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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. How do you find the pH for a dibasic acid? (H2A)?
proton donor base
chemically (ex: with carbon)
Perform ICE BOX calculation based on K1
Group I metals (soft metals) are stored under oil

2. Which alkali metals float on water?
T increases exponentially the proportion of molecules with E > Ea
Iodine and CO2 (dry ice)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
All except for lithium

3. What do metal oxides plus non- metal oxides form?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Salts (ex: CaO + SO2 ? CaSO3)
Decant
benzene is less reactive than alkenes

4. What steps do organic labs consist of?
Soluble
Insoluble except group 1 and ammonium
Synthesis - separation and purification of the product and its identification.
Ksp = 108s5

5. How many ligands attach to a central ion in a complex ion?
The one with most oxygen atoms (highest oxidation number)
red - green - blue
K1 x K2
#ligands=charge x2

6. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
'non-active' metals such as Cu - Ag - Au - Pt - etc.
The benzene ring (or more correctly the phenyl group - C6H5)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

7. What are amphoteric oxides?
Hg2²?
chemically (ex: with carbon)
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
ClO4?

8. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Anode - oxygen. Cathode - hydrogen
More chaotic (ex: gases made)
Saturated - Substitution (which requires more radical conditions)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

9. silver compounds
Exothermic
The benzene ring (or more correctly the phenyl group - C6H5)
Insoluble except for nitrate and acetate
zero

10. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
Ksp = 4s³
it is lower and occurs over less sharp a range
Greenish-yellow gas

11. dihydrogen phosphate
water and substances with (s) less dense than
H2PO4?
Soluble except Ag - Pb - Ca - Sr Ba)
CO3²?

12. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Concentration
redox reaction
Salt + water.

13. How does half life change for zero-th order - first order - and second order processes?
Identity and purity (impure compounds usually have broad & low melting points)
zero-th: decreases - first: constant - second: increases
zero
do not change

14. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
RCOOR
same KE - but PEice<PEwater
fruit - fish - bases
Tetrahedral

15. What electrons are lost/gained first in transition element ions?
The dilution effect when the solutions mix. M1V1 = M2V2
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
ns² electrons (first in-first out)
Exothermic

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

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17. What is the slope of the graph of lnk vs. 1/T?
Evaporation
Pale yellow
Ppt will NOT form (unsaturated)
-Ea/R

18. What is the name of S2Cl2? (Know how to name others like this - too)
diamond and graphite
C4H10
CO (poisonous)
Disulfur dichloride

19. bromine
The benzene ring (or more correctly the phenyl group - C6H5)
brown volatile liquid
Nothing
Group 1 hydroxides (ex: NaOH)

20. What is the formula for alkynes?
blue (BTB)
a-IMFs - b-molecular volume
strong acids/bases are written as H+ or OH- ions
CnH2n-2

21. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Insoluble except nitrate and acetate
Unsaturated - addition (ex: decolorize bromine solution)

22. silver iodide
Increases.
acids
Acidified
Pale yellow

23. oxalate
RNH2
C2O4²?
NH2?
K2

24. Colorless doesn't mean ______
Clear
q=mc?T q=mL (or n x ?h)
P2O5
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)

25. What is the general formula for an alcohol?
Molecules with the same molecular formulas - but different structural formulas
H3PO4
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
ROH

26. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
Distillation
zero
Ksp = s²
P2O5

27. What is the second law of thermodynamics?
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)
Suniverse increases for spontaneous processes
Saturated - Substitution (which requires more radical conditions)
Hg2²?

28. What process do you use to obtain a solvent from a solution?
Greenish-yellow gas
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)
The compound with the lowest Ksp value.
Distillation

29. Alkenes are ________ and react by __________
Ksp = 4s³
Unsaturated - addition (ex: decolorize bromine solution)
Pour liquids using a funnel or down a glass rod
OH?

30. 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?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
The compound with the lowest Ksp value.
Monomer + monomer = polymer product + a simple molecule such as water or HCl

31. Name C7H16
OH?
Add acid to water so that the acid doesn't boil and spit
10?8
Heptane

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

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33. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
zero
K2
-Ea/R

34. What equipment do you need for a titration?
Insoluble
water and substances with (s) less dense than
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

35. What is HCOOCH3?
allow for the vapor pressure of water and make sure to level levels
The benzene ring (or more correctly the phenyl group - C6H5)
Acids; HCOOCH3 is an ester
redox reaction

36. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
no - they're written undissociated (HAaq)

37. What apparatus do you use to separate 2 immiscible liquids?
RX
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Only temperature
Separating funnel

38. What measuring device would you use for very small volumes of liquids?
Soluble except Ag - Pb - Ca - Sr Ba)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Pipette (burette if need repetition)
NO3?

39. What do group I/II metal oxides plus water form?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Group I metals (soft metals) are stored under oil
catalyst=conc H2SO4
bases

40. dichromate (soln + most solids)
[A?]/[HA] x 100 or [BH?]/[B] x 100
zero
Synthetic condensation polymer (aka a polyamide)
Orange

41. lead compounds
A salt solution.
CO (poisonous)
Insoluble except nitrate and acetate
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

42. nitrate
NO3?
Iodine and CO2 (dry ice)
Decant
The Faraday or Faraday's constant.

43. What kind of bonding structure does benzene have?
C4H10
benzene has a delocalized pi ring structure
diamond and graphite
Nothing

44. How are primary alcohols turned into acids?
allow for the vapor pressure of water and make sure to level levels
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
R=8.31 J/mol/K
#ligands=charge x2

45. What is the general formula for an amine?
More chaotic (ex: gases made)
RNH2
fruit - fish - bases
linear

46. What effect does increasing the size/surface area of a voltaic cell have on the cell?
benzene has a delocalized pi ring structure
Insoluble except for nitrate and acetate
bright yellow
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

47. What do you need to make a polymer?
S2O3²?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
yellow
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)

48. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
Anode - oxygen. Cathode - hydrogen
Most are soluble except Ag - Pb
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

49. How does benzene compare in reactivity to alkenes?
Cu3(PO4)2
benzene is less reactive than alkenes
Combine the equations for the half reactions in the non-spontaneous direction
Acid rain - dissolves marble buildings/statues and kills trees.

50. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
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)
fruit - fish - bases
Most are soluble except Ag - Pb