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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 can supercooling occur? What does it look like on a cooling curve?
2. The definition of acidic basic and neutral aqueous solutions is:
fruit - fish - bases
E=q + w (negative is by system - positive is on system)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
3. What is the formula of butane?
Identity and purity (impure compounds usually have broad & low melting points)
blue (BTB)
C4H10
ion pairing
4. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Pour liquids using a funnel or down a glass rod
Hg2²?
CO2 and H2O
K1 x K2
5. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
Iodine and CO2 (dry ice)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Ksp = 4s³
6. carbonate
No - it depends on the number of ions produced on dissolving.
RCHO (carbonyl at end)
CO3²?
bent
7. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Glacial acetic acid
Nothing
catalyst=conc H2SO4
a-IMFs - b-molecular volume
8. If a free element is involved - what type of reaction must be involved?
voltaic: + electrolytic: -
Eudiometer
Greenish-yellow gas
redox reaction
9. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
K2
zero
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
10. nitrates
Eudiometer
Soluble
The one with most oxygen atoms (highest oxidation number)
Pour liquids using a funnel or down a glass rod
11. Are weak acids (and bases) written dissociated?
12. Can you collect soluble gases over water?
it is lower and occurs over less sharp a range
S crystal at 0K=0
No - NH3 and HCl gases are extremely soluble
zero-th: decreases - first: constant - second: increases
13. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
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.
voltaic: + electrolytic: -
H2O + CO2 (it decomposes readily)
14. group 1 ions/compounds
?G=negative - E° must be positive
bases
Soluble
redox reaction
15. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Group I metals (soft metals) are stored under oil
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
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.
CO (poisonous)
16. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Equivalence point is the titrant volume when the moles of acid and base are stoichiometrically equal; end point is the titrant volume when the color of the indicator permanently changes. If you choose the correct indicator - they should occur at the
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.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Acid rain - dissolves marble buildings/statues and kills trees.
17. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Synthesis - separation and purification of the product and its identification.
At half equivalence - pH=pKa
zero
ROH
18. What is the slope of the graph of lnk vs. 1/T?
Selective absorption
-Ea/R
ethers
zero
19. thiosulfate
it's lower and occurs over less sharp a range
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
S2O3²?
fruit - fish - bases
20. What two types of substances are present in all redox reactions?
CH3COO?
allow for the vapor pressure of water and make sure to level levels
a-IMFs - b-molecular volume
an oxidized and reduced substance
21. What things should you remember to do when collecting gas over water?
blue
|experimental - accepted|/accepted X 100
Salt + water
allow for the vapor pressure of water and make sure to level levels
22. What are isotopes?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
different forms of the same element
[A?]/[HA] x 100 or [BH?]/[B] x 100
an oxidized and reduced substance
23. What are the common strong bases?
A) any range. b) 8-10 c) 4-6
ion pairing
Group 1 hydroxides (ex: NaOH)
They stay the same.
24. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
A) any range. b) 8-10 c) 4-6
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
ionic and form hydrogen and hydroxide
basic
25. What is the conjugate acid of H2PO4?
E=q + w (negative is by system - positive is on system)
H3PO4
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
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)
26. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
Salt + water
Synthetic condensation polymer (aka a polyamide)
Clear
27. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
An active metal.
Soluble
Mn²? - Cr³? - Cr³
R=8.31 J/mol/K
28. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
CnH2n+2
Evaporation
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
29. What type of compounds do Group 14 form?
Soluble
Read the bottom of the meniscus
Conjugate pair (one must be a weak base or acid)
+4-covalent - +2-ionic
30. What are allotropes?
proton acceptor.
CO (poisonous)
0 and 14
different forms of the same element
31. What value of R do you use for thermo calculations? gas calculations?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
catalyst=conc H2SO4
atoms
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
32. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
NH4?
The compound with the lowest Ksp value.
Mn²? - Cr³? - Cr³
neutralization: high K - H2O product dissociation: low K - H2O reactant
33. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
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)
C4H10
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
34. What is the general formula for an amine?
Identity and purity (impure compounds usually have broad & low melting points)
no - they're written undissociated (HAaq)
RNH2
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
35. What is H2CO3 (carbonate acid) usually written as?
Nothing
NO3?
H2O + CO2 (it decomposes readily)
Ppt will NOT form (unsaturated)
36. What do hydrocarbons form when they burn in air (oxygen)?
RX
CO2 and H2O
S crystal at 0K=0
Most INsoluble except group 1 and ammonium
37. What changes Keq?
Only temperature
linear
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
ClO4?
38. What is Big K in terms of kf and kr?
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)
E=q + w (negative is by system - positive is on system)
Transition element compounds (except if it has a full or empty d shell)
Big K=kf/kr
39. What effect does increasing the size/surface area of a voltaic cell have on the cell?
The Faraday or Faraday's constant.
Ionic compounds
strong acids/bases are written as H+ or OH- ions
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
40. mercury (II) ion
Hg²?
10?8
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
left - ppt will form
41. What reacts with an acid to create hydrogen gas?
At half equivalence - pH=pKa
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.
An active metal.
RX
42. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
0 and 14
#ligands=charge x2
Decant
43. ammonium/ammonium compounds
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Soluble
Selective absorption
water and substances with (s) less dense than
44. Give an example of a concentrated weak acid.
?G=negative - E° must be positive
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Insoluble except for nitrate and acetate
Glacial acetic acid
45. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Purple
Check for air bubbles in the buret and remove the buret funnel from the buret
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
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
46. How does the melting point of a mixture compare to the MP of a pure substance?
47. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
Only temperature
Insoluble (except group 1 ammonium and Ba)
Cu3(PO4)2
48. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
CN?
basic
Ksp = s²
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
49. acetates
Iodine and CO2 (dry ice)
Soluble
same KE - but PEice<PEwater
benzene is less reactive than alkenes
50. What do group I/II metal oxides and acids form?
Making sigma bonds and holding lone pairs
Salt and water
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)
Glacial acetic acid