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. Alkenes are ________ and react by __________
-Ea/R
Unsaturated - addition (ex: decolorize bromine solution)
diamond and graphite
OH- and NH3


2. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
RCHO (carbonyl at end)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
All except for lithium


3. 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.
Add acid to water so that the acid doesn't boil and spit
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Conjugate pair (one must be a weak base or acid)


4. hypochlorite
CN?
ClO?
Mono; di; tri; tetra; penta; hexa.
CrO4²?


5. nitrate
allow for the vapor pressure of water and make sure to level levels
ROH
NO3?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties


6. What is a dipeptide? polypeptide? protein?
It ceases - the circuit is broken.
are less dense than water
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
'non-active' metals such as Cu - Ag - Au - Pt - etc.


7. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
Nothing
OH?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2


8. What is the formula for summation?

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9. How can metals like iron and zinc be reduced?
brown volatile liquid
Pour liquids using a funnel or down a glass rod
chemically (ex: with carbon)
no - they're written undissociated (HAaq)


10. What are isomers?
Heat a test tube at an angle at the side of the tube (not bottom)
Molecules with the same molecular formulas - but different structural formulas
Nothing
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)


11. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
?G=negative - E° must be positive
Greenish-yellow gas
Ksp = 27s4
zero


12. If a weak acid is diluted more - what happens to its % dissociation value?
ROR
H2PO4?
Increases.
look for changes in oxidation # - the one that goes up is oxidized and is the RA


13. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Add acid to water so that the acid doesn't boil and spit
blue (BTB)
water and substances with (s) less dense than
RCOOH


14. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Increases.
No - it depends on the number of ions produced on dissolving.
+4-covalent - +2-ionic


15. What do the 'a' and 'b' in Van Der Waal's equation allow for?
linear
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
a-IMFs - b-molecular volume
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell


16. What is the general formula of an alkane?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
CnH(2n+2)
Iodine and CO2 (dry ice)
zero-th: decreases - first: constant - second: increases


17. dichromate (soln + most solids)
Orange
Products - reactants (except for BDE when it's reactants - products)
voltaic: - electrolytic: +
Ignore 'x' if its K is very small compared to [reactant] (5% rule)


18. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
C4H10
CnH2n+1 often designated 'R' ex C3H7 is propyl
ClO4?


19. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
red - green - blue
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
no - they're written undissociated (HAaq)
neutralization: high K - H2O product dissociation: low K - H2O reactant


20. If a free element is involved - what type of reaction must be involved?
redox reaction
Read the bottom of the meniscus
OH?
bases


21. What is the word equation for addition polymerisation?
Sigma bonds are stronger than pi bonds
bent
hydroxides (ex: Ba(OH)2)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)


22. What is an Alkyl group?

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23. One mole of electrons carries 96500Coulombs - what is this quantity called?

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

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25. What do you need to make a polymer?
linear
Sigma bonds are stronger than pi bonds
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)
White precipitate


26. What does the solubility of organic compounds depend on?
Pale purple - (orange)-yellow - red - blue - green.
CnH2n+1 often designated 'R' ex C3H7 is propyl
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell


27. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
small size and high charge
Reduction always takes place at the cathode (RED CAT) In both types of cell!
An active metal.


28. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Iodine and CO2 (dry ice)
Disulfur dichloride
Acids; HCOOCH3 is an ester


29. mercury (II) ion
OH- and NH3
NH2?
Hg²?
E=q + w (negative is by system - positive is on system)


30. What process do you use to obtain the precipitate from a solution?
How close results are to the accepted value
How grouped results are
Group I metals (soft metals) are stored under oil
Filtration


31. ammonium
NH2?
acid + alcohol
NH4?
Salt + water.


32. What are amphoteric oxides?
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?)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Read the bottom of the meniscus
Mono; di; tri; tetra; penta; hexa.


33. What shape is methane?
bent
More chaotic (ex: gases made)
Tetrahedral
White precipitate


34. BaSO4
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Transition element compounds (except if it has a full or empty d shell)
Read the bottom of the meniscus
Insoluble


35. What type of polymer is nylon?
fruit - fish - bases
ClO2?
Synthetic condensation polymer (aka a polyamide)
ethers


36. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
water and substances with (s) less dense than
diamond and graphite
A) any range. b) 8-10 c) 4-6


37. What are two substances that sublime at 1 atm when heated?
A) any range. b) 8-10 c) 4-6
Iodine and CO2 (dry ice)
Glacial acetic acid
RCOOH


38. How do you heat a test tube?
CO3²?
Heat a test tube at an angle at the side of the tube (not bottom)
ion pairing
Experimental mass/theoretical mass X 100


39. permanganate
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
MnO4?


40. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
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)


41. If Q < Ksp a ppt ______
T increases exponentially the proportion of molecules with E > Ea
Evaporation
a-IMFs - b-molecular volume
Ppt will NOT form (unsaturated)


42. What shape is carbon dioxide?
H2PO4?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
linear
Ions go through the salt bridge - electrons go through metal wires in the external circuit


43. Is the standard entropy (S°) of an element zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
But S° of element is not zero (except at 0K)
Heptane
Iodine and CO2 (dry ice)


44. How does the melting point of a mixture compare to the MP of a pure substance?

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45. What things should you remember to do when collecting gas over water?
H3PO4
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
allow for the vapor pressure of water and make sure to level levels


46. acetate
CH3COO?
Group 1 hydroxides (ex: NaOH)
left - ppt will form
it's lower and occurs over less sharp a range


47. At what point during titration do you have the perfect buffer - and what is the pH at this point?
left - ppt will form
At half equivalence - pH=pKa
Mn²? - Cr³? - Cr³
Ions go through the salt bridge - electrons go through metal wires in the external circuit


48. What apparatus do you use to pour liquids?
red - green - blue
OH- and NH3
Pour liquids using a funnel or down a glass rod
water and substances with (s) less dense than


49. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
Greenish-yellow gas
Increases.
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
There's one normal boiling point (1 atm) - but many boiling points (P dependent)


50. What are the common strong bases?
Group 1 hydroxides (ex: NaOH)
Sulfur
Add acid to water so that the acid doesn't boil and spit
Clear