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. What is precision?
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)
SO4²?
How grouped results are
Perform ICE BOX calculation based on K1

2. iodine - iodine solution - iodine vapor
Insoluble (except group 1 ammonium and Ba)
Silvery gray solid - brown - purple
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
CnH2n-2

3. What element is used to vulcanize rubber?
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)
Sulfur
A salt solution.
Group I metals (soft metals) are stored under oil

4. chlorine
blue (BTB)
Greenish-yellow gas
RCOOH
Concentration

5. acetate
ethers
Synthetic condensation polymer (aka a polyamide)
S2O3²?
CH3COO?

6. How do you clean a buret/pipette for a titration?
OH?
Soluble
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Soluble

7. What is H2CO3 (carbonate acid) usually written as?
fractional distillation
10?8
RCHO (carbonyl at end)
H2O + CO2 (it decomposes readily)

8. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
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
are less dense than water
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

9. Color is due to ______ _______ of light.
Making sigma bonds and holding lone pairs
Selective absorption
H2O + CO2 (it decomposes readily)
Salt and water

10. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
blue glass - it filters UV
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Salt + water.

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

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

12. Nonmetals are good _____ agents. Metals are good _______ agents.
Soluble
Soluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
CnH2n+1 often designated 'R' ex C3H7 is propyl

13. What is the word equation for addition polymerisation?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
neutralization: high K - H2O product dissociation: low K - H2O reactant
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

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

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

15. carbonate
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Group 1 hydroxides (ex: NaOH)
CnH2n+2
CO3²?

16. A Bronsted-Lowry base is...
C4H10
They stay the same.
proton acceptor.
Combine the equations for the half reactions in the non-spontaneous direction

17. 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

18. How many faradays of electric charge do you need to produce one mole of O2? H2?
CnH2n+1 often designated 'R' ex C3H7 is propyl
zero-th: decreases - first: constant - second: increases
Insoluble except group 1 and ammonium
O2 needs 4F/mol H2 needs 2F/mol

19. Alkenes are ________ and react by __________
Soluble
Unsaturated - addition (ex: decolorize bromine solution)
Insoluble (except group 1 ammonium and Ba)
The benzene ring (or more correctly the phenyl group - C6H5)

20. How do you identify which is oxidized or otherwise?
Cu3(PO4)2
look for changes in oxidation # - the one that goes up is oxidized and is the RA
RCHO (carbonyl at end)
Selective absorption

21. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Most INsoluble except group 1 and ammonium
Anode - oxygen. Cathode - hydrogen
RCOR
Transition element compounds (except if it has a full or empty d shell)

22. permanganate
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)
C4H10
More chaotic (ex: gases made)
MnO4?

23. dichromate
zero
No - NH3 and HCl gases are extremely soluble
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Cr2O7²?

24. How do you get Ecell for spontaneous reactions?
Ksp = 27s4
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.
Synthesis - separation and purification of the product and its identification.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

25. How do you get the equation for a net electrolysis reaction?
allow for the vapor pressure of water and make sure to level levels
Combine the equations for the half reactions in the non-spontaneous direction
Only temperature
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

26. When is ?G zero?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
ClO?
Insoluble
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

27. What device would you use to measure a volume of gas?
Acids; HCOOCH3 is an ester
Reduction always takes place at the cathode (RED CAT) In both types of cell!
?G=negative - E° must be positive
Eudiometer

28. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
neutralization: high K - H2O product dissociation: low K - H2O reactant
+4-covalent - +2-ionic
Orange

29. 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
Salt + water.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Insoluble except for nitrate and acetate

30. What is the test for hydrogen?
lighted splint (positive result=pop)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Insoluble except group 1 and ammonium
Read the bottom of the meniscus

31. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
NO3?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
ClO3?

32. What should you check for before you begin titrating?
a-IMFs - b-molecular volume
Check for air bubbles in the buret and remove the buret funnel from the buret
zero
acid + alcohol

33. How do you explain trends in atomic properties using Coulomb's Law?
Iodine and CO2 (dry ice)
Soluble
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

34. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
are less dense than water
CO (poisonous)
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)

35. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
#ligands=charge x2
H+
different forms of the same element
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.

36. potassium permanganate
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
it is lower and occurs over less sharp a range
Purple
How grouped results are

37. halides
Suniverse increases for spontaneous processes
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Most are soluble except Ag - Pb
Conjugate pair (one must be a weak base or acid)

38. What measuring device would you use for very small volumes of liquids?
Sigma bonds are stronger than pi bonds
Pipette (burette if need repetition)
Insoluble except nitrate and acetate
Nothing

39. hydroxide
E=q + w (negative is by system - positive is on system)
zero
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
OH?

40. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Insoluble except for nitrate and acetate
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
ion pairing
Soluble

41. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
A salt solution.
diamond and graphite
Selective absorption

42. What are two substances that sublime at 1 atm when heated?
#ligands=charge x2
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
All except for lithium
Iodine and CO2 (dry ice)

43. What process do you use to obtain a solvent from a solution?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Distillation
'non-active' metals such as Cu - Ag - Au - Pt - etc.
yellow

44. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
The Faraday or Faraday's constant.
Evaporation
ionic and form hydrogen and hydroxide

45. When a cell is 'flat' What is its voltage?
zero
?G= -ve - E°= +ve
lighted splint (positive result=pop)
acids

46. bromine
Combine the equations for the half reactions in the non-spontaneous direction
Reduction always takes place at the cathode (RED CAT) In both types of cell!
RCOR
brown volatile liquid

47. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Kc=Kp
How grouped results are
R=8.31 J/mol/K

48. silver compounds
strong acids/bases are written as H+ or OH- ions
Reduction always takes place at the cathode (RED CAT) In both types of cell!
NO3?
Insoluble except for nitrate and acetate

49. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
bases
neutralization: high K - H2O product dissociation: low K - H2O reactant
How close results are to the accepted value

50. Alcohols and _______ are FG isomers
ethers
zero
Current - time and charge on ion (moles of e used in half cell reaction)
ns² electrons (first in-first out)