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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.
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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 do you identify which is oxidized or otherwise?
K1 x K2
metal oxides and hydrides are ionically bonded and basic
look for changes in oxidation # - the one that goes up is oxidized and is the RA
bases

2. What is the general formula for an ester?
RCOOR
ionic and form hydrogen and hydroxide
The compound with the lowest Ksp value.
CN?

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

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4. What is the first law of thermodynamics?
NO3?
?G=negative - E° must be positive
E=q + w (negative is by system - positive is on system)
ionic and form hydrogen and hydroxide

5. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Unsaturated - addition (ex: decolorize bromine solution)
Ksp = 108s5
RNH2
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

6. What is the general formula for an amine?
are less dense than water
RNH2
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Increases.

7. What type of compounds do Group 14 form?
E=q + w (negative is by system - positive is on system)
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
+4-covalent - +2-ionic
The Faraday or Faraday's constant.

8. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Products - reactants (except for BDE when it's reactants - products)
H2PO4?
voltaic: + electrolytic: -
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

9. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Clear
Iodine and CO2 (dry ice)
boiling without losing volatile solvents/reactants
Ksp = s²

10. How do you find the pH for a dibasic acid? (H2A)?
proton donor base
Perform ICE BOX calculation based on K1
Decant
same KE - but PEice<PEwater

11. bromine
Mono; di; tri; tetra; penta; hexa.
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)
CH3COO?
brown volatile liquid

12. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
Big K=kf/kr
Salt and water
OH- and NH3

13. group 1 ions/compounds
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.
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Group 1 hydroxides (ex: NaOH)
Soluble

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

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15. What things should you remember to do when collecting gas over water?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
allow for the vapor pressure of water and make sure to level levels
a-IMFs - b-molecular volume
S crystal at 0K=0

16. 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?
Evaporation
The compound with the lowest Ksp value.
Read the bottom of the meniscus
Separating funnel

17. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
S2O3²?
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)
boiling without losing volatile solvents/reactants
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

18. If ?S is positive - are the products more or less chaotic than the reactants?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Unsaturated - addition (ex: decolorize bromine solution)
More chaotic (ex: gases made)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

19. Where are group I metals stored?
are less dense than water
Group I metals (soft metals) are stored under oil
Identity and purity (impure compounds usually have broad & low melting points)
An active metal.

20. mercury (II) ion
RCOOR
Hg²?
Tetrahedral
Sigma bonds are stronger than pi bonds

21. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
blue glass - it filters UV
a-IMFs - b-molecular volume
CO3²?

22. Generally - which oxy acid is strongest?
Experimental mass/theoretical mass X 100
The one with most oxygen atoms (highest oxidation number)
hydroxides (ex: Ba(OH)2)
Only temperature

23. potassium permanganate
?G=negative - E° must be positive
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)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Purple

24. One mole of electrons carries 96500Coulombs - what is this quantity called?

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25. What is the relationship in strength between sigma and pi bonds?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Sigma bonds are stronger than pi bonds
Evaporation
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

26. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
blue (BTB)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
H+
Tetrahedral

27. Alkanes are _________ and react by _________
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Saturated - Substitution (which requires more radical conditions)
NO3?
H3PO4

28. What device would you use to measure a volume of gas?
a-IMFs - b-molecular volume
Suniverse increases for spontaneous processes
Eudiometer
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

29. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Transition element compounds (except if it has a full or empty d shell)
zero
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
No - it depends on the number of ions produced on dissolving.

30. What shape is ammonia?
Trigonal pyramidal
Only temperature
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Most are soluble except Ag - Pb

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

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32. How many ligands attach to a central ion in a complex ion?
neutralization: high K - H2O product dissociation: low K - H2O reactant
voltaic: - electrolytic: +
Soluble
#ligands=charge x2

33. What is the catalyst for this reaction Ester + ?
brown volatile liquid
CO3²?
Hg2²?
catalyst=conc H2SO4

34. If Q > Ksp - then system shifts _______ and ppt ______
Iodine and CO2 (dry ice)
Soluble except Ag - Pb - Ca - Sr Ba)
left - ppt will form
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)

35. What is precision?
HClO4
S crystal at 0K=0
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
How grouped results are

36. Neutralization is an ________ reaction.
?H-kJ - ?S-J - ?G-kJ
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Only temperature
Eudiometer

37. Do anions flow to the cathode or anode?
Check for air bubbles in the buret and remove the buret funnel from the buret
Anode
Salt + water.
Insoluble except nitrate and acetate

38. How do you heat a test tube?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Heat a test tube at an angle at the side of the tube (not bottom)

39. What is the word equation for addition polymerisation?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Increases.
Selective absorption
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

40. bromothymol
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
blue (BTB)
basic
Separating funnel

41. What is the slope of the graph of lnk vs. 1/T?
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.
-Ea/R
More chaotic (ex: gases made)
CN?

42. What process do you use to obtain a solvent from a solution?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Most INsoluble except group 1 and ammonium
Distillation
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

43. chromate ion (soln + most solids)
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
a-IMFs - b-molecular volume
yellow
Monomer + monomer = polymer product + a simple molecule such as water or HCl

44. Ca - Sr - Ba
do not change
C2O4²?
hydroxides (ex: Ba(OH)2)
Kc=Kp

45. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
CO (poisonous)
Ksp = 27s4
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
H2PO4?

46. Which of the rates changes more when temperature is increased?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Products - reactants (except for BDE when it's reactants - products)
CO3²?
boiling without losing volatile solvents/reactants

47. Acids + Carbonates (bicarbonates) make?
acids
Insoluble (except group 1 ammonium and Ba)
SO4²?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

48. Why are i factors (Van't Hoff factors) often less than ideal?
CnH(2n+2)
Acid rain - dissolves marble buildings/statues and kills trees.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
ion pairing

49. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
RX
CnH2n-2

50. The definition of acidic basic and neutral aqueous solutions is:
RX
proton donor base
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]