Consider the following molecules: Br_3O_8,F_2 | vedclass

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(D) $1$. For $Br_3O_8$: The structure shows bromine atoms in $+6$ and $+4$ oxidation states. Number of atoms with zero oxidation state = $0$.$2$. For

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$6$

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(D) $1$. For $Br_3O_8$: The structure shows bromine atoms in $+6$ and $+4$ oxidation states. Number of atoms with zero oxidation state = $0$.$2$. For $F_2O$: The oxygen atom is in $+2$ oxidation state. Number of atoms with zero oxidation state = $0$.$3$. For $H_2S_4O_6$: The structure contains two central sulfur atoms in $0$ oxidation state. Number of atoms with zero oxidation state = $2$.$4$. For $H_2S_5O_6$: The structure contains three central sulfur atoms in $0$ oxidation state. Number of atoms with zero oxidation state = $3$.$5$. For $C_3O_2$: The central carbon atom is in $0$ oxidation state. Number of atoms with zero oxidation state = $1$.$6$. Total sum = $0 + 0 + 2 + 3 + 1 = 6$.

Consider the following molecules: $Br_3O_8$,$F_2O$,$H_2S_4O_6$,$H_2S_5O_6$,and $C_3O_2$. Count the number of atoms existing in their zero oxidation state in each molecule. Their sum is . . . . .

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