redox: content Flashcards
what type of equation do we use to show reduction and oxidation
half equation
half equation for oxidation
X → X⁺ⁿ + n(e⁻)
half equation for reduction
X + n(e⁻) → X⁻ⁿ
oxidation number of elements
0
oxidation numbers of metals (when in compounds)
group one: +1
group two: +2
group three: +3
oxidation number of fluorine
ALWAYS -1
usual oxidation number of hydrogen
+1
(exception: metal hydrides)
oxidation number of hydrogen in metal hydrides
-1 (ANOMALY)
usual oxidation number of oxygen
-2
(exceptions: peroxides and fluoridates)
oxidation number of oxygen in peroxides
-1 (ANOMALY)
oxidation number of oxygen when combined with fluorine
positive
(fluorine ALWAYS -1)
usual oxidation number of chlorine
-1
(Cl has lots of variable oxidation states)
oxidation number in compound ions
sum of the individual oxidation states is equal to the charge on the ion
what makes the best oxidising agents
species with high electronegativities
metals undergo ____ in redox reactions
oxidation
(tend to be reducing agents)
nonmetals undergo ____ in redox reactions
reduction
(tend to be oxidising agents)
structure for answering redox questions
A loses n electrons and is oxidised
B gains n electrons and is reduced
Give oxidation numbers (and the compounds they’re part of) if needed
how to spot redox reactions easy
is something exists as an element on one side and within a compound on the other, it must be a redox reaction
redox reactions of metals with acids form
metal + acid → salt + hydrogen
