1c:["$","section",null,{"className":"science-method","id":"worked-examples","children":["$","details",null,{"open":true,"children":[["$","summary",null,{"children":"Method and worked examples"}],["$","div",null,{"className":"science-method-copy","children":[[["$","p","0",{"children":[[["$","link","css:/_next/static/css/math-text.ClrOCYwY.css",{"rel":"stylesheet","precedence":"vite-rsc/importer-resources","href":"/_next/static/css/math-text.ClrOCYwY.css","data-rsc-css-href":"/_next/static/css/math-text.ClrOCYwY.css"}],"$undefined"],["$","span",null,{"className":"gm-math gm-typeset","aria-label":"Oxidation is electron loss and an increase in oxidation number; reduction is electron gain and a decrease in oxidation number. Both occur together in a redox reaction. An element in its uncombined form has oxidation number zero. A monatomic ion has oxidation number equal to its charge. In usual compounds hydrogen is +1 and oxygen −2, with stated exceptions such as metal hydrides or peroxides.","children":["$","span",null,{"aria-hidden":"true","children":[["$","span","0",{"children":"Oxidation is electron loss and an increase in oxidation number; reduction is electron gain and a decrease in oxidation number. Both occur together in a redox reaction. An element in its uncombined form has oxidation number zero. A monatomic ion has oxidation number equal to its charge. In usual compounds hydrogen "}],["$","span","1",{"className":"gm-latex","dangerouslySetInnerHTML":{"__html":"is+1"}}],["$","span","2",{"children":" and oxygen "}],["$","span","3",{"className":"gm-latex","dangerouslySetInnerHTML":{"__html":"−2,"}}],["$","span","4",{"children":" with stated exceptions such as metal hydrides or peroxides."}]]}]}]]}],["$","p","1",{"children":[[["$","link","css:/_next/static/css/math-text.ClrOCYwY.css",{"rel":"stylesheet","precedence":"vite-rsc/importer-resources","href":"/_next/static/css/math-text.ClrOCYwY.css","data-rsc-css-href":"/_next/static/css/math-text.ClrOCYwY.css"}],"$undefined"],["$","span",null,{"className":"gm-math gm-typeset","aria-label":"The sum equals zero for a neutral compound and the ion charge for a polyatomic ion. Solve for an unknown using that total. The oxidising agent accepts electrons and is reduced. The reducing agent donates electrons and is oxidised. Oxidation number is bookkeeping; it does not imply that a covalently bonded atom carries that full ionic charge.","children":["$","span",null,{"aria-hidden":"true","children":[["$","span","0",{"children":"The sum equals zero for a neutral compound and the ion charge for a polyatomic ion. Solve for an unknown using that total. The oxidising agent accepts electrons and is reduced. The reducing agent donates electrons and is oxidised. Oxidation number is bookkeeping; it does not imply that a covalently bonded atom carries that full ionic charge."}]]}]}]]}]],[["$","article","0",{"children":[["$","h2",null,{"children":["Example ",1]}],["$","p",null,{"children":[[["$","link","css:/_next/static/css/math-text.ClrOCYwY.css",{"rel":"stylesheet","precedence":"vite-rsc/importer-resources","href":"/_next/static/css/math-text.ClrOCYwY.css","data-rsc-css-href":"/_next/static/css/math-text.ClrOCYwY.css"}],"$undefined"],"$L1f"]}],"$L20"]}],"$L21"],"$L22"]}]]}]}]

Example 1

Example 2