Analysis show that iron oxide consist of Iron ion with 94 % ions having d6 configuration and 6 % having d5 configuration. Which amongst the following best represents the formula of the oxide?

Question

Analysis show that iron oxide consist of Iron ion with 94 % ions having d6 configuration and 6 % having d5 configuration. Which amongst the following best represents the formula of the oxide? (A) Fe0.97O (B)  Fe1.03O (C)  Fe0.60O (D)  Fe0.94O0.94

Tardigrade Admin · Accepted Answer

d6 arrow Fe+ 2,d5 arrow Fe+ 3 Total charge of Iron =(0.94 × 2)+(0.06 × 3)=1.88+0.18=2.06 Number of O- 2ion=(2.06/2)=1.03 Formula of solid =FeO1.03=Fe0.97O

Q. Analysis show that iron oxide consist of Iron ion with $94%$ ions having $d^{6}$ configuration and $6%$ having $d^{5}$ configuration. Which amongst the following best represents the formula of the oxide?

$F e_{0.97} O$

$F e_{1.03} O$

$F e_{0.60} O$

$F e_{0.94} O_{0.94}$

$d^{6} \to F e^{+ 2}, d^{5} \to F e^{+ 3}$

Total charge of Iron

$= (0.94 \times 2) + (0.06 \times 3) = 1.88 + 0.18 = 2.06$

Number of $O^{- 2} i o n = \frac{2.06}{2} = 1.03$

Formula of solid $= F e O_{1.03} = F e_{0.97} O$

Q. Analysis show that iron oxide consist of Iron ion with 94% ions having d6 configuration and 6% having d5 configuration. Which amongst the following best represents the formula of the oxide?

Fe0.97​O

Fe1.03​O

Fe0.60​O

Fe0.94​O0.94​