremely soluble
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

23. Neutralization is an ________ reaction.
Ppt will NOT form (unsaturated)
a-IMFs - b-molecular volume
catalyst=conc H2SO4
Exothermic (?H for ANY sa/sb = -57kJ/mol)

24. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

25. What are isotopes?
No - NH3 and HCl gases are extremely soluble
Read the bottom of the meniscus
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Clear

26. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
zero
Kc=Kp
Group I metals (soft metals) are stored under oil

27. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Products - reactants (except for BDE when it's reactants - products)
Anode - oxygen. Cathode - hydrogen
Glowing splint (positive result=relights)
CnH2n-2

28. What is the pH of 1.0M HCl? 1M NaOH?
NH4?
Insoluble (except group 1 ammonium and Ba)
Greenish-yellow gas
0 and 14

29. If ?S is positive - are the products more or less chaotic than the reactants?
Unsaturated - addition (ex: decolorize bromine solution)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Current - time and charge on ion (moles of e used in half cell reaction)
More chaotic (ex: gases made)

30. dichromate (soln + most solids)
Orange
Current - time and charge on ion (moles of e used in half cell reaction)
zero
Exothermic

31. Which value of R do you use for all energy and kinetics calculations?
Heptane
R=8.31 J/mol/K
CO (poisonous)
CnH2n+2

32. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
catalyst=conc H2SO4
red - green - blue
a-IMFs - b-molecular volume

33. How many normal boiling points and boiling points are there?

34. What is the catalyst for this reaction Ester + ?
Sigma bonds are stronger than pi bonds
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Salt + water
catalyst=conc H2SO4

35. bromine
no - they're written undissociated (HAaq)
ns² electrons (first in-first out)
C4H10
brown volatile liquid

36. What is the formula for obtaining charge flowing in a cell?
NH4?
Q=It (time in seconds)
ionic and form hydrogen and hydroxide
Most are soluble except Ag - Pb

37. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Exothermic
?G= -ve - E°= +ve
H+

38. Name some properties of Group 17
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Acidified
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
|experimental - accepted|/accepted X 100

39. Which of the rates changes more when temperature is increased?
bright yellow
linear
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
are less dense than water

40. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
non-metal oxides and hydrides are covalently bonded and are acidic.
acids
water and substances with (s) less dense than
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

41. perchlorate
An active metal.
ClO4?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

42. What is the general formula for an acid?
Salt and water
More chaotic (ex: gases made)
RCOOH
Greenish-yellow gas

43. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
NO3?
are less dense than water
methyl formate

44. What is the third law of thermodynamics?
S2O3²?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
S crystal at 0K=0
Transition element compounds (except if it has a full or empty d shell)

45. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Ksp = s²
Distillation
Acidified

46. What are two substances that sublime at 1 atm when heated?
Q=It (time in seconds)
Iodine and CO2 (dry ice)
water and substances with (s) less dense than
ClO4?

47. If a weak acid is diluted more - what happens to its % dissociation value?
Increases.
A salt solution.
blue (BTB)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

48. Why are noble gases stable?
strong acids/bases are written as H+ or OH- ions
ethers
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

49. barium sulfate
RCOOR
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
The benzene ring (or more correctly the phenyl group - C6H5)
White precipitate

50. When combining half equations - what do you do to E° values when multiplying coefficients?
CO (poisonous)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
ion pairing
Nothing