Test your basic knowledge |

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. Colorless doesn't mean ______
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?)
Clear
A) any range. b) 8-10 c) 4-6
The Faraday or Faraday's constant.

2. How do you clean a buret/pipette for a titration?
ROH
Disulfur dichloride
C2O4²?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

3. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Kc=Kp
10?8
They stay the same.
Soluble

4. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
ROR
H2PO4?
diamond and graphite
Ksp = 108s5

5. How do you explain trends in atomic properties using Coulomb's Law?
Nothing
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Eudiometer
H3PO4

6. What shape is carbon dioxide?
Experimental mass/theoretical mass X 100
linear
Insoluble except for nitrate and acetate
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

7. copper sulfate
Mono; di; tri; tetra; penta; hexa.
Iodine and CO2 (dry ice)
blue (BTB)
blue

8. What is the conjugate base of NH3?
+4-covalent - +2-ionic
NH2?
Concentration
-Ea/R

9. What do you use to look at burning magnesium? why?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
blue glass - it filters UV
Pale yellow
Synthesis - separation and purification of the product and its identification.

10. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
a-IMFs - b-molecular volume
Current - time and charge on ion (moles of e used in half cell reaction)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

11. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Conjugate pair (one must be a weak base or acid)
An active metal.

12. What is the formula for alkanes?
allow for the vapor pressure of water and make sure to level levels
H+
CH3COO?
CnH2n+2

13. halides
basic
Most are soluble except Ag - Pb
Identity and purity (impure compounds usually have broad & low melting points)
Perform ICE BOX calculation based on K1

14. silver iodide
Pale yellow
+4-covalent - +2-ionic
CrO4²?
H3PO4

15. How are primary alcohols turned into acids?
Soluble
Ppt will NOT form (unsaturated)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Cr2O7²?

16. Does Kw increase or decrease with T? Why?
allow for the vapor pressure of water and make sure to level levels
fractional distillation
Nothing
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

17. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
ion pairing
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

18. What should you check for before you begin titrating?
Anode
Check for air bubbles in the buret and remove the buret funnel from the buret
Decant
Group I metals (soft metals) are stored under oil

19. What are isomers?
methyl formate
Molecules with the same molecular formulas - but different structural formulas
Most are soluble except Ag - Pb
ns² electrons (first in-first out)

20. How do you compute % dissociation?
Ksp = s²
Ksp = 27s4
Glowing splint (positive result=relights)
[A?]/[HA] x 100 or [BH?]/[B] x 100

21. How are non-metal oxides and hydrides bonded? are they acidic or basic?
acids
Making sigma bonds and holding lone pairs
non-metal oxides and hydrides are covalently bonded and are acidic.
R=8.31 J/mol/K

22. thiosulfate
zero
S2O3²?
Insoluble except for nitrate and acetate
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

23. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
CnH2n+1 often designated 'R' ex C3H7 is propyl
Combine the equations for the half reactions in the non-spontaneous direction
neutralization: high K - H2O product dissociation: low K - H2O reactant

24. If a free element is involved - what type of reaction must be involved?
redox reaction
Acidified
Identity and purity (impure compounds usually have broad & low melting points)
T increases exponentially the proportion of molecules with E > Ea

25. What do you need to make a polymer?
R=8.31 J/mol/K
Cr2O7²?
P2O5
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)

26. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Soluble
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

27. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Purple
ion pairing
Both electrons come from the same atom (just as good as a regular bond)

28. What are the prefixes for the naming of binary molecular compound formulas (up to six)
same KE - but PEice<PEwater
zero
How grouped results are
Mono; di; tri; tetra; penta; hexa.

29. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
allow for the vapor pressure of water and make sure to level levels
Perform ICE BOX calculation based on K1

30. What shape is water?
lighted splint (positive result=pop)
bent
Both electrons come from the same atom (just as good as a regular bond)
Decant

31. What reacts with an acid to create hydrogen gas?
Conjugate pair (one must be a weak base or acid)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
An active metal.
Greenish-yellow gas

32. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Ionic compounds
ROH
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
basic

33. dichromate
H2O + CO2 (it decomposes readily)
Conjugate pair (one must be a weak base or acid)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Cr2O7²?

34. What is reflux?
boiling without losing volatile solvents/reactants
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
zero
are less dense than water

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

36. barium sulfate
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
White precipitate
fruit - fish - bases
The Faraday or Faraday's constant.

37. What do group I/II metal oxides and acids form?
a-IMFs - b-molecular volume
Salt and water
Soluble
Sulfur

38. Aromatic compounds contain what?
The benzene ring (or more correctly the phenyl group - C6H5)
CnH(2n+2)
q=mc?T q=mL (or n x ?h)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

39. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Soluble
At half equivalence - pH=pKa
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Glowing splint (positive result=relights)

40. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Perform ICE BOX calculation based on K1

41. mercury (I) ion
Monomer + monomer = polymer product + a simple molecule such as water or HCl
RCOOR
Anode
Hg2²?

42. What are two substances that sublime at 1 atm when heated?
K1 x K2
Iodine and CO2 (dry ice)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Soluble

43. Color is due to ______ _______ of light.
It ceases - the circuit is broken.
fruit - fish - bases
no - they're written undissociated (HAaq)
Selective absorption

44. Which alkali metals float on water?
acid + alcohol
Conjugate pair (one must be a weak base or acid)
Distillation
All except for lithium

45. If a weak acid is diluted more - what happens to its % dissociation value?
Increases.
CnH(2n+2)
blue (BTB)
H2O + CO2 (it decomposes readily)

46. Neutralization is an ________ reaction.
Products - reactants (except for BDE when it's reactants - products)
same KE - but PEice<PEwater
0 and 14
Exothermic (?H for ANY sa/sb = -57kJ/mol)

47. What is Big K in terms of kf and kr?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
?G=negative - E° must be positive
Big K=kf/kr
Time?¹ - (ex. s?¹ - hr?¹ - etc)

48. How do you find the pH for a dibasic acid? (H2A)?
Concentration
ns² electrons (first in-first out)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Perform ICE BOX calculation based on K1

49. What type of compounds do metals/non metals form?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Ionic compounds
#ligands=charge x2
zero

50. chlorine
Greenish-yellow gas
a-IMFs - b-molecular volume
-Ea/R
S2O3²?