Extra Credit 44
- Page ID
- 83441
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Sketch a voltaic cell. Label anode and cathode. Indicate direction of electron flow, write balanced equation for reaction and calculate E∘cell.
- Fe2+(aq) displaced from solution by Li(s)
- Sn(s)+H+(aq)+NO−3(aq)→Sn2+(aq)+H2O(l)+NO(g)
- F2(g)+H2O(l)→F−(aq)+O2(g)+H+(aq)
- Cu(s)+F2(g)→Cu2+(aq)+2F−(aq)
S19.22B
Q20.3C
Determine and balance the equation (the aluminum is oxidized):
Al(s)+MoO3(s)→?Al(s)+MoO3(s)→?
Q24.23A
If a first order decomposition reaction has a half-life of 107 minutes, in what amount of time will the original reactant be ¼ of its original concentration?
S20.3C & S24.23A
Q21.17A
How does crystal field theory explain the coloration of so many transition metals?
S21.17A
The Crystal Field Theory is a bonding theory used in describing the characteristic colors and magnetic properties of complex ions due to the repulsions between the negatively charged d electrons of the central metal atom and the negatively charged electrons in the ligands. Depending on the magnitude of the repulsion, the degenerate (same energy) d orbitals can either be raised to a higher energy level or dropped to a lower energy level both with respect to the average energy of the d orbitals in a ligand field. This energy, known as delta, Δ, corresponds to a specific wavelength of a photon, λ, in the following equation Δ=hc/λ. The wavelength of the photon relates to a specific color absorbed. The complementary color to the absorbed color is reflected and is the color we see. Many transition metals are colored because they have d electrons that can “jump” up to higher energy levels.
However, if there are no electrons to move up to the next energy level (as in d0compounds) or if there are no spaces to move up electrons (as in d10compounds) then there is no Δ and therefore no corresponding λ. Thus, the compound is colorless.
Q25.5A
A sample with Sb-124 has an activity 100 times the detectable limit. How long would an experiment run before the radioactivity could no longer be detected?
Q21.2.23
Using the information provided in Chapter 33, complete each reaction and calculate the amount of energy released from each in kilojoules per mole.
\(_{91}^{234}\textrm{Pa}\rightarrow \,?+\,_{-1}^0\beta\) - \(_{88}^{226}\textrm{Ra}\rightarrow \,?+\,_2^4\alpha\)
S25.5A & S21.2.23
Q25.41B
Which member of the following pairs of nuclide would you expect most abundant in natural sources. Explain your answer
a. Ar-40 or Ar 42
b. Cl-36 or Cl-38
S25.41B
The closer an isotope is to its average atomic mass, the more abundant it is.
a. Ar-40 is more abundant than Ar-42 since it is closer to the average atomic mass of Ar which is 39.95.
b. Cl-36 is more abundant than Cl-38 since it is closer to the average atomic mass of Cl which is 35.45.
Q20.3.9
The reaction \[Pb(s) + 2VO^{2+}(aq) + 4H^+(aq) → Pb^{2+}(aq) + 2V^{3+}(aq) + 2H_2O(l)\] occurs spontaneously.
- Write the two half-reactions for this redox reaction.
- If the reaction is carried out in a galvanic cell using an inert electrode in each compartment, which reaction occurs at the cathode and which occurs at the anode?
- Which electrode is positively charged, and which is negatively charged?
