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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. carbonates
Insoluble except group 1 and ammonium
Acid rain - dissolves marble buildings/statues and kills trees.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
The compound with the lowest Ksp value.

2. Color is due to ______ _______ of light.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
NH4?
Selective absorption
HClO4

3. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
basic
bright yellow
water and substances with (s) less dense than

4. Alcohols and _______ are FG isomers
acid + alcohol
Anode
ethers
Eudiometer

5. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
CO (poisonous)
water and substances with (s) less dense than
q=mc?T q=mL (or n x ?h)
bases

6. When is ?G zero?
NH4?
Hg²?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
water and substances with (s) less dense than

7. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
it reacts by substitution NOT addition
water and substances with (s) less dense than
Identity and purity (impure compounds usually have broad & low melting points)

8. What process do you use to obtain the precipitate from a solution?
Filtration
Big K=kf/kr
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
It ceases - the circuit is broken.

9. How do you get the equation for a net electrolysis reaction?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Decant
Salt + water
Combine the equations for the half reactions in the non-spontaneous direction

10. What is the basic structure of an optical isomer?
ClO?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
different forms of the same element
lighted splint (positive result=pop)

11. Ions are not ______.
Ksp = 27s4
-Ea/R
?H-kJ - ?S-J - ?G-kJ
atoms

12. What is the conjugate acid of H2PO4?
H3PO4
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
it's lower and occurs over less sharp a range
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

13. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
|experimental - accepted|/accepted X 100
are less dense than water
Soluble except Ag - Pb - Ca - Sr Ba)

14. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Combine the equations for the half reactions in the non-spontaneous direction
Increases.
red - green - blue
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

15. Are weak acids (and bases) written dissociated?

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16. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
CnH(2n+2)
water and substances with (s) less dense than
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)
ethers

17. bromine
a-IMFs - b-molecular volume
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
brown volatile liquid

18. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
Pour liquids using a funnel or down a glass rod
Distillation
10?8
do not change

19. What process do you use to obtain a solvent from a solution?
Ksp = 27s4
Pipette (burette if need repetition)
Distillation
Trigonal pyramidal

20. If Q > Ksp - then system shifts _______ and ppt ______
Group 1 hydroxides (ex: NaOH)
boiling without losing volatile solvents/reactants
left - ppt will form
More chaotic (ex: gases made)

21. What type of solutions do small - highly charged cations tend to form?
are less dense than water
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
RCOOR
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

22. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
fractional distillation
neutralization: high K - H2O product dissociation: low K - H2O reactant
NO3?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

23. If a free element is involved - what type of reaction must be involved?
redox reaction
It ceases - the circuit is broken.
proton donor base
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

24. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
zero
HClO4
water and substances with (s) less dense than

25. Both Acetic acid and ____________ are also functional isomers.
ion pairing
Conjugate pair (one must be a weak base or acid)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
methyl formate

26. hydroxide
Iodine and CO2 (dry ice)
Perform ICE BOX calculation based on K1
OH?
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

27. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
CnH2n+1 often designated 'R' ex C3H7 is propyl
Insoluble (except group 1 ammonium and Ba)
Hg2²?

28. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
|experimental - accepted|/accepted X 100
Group 1 hydroxides (ex: NaOH)
It ceases - the circuit is broken.

29. Ca - Sr - Ba
brown volatile liquid
hydroxides (ex: Ba(OH)2)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
atoms

30. cyanide
How grouped results are
P2O5
Decant
CN?

31. What kind of bonding structure does benzene have?
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)
acids
benzene has a delocalized pi ring structure
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

32. dichromate (soln + most solids)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
blue glass - it filters UV
Orange
same KE - but PEice<PEwater

33. What apparatus do you use to separate 2 immiscible liquids?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Insoluble (except group 1 ammonium and Ba)
Separating funnel
Most INsoluble except group 1 and ammonium

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

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35. Colorless doesn't mean ______
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Clear
A salt solution.
CN?

36. How are non-metal oxides and hydrides bonded? are they acidic or basic?
A) any range. b) 8-10 c) 4-6
Salt + water
non-metal oxides and hydrides are covalently bonded and are acidic.
The compound with the lowest Ksp value.

37. Give an example of a dilute strong acid.
Add acid to water so that the acid doesn't boil and spit
Insoluble (except group 1 ammonium and Ba)
Exothermic
HClO4

38. acetates
Group I metals (soft metals) are stored under oil
Soluble
a-IMFs - b-molecular volume
Group 1 hydroxides (ex: NaOH)

39. Name 2 ways in which you can create a buffer?
H3PO4
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)
Insoluble except for nitrate and acetate
ethers

40. 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.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
P2O5
A) any range. b) 8-10 c) 4-6
Group I metals (soft metals) are stored under oil

41. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Evaporation
ion pairing
K1 x K2
SO4²?

42. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
The dilution effect when the solutions mix. M1V1 = M2V2
no - they're written undissociated (HAaq)
Pale yellow

43. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Orange
Heat a test tube at an angle at the side of the tube (not bottom)
Anode - oxygen. Cathode - hydrogen
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

44. Which would cause the bulb in a conductivity apparatus to be brightest?
Decant
More chaotic (ex: gases made)
0.10M HCl (more ions)
Ksp = 27s4

45. A Bronsted-Lowry base is...
proton acceptor.
Saturated - Substitution (which requires more radical conditions)
atoms
But S° of element is not zero (except at 0K)

46. sulfates
Increases.
boiling without losing volatile solvents/reactants
Soluble except Ag - Pb - Ca - Sr Ba)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

47. When the salt bridge is removed what happens to the cell reaction?
CO (poisonous)
Experimental mass/theoretical mass X 100
Sulfur
It ceases - the circuit is broken.

48. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Soluble
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Molecules with the same molecular formulas - but different structural formulas

49. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Ksp = 108s5
Distillation
+4-covalent - +2-ionic

50. Give an example of a concentrated weak acid.
Eudiometer
The one with most oxygen atoms (highest oxidation number)
CH3COO?
Glacial acetic acid