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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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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 gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Initiation energy (NOT Ea)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

2. How are primary alcohols turned into acids?
do not change
More chaotic (ex: gases made)
RCOOR
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

3. An amphiprotic (amphoteric) species is...
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

4. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
NH4?
P2O5
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

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

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6. chromate ion (soln + most solids)
Sigma bonds are stronger than pi bonds
yellow
Anode
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

7. thiosulfate
S2O3²?
NO3?
?G=negative - E° must be positive
it's lower and occurs over less sharp a range

8. What is precision?
Increases down group 1 decreases down group 17
How grouped results are
brown volatile liquid
RCHO (carbonyl at end)

9. 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
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
H3PO4
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

10. What do ions and electrons travel through in a voltaic/electrolytic cell?
Separating funnel
C2O4²?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
zero

11. What is the general formula for an alcohol?
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
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
ROH
K1 x K2

12. What are the signs for ?G and E° for spontaneous reactions?
proton donor base
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
ion pairing
?G= -ve - E°= +ve

13. Which would cause the bulb in a conductivity apparatus to be brightest?
Ksp = 27s4
0.10M HCl (more ions)
Cr2O7²?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

14. What is the word equation for addition polymerisation?
CN?
NH4?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

15. What are the signs of ?G and E° for spontaneous reactions?
0 and 14
?G=negative - E° must be positive
same KE - but PEice<PEwater
CnH2n+1 often designated 'R' ex C3H7 is propyl

16. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Group 1 hydroxides (ex: NaOH)
same KE - but PEice<PEwater
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
RNH2

17. nitrates
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Soluble
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
voltaic: + electrolytic: -

18. How does the melting point of a mixture compare to the MP of a pure substance?

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19. What do the 'a' and 'b' in Van Der Waal's equation allow for?
No - NH3 and HCl gases are extremely soluble
ionic and form hydrogen and hydroxide
a-IMFs - b-molecular volume
RCHO (carbonyl at end)

20. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Separating funnel
No - it depends on the number of ions produced on dissolving.
How close results are to the accepted value
Monomer + monomer = polymer product + a simple molecule such as water or HCl

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?
allow for the vapor pressure of water and make sure to level levels
They stay the same.
MnO4?
zero-th: decreases - first: constant - second: increases

22. Can you collect soluble gases over water?
benzene is less reactive than alkenes
Unsaturated - addition (ex: decolorize bromine solution)
No - NH3 and HCl gases are extremely soluble
R=8.31 J/mol/K

23. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
zero-th: decreases - first: constant - second: increases
Big K=kf/kr
CnH(2n+2)

24. What are isomers?
Glowing splint (positive result=relights)
chemically (ex: with carbon)
Molecules with the same molecular formulas - but different structural formulas
boiling without losing volatile solvents/reactants

25. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
ion pairing
Most INsoluble except group 1 and ammonium
Insoluble except for nitrate and acetate
Current - time and charge on ion (moles of e used in half cell reaction)

26. What is the sign of the anode in voltaic cells? in electrolytic cells?
Current - time and charge on ion (moles of e used in half cell reaction)
voltaic: - electrolytic: +
Acidified
Sulfur

27. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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28. Colorless doesn't mean ______
Soluble
ROR
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Clear

29. What type of compounds do metals/non metals form?
S2O3²?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
All except for lithium
Ionic compounds

30. bromothymol
blue (BTB)
RCOOH
Exothermic
Perform ICE BOX calculation based on K1

31. How does half life change for zero-th order - first order - and second order processes?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
zero-th: decreases - first: constant - second: increases
Concentration
ionic and form hydrogen and hydroxide

32. How do you get Ecell for spontaneous reactions?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Heptane
Filtration

33. What type of compounds do Group 14 form?
|experimental - accepted|/accepted X 100
Tetrahedral
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
+4-covalent - +2-ionic

34. What is the formula for alkenes?
CnH2n
red - green - blue
0.10M HCl (more ions)
zero

35. Which of the rates changes more when temperature is increased?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
fractional distillation
bent

36. Give an example of a dilute strong acid.
chemically (ex: with carbon)
HClO4
Soluble
fractional distillation

37. What do group I/II metal oxides and acids form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Soluble except Ag - Pb - Ca - Sr Ba)
Salt and water
Big K=kf/kr

38. chlorine
ionic and form hydrogen and hydroxide
No - it depends on the number of ions produced on dissolving.
They stay the same.
Greenish-yellow gas

39. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
R=8.31 J/mol/K
Increases.

40. Alkenes are ________ and react by __________
q=mc?T q=mL (or n x ?h)
Unsaturated - addition (ex: decolorize bromine solution)
OH- and NH3
it's lower and occurs over less sharp a range

41. A Bronsted-Lowry acid is...
10?8
How close results are to the accepted value
HClO4
proton donor base

42. What do the 'a' and 'b' in Van Der Waal's equation allow for?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
non-metal oxides and hydrides are covalently bonded and are acidic.
a-IMFs - b-molecular volume
?H-kJ - ?S-J - ?G-kJ

43. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
?G= -ve - E°= +ve
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.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
ROH

44. How does benzene compare in reactivity to alkenes?
E=q + w (negative is by system - positive is on system)
K2
benzene is less reactive than alkenes
CO (poisonous)

45. What is the formula for summation?

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46. What is the energy you must put into a reaction to make it start called?
But S° of element is not zero (except at 0K)
Initiation energy (NOT Ea)
zero
Silvery gray solid - brown - purple

47. What is the formula for alkanes?
CnH2n+2
S2O3²?
CO (poisonous)
CN?

48. Where are group I metals stored?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Group I metals (soft metals) are stored under oil
Reduction always takes place at the cathode (RED CAT) In both types of cell!
They decrease (or could be the same if the solid has ONLY JUST disappeared)

49. halides
Ions go through the salt bridge - electrons go through metal wires in the external circuit
HClO4
Most are soluble except Ag - Pb
Cr2O7²?

50. Aromatic compounds contain what?
Eudiometer
a-IMFs - b-molecular volume
The benzene ring (or more correctly the phenyl group - C6H5)
same KE - but PEice<PEwater