Question

some chemical reactants are listed in the table below. complete the table by filling in the oxidation state of the highlighted atom. species oxidation state of highlighted atom ag⁺(aq) 0 sio₂(s) 0 h₂o(l) 0 h₂(g) 0

Explanation:

Step1: Determine oxidation state of $Ag^+$

The oxidation state of a monatomic ion is equal to its charge. So for $Ag^+$, the oxidation state of silver is + 1.

Step2: Determine oxidation state of $Si$ in $SiO_2$

Oxygen has an oxidation state of - 2 in most compounds. Let the oxidation state of $Si$ be $x$. In $SiO_2$, using the rule that the sum of oxidation states in a neutral compound is 0, we have $x+2\times(-2)=0$. Solving for $x$ gives $x = + 4$.

Step3: Determine oxidation state of $O$ in $H_2O$

Hydrogen has an oxidation state of + 1 in most compounds. Let the oxidation state of $O$ be $y$. In $H_2O$, using the sum - of - oxidation - states rule ($2\times(+1)+y = 0$), we find $y=-2$.

Step4: Determine oxidation state of $H$ in $H_2$

In an elemental form, the oxidation state of an atom is 0. So for $H_2$, the oxidation state of hydrogen is 0.

Answer:

species	oxidation state of highlighted atom
$SiO_2(s)$	+ 4
$H_2O(l)$	- 2
$H_2(g)$	0