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. How do you heat a test tube?
K2
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
No - it depends on the number of ions produced on dissolving.
Heat a test tube at an angle at the side of the tube (not bottom)


2. What type of polymer is nylon?
Products - reactants (except for BDE when it's reactants - products)
Synthetic condensation polymer (aka a polyamide)
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.
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)


3. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
Iodine and CO2 (dry ice)
acid + alcohol
Time?¹ - (ex. s?¹ - hr?¹ - etc)


4. 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?
Ionic compounds
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
The compound with the lowest Ksp value.
Insoluble except nitrate and acetate


5. What is the sign of the anode in voltaic cells? in electrolytic cells?
The one with most oxygen atoms (highest oxidation number)
Q=It (time in seconds)
voltaic: - electrolytic: +
Time?¹ - (ex. s?¹ - hr?¹ - etc)


6. When driving off water from a hydrate - how do you tell you're done?
NH4?
Add acid to water so that the acid doesn't boil and spit
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)


7. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
Perform ICE BOX calculation based on K1
S crystal at 0K=0
CnH(2n+2)


8. If ?S is positive - are the products more or less chaotic than the reactants?
metal oxides and hydrides are ionically bonded and basic
More chaotic (ex: gases made)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
proton donor base


9. How are strong ones written?
Q=It (time in seconds)
Glowing splint (positive result=relights)
Current - time and charge on ion (moles of e used in half cell reaction)
strong acids/bases are written as H+ or OH- ions


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

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11. What equipment do you need for a titration?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Combine the equations for the half reactions in the non-spontaneous direction
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask


12. What do metal oxides plus non- metal oxides form?
fractional distillation
Insoluble except group 1 and ammonium
Ksp = 4s³
Salts (ex: CaO + SO2 ? CaSO3)


13. carbonates
?G=negative - E° must be positive
Insoluble except group 1 and ammonium
RNH2
0 and 14


14. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Insoluble except group 1 and ammonium
Perform ICE BOX calculation based on K1
small size and high charge
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2


15. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Increases.
fruit - fish - bases
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)


16. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Ksp = 108s5
0 and 14
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.


17. What changes Keq?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Only temperature
a-IMFs - b-molecular volume
left - ppt will form


18. ammonium
NH4?
ethers
no - they're written undissociated (HAaq)
Suniverse increases for spontaneous processes


19. ammonium/ammonium compounds
Ksp = 4s³
Salts (ex: CaO + SO2 ? CaSO3)
Soluble
Increases down group 1 decreases down group 17


20. What is the general formula for an amine?
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)
Salt + water.
RNH2
blue


21. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Eudiometer
H+
Conjugate pair (one must be a weak base or acid)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)


22. How do you compute % dissociation?
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
No - it depends on the number of ions produced on dissolving.
[A?]/[HA] x 100 or [BH?]/[B] x 100
MnO4?


23. How are metal oxides and hydrides bonded? are they acidic or basic?
metal oxides and hydrides are ionically bonded and basic
Distillation
fruit - fish - bases
methyl formate


24. How do you dilute an acid?

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25. Esterification is...
acid + alcohol
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Hg²?
are less dense than water


26. Colorless doesn't mean ______
Silvery gray solid - brown - purple
CnH(2n+2)
a-IMFs - b-molecular volume
Clear


27. carbonate
CO3²?
Heat a test tube at an angle at the side of the tube (not bottom)
neutralization: high K - H2O product dissociation: low K - H2O reactant
Orange


28. chlorine
Ksp = 27s4
All except for lithium
PO4³?
Greenish-yellow gas


29. What type of solutions do small - highly charged cations tend to form?
Anode
lighted splint (positive result=pop)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Clear


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

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31. What process do you use to obtain the solute from a solution?
H+
P2O5
Evaporation
Synthesis - separation and purification of the product and its identification.


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

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33. What is the formula for alkenes?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
K2
CnH2n


34. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
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)
CnH2n-2
Disulfur dichloride
Current - time and charge on ion (moles of e used in half cell reaction)


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

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36. What is the general formula for an ether?
ROR
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
More chaotic (ex: gases made)
Filtration


37. What is the third law of thermodynamics?
Soluble
They stay the same.
S crystal at 0K=0
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]


38. How many ligands attach to a central ion in a complex ion?
methyl formate
acids
#ligands=charge x2
Ions go through the salt bridge - electrons go through metal wires in the external circuit


39. Name some properties of Group 17
The one with most oxygen atoms (highest oxidation number)
NH4?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant


40. What are hybrid orbitals used for?
CO3²?
it's lower and occurs over less sharp a range
Making sigma bonds and holding lone pairs
CnH2n-2


41. How does the melting point of a mixture compare to the MP of a pure substance?
CO2 and H2O
But S° of element is not zero (except at 0K)
it is lower and occurs over less sharp a range
basic


42. phosphate
Greenish-yellow gas
PO4³?
An active metal.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.


43. What element is used to vulcanize rubber?
Sulfur
Most are soluble except Ag - Pb
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Ksp = s²


44. nitrates
Soluble
Hg2²?
blue glass - it filters UV
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K


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

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46. What is the energy you must put into a reaction to make it start called?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Initiation energy (NOT Ea)
non-metal oxides and hydrides are covalently bonded and are acidic.
Combine the equations for the half reactions in the non-spontaneous direction


47. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
The one with most oxygen atoms (highest oxidation number)
-Ea/R


48. What is a coordinate covalent bond?
Sulfur
Both electrons come from the same atom (just as good as a regular bond)
An active metal.
Making sigma bonds and holding lone pairs


49. potassium permanganate
Purple
Heptane
Evaporation
lighted splint (positive result=pop)


50. Acid plus base make?
Acid rain - dissolves marble buildings/statues and kills trees.
K2
methyl formate
Salt + water.