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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 things should you remember to do when collecting gas over water?
Identity and purity (impure compounds usually have broad & low melting points)
allow for the vapor pressure of water and make sure to level levels
brown volatile liquid
neutralization: high K - H2O product dissociation: low K - H2O reactant

2. What process do you use to obtain the precipitate from a solution?
Soluble
A salt solution.
Ksp = 108s5
Filtration

3. phosphate
PO4³?
Soluble
Ionic compounds
CO3²?

4. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
H3PO4
same KE - but PEice<PEwater
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
blue

5. What does the solubility of organic compounds depend on?
blue (BTB)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
ClO4?
Pale purple - (orange)-yellow - red - blue - green.

6. What is Big K in terms of kf and kr?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
At half equivalence - pH=pKa
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Big K=kf/kr

7. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
proton acceptor.
H2O + CO2 (it decomposes readily)
ion pairing

8. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
SO4²?
Hg2²?
Products - reactants (except for BDE when it's reactants - products)
Pale purple - (orange)-yellow - red - blue - green.

9. Where are group I metals stored?
Unsaturated - addition (ex: decolorize bromine solution)
Trigonal pyramidal
HClO4
Group I metals (soft metals) are stored under oil

10. thiosulfate
Reduction always takes place at the cathode (RED CAT) In both types of cell!
?H formation of an element in standard state=0
S2O3²?
do not change

11. How are metal oxides and hydrides bonded? are they acidic or basic?
Salts (ex: CaO + SO2 ? CaSO3)
metal oxides and hydrides are ionically bonded and basic
Insoluble except group 1 and ammonium
Read the bottom of the meniscus

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

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13. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
red - green - blue
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
catalyst=conc H2SO4
Orange

14. Alkenes are ________ and react by __________
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Unsaturated - addition (ex: decolorize bromine solution)
The Faraday or Faraday's constant.
redox reaction

15. Ca - Sr - Ba
same KE - but PEice<PEwater
hydroxides (ex: Ba(OH)2)
Experimental mass/theoretical mass X 100
Increases.

16. What are hybrid orbitals used for?
CnH2n+1 often designated 'R' ex C3H7 is propyl
ethers
ClO2?
Making sigma bonds and holding lone pairs

17. Which alkali metals float on water?
?H formation of an element in standard state=0
Read the bottom of the meniscus
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
All except for lithium

18. What measuring device would you use for very small volumes of liquids?
it is lower and occurs over less sharp a range
Transition element compounds (except if it has a full or empty d shell)
Pipette (burette if need repetition)
How close results are to the accepted value

19. What do nonmetal oxides plus water form?
Check for air bubbles in the buret and remove the buret funnel from the buret
Read the bottom of the meniscus
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
acids

20. What is the formula for alkynes?
CnH2n-2
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
The compound with the lowest Ksp value.
K2

21. A Bronsted-Lowry acid is...
proton donor base
no - they're written undissociated (HAaq)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
blue

22. A Bronsted-Lowry base is...
benzene has a delocalized pi ring structure
proton acceptor.
Purple
Pale purple - (orange)-yellow - red - blue - green.

23. What apparatus do you use to pour liquids?
Anode
Ksp = 27s4
Pour liquids using a funnel or down a glass rod
a-IMFs - b-molecular volume

24. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
A) any range. b) 8-10 c) 4-6
OH?
neutralization: high K - H2O product dissociation: low K - H2O reactant

25. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
OH- and NH3
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Soluble

26. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
zero
O2 needs 4F/mol H2 needs 2F/mol
H2O + CO2 (it decomposes readily)

27. Does Kw increase or decrease with T? Why?
SO4²?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
are less dense than water
H3PO4

28. What type of compounds do metals/non metals form?
Increases down group 1 decreases down group 17
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
0 and 14
Ionic compounds

29. What is an Alkyl group?

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30. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
water and substances with (s) less dense than

31. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
Sigma bonds are stronger than pi bonds
chemically (ex: with carbon)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

32. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
The benzene ring (or more correctly the phenyl group - C6H5)
CH3COO?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
small size and high charge

33. How are strong ones written?
R=8.31 J/mol/K
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
strong acids/bases are written as H+ or OH- ions
H+

34. Is the ?H formation of an element in standard state zero?
zero
?H formation of an element in standard state=0
-Ea/R
Salts (ex: CaO + SO2 ? CaSO3)

35. What is the pH of 1.0M HCl? 1M NaOH?
Increases.
R=8.31 J/mol/K
0 and 14
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

36. What do the 'a' and 'b' in Van Der Waal's equation allow for?
H2PO4?
Most are soluble except Ag - Pb
Ionic compounds
a-IMFs - b-molecular volume

37. chromate ion (soln + most solids)
Increases.
Hg²?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
yellow

38. acetate
Soluble
CH3COO?
Ksp = 108s5
The compound with the lowest Ksp value.

39. halides
H2PO4?
Most are soluble except Ag - Pb
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
P2O5

40. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
ROH
Salts (ex: CaO + SO2 ? CaSO3)
water and substances with (s) less dense than
fruit - fish - bases

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

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42. ammonium
NH4?
Glowing splint (positive result=relights)
linear
by electrolysis

43. What changes Keq?
Acids; HCOOCH3 is an ester
small size and high charge
But S° of element is not zero (except at 0K)
Only temperature

44. An amphiprotic (amphoteric) species is...
Salt and water
ROH
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

45. bromine
RCOOH
Anode
brown volatile liquid
metal oxides and hydrides are ionically bonded and basic

46. Why are noble gases stable?
small size and high charge
blue
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
A salt solution.

47. What shape is methane?
allow for the vapor pressure of water and make sure to level levels
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Tetrahedral

48. If a free element is involved - what type of reaction must be involved?
redox reaction
Making sigma bonds and holding lone pairs
Cu3(PO4)2
Salt and water

49. How do you explain trends in atomic properties using Coulomb's Law?
proton donor base
redox reaction
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Pale purple - (orange)-yellow - red - blue - green.

50. If ?S is positive - are the products more or less chaotic than the reactants?
No - NH3 and HCl gases are extremely soluble
More chaotic (ex: gases made)
it reacts by substitution NOT addition
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.