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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 does saturated mean? Unsaturated?
O2 needs 4F/mol H2 needs 2F/mol
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
0.10M HCl (more ions)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

2. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
zero-th: decreases - first: constant - second: increases
water and substances with (s) less dense than
ClO3?
strong acids/bases are written as H+ or OH- ions

3. What do nonmetal oxides plus water form?
Tetrahedral
Conjugate pair (one must be a weak base or acid)
acids
neutralization: high K - H2O product dissociation: low K - H2O reactant

4. When combining half equations - what do you do to E° values when multiplying coefficients?
Most are soluble except Ag - Pb
OH?
Nothing
Combine the equations for the half reactions in the non-spontaneous direction

5. What is the general formula of an alkane?
CnH(2n+2)
brown volatile liquid
zero
Insoluble except for nitrate and acetate

6. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
bases
Insoluble
Check for air bubbles in the buret and remove the buret funnel from the buret

7. What is the general formula for an aldehyde?
blue glass - it filters UV
RCHO (carbonyl at end)
Read the bottom of the meniscus
acids

8. What is the formula for alkanes?
small size and high charge
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
CnH2n+2
They stay the same.

9. If ?S is positive - are the products more or less chaotic than the reactants?
methyl formate
[A?]/[HA] x 100 or [BH?]/[B] x 100
CnH2n+2
More chaotic (ex: gases made)

10. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
different forms of the same element
Acids; HCOOCH3 is an ester
a-IMFs - b-molecular volume

11. What are the units of the first order rate constant?
Soluble
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Perform ICE BOX calculation based on K1
The Faraday or Faraday's constant.

12. If Q > Ksp - then system shifts _______ and ppt ______
a-IMFs - b-molecular volume
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
left - ppt will form
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

13. How many ligands attach to a central ion in a complex ion?
chemically (ex: with carbon)
Initiation energy (NOT Ea)
#ligands=charge x2
Evaporation

14. dihydrogen phosphate
H2PO4?
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)
Insoluble except group 1 and ammonium
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

15. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
P2O5
H3PO4
Orange
Q=It (time in seconds)

16. What is an Alkyl group?

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17. What should you check for before you begin titrating?
a-IMFs - b-molecular volume
ion pairing
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Check for air bubbles in the buret and remove the buret funnel from the buret

18. hydroxides
ROH
Insoluble (except group 1 ammonium and Ba)
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)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

19. The oxidation # for acid base reactions...
do not change
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
basic
ethers

20. mercury (I) ion
Hg2²?
Mono; di; tri; tetra; penta; hexa.
How grouped results are
it's lower and occurs over less sharp a range

21. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
a-IMFs - b-molecular volume
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
NH2?

22. What two compounds are great oxidizing agents?

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23. Acid plus base make?
fruit - fish - bases
Salt + water.
CnH2n+1 often designated 'R' ex C3H7 is propyl
10?8

24. What measuring device would you use for very small volumes of liquids?
White precipitate
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Pipette (burette if need repetition)
Salt + water.

25. Name six characteristics of transition elements (or their compounds)
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)
CnH2n+1 often designated 'R' ex C3H7 is propyl
CO2 and H2O
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)

26. What shape is carbon dioxide?
fruit - fish - bases
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?)
PO4³?
linear

27. What is the slope of the graph of lnk vs. 1/T?
Insoluble except for nitrate and acetate
Check for air bubbles in the buret and remove the buret funnel from the buret
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
-Ea/R

28. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Ksp = 27s4
Pipette (burette if need repetition)
RX

29. Buffer capacity must contain decent amounts of a ________ ________
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Experimental mass/theoretical mass X 100
Conjugate pair (one must be a weak base or acid)

30. What are hybrid orbitals used for?
Ionic compounds
Insoluble except for nitrate and acetate
Making sigma bonds and holding lone pairs
acids

31. What causes the dramatic effect of T on rate?
Pale yellow
acids
bright yellow
T increases exponentially the proportion of molecules with E > Ea

32. How does group 1 metals' density compare to water's?
left - ppt will form
S crystal at 0K=0
Hg²?
are less dense than water

33. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Purple
Add acid to water so that the acid doesn't boil and spit
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
basic

34. halides
allow for the vapor pressure of water and make sure to level levels
C4H10
Transition element compounds (except if it has a full or empty d shell)
Most are soluble except Ag - Pb

35. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Glacial acetic acid
?G= -ve - E°= +ve
Salt and water

36. What do you do to get rid of most of the solution from a precipitate?
no - they're written undissociated (HAaq)
Decant
All except for lithium
C2O4²?

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

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38. What is the formula for alkynes?
Iodine and CO2 (dry ice)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
CnH2n-2
?G= -ve - E°= +ve

39. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
H3PO4
K2
Ksp = s²

40. If a free element is involved - what type of reaction must be involved?
Glowing splint (positive result=relights)
redox reaction
Add acid to water so that the acid doesn't boil and spit
H2O + CO2 (it decomposes readily)

41. What are the common strong bases?
Graduated cylinder
Sulfur
Group 1 hydroxides (ex: NaOH)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

42. What type of compounds do Group 14 form?
Big K=kf/kr
Glowing splint (positive result=relights)
+4-covalent - +2-ionic
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

43. Do anions flow to the cathode or anode?
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
hydroxides (ex: Ba(OH)2)
Increases down group 1 decreases down group 17
Anode

44. What is the difference between equivalence point and end point of a titration.
Read the bottom of the meniscus
RNH2
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
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

45. chromate ion (soln + most solids)
O2 needs 4F/mol H2 needs 2F/mol
K1 x K2
yellow
H2PO4?

46. acetate
CH3COO?
blue glass - it filters UV
fractional distillation
CrO4²?

47. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Glowing splint (positive result=relights)
Increases down group 1 decreases down group 17
Acid rain - dissolves marble buildings/statues and kills trees.
CrO4²?

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

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49. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Mn²? - Cr³? - Cr³
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
catalyst=conc H2SO4
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

50. What kind of bonding structure does benzene have?
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.
H2O + CO2 (it decomposes readily)
benzene has a delocalized pi ring structure
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties