Oxidation-reduction Flashcards
Reduces other species by losing electrons
reducing agent
Oxidizes other species by gaining electrons
oxidizing agent
Common oxidizing agents are __, __, __ and _____, which favor gaining an electron to have a full octet
O2, O3, H2SO4, halogens
Common reducing agents are __, __, __ and ___ __ which favor losing an electron to have a full octet
H2, Fe, Zn, alkali metals
the total number of electrons that an atoms gains or loses electrons when a bond is formed
oxidation states
atoms in their ___ ___ have an oxidation number of zero. Oxidation numbers for atoms in ____ ___ are equal to their charge. __ is always assigned an oxidation number of -1, oxygen is often ___, and hydrogen is usually ___
elemental state, monoatomic ions, fluorine, +2, +1
__ ___ often have an oxidation number of +1, and ___ __ ____ often have an oxidation number of +2
alkali metals, alkaline earth metals
Exceptions are, if oxygen is in a ___, (___), it’s oxidation number is -1. If oxygen is bonded to fluorine the oxidation number of oxygen is ____. If hydrogen is part of a __ ___, the oxidation number is ____
peroxide, H2O2, +1, metal hydride, -1
To balance the redox reaction under acidic conditions, each ___ reaction must be written and firstly all atoms must be balanced other than __ and ___. Then balance the number of oxygen atoms by adding the same number of __ molecules to the opposite side. Balance the hydrogen atoms by adding __ to the opposite side. Balance the charges by adding ____. Multiply the equations to make sure each half reaction has the same number of ___, then add them together and cancel common terms
half, oxygen hydrogen, H2O, H+, electrons, electrons
In basic reactions the H+ must be balanced with ___ and then combined to create ____.
OH-, H2O
Electrochemical cells convert ___ energy to ___ energy or vice versa using __ __ and the movement of ___
chemical energy, electrical, redox reactions, electrons
Electrons always flow from the ___ to the ___
anode, cathode
energy produced from chemical reactions from energy stored in the bonds of atoms and molecules
chemical energy
energy produced from the flow of electrons
electrical energy
a cell that is spontaneous like a battery
galvanic (voltaic) cell