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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. When driving off water from a hydrate - how do you tell you're done?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
fruit - fish - bases
Anode - oxygen. Cathode - hydrogen
acid + alcohol

2. What equipment do you need for a titration?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
redox reaction
They decrease (or could be the same if the solid has ONLY JUST disappeared)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

3. What shape is ammonia?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Trigonal pyramidal
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.
CnH2n

4. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
voltaic: - electrolytic: +
Heptane
left - ppt will form

5. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Pour liquids using a funnel or down a glass rod
yellow

6. When the salt bridge is removed what happens to the cell reaction?
Current - time and charge on ion (moles of e used in half cell reaction)
It ceases - the circuit is broken.
Hg²?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

7. What do you do to get rid of most of the solution from a precipitate?
hydroxides (ex: Ba(OH)2)
#ligands=charge x2
Distillation
Decant

8. When a cell is 'flat' What is its voltage?
Filtration
zero
Combine the equations for the half reactions in the non-spontaneous direction
CnH(2n+2)

9. dichromate
boiling without losing volatile solvents/reactants
Cr2O7²?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Trigonal pyramidal

10. What are the prefixes for the naming of binary molecular compound formulas (up to six)
ClO4?
Mono; di; tri; tetra; penta; hexa.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Separating funnel

11. A Bronsted-Lowry acid is...
proton donor base
It ceases - the circuit is broken.
ClO2?
do not change

12. What do metal oxides plus acids form?
RX
Salt + water
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
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.

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

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14. What do the 'a' and 'b' in Van Der Waal's equation allow for?
CH3COO?
a-IMFs - b-molecular volume
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
it is lower and occurs over less sharp a range

15. What is the general formula for a ketone?
RCOR
zero
linear
K2

16. primary colors
Evaporation
red - green - blue
S2O3²?
an oxidized and reduced substance

17. Which alkali metals float on water?
CO3²?
Sulfur
All except for lithium
Group I metals (soft metals) are stored under oil

18. What do the 'a' and 'b' in Van Der Waal's equation allow for?
NH2?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
a-IMFs - b-molecular volume
Distillation

19. Alcohols and _______ are FG isomers
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
ethers
ns² electrons (first in-first out)
Mono; di; tri; tetra; penta; hexa.

20. hypochlorite
ClO?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
A) any range. b) 8-10 c) 4-6
#ligands=charge x2

21. What is precision?
ClO2?
Acidified
They stay the same.
How grouped results are

22. Is the freezing of ice endothermic or exothermic?
Exothermic
+4-covalent - +2-ionic
Identity and purity (impure compounds usually have broad & low melting points)
Heat a test tube at an angle at the side of the tube (not bottom)

23. How can metals like iron and zinc be reduced?
Transition element compounds (except if it has a full or empty d shell)
Perform ICE BOX calculation based on K1
chemically (ex: with carbon)
bases

24. chlorine
Insoluble (except group 1 ammonium and Ba)
CO3²?
Greenish-yellow gas
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

25. Aromatic compounds contain what?
Salt + water.
Anode
it's lower and occurs over less sharp a range
The benzene ring (or more correctly the phenyl group - C6H5)

26. chromate
But S° of element is not zero (except at 0K)
CN?
OH?
CrO4²?

27. What is an Alkyl group?

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28. What is the word equation for addition polymerisation?
ClO3?
HClO4
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

29. carbonate
allow for the vapor pressure of water and make sure to level levels
CO3²?
Pale purple - (orange)-yellow - red - blue - green.
Purple

30. What are hybrid orbitals used for?
Acids; HCOOCH3 is an ester
Q=It (time in seconds)
Making sigma bonds and holding lone pairs
Ksp = 27s4

31. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
OH- and NH3
Separating funnel
Exothermic (?H for ANY sa/sb = -57kJ/mol)

32. Which value of R do you use for all energy and kinetics calculations?
Transition element compounds (except if it has a full or empty d shell)
zero
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
R=8.31 J/mol/K

33. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
RX
?G= -ve - E°= +ve
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
ion pairing

34. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
All except for lithium
hydroxides (ex: Ba(OH)2)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

35. ammonium
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
NH4?
do not change
How grouped results are

36. What is HCOOCH3?
?G=negative - E° must be positive
benzene is less reactive than alkenes
Pale yellow
Acids; HCOOCH3 is an ester

37. If Q > Ksp - then system shifts _______ and ppt ______
Salt + water
OH- and NH3
Exothermic (?H for ANY sa/sb = -57kJ/mol)
left - ppt will form

38. Ions are not ______.
Insoluble except nitrate and acetate
atoms
proton acceptor.
Conjugate pair (one must be a weak base or acid)

39. What is the conjugate acid of H2PO4?
NH4?
H3PO4
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.
Pour liquids using a funnel or down a glass rod

40. Acid plus base make?
RCHO (carbonyl at end)
Salt + water.
P2O5
[A?]/[HA] x 100 or [BH?]/[B] x 100

41. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
0.10M HCl (more ions)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
All except for lithium
H+

42. halides
'non-active' metals such as Cu - Ag - Au - Pt - etc.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Most are soluble except Ag - Pb
by electrolysis

43. What apparatus do you use to separate 2 immiscible liquids?
10?8
Synthetic condensation polymer (aka a polyamide)
Separating funnel
OH- and NH3

44. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
C4H10
ClO2?
by electrolysis
same KE - but PEice<PEwater

45. How do you clean a buret/pipette for a titration?
Ksp = s²
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.
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)

46. If a free element is involved - what type of reaction must be involved?
voltaic: - electrolytic: +
redox reaction
Increases.
H3PO4

47. What is the sign of the anode in voltaic cells? in electrolytic cells?
?G= -ve - E°= +ve
proton acceptor.
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)
voltaic: - electrolytic: +

48. How are strong ones written?
zero
CrO4²?
strong acids/bases are written as H+ or OH- ions
Only temperature

49. mercury (I) ion
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
bright yellow
Saturated - Substitution (which requires more radical conditions)
Hg2²?

50. Generally - which oxy acid is strongest?
linear
OH- and NH3
The one with most oxygen atoms (highest oxidation number)
OH?