MCQs || B21

Most agents are oxidizing agents

CH 4 (g) + 2O (g) —-> CO 2 2 (g) + 2H 2 O(g) Oxidation he is

of Fossil Fuels – Example: natural gas furnaces

the deterioration of metals caused by an oxidation-reduction process

Assigning Oxidation Numbers: Na^+

In peroxides O has oxidation number of –1. • Examples

4.In a polyatomic ion, the sum of the oxidation numbers of the constituent elements is equal to the charge on the ion (e.g. overall oxidation number = -2 in SO4^-2

In the formula for any compound, the sum of the oxidation numbers of all elements in the compound is zero (e.g. overall oxidation number = zero in H2SO4

The oxidation number of an element in a simple (monatomic) ion is the charge on the ion

The oxidation number of any free, uncombined element is zero

Oxd. State = Oxid. # = the # of electron gained or lost by an atom of that element when it forms the compound. It is oxidation state

Oxidized is

Zn(s) + Cu2+(aq)  Zn2+(aq) + Cu(s)

Zn(s) + Cu2+(aq)  Zn2+(aq) + Cu(s) Zn is being

electrochemical cell that converts stored chemical energy into electrical energy

Is oxidized • Loses electrons

Is reduced • Gains electrons

Cannot have oxidation without reduction

Reduction properties

Double- Replacement Reactions