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Chapter 17: Q1Q (page 412)

Is B-doped diamond p-type or n-type? Consult Figure 15-37

Short Answer

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Diamond doped with boron is P-type semiconductor

Step by step solution

01

Introduction

P-type semiconductor:

Intrinsic or pure semiconductors (silicon or germanium) with trivalent impurities is called p-type semiconductor. Gallium (G), Boron (B), Aluminium (Al), Indium (In), etc. are trivalent impurities.

N-type semiconductor:

Intrinsic or pure semiconductors (silicon or germanium) with pentavalent impurity is called n-type semiconductor. Arsenic, phosphorus, antimony etc are pentavalent impurities.

02

Check whether Is B-doped diamond p-type or n-type

Silicon or germanium is used as the intrinsic semiconductor, silicon and germanium has four valence electrons. Carbon also has four valence electrons.

diamond doped with boron is P-type semiconductor, because, when trivalent impurity is added to diamond is called as p-type semiconductor. Boron (B) is one of the trivalent impurities which are also known as acceptor impurity.

Trivalent is added to the diamond it will form three covalent bonds with carbon and there is no electron to formation of the bond because due to the absence of valence electron of boron, which cause one hole is remaining therefore which is called acceptor impurity and is called as P-type semiconductor.

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Most popular questions from this chapter

Coulometric titration of sulfite in wine. Sulfur dioxide is added to many foods as a preservative. In aqueous solution, the following species are in equilibrium:

Bisulfite reacts with aldehydes in food near neutral pH:

Sulfite is released from the adduct in 2MNaOH and can be analyzed by its reaction with $I_{3}^{-}$ to give $I^{-}$ and sulfate. Excess $I_{3}^{-}$ must be present for quantitative reaction.

Here is a coulometric procedure for analysis of total sulfite in white wine. Total sulfite means all species in Reaction and the adduct in Reaction . We use white wine so that we can see the color of a starch-iodine end point.

1. Mix 9.00 mL of wine plus 0.8gNaOH and dilute to 10.00mL. The releases sulfite from its organic adducts.

2. Generate $I_{3}^{-}$ at the working electrode (the anode) by passing a known current for a known time through the cell in Figure 17 - 10. The cell containsofacetate buffer () plus. In the cathode compartment, is reduced to $H_{2} + {OH}^{-}$ . The frit retards diffusion of into the main compartment, where it would react with $I_{3}^{-}$ to give ${IO}^{-}$ .

3. Generate $I_{3}^{-}$ at the anode with a current of for.

4. Inject 2.000mL of the wine/ solution into the cell, where the sulfite reacts with leaving excess.

5. Add of thiosulfate to consume by Reaction and leave excess thiosulfate.

6. Add starch indicator to the cell and generate fresh $I_{3}^{-}$ with a constant current of 10.0mA. A time of 131s was required to consume excess thiosulfate and reach the starch end point.

(a) In what pH range is each form of sulfurous acid predominant?

(b) Write balanced half-reactions for the anode and cathode.

(c) At pH 3.7, the dominant form of sulfurous acid isand the dominant form of sulfuric acid is ${HSO}_{4}^{2 -}$ . Write balanced reactions between andand between $I_{3}^{-}$ and ${HSO}_{3}^{-}$ thiosulfate.

(d) Find the concentration of total sulfite in undiluted wine.

Ions that react with $A g^{+}$ can be determined electrogravimetrically by deposition on a silver working anode:

$A g (s) + X^{-} \to A g X (s) + e^{-}$

(a) What will be the final mass of a silver anode used to electrolyze 75.00 mL of 0.02380 M KSCN if the initial mass of the anode is 12.4638 g?

(b) At what electrolysis voltage (versus S.C.E.) will AgBr(s) be deposited from 0.10M Br? (Consider negligible current flow, so that there is no ohmic potential, concentration polarization, or overpotential.)

(c) Is it theoretically possible to separate 99.99% of0.10M Klfrom0.10MKBr by controlled-potential electrolysis?

How many hours are required for 0.100 mol of electrons to flow through a circuit if the current is 1.00 A?

Consider the cyclic voltammogram of the ${Co}^{3 +}$ compoundrole="math" localid="1663646447735" $Co {(B_{9} C_{2} H_{11})}_{2}^{-}$ . Suggest a chemical reaction to account for each wave. Are the reactions reversible? How many electrons are involved in each step? Sketch the sampled current and square wave polarograms expected for this compound.

Cyclic voltammogramofrole="math" localid="1663646461802" $Co {(B_{9} C_{2} H_{11})}_{2}^{-}$ . [Data from W. E. Geiger, Jr., W. L. Bowden, and N. El Murr, "An Electrochemical Study of the Protonation Site of the Cobaltocene Anion and of Cyclopentadienylcobalt(I) Dicarbollides," Inorg. Chem. 1979,18,2358.]

Fundamentals of Electrolysis

17 - 6.The cell in Figure 17 - 4 is:

$Cu | 1.0 {MCuSO}_{4} (aq) | KCL (aq, 3 M) | AgCI (s) | Ag (s)$

Write half-reactions for this cell. Neglecting activity coefficients and the junction potential between ${CuSO}_{4} (aq)$ and KCI(aq), predict the equilibrium (zero-current) voltage expected when the Lugging capillary contacts the electrode. For this purpose, suppose that the reference electrode potential is 0.197Vvs. S.H.E. Why is the observed equilibrium potential+109mV, not the value you calculated?

How would the over potentials change if>1.000Vwere imposed by the

Potentiostat?

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