Chapter 12 Flashcards
theoretical definition of oxidization
the loss of electrons, results in an increase in ON
theoretical definition of reduction
the gain of electrons, results in a decrease in ON
operational definition of oxidization
the reaction with molecular oxygen
operational definition of reduction
the extraction of metals from metal ore
oxidizing agent definition
reactant being reduced, causing another reagent to be oxidized
reducing agent
reactant being oxidized, causing another reagent to be reduced
redox reactions happen betweeen a ______ and a ______
oxidizing and reducing agent
in redox reactions electrons are _____
gained by one atom or ion and lost by another
oxidization numbers definition
hypothetical numbers used to determine the degree of oxidization of an atom
redox reactions involve ____ of electrons
transfer
what indicates a redox reaction
a change in an element’s ON
steps for determining if reactions are redox or non-redox
1) assign ON’s
2) determine if reactions are redox or non redox
- non redox=no change in ON
- redox=change in ON
definition of spontaneous redox reaction
takes place without the input of electricity
if OA is above RA, the reaction is _______
spontaneous/ does happen
if OA is below RA, the reaction is _____
non-spontaneous/ doesn’t happen
oxidizing agents are on the ___ side of the redox table
left
reducing agents are on the ___ side of the table
right
the SOA is at the ____ of the table
top
the SRA is at the _____ of the table
bottom
the WOA is at the ____ of the table
bottom
the WRA is at the ____ of the table
top
copy out reduction reactions from ____ to ____
left to right (regular)
copy out oxidization reactions from ___ to ___
right to left (opposite)
steps for determine if a redox reaction is spontaneous or non spontaneous
1) determine OA and RA by assigning oxidization numbers
2) consult redox table to determine or spontaneous or not
- spontaneous= OA is above RA
- non spontaneous= OA is below RA
steps for building a redox table
1) determine OA and RA of each equation by assigning oxidization numbers
- metals are always RA
2) place the OA and RA in each equation relative to each other on the table
- each OA and RA has a corresponding element
what is an oxidization half reaction
separating a redox reaction into its oxidization component
what is a reduction half reaction
separating a redox reaction into its reduction component
oxidization half reactions have electrons on ____ side
product
reduction half reactions have electrons on ____ side
reactant
balancing steps
1) write half reactions
2) balance any atoms other than H and O
3) balance oxygen by adding H2O
4) balance hydrogen by adding H+
5) balance any charges by adding electrons
6) multiply half reaction by LCM to cancel out electrons
7) add the balance half reactions
8) cancel out any ions present on both sides
9) add spectator ions back in if they were removed when writting half reaction
steps for balancing equations using half reactions from data booklet (and what format is this question usually in)
usually in all word format
1) list all things you have
acidified/acid=H+
solution=H2O
2) find SOA (consult table) and copy out half reaction
3) find SRA (consult table) and copy out half reaction
6) continue steps for regular balancing
what do you make sure of when copying out half reaction
that you’re copying them out in the CORRECT direction
disproportionation definition
sometimes some atoms of an element can undergo oxidization while some atoms of the same element undergo reduction
steps for determine which element undergoes disproportionation
1) assign ON’s
2) determine which element is being both oxidized and reduced
step for balancing disproportionation reactions:
1) assign ON’s
2) determine which element is being both oxidized and reduced
3) start and finish steps for regular balancing
titration definition
process used to determine the concentration of an unknown solution
titrant definition
solution of KNOWN concentration
sample definition
solution of UNKOWN concentration
titration process
a solution of known concentration (titrant) is added slowly to the solution of unknown concentration (sample) until the reaction is complete
endpoint definition
point when you observe a sudden change in colour
what is the endpoint dependent on
the indicator in acid-base titration
equivalence point definition
point where the chemical amount of the titrant is stoichiometrically equal to the chemical amount present in the solution of unknown concentration
acid-base indicator definition
a compound that changes colour over a given pH range
the ___ is in the buret (titrant or sample)
titrant
the ___ is in the erlenmeyer flask (titrant or sample)
sample
where is the stopcock (relative to the buret)
at the bottom of the buret
what is the retort stand
the thing holding everything up
where is the buret clamp
attached to the retort stand, hold the buret
why do we commonly us OA/RA’s that change colour themselves in redox titrations?
so we don’t have to add an additional indicator
photosynthesis equation
6 CO2(g)+ 6 H2O(l) + energy —>
C6H12O6(s) + 6 O2(g)
cellular respiration equation
C6H12O6(s) + 6 O2(g) —->
6 CO2(g) + 6 H2O(l) + energy
what is the OA in cellular respiration
oxygen
what is the RA in cellular respiration
sugar
what is the OA in photosynthesis
CO2
what is the RA in photosynthesis
water
increase in ph ( in terms of hydrogen ions and acidity)
taking hydrogen ions and converting them to water (H+ on reactant side)
becomes LESS acidic
decrease in ph ( in terms of hydrogen ions and acidity)
when your producing hydrogen ions
becomes MORE acidic
