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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. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
brown volatile liquid
water and substances with (s) less dense than
Salt and water
Clear

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

3. What is the name of S2Cl2? (Know how to name others like this - too)
Insoluble except for nitrate and acetate
Disulfur dichloride
But S° of element is not zero (except at 0K)
Purple

4. What is the formula for summation?

5. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
MnO4?
voltaic: - electrolytic: +
water and substances with (s) less dense than

6. What do the 'a' and 'b' in Van Der Waal's equation allow for?
NO3?
a-IMFs - b-molecular volume
ROR
Group 1 hydroxides (ex: NaOH)

7. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
?G=negative - E° must be positive
do not change
How grouped results are
How close results are to the accepted value

8. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
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
K1 x K2
More chaotic (ex: gases made)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

9. Which alkali metals float on water?
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
All except for lithium
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
ion pairing

10. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
left - ppt will form
Hg2²?
The compound with the lowest Ksp value.
#ligands=charge x2

11. acetates
Insoluble except nitrate and acetate
Soluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
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

12. Acid plus base make?
Soluble except Ag - Pb - Ca - Sr Ba)
Salt + water.
Distillation
ethers

13. What is the formula for percent error?
|experimental - accepted|/accepted X 100
a-IMFs - b-molecular volume
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
benzene is less reactive than alkenes

14. When a cell is 'flat' What is its voltage?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Soluble
Combine the equations for the half reactions in the non-spontaneous direction
zero

15. What is the difference between equivalence point and end point of a titration.
left - ppt will form
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
PO4³?
bent

16. Where are group I metals stored?
Acid rain - dissolves marble buildings/statues and kills trees.
Group I metals (soft metals) are stored under oil
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Silvery gray solid - brown - purple

17. If a free element is involved - what type of reaction must be involved?
water and substances with (s) less dense than
redox reaction
A) any range. b) 8-10 c) 4-6
acids

18. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
RCOOR
Increases.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

19. If Q < Ksp a ppt ______
NO3?
Products - reactants (except for BDE when it's reactants - products)
Pipette (burette if need repetition)
Ppt will NOT form (unsaturated)

20. How are strong ones written?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
strong acids/bases are written as H+ or OH- ions
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

21. phosphates
Most INsoluble except group 1 and ammonium
Perform ICE BOX calculation based on K1
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
it's lower and occurs over less sharp a range

22. What is a dipeptide? polypeptide? protein?
RNH2
brown volatile liquid
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
acid + alcohol

23. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Insoluble except group 1 and ammonium
At half equivalence - pH=pKa
Salt + water.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

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

25. What is the general formula of an alkane?
CnH(2n+2)
CnH2n
Add acid to water so that the acid doesn't boil and spit
non-metal oxides and hydrides are covalently bonded and are acidic.

26. What is the general formula for an aldehyde?
RCHO (carbonyl at end)
fractional distillation
Greenish-yellow gas
-Ea/R

27. What does a short - sharp melting point indicate?
a-IMFs - b-molecular volume
ClO3?
Identity and purity (impure compounds usually have broad & low melting points)
The dilution effect when the solutions mix. M1V1 = M2V2

28. What is reflux?
blue (BTB)
boiling without losing volatile solvents/reactants
10?8
zero

29. Color is due to ______ _______ of light.
water and substances with (s) less dense than
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Sulfur
Selective absorption

30. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
O2 needs 4F/mol H2 needs 2F/mol
S crystal at 0K=0
hydroxides (ex: Ba(OH)2)

31. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Silvery gray solid - brown - purple
Nothing

32. How do you identify which is oxidized or otherwise?
same KE - but PEice<PEwater
Selective absorption
look for changes in oxidation # - the one that goes up is oxidized and is the RA
ROH

33. What is the formula for alkenes?
Graduated cylinder
The one with most oxygen atoms (highest oxidation number)
CnH2n
Iodine and CO2 (dry ice)

34. What is the catalyst for this reaction Ester + ?
methyl formate
Soluble
strong acids/bases are written as H+ or OH- ions
catalyst=conc H2SO4

35. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
bent
boiling without losing volatile solvents/reactants
Pale purple - (orange)-yellow - red - blue - green.

36. Which value of R do you use for all energy and kinetics calculations?
Kc=Kp
Pale yellow
Salts (ex: CaO + SO2 ? CaSO3)
R=8.31 J/mol/K

37. cyanide
CN?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
K2
chemically (ex: with carbon)

38. What should you check for before you begin titrating?
Ksp = s²
No - it depends on the number of ions produced on dissolving.
Transition element compounds (except if it has a full or empty d shell)
Check for air bubbles in the buret and remove the buret funnel from the buret

39. dichromate
Glacial acetic acid
White precipitate
Cr2O7²?
ionic and form hydrogen and hydroxide

40. What are the units of the first order rate constant?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Silvery gray solid - brown - purple

41. primary colors
red - green - blue
Heat a test tube at an angle at the side of the tube (not bottom)
The benzene ring (or more correctly the phenyl group - C6H5)
CO2 and H2O

42. What apparatus do you use to separate 2 immiscible liquids?
fruit - fish - bases
Separating funnel
Products - reactants (except for BDE when it's reactants - products)
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia

43. halides
boiling without losing volatile solvents/reactants
Most are soluble except Ag - Pb
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
HClO4

44. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Conjugate pair (one must be a weak base or acid)
voltaic: + electrolytic: -
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
K2

45. What electrons are lost/gained first in transition element ions?
Increases down group 1 decreases down group 17
ROH
ns² electrons (first in-first out)
Acids; HCOOCH3 is an ester

46. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
ClO?
it reacts by substitution NOT addition
RCOOR

47. What is the second law of thermodynamics?
Suniverse increases for spontaneous processes
Salt and water
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
The benzene ring (or more correctly the phenyl group - C6H5)

48. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

49. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
White precipitate
Ksp = 27s4
benzene is less reactive than alkenes

50. Is the ?H formation of an element in standard state zero?
Ionic compounds
NO3?
?H formation of an element in standard state=0
RNH2