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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. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Eudiometer
non-metal oxides and hydrides are covalently bonded and are acidic.
Most are soluble except Ag - Pb
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

2. What type of compounds do metals/non metals form?
RCHO (carbonyl at end)
Ionic compounds
?G=negative - E° must be positive
Salt + water

3. Color is due to ______ _______ of light.
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Selective absorption
Ksp = s²
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

4. What are the signs for ?G and E° for spontaneous reactions?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
NH4?
?G= -ve - E°= +ve
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

5. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
Kc=Kp
ClO2?
Sulfur

6. Nonmetals are good _____ agents. Metals are good _______ agents.
Soluble except Ag - Pb - Ca - Sr Ba)
Mn²? - Cr³? - Cr³
Salt and water
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

7. Esters smell like _______ and amines smell like _______ and are ______.
Soluble
fruit - fish - bases
The Faraday or Faraday's constant.
Ionic compounds

8. ammonium/ammonium compounds
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Tetrahedral
Soluble
atoms

9. mercury (II) ion
benzene has a delocalized pi ring structure
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Hg²?
RX

10. What measuring device would you use for very small volumes of liquids?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Pipette (burette if need repetition)
+4-covalent - +2-ionic
CnH2n

11. When combining half equations - what do you do to E° values when multiplying coefficients?
The benzene ring (or more correctly the phenyl group - C6H5)
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)
benzene has a delocalized pi ring structure
Nothing

12. Which alkali metals float on water?
RNH2
All except for lithium
same KE - but PEice<PEwater
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

13. potassium permanganate
same KE - but PEice<PEwater
Heat a test tube at an angle at the side of the tube (not bottom)
Purple
neutralization: high K - H2O product dissociation: low K - H2O reactant

14. 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 except for lithium
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
strong acids/bases are written as H+ or OH- ions
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)

15. For a dibasic acid (H2A) - [A²?]= ____ ?
Separating funnel
RCOOR
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
K2

16. silver iodide
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
#ligands=charge x2
Pale yellow

17. What type of metals don't react with water or acids to form H2?

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18. permanganate
NO3?
acids
MnO4?
H3PO4

19. Give an example of a dilute strong acid.
MnO4?
Ksp = 4s³
Distillation
HClO4

20. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Pour liquids using a funnel or down a glass rod
Anode - oxygen. Cathode - hydrogen
But S° of element is not zero (except at 0K)
CnH2n

21. What type of compounds are almost always colored?
Read the bottom of the meniscus
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Transition element compounds (except if it has a full or empty d shell)
CO3²?

22. What value of R do you use for thermo calculations? gas calculations?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Distillation
ClO?

23. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
boiling without losing volatile solvents/reactants
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

24. lead iodide
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
proton acceptor.
bright yellow
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

25. 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?
CrO4²?
RCOOH
Insoluble except nitrate and acetate
The compound with the lowest Ksp value.

26. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
are less dense than water
How grouped results are
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

27. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Anode
E=q + w (negative is by system - positive is on system)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
CO (poisonous)

28. oxalate
How grouped results are
C2O4²?
The dilution effect when the solutions mix. M1V1 = M2V2
zero-th: decreases - first: constant - second: increases

29. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
The dilution effect when the solutions mix. M1V1 = M2V2
water and substances with (s) less dense than
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
voltaic: - electrolytic: +

30. Name six characteristics of transition elements (or their compounds)
ClO3?
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
RCOOR
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)

31. Both Acetic acid and ____________ are also functional isomers.
methyl formate
diamond and graphite
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)
ion pairing

32. How does benzene compare in reactivity to alkenes?
Conjugate pair (one must be a weak base or acid)
[A?]/[HA] x 100 or [BH?]/[B] x 100
benzene is less reactive than alkenes
SO4²?

33. Buffer capacity must contain decent amounts of a ________ ________
Increases down group 1 decreases down group 17
Conjugate pair (one must be a weak base or acid)
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?)
Insoluble

34. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Current - time and charge on ion (moles of e used in half cell reaction)
same KE - but PEice<PEwater
benzene has a delocalized pi ring structure
non-metal oxides and hydrides are covalently bonded and are acidic.

35. perchlorate
zero
Add acid to water so that the acid doesn't boil and spit
ClO4?
a-IMFs - b-molecular volume

36. Is the freezing of ice endothermic or exothermic?
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
A) any range. b) 8-10 c) 4-6
A salt solution.
Exothermic

37. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
redox reaction
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
no - they're written undissociated (HAaq)
Evaporation

38. Color (absorbance) is proportional to ________
CnH2n+1 often designated 'R' ex C3H7 is propyl
More chaotic (ex: gases made)
The Faraday or Faraday's constant.
Concentration

39. What is the formula for alkanes?
CnH2n+2
q=mc?T q=mL (or n x ?h)
10?8
They stay the same.

40. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Tetrahedral
Ksp = 4s³
Combine the equations for the half reactions in the non-spontaneous direction
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

41. How do you find the pH for a dibasic acid? (H2A)?
Perform ICE BOX calculation based on K1
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
They stay the same.
bent

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

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43. What is an Alkyl group?

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44. What is Big K in terms of kf and kr?
Big K=kf/kr
O2 needs 4F/mol H2 needs 2F/mol
bright yellow
blue glass - it filters UV

45. Does Kw increase or decrease with T? Why?
Soluble except Ag - Pb - Ca - Sr Ba)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
O2 needs 4F/mol H2 needs 2F/mol
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

46. hypochlorite
ClO?
Pale purple - (orange)-yellow - red - blue - green.
fractional distillation
ROH

47. What is the test for oxygen?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
-Ea/R
Glowing splint (positive result=relights)
same KE - but PEice<PEwater

48. thiosulfate
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Only temperature
blue (BTB)
S2O3²?

49. Alcohols and _______ are FG isomers
ethers
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Iodine and CO2 (dry ice)
Add acid to water so that the acid doesn't boil and spit

50. Give an example of a concentrated weak acid.
Glacial acetic acid
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Increases down group 1 decreases down group 17