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. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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


2. permanganate
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ns² electrons (first in-first out)
MnO4?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.


3. What do acids plus active metals form?
ns² electrons (first in-first out)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
ethers
chemically (ex: with carbon)


4. A Bronsted-Lowry acid is...
voltaic: - electrolytic: +
allow for the vapor pressure of water and make sure to level levels
proton donor base
methyl formate


5. What are isomers?
atoms
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
How close results are to the accepted value
Molecules with the same molecular formulas - but different structural formulas


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

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


7. 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


8. What shape is carbon dioxide?
Insoluble except nitrate and acetate
Hg²?
linear
ethers


9. What is H2CO3 (carbonate acid) usually written as?
Most are soluble except Ag - Pb
blue (BTB)
H2O + CO2 (it decomposes readily)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)


10. What is the general formula for an amine?
RNH2
Read the bottom of the meniscus
Transition element compounds (except if it has a full or empty d shell)
Insoluble except for nitrate and acetate


11. What word is a clue for a redox reaction?
Conjugate pair (one must be a weak base or acid)
Acidified
Both electrons come from the same atom (just as good as a regular bond)
acid + alcohol


12. How do you clean a buret/pipette for a titration?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
ns² electrons (first in-first out)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.


13. What are the units of the first order rate constant?
Making sigma bonds and holding lone pairs
Exothermic
RX
Time?¹ - (ex. s?¹ - hr?¹ - etc)


14. How many normal boiling points and boiling points are there?

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


15. mercury (II) ion
Hg²?
Clear
Greenish-yellow gas
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?


16. lead compounds
Insoluble except nitrate and acetate
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Ksp = s²
Acids; HCOOCH3 is an ester


17. What are amphoteric oxides?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
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?)
Synthetic condensation polymer (aka a polyamide)
More chaotic (ex: gases made)


18. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
How grouped results are
They decrease (or could be the same if the solid has ONLY JUST disappeared)
?G= -ve - E°= +ve
Anode - oxygen. Cathode - hydrogen


19. What is the general formula for an ether?
bright yellow
Salt + water
Experimental mass/theoretical mass X 100
ROR


20. Which value of R do you use for all energy and kinetics calculations?
No - it depends on the number of ions produced on dissolving.
water and substances with (s) less dense than
brown volatile liquid
R=8.31 J/mol/K


21. Ions are not ______.
ROR
atoms
metal oxides and hydrides are ionically bonded and basic
Big K=kf/kr


22. What process do you use to separate two liquids with different boiling points?
fractional distillation
Insoluble except nitrate and acetate
0 and 14
acid + alcohol


23. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
ethers
CrO4²?
Identity and purity (impure compounds usually have broad & low melting points)


24. What is the basic structure of an optical isomer?
Cu3(PO4)2
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
H3PO4
basic


25. How are metal oxides and hydrides bonded? are they acidic or basic?
Synthesis - separation and purification of the product and its identification.
K2
CnH2n+1 often designated 'R' ex C3H7 is propyl
metal oxides and hydrides are ionically bonded and basic


26. What is an Alkyl group?

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


27. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Insoluble except group 1 and ammonium
a-IMFs - b-molecular volume
blue glass - it filters UV
hydroxides (ex: Ba(OH)2)


28. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
SO4²?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
#ligands=charge x2


29. What are two allotropes of carbon?
Hg²?
Initiation energy (NOT Ea)
Heat a test tube at an angle at the side of the tube (not bottom)
diamond and graphite


30. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
#ligands=charge x2
They decrease (or could be the same if the solid has ONLY JUST disappeared)
The compound with the lowest Ksp value.


31. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
blue (BTB)
K1 x K2
Ksp = 4s³
Reduction always takes place at the cathode (RED CAT) In both types of cell!


32. carbonate
CO3²?
Soluble
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Ksp = 4s³


33. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
a-IMFs - b-molecular volume
'non-active' metals such as Cu - Ag - Au - Pt - etc.


34. 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


35. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
allow for the vapor pressure of water and make sure to level levels
H+
Only temperature
Both electrons come from the same atom (just as good as a regular bond)


36. How many faradays of electric charge do you need to produce one mole of O2? H2?
voltaic: + electrolytic: -
O2 needs 4F/mol H2 needs 2F/mol
zero
Acids; HCOOCH3 is an ester


37. What device would you use to measure a volume of gas?
Eudiometer
it's lower and occurs over less sharp a range
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
Silvery gray solid - brown - purple


38. barium sulfate
Heat a test tube at an angle at the side of the tube (not bottom)
White precipitate
neutralization: high K - H2O product dissociation: low K - H2O reactant
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.


39. How are strong ones written?
Saturated - Substitution (which requires more radical conditions)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Pale yellow
strong acids/bases are written as H+ or OH- ions


40. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
neutralization: high K - H2O product dissociation: low K - H2O reactant
RCOOR
CO2 and H2O


41. Both Acetic acid and ____________ are also functional isomers.
methyl formate
Insoluble except for nitrate and acetate
CH3COO?
H+


42. Colorless doesn't mean ______
Clear
q=mc?T q=mL (or n x ?h)
CnH2n-2
Current - time and charge on ion (moles of e used in half cell reaction)


43. The definition of acidic basic and neutral aqueous solutions is:
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Combine the equations for the half reactions in the non-spontaneous direction
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
ethers


44. What are the formulas for q?
H2PO4?
atoms
q=mc?T q=mL (or n x ?h)
Soluble


45. sulfate
Iodine and CO2 (dry ice)
SO4²?
Glacial acetic acid
CO2 and H2O


46. What are two substances that sublime at 1 atm when heated?
S crystal at 0K=0
CnH2n+1 often designated 'R' ex C3H7 is propyl
Combine the equations for the half reactions in the non-spontaneous direction
Iodine and CO2 (dry ice)


47. Esterification is...
voltaic: + electrolytic: -
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
They stay the same.
acid + alcohol


48. What is the name of S2Cl2? (Know how to name others like this - too)
zero
NH4?
Disulfur dichloride
Insoluble


49. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
Pale yellow
Increases down group 1 decreases down group 17
ClO3?


50. For a dibasic acid (H2A) - [A²?]= ____ ?
red - green - blue
Identity and purity (impure compounds usually have broad & low melting points)
K2
CN?