The oxidation number of all metals on the periodic table have a positive (+) charge. which of these best explains why? a) metals are known to add protons to their nuclei causing them to become positively charged. b) all metals lose one or more valence electrons to become stable, giving them a positive oxidation number. c) all metals gain one or more valence electrons to become stable, giving them a positive oxidation number. d) metals are known to lose protons and add neutrons to their nuclei causing them to become positively charged.

Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. in general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number. the species that is oxidized is called the reducing agent or reductant. the species that is reduced is called the oxidizing agent or oxidant. to sum up: oxidation = increase in oxidation state = loss of electrons = reducing agent reduction = decrease in oxidation state = gain of electrons = oxidizing agent part a which element is oxidized in this reaction? fe2o3+3co→2fe+3co2 enter the elemental symbol. view available hint(s) is oxidized part b which element is reduced in this reaction? 2hcl+2kmno4+3h2c2o4→6co2+2mno2+2kcl +4h2o enter the elemental symbol. view available hint(s) is reduced

In which situation can a mixture always be called a solution

Which metal exist in liquid state and can be cut with knife ?