Reduction Oxidation Flashcards
Electronegativity trend in the periodic table
Electronegativity increases as we go to the top right of the periodic table.
The more electronegative an atom is, the more it wants to _______ electrons.
Gain
The less electronegative an atom is, the more it wants to ________ electrons.
Lose
Na⁺ has ____an electron
Lost
Cl⁻ has ______ an electron
Gained
What is an oxidation state?
In a covalent bond with partial charges (δ⁺ δ⁻) an oxidation state is a hypothetical ionic state where electrons are taken by the more electronegative atom.
H₂O oxidation explanation
In H₂O (oxidation state H₂+ O²⁻), oxygen took the electrons from hydrogen so hydrogen was OXYdised.
Reduction: Oxygen the charge on oxygen was reduced to 2⁻
Atom with positive charge is __________
Oxidized (as if it had been oxygen-ised) like H in H²O
Atom with hypothetical _______ charge is reduced.
Negative
OIL RIG
Oxidation is losing electrons, reduction is gaining.
Usual oxidation state of Oxygen
2-
OF₂ oxidation states
Exception to oxygen’s oxidation state. F is more electronegative so it’s O⁺² and each F is ⁻1 check
H₂O₂ oxidation state
O usually 2 minus but here each O is bonded with a H and another O so eash H is plus 1 which is normal but each O is minus 1. This is an unusual oxidation state.
What is the reducing agent?
The reactant being oxidized (thus causing something else to be reduced)
What is the oxidizing agent?
The reactant that is being reduced (thus causing something else to be oxidized)
