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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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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 the conjugate base of NH3?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
boiling without losing volatile solvents/reactants
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
NH2?

2. hydroxides
CnH(2n+2)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Insoluble (except group 1 ammonium and Ba)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

3. BaSO4
Read the bottom of the meniscus
0.10M HCl (more ions)
Insoluble
CnH2n+2

4. How are more active metals reduced?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
by electrolysis
An active metal.
NH2?

5. What do you do to get rid of most of the solution from a precipitate?
Current - time and charge on ion (moles of e used in half cell reaction)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
allow for the vapor pressure of water and make sure to level levels
Decant

6. group 1 ions/compounds
Soluble
Unsaturated - addition (ex: decolorize bromine solution)
bright yellow
RCOOR

7. Which value of R do you use for all energy and kinetics calculations?
proton acceptor.
R=8.31 J/mol/K
Perform ICE BOX calculation based on K1
But S° of element is not zero (except at 0K)

8. What is the sign of the anode in voltaic cells? in electrolytic cells?
Soluble except Ag - Pb - Ca - Sr Ba)
voltaic: - electrolytic: +
Insoluble except group 1 and ammonium
Synthesis - separation and purification of the product and its identification.

9. How do you compute % dissociation?
HClO4
acids
[A?]/[HA] x 100 or [BH?]/[B] x 100
bright yellow

10. hydroxide
OH?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Salt + water.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

11. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
H3PO4
10?8
a-IMFs - b-molecular volume

12. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
The benzene ring (or more correctly the phenyl group - C6H5)
MnO4?
Pour liquids using a funnel or down a glass rod

13. potassium permanganate
MnO4?
Salt + water
Purple
brown volatile liquid

14. Acidic gases like SO2 in the atmosphere cause what environmental problems?
ROR
Transition element compounds (except if it has a full or empty d shell)
Acid rain - dissolves marble buildings/statues and kills trees.
strong acids/bases are written as H+ or OH- ions

15. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
S crystal at 0K=0
ion pairing
benzene is less reactive than alkenes

16. What is the general formula for an acid?
a-IMFs - b-molecular volume
Increases down group 1 decreases down group 17
diamond and graphite
RCOOH

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

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18. How do you explain trends in atomic properties using Coulomb's Law?
Glowing splint (positive result=relights)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Most INsoluble except group 1 and ammonium
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

19. What should you check for before you begin titrating?
NO3?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Check for air bubbles in the buret and remove the buret funnel from the buret
Initiation energy (NOT Ea)

20. What is the charge on a chlorine atom?
it reacts by substitution NOT addition
The Faraday or Faraday's constant.
Saturated - Substitution (which requires more radical conditions)
zero

21. Name six characteristics of transition elements (or their compounds)
NH4?
proton acceptor.
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)
H3PO4

22. acetates
Eudiometer
Kc=Kp
Soluble
left - ppt will form

23. What are the formulas for q?
an oxidized and reduced substance
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
neutralization: high K - H2O product dissociation: low K - H2O reactant
q=mc?T q=mL (or n x ?h)

24. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
bent

25. 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
Acidified
Acid rain - dissolves marble buildings/statues and kills trees.
Evaporation

26. Ions are not ______.
Add acid to water so that the acid doesn't boil and spit
Group 1 hydroxides (ex: NaOH)
NH2?
atoms

27. What process do you use to obtain the solute from a solution?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
NH4?
water and substances with (s) less dense than
Evaporation

28. What are isomers?
strong acids/bases are written as H+ or OH- ions
Molecules with the same molecular formulas - but different structural formulas
Most INsoluble except group 1 and ammonium
Q=It (time in seconds)

29. carbonates
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Ionic compounds
Graduated cylinder
Insoluble except group 1 and ammonium

30. What is the word equation for addition polymerisation?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
proton donor base
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

31. What type of compounds are almost always colored?
CrO4²?
same KE - but PEice<PEwater
Transition element compounds (except if it has a full or empty d shell)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

32. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Salt + water
Tetrahedral
Sulfur
Ksp = 4s³

33. Lattice energy is high for ions with _____ size and _____ charge
Ksp = s²
different forms of the same element
small size and high charge
Increases.

34. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
CnH(2n+2)
Acids; HCOOCH3 is an ester

35. What is the general formula for an alcohol?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
zero
Ppt will NOT form (unsaturated)
ROH

36. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
water and substances with (s) less dense than
benzene is less reactive than alkenes
T increases exponentially the proportion of molecules with E > Ea

37. Alkenes are ________ and react by __________
ROH
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Most are soluble except Ag - Pb
Unsaturated - addition (ex: decolorize bromine solution)

38. What is the second law of thermodynamics?
allow for the vapor pressure of water and make sure to level levels
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Saturated - Substitution (which requires more radical conditions)
Suniverse increases for spontaneous processes

39. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
CN?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
same KE - but PEice<PEwater
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

40. 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)
ion pairing
White precipitate
ClO3?

41. bromine
diamond and graphite
Glowing splint (positive result=relights)
brown volatile liquid
Cr2O7²?

42. When a cell is 'flat' What is its voltage?
Big K=kf/kr
zero
Salt + water
P2O5

43. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
brown volatile liquid
Anode - oxygen. Cathode - hydrogen
Transition element compounds (except if it has a full or empty d shell)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

44. Acid plus base make?
An active metal.
S crystal at 0K=0
Salt + water.
fruit - fish - bases

45. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Pale purple - (orange)-yellow - red - blue - green.
Sigma bonds are stronger than pi bonds
?G= -ve - E°= +ve
Suniverse increases for spontaneous processes

46. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
same KE - but PEice<PEwater
basic
10?8
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

47. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
CO (poisonous)
Read the bottom of the meniscus
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
H2O + CO2 (it decomposes readily)

48. How do you dilute an acid?

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49. permanganate
10?8
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Iodine and CO2 (dry ice)
MnO4?

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

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