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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 process do you use to obtain the precipitate from a solution?
Filtration
bases
H2O + CO2 (it decomposes readily)
Ionic compounds

2. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Iodine and CO2 (dry ice)
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 type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
P2O5
look for changes in oxidation # - the one that goes up is oxidized and is the RA
It ceases - the circuit is broken.

4. What shape is methane?
brown volatile liquid
Synthetic condensation polymer (aka a polyamide)
Tetrahedral
?H formation of an element in standard state=0

5. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
T increases exponentially the proportion of molecules with E > Ea
The dilution effect when the solutions mix. M1V1 = M2V2
proton donor base

6. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
small size and high charge
Salts (ex: CaO + SO2 ? CaSO3)
CO2 and H2O

7. hydroxides
Filtration
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Insoluble (except group 1 ammonium and Ba)

8. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
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.
it reacts by substitution NOT addition
voltaic: + electrolytic: -
H+

9. What type of solutions do small - highly charged cations tend to form?
Eudiometer
Salt + water.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Tetrahedral

10. What do you need to make a polymer?
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
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)
Heat a test tube at an angle at the side of the tube (not bottom)
0.10M HCl (more ions)

11. acetates
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
no - they're written undissociated (HAaq)
More chaotic (ex: gases made)
Soluble

12. silver iodide
left - ppt will form
Pale yellow
allow for the vapor pressure of water and make sure to level levels
different forms of the same element

13. What do group I/II metal oxides plus water form?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Filtration
bases
The compound with the lowest Ksp value.

14. What are the common strong bases?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
The Faraday or Faraday's constant.
Group 1 hydroxides (ex: NaOH)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

15. chlorine
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Greenish-yellow gas
CN?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

16. Give an example of a dilute strong acid.
it is lower and occurs over less sharp a range
zero
boiling without losing volatile solvents/reactants
HClO4

17. How do you explain trends in atomic properties using Coulomb's Law?
it is lower and occurs over less sharp a range
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Pour liquids using a funnel or down a glass rod

18. What is the relationship in strength between sigma and pi bonds?
Glowing splint (positive result=relights)
Sigma bonds are stronger than pi bonds
do not change
OH?

19. What are the units of the first order rate constant?
CnH2n-2
Time?¹ - (ex. s?¹ - hr?¹ - etc)
diamond and graphite
redox reaction

20. What is the formula for percent yield?
H3PO4
Soluble
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Experimental mass/theoretical mass X 100

21. Name some properties of Group 17
acids
C4H10
water and substances with (s) less dense than
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

22. Is the freezing of ice endothermic or exothermic?
Sulfur
Acids; HCOOCH3 is an ester
Clear
Exothermic

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

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24. What process do you use to separate two liquids with different boiling points?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
ROR
fractional distillation

25. How are non-metal oxides and hydrides bonded? are they acidic or basic?
benzene is less reactive than alkenes
benzene has a delocalized pi ring structure
non-metal oxides and hydrides are covalently bonded and are acidic.
same KE - but PEice<PEwater

26. What do acids plus active metals form?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
MnO4?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

27. Name 2 ways in which you can create a buffer?
chemically (ex: with carbon)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
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)

28. What are the names and formulas of the 6 strong acids?
a-IMFs - b-molecular volume
Evaporation
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Iodine and CO2 (dry ice)

29. What is the conjugate base of NH3?
Salt + water.
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)
NH2?
The Faraday or Faraday's constant.

30. What is the general formula for an ether?
Soluble
CH3COO?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
ROR

31. What is accuracy?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Insoluble except for nitrate and acetate
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
How close results are to the accepted value

32. chlorite
ClO2?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

33. BaSO4
ns² electrons (first in-first out)
Insoluble
yellow
Identity and purity (impure compounds usually have broad & low melting points)

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

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35. chlorate
ClO3?
Pale yellow
0.10M HCl (more ions)
voltaic: - electrolytic: +

36. What are isotopes?
#ligands=charge x2
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Saturated - Substitution (which requires more radical conditions)
Iodine and CO2 (dry ice)

37. What is the general formula for an ester?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
C2O4²?
RCOOR
R=8.31 J/mol/K

38. What do metal oxides plus non- metal oxides form?
NH4?
Graduated cylinder
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Salts (ex: CaO + SO2 ? CaSO3)

39. What do group I/II metal oxides and acids form?
Salt and water
zero-th: decreases - first: constant - second: increases
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Ksp = 27s4

40. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
?G=negative - E° must be positive
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Products - reactants (except for BDE when it's reactants - products)

41. What does saturated mean? Unsaturated?
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.
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
The dilution effect when the solutions mix. M1V1 = M2V2

42. What word is a clue for a redox reaction?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Acidified
ClO3?
CnH2n-2

43. How do you clean a buret/pipette for a titration?
Purple
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
fractional distillation
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

44. What are two allotropes of carbon?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
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.
diamond and graphite
acid + alcohol

45. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
zero
Kc=Kp
H2O + CO2 (it decomposes readily)
non-metal oxides and hydrides are covalently bonded and are acidic.

46. What is the difference between equivalence point and end point of a titration.
Pale purple - (orange)-yellow - red - blue - green.
ClO2?
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
it is lower and occurs over less sharp a range

47. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
#ligands=charge x2
Experimental mass/theoretical mass X 100
0.10M HCl (more ions)

48. lead compounds
No - NH3 and HCl gases are extremely soluble
Insoluble except nitrate and acetate
Group 1 hydroxides (ex: NaOH)
K2

49. When the salt bridge is removed what happens to the cell reaction?
Mono; di; tri; tetra; penta; hexa.
They stay the same.
It ceases - the circuit is broken.
Separating funnel

50. What is the test for hydrogen?
lighted splint (positive result=pop)
Clear
Soluble except Ag - Pb - Ca - Sr Ba)
ROR