Test your basic knowledge |

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. What is the formula for obtaining charge flowing in a cell?
Big K=kf/kr
Q=It (time in seconds)
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)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

2. What things should you remember to do when collecting gas over water?
0.10M HCl (more ions)
allow for the vapor pressure of water and make sure to level levels
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
neutralization: high K - H2O product dissociation: low K - H2O reactant

3. What is the second law of thermodynamics?
Suniverse increases for spontaneous processes
zero
benzene has a delocalized pi ring structure
methyl formate

4. Are weak acids (and bases) written dissociated?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

5. hydroxide
strong acids/bases are written as H+ or OH- ions
Filtration
OH?
CnH2n+1 often designated 'R' ex C3H7 is propyl

6. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
Glacial acetic acid
diamond and graphite
0 and 14

7. What do group I/II metal oxides plus water form?
?G=negative - E° must be positive
bases
bright yellow
ns² electrons (first in-first out)

8. What type of metals don't react with water or acids to form H2?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

9. What value of R do you use for thermo calculations? gas calculations?
Ksp = 4s³
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
lighted splint (positive result=pop)
Acid rain - dissolves marble buildings/statues and kills trees.

10. What is the general formula of an alkane?
CnH(2n+2)
it reacts by substitution NOT addition
Disulfur dichloride
Acid rain - dissolves marble buildings/statues and kills trees.

11. silver iodide
Monomer + monomer = polymer product + a simple molecule such as water or HCl
ns² electrons (first in-first out)
Pale yellow
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

12. What kind of bonding structure does benzene have?
Tetrahedral
benzene has a delocalized pi ring structure
atoms
Trigonal pyramidal

13. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
Molecules with the same molecular formulas - but different structural formulas
MnO4?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

15. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
Separating funnel
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

16. Is the standard entropy (S°) of an element zero?
Soluble
But S° of element is not zero (except at 0K)
ion pairing
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

17. What is the formula for alkenes?
+4-covalent - +2-ionic
CnH2n
Acid rain - dissolves marble buildings/statues and kills trees.
OH?

18. An amphiprotic (amphoteric) species is...
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)
No - it depends on the number of ions produced on dissolving.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Graduated cylinder

19. 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.
ClO2?
proton donor base
A) any range. b) 8-10 c) 4-6
blue (BTB)

20. What are the prefixes for the naming of binary molecular compound formulas (up to six)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Products - reactants (except for BDE when it's reactants - products)
Mono; di; tri; tetra; penta; hexa.
Iodine and CO2 (dry ice)

21. When the salt bridge is removed what happens to the cell reaction?
The dilution effect when the solutions mix. M1V1 = M2V2
RCOOR
Unsaturated - addition (ex: decolorize bromine solution)
It ceases - the circuit is broken.

22. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
a-IMFs - b-molecular volume
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Insoluble except nitrate and acetate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

23. primary colors
ionic and form hydrogen and hydroxide
red - green - blue
?H-kJ - ?S-J - ?G-kJ
Insoluble except nitrate and acetate

24. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Purple
ClO2?

25. How do you identify which is oxidized or otherwise?
same KE - but PEice<PEwater
Synthesis - separation and purification of the product and its identification.
look for changes in oxidation # - the one that goes up is oxidized and is the RA
q=mc?T q=mL (or n x ?h)

26. What is a coordinate covalent bond?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Both electrons come from the same atom (just as good as a regular bond)
Only temperature
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

27. barium sulfate
no - they're written undissociated (HAaq)
White precipitate
Sulfur
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

28. chlorine
H2PO4?
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)
Greenish-yellow gas
C4H10

29. Do you use J or kJ for ?H - ?S - and ?G?
Graduated cylinder
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
ClO?
?H-kJ - ?S-J - ?G-kJ

30. nitrates
Heptane
Soluble
An active metal.
+4-covalent - +2-ionic

31. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
ROH
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
0.10M HCl (more ions)

32. chlorate
H2PO4?
allow for the vapor pressure of water and make sure to level levels
ClO3?
Identity and purity (impure compounds usually have broad & low melting points)

33. Ca - Sr - Ba
RCOR
Both electrons come from the same atom (just as good as a regular bond)
hydroxides (ex: Ba(OH)2)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

34. What steps do organic labs consist of?
Synthesis - separation and purification of the product and its identification.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Read the bottom of the meniscus
different forms of the same element

35. Alcohols and _______ are FG isomers
ethers
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
OH- and NH3
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

36. What is the formula for percent yield?
Insoluble except for nitrate and acetate
Experimental mass/theoretical mass X 100
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Salts (ex: CaO + SO2 ? CaSO3)

37. When is ?G zero?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Big K=kf/kr
chemically (ex: with carbon)

38. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
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)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
same KE - but PEice<PEwater
Kc=Kp

39. What is HCOOCH3?
neutralization: high K - H2O product dissociation: low K - H2O reactant
left - ppt will form
Only temperature
Acids; HCOOCH3 is an ester

40. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
RCOOH
CnH(2n+2)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

41. 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?
redox reaction
Anode
The compound with the lowest Ksp value.
yellow

42. When driving off water from a hydrate - how do you tell you're done?
Decant
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Insoluble
proton acceptor.

43. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Making sigma bonds and holding lone pairs

44. Give an example of a dilute strong acid.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
RX
HClO4
Exothermic

45. What is the relationship in strength between sigma and pi bonds?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
S crystal at 0K=0
q=mc?T q=mL (or n x ?h)
Sigma bonds are stronger than pi bonds

46. Name C7H16
Mn²? - Cr³? - Cr³
Synthetic condensation polymer (aka a polyamide)
Heptane
'non-active' metals such as Cu - Ag - Au - Pt - etc.

47. Name six characteristics of transition elements (or their compounds)
S crystal at 0K=0
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)
Ksp = s²
Salt + water.

48. What are two allotropes of carbon?
acids
ns² electrons (first in-first out)
Selective absorption
diamond and graphite

49. What is precision?
zero
Eudiometer
Initiation energy (NOT Ea)
How grouped results are

50. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
Salt and water
CN?
water and substances with (s) less dense than