Metal deficiency defect is shown by Fe_{0.93} | vedclass

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(A) Let the number of $Fe^{2+}$ ions be $x$ and the number of $Fe^{3+}$ ions be $y$.Total number of $Fe$ ions is $x + y = 0.93$.Since the crystal is e

Vedclass · Accepted Answer

$85$

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(A) Let the number of $Fe^{2+}$ ions be $x$ and the number of $Fe^{3+}$ ions be $y$.Total number of $Fe$ ions is $x + y = 0.93$.Since the crystal is electrically neutral,the total positive charge must equal the total negative charge ($-2$ for $O^{2-}$).$2x + 3y = 2$.Substituting $y = 0.93 - x$ into the charge equation:$2x + 3(0.93 - x) = 2$$2x + 2.79 - 3x = 2$$-x = -0.79$$x = 0.79$.Thus,the number of $Fe^{2+}$ ions is $0.79$.The percentage of $Fe^{2+}$ ions is $\frac{0.79}{0.93} 	imes 100 \approx 84.94\%$.The nearest integer is $85\%$.

List-$I$ (Defect)	List-$II$ (Examples)
$A$. Frenkel defects	$1$. $FeO$
$B$. Schottky defects	$2$. $NaCl$
$C$. Vacancy defects	$3$. $AgCl$
$D$. Metal deficiency defects	$4$. Crystals with vacant lattice sites

Metal deficiency defect is shown by $Fe_{0.93}O$. In the crystal,some $Fe^{2+}$ cations are missing and loss of positive charge is compensated by the presence of $Fe^{3+}$ ions. The percentage of $Fe^{2+}$ ions in the $Fe_{0.93}O$ crystals is $....$ (Nearest integer)

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Identify the defect developed when an ion of an ionic compound is missing from its regular site and occupies an interstitial position between lattice points.

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Match List-$I$ with List-$II$.

List-$I$ (Defect) List-$II$ (Examples)

$A$. Frenkel defects $1$. $FeO$

$B$. Schottky defects $2$. $NaCl$

$C$. Vacancy defects $3$. $AgCl$

$D$. Metal deficiency defects $4$. Crystals with vacant lattice sites

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