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Test your basic knowledge |
AP Chemistry 2
Start Test
Study First
Subjects
:
science
,
ap
,
chemistry
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?