426097
Chemical Reactions Lab
- three types of reactions
- precipiatation
- redox reactions
- combination
reactions:
X+Y=Z
- decomposition
reactions: Z=
X+Y
- displacement reactions:
X+YZ=XZ+Y
- main focus of the lab was
single displacement
- types of displacement
reactions
- metal and an
aqueous solution
of a strong acid
- metal displacing a second
metal from solution of
second metal's ions
- metal and an
aqueous solution
of a strong acid
- main focus of the lab was
single displacement
- combination
reactions:
X+Y=Z
- acid-base reactions
- precipiatation
- key terms
- oxidation
- loss of electrons
- reducing agent since it causes a
reduction
- loss of electrons
- reduction
- gain of electrons
- oxidizing agent since it
causes an oxidation
- gain of electrons
- oxidation number
- charge each atom would have if all shared
electrons were transferred to the atom that more
strongly attracts the electrons
- rules
- oxidation # for an
atom in elemental
form is always 0
- oxidation # for an
element in a
monoatomic ion is
the same as the
charge (ex: O2-)
- sum of
oxidation
numbers in
neutral
covalent/
ionic
compound is
0
- rules for
oxidation
numbers in
compounds or
polyatomic ions
- F is -1
- Group 1A metals are +1
- Group 2A metals are +2
- O is -1 in peroxides and -2 in all
other compounds (except when
bounded to F
- H is =1 in all
compounds with metals
or boron, but +1 in
compounds with
nonmetals
- Group 7A metals (halogens) are -1
when bonded with metals,
nonmetals, and other halogens
lower in the group (except O is -2
when bonded to halogens except F
- F is -1
- oxidation # for an
atom in elemental
form is always 0
- charge each atom would have if all shared
electrons were transferred to the atom that more
strongly attracts the electrons
- molecular equaiton
- shows all of the
reactants & products
as if they were intact,
undissociated
compounds
- shows all of the
reactants & products
as if they were intact,
undissociated
compounds
- ionic equaiton
- shows all the
soluble ionic
substances
dissociated into
their component
ions
- shows all the
soluble ionic
substances
dissociated into
their component
ions
- net ionic equaiton
- eliminates all spectator ions
and shows reactions in
simplest form
- eliminates all spectator ions
and shows reactions in
simplest form
- oxidation
- activity series
- balancing a redox rection
- steps:
- 1) determine the oxidation numbers of all elements in the reactant and products
- 2) identify the oxidized and the reduced species from the changes in oxidation numbers
and electrons to the now two separate equations in order to make the charges balanced
- 3) balance number of electrons gained and lost (reduction reactions are always multiplied by 2)
- 4) add the oxidation and reduction reactions together to cancel electrons
- 5) add back in the additional atoms for the balance of charge and mass
- 1) determine the oxidation numbers of all elements in the reactant and products
- steps:
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