Oxidation/Reduction reactions Flashcards
An oxidizing agent ___ other species and ___ itself
Oxidizes other species and reduces itself
A reducing agent ___ other species and ____ itself
Reduces other species and oxidizes itself
Oxidation is ____ of electrons while reducing is ___ of electrons
Loss
Gain
OIL RIG
The oxidation number of a free element is __
0
The oxidation number of a monotonic ion is equal to its ___
Charge
(-2, +3, +1)
The oxidation number of the group 1 elements is ___
+1
The oxidation number of the group 2 elements is ___
+2
The oxidation number of the group 7 elements is ___, unless paired with an atom that’s more electronegative
-1
(Ex: HCL, Cl= -1. HOCL, Cl= +1)
The oxidation number of H is always ___, unless paired with a less electronegative atom (like Na)
+1
The oxidation number of O is always ___, unless in a peroxide or with a more electronegative element
-2
The sum of all oxidation numbers is __ for neutral atoms and ___ for charged atoms
0
Equal to the charge
What is the difference between oxidation number and formal charge?
The oxidation number awards electrons to the most electronegative atom (which is why some are positive and some are negative)
Formal charge is an even division of electrons between bonds
What is the half reaction method?
When you separate the overall equation into the reduction and oxidation reaction
What is the difference between net ionic equation and complete ionic equation?
The net ionic equation removes the spectator ions (those not involved in the oxidation or reduction reaction) and keeps only the atoms that participate in the reaction. Solid salts stay together but aqueous compounds are split up into their components
The complete ionic equation splits all the compounds up into their separate components
In a ____ reaction, an element will undergo both oxidation and reduction
Disproportionation
