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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. chromate
CrO4²?
An active metal.
Tetrahedral
O2 needs 4F/mol H2 needs 2F/mol

2. What is the test for oxygen?
Glowing splint (positive result=relights)
But S° of element is not zero (except at 0K)
allow for the vapor pressure of water and make sure to level levels
it's lower and occurs over less sharp a range

3. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
yellow
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

4. Name 2 ways in which you can create a buffer?
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)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Insoluble
K1 x K2

5. Is the freezing of ice endothermic or exothermic?
C2O4²?
Acidified
Exothermic
Decant

6. Why are i factors (Van't Hoff factors) often less than ideal?
0 and 14
Current - time and charge on ion (moles of e used in half cell reaction)
RCHO (carbonyl at end)
ion pairing

7. When is ?G zero?
?G= -ve - E°= +ve
An active metal.
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
lighted splint (positive result=pop)

8. 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)
water and substances with (s) less dense than
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Tetrahedral

9. If a weak acid is diluted more - what happens to its % dissociation value?
All except for lithium
Tetrahedral
The benzene ring (or more correctly the phenyl group - C6H5)
Increases.

10. What is Big K in terms of kf and kr?
non-metal oxides and hydrides are covalently bonded and are acidic.
RNH2
Big K=kf/kr
different forms of the same element

11. What are two allotropes of carbon?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
OH?
diamond and graphite
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

12. Esterification is...
Check for air bubbles in the buret and remove the buret funnel from the buret
Cu3(PO4)2
acid + alcohol
MnO4?

13. What word is a clue for a redox reaction?
CO3²?
Acidified
How close results are to the accepted value
ClO3?

14. What are two substances that sublime at 1 atm when heated?
Initiation energy (NOT Ea)
ethers
Ksp = 27s4
Iodine and CO2 (dry ice)

15. What are hybrid orbitals used for?
Saturated - Substitution (which requires more radical conditions)
Making sigma bonds and holding lone pairs
Trigonal pyramidal
bases

16. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Decant
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
a-IMFs - b-molecular volume
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

17. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
MnO4?
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
CO2 and H2O
CnH(2n+2)

18. What is the conjugate acid of H2PO4?
methyl formate
H3PO4
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
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)

19. What are two substances that sublime at 1 atm when heated?
Both electrons come from the same atom (just as good as a regular bond)
Iodine and CO2 (dry ice)
H2O + CO2 (it decomposes readily)
10?8

20. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
red - green - blue

21. How are primary alcohols turned into acids?
Acidified
Products - reactants (except for BDE when it's reactants - products)
NO3?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

22. What part of a liquid do you look at to measure its volume?
Molecules with the same molecular formulas - but different structural formulas
Read the bottom of the meniscus
ethers
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

23. What is an Alkyl group?

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24. How can metals like iron and zinc be reduced?
ns² electrons (first in-first out)
chemically (ex: with carbon)
A salt solution.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

25. What do you do to get rid of most of the solution from a precipitate?
Experimental mass/theoretical mass X 100
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
CH3COO?
Decant

26. ________ are Lewis bases - because they can donate a lone pair of electrons.
OH?
Separating funnel
Perform ICE BOX calculation based on K1
OH- and NH3

27. What value of R do you use for thermo calculations? gas calculations?
ClO2?
Products - reactants (except for BDE when it's reactants - products)
CnH2n+2
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

28. Acidic gases like SO2 in the atmosphere cause what environmental problems?
RCHO (carbonyl at end)
proton donor base
Acid rain - dissolves marble buildings/statues and kills trees.
NH4?

29. What two types of substances are present in all redox reactions?
PO4³?
no - they're written undissociated (HAaq)
Salt and water
an oxidized and reduced substance

30. ammonium/ammonium compounds
Soluble
Iodine and CO2 (dry ice)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

31. What two compounds are great oxidizing agents?

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32. What are the formulas for q?
RCOOR
q=mc?T q=mL (or n x ?h)
C2O4²?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

33. Does reactivity increase/decrease going down group 1 and group 17?
Eudiometer
Increases down group 1 decreases down group 17
Concentration
Anode

34. How does half life change for zero-th order - first order - and second order processes?
R=8.31 J/mol/K
Glacial acetic acid
CnH2n-2
zero-th: decreases - first: constant - second: increases

35. What is the formula for alkanes?
Insoluble except group 1 and ammonium
allow for the vapor pressure of water and make sure to level levels
CnH2n+2
Ksp = s²

36. silver iodide
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?)
Pale yellow
benzene is less reactive than alkenes
zero

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

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38. What process do you use to separate two liquids with different boiling points?
do not change
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)
fractional distillation
The dilution effect when the solutions mix. M1V1 = M2V2

39. What do nonmetal oxides plus water form?
NO3?
acids
Exothermic (?H for ANY sa/sb = -57kJ/mol)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

40. What is the basic structure of an optical isomer?
K2
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
it's lower and occurs over less sharp a range
ROH

41. How do you get the equation for a net electrolysis reaction?
K1 x K2
Mono; di; tri; tetra; penta; hexa.
Combine the equations for the half reactions in the non-spontaneous direction
Glacial acetic acid

42. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
The one with most oxygen atoms (highest oxidation number)
R=8.31 J/mol/K
NH4?

43. What does a short - sharp melting point indicate?
RCOR
Pour liquids using a funnel or down a glass rod
Identity and purity (impure compounds usually have broad & low melting points)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

44. What do you use to look at burning magnesium? why?
Cr2O7²?
blue glass - it filters UV
Time?¹ - (ex. s?¹ - hr?¹ - etc)
At half equivalence - pH=pKa

45. What is the general formula of an alkane?
CnH(2n+2)
More chaotic (ex: gases made)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

46. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
water and substances with (s) less dense than
bases
red - green - blue

47. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
small size and high charge
CnH2n+1 often designated 'R' ex C3H7 is propyl
Both electrons come from the same atom (just as good as a regular bond)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

48. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
The Faraday or Faraday's constant.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
non-metal oxides and hydrides are covalently bonded and are acidic.
Conjugate pair (one must be a weak base or acid)

49. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
do not change
E=q + w (negative is by system - positive is on system)

50. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
blue
Time?¹ - (ex. s?¹ - hr?¹ - etc)
redox reaction