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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. What does saturated mean? Unsaturated?
blue (BTB)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
zero

2. nitrate
Initiation energy (NOT Ea)
Hg2²?
voltaic: + electrolytic: -
NO3?

3. What shape is carbon dioxide?
linear
CnH(2n+2)
CN?
Anode

4. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
No - it depends on the number of ions produced on dissolving.
Big K=kf/kr
S crystal at 0K=0
Ksp = s²

5. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
catalyst=conc H2SO4
Insoluble except nitrate and acetate
water and substances with (s) less dense than
Ions go through the salt bridge - electrons go through metal wires in the external circuit

6. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Selective absorption
The benzene ring (or more correctly the phenyl group - C6H5)

7. lead iodide
Hg2²?
by electrolysis
10?8
bright yellow

8. What are the signs for ?G and E° for spontaneous reactions?
Concentration
Salt + water
?G= -ve - E°= +ve
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)

9. Can you collect soluble gases over water?
red - green - blue
No - NH3 and HCl gases are extremely soluble
T increases exponentially the proportion of molecules with E > Ea
?H-kJ - ?S-J - ?G-kJ

10. What is the test for oxygen?
Increases down group 1 decreases down group 17
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
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
Glowing splint (positive result=relights)

11. What do acids plus active metals form?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
C4H10
Ksp = s²
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

12. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
Add acid to water so that the acid doesn't boil and spit
R=8.31 J/mol/K
Ksp = 27s4

13. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
More chaotic (ex: gases made)
How close results are to the accepted value
it's lower and occurs over less sharp a range

14. Name 2 ways in which you can create a buffer?
Ksp = 27s4
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)
PO4³?
Tetrahedral

15. What is a coordinate covalent bond?
Heptane
proton acceptor.
Pale purple - (orange)-yellow - red - blue - green.
Both electrons come from the same atom (just as good as a regular bond)

16. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Soluble
neutralization: high K - H2O product dissociation: low K - H2O reactant
Soluble except Ag - Pb - Ca - Sr Ba)

17. When can supercooling occur? What does it look like on a cooling curve?

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18. If Q > Ksp - then system shifts _______ and ppt ______
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
bases
left - ppt will form
The compound with the lowest Ksp value.

19. Alkanes are _________ and react by _________
Saturated - Substitution (which requires more radical conditions)
ns² electrons (first in-first out)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
methyl formate

20. What is the formula for alkenes?
Making sigma bonds and holding lone pairs
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
CnH2n
strong acids/bases are written as H+ or OH- ions

21. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Graduated cylinder
CO2 and H2O

22. How are strong ones written?
Increases down group 1 decreases down group 17
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Anode - oxygen. Cathode - hydrogen
strong acids/bases are written as H+ or OH- ions

23. What is the sign of the anode in voltaic cells? in electrolytic cells?
CrO4²?
Mn²? - Cr³? - Cr³
proton acceptor.
voltaic: - electrolytic: +

24. What is the difference between equivalence point and end point of a titration.
boiling without losing volatile solvents/reactants
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
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
?G=negative - E° must be positive

25. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
ClO?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
small size and high charge

26. BaSO4
Insoluble
Time?¹ - (ex. s?¹ - hr?¹ - etc)
zero
Mn²? - Cr³? - Cr³

27. How do you get Ecell for spontaneous reactions?
-Ea/R
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
The Faraday or Faraday's constant.
?G=negative - E° must be positive

28. Which alkali metals float on water?
CnH2n+1 often designated 'R' ex C3H7 is propyl
atoms
Glowing splint (positive result=relights)
All except for lithium

29. What do group I/II metal oxides plus water form?
-Ea/R
H3PO4
No - NH3 and HCl gases are extremely soluble
bases

30. What is reflux?
acids
boiling without losing volatile solvents/reactants
H2O + CO2 (it decomposes readily)
an oxidized and reduced substance

31. Where are group I metals stored?
Group 1 hydroxides (ex: NaOH)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Nothing
Group I metals (soft metals) are stored under oil

32. How does benzene compare in reactivity to alkenes?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
benzene is less reactive than alkenes
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Suniverse increases for spontaneous processes

33. What is the test for hydrogen?
Insoluble except nitrate and acetate
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
RCOOH
lighted splint (positive result=pop)

34. mercury (II) ion
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
voltaic: + electrolytic: -
Hg²?
Soluble

35. What apparatus do you use to pour liquids?
q=mc?T q=mL (or n x ?h)
Anode
ROH
Pour liquids using a funnel or down a glass rod

36. iodine - iodine solution - iodine vapor
S crystal at 0K=0
0.10M HCl (more ions)
Silvery gray solid - brown - purple
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

37. primary colors
different forms of the same element
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
red - green - blue
ns² electrons (first in-first out)

38. What things should you remember to do when collecting gas over water?
Separating funnel
allow for the vapor pressure of water and make sure to level levels
ROR
[A?]/[HA] x 100 or [BH?]/[B] x 100

39. What are the products of the reaction between group 1 metals and water?

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40. When driving off water from a hydrate - how do you tell you're done?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
redox reaction
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

41. Color (absorbance) is proportional to ________
Mn²? - Cr³? - Cr³
no - they're written undissociated (HAaq)
Concentration
ionic and form hydrogen and hydroxide

42. Lattice energy is high for ions with _____ size and _____ charge
A salt solution.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
zero
small size and high charge

43. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
boiling without losing volatile solvents/reactants
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Clear

44. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
do not change
Pour liquids using a funnel or down a glass rod
blue (BTB)

45. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
Purple
Molecules with the same molecular formulas - but different structural formulas
0 and 14

46. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
Pipette (burette if need repetition)
Nothing
it is lower and occurs over less sharp a range

47. How do you clean a buret/pipette for a titration?
0 and 14
The benzene ring (or more correctly the phenyl group - C6H5)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

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

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49. What equipment do you need for a titration?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Ksp = s²
Acid rain - dissolves marble buildings/statues and kills trees.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

50. What do ions and electrons travel through in a voltaic/electrolytic cell?
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)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Big K=kf/kr
Ions go through the salt bridge - electrons go through metal wires in the external circuit