Unit 4 Flashcards
Synthesis/ Combination Reaction
where two substances combine to form a compound
Decomposition Reaction
Where a substance comes apart into multiple substances
Metathesis Reactions
bonds between two chemical species are exchanged
Acid - Base Reaction
where an acid and base react to form their conjugate pairs
Oxidation - Reduction Reaction
the exchange of e-, causing different oxidation numbers
Combustion Reaction
where a hydrocarbon and O2 form CO2 + H2O + whatever else
Precipitation Reaction
ionic aqueous are mixed and two ions combine, solidifying
Spector Ion
the ions that do no solidify in an ionic substance
Alkali metal cations are….
always soluble
Ammonium Cations (NH4+) are…
always soluble
Nitrate Anion (NO3)4- are…
always soluble
Why do some ionic substances dissolve?
if…
Dipole H2O > Electrostatic Attraction
Why do some ionic substances solidify?
If…
Dipole H2O < Electrostatic Attraction
Hydroxide
OH-
Nitrate
(NO3) -
Acetate
(C2H3O2)-
Cynaide
(CN)-
Permanganate
(MnO4) -
Carbonate
(CO3)2-
Sulfate
(SO4)2-
Dichromate
(Cr2O7) 2-
Phosphate
(PO4) 3-
Ammonium
(NH4) +
Chromate
(CrO4) 2-
Peroxide
(O2) 2-
Oxalate
(C2O4) 2-
Thiosulfate
(S2O3) 2-
What is the trick for balancing reactions?
PLUG IN!
Law of Conservation of Mass
Mass is neither created or destroyed
In combustion all the carbon from the hydrocarbon…
ends up in CO2
In combustion all the hydrogen from the hydrocarbon…
ends up in H2O
Gravimetrical Analysis
Determining the unknown substance of a chemical reaction
Oxidative State
a HYPOTHETICAL charge assigned to an atom in a chemical compound, representing the number of electrons it would gain or lose if all its bonds were completely ionic
non bonded, neutral atoms have a oxidative state of…
0
oxidative charge of an ion/polyatomic ion…
ionic charge
oxidative state of Oxygen is 2- EXCEPT when..
(H2O2)
O = -1
oxidative state of H in metal is..
-1
oxidative state of H in nonmetal is..
+1
If there is no Oxygen is in the compound the most ________, takes the most common charge for oxidative charge.
electronegative
For oxidative change, individual charges added together…
is the charge of the atom
Redox reactions
The change in oxidative state due to the exchange of e-
LEO the lion says GER
explain
What do half reactions in redox reactions show?
it shows the loss/gain of e-
activity series
a list of elements arranged in decreasing order of their reactivity
(redox reaction)
the higher the activity series ranking, the…
more likely to engage in redox
Oxidating agent
the molecule being reduced
Reducing agent
the molecule being oxidized
Redox titrations
slowly adding solution with known concentrations to an unknown solution to determine concentration of that unknown solution
Bronsted Acid
capable of donating a proton/H+
Bronsted Base
Capable of accepting a proton/H+
Why is H+ a proton?
because a proton is an e- + proton.
take away the e- and you have a proton
conjugated pair
the acid version and base version of a molecule
Amphoretic
can be either base or acid
ex: H2O - OH- and H3O+
Types of Redox reactions
- Combination
- Decomposition
- Combustion
what is the oxidation number for F in all compounds?
-1
How do we determine if a reaction is redox?
We assign oxidation numbers
end point
the point in a titration where all the substances have been reacted to make products
Molecular Equation
the full, balanced equation
Complete Ionic Equation
Shows the DISSOLVED IONS
Net ionic
reaction which does not show the spectator ions (!)
also includes the charge
theoretical yield
the amount that SHOULD be made up with the limiting agent
Percent yield
[(actual yield)/(theoretical yield)] x 100%
How do I balance normal redox reactions?
- write the half reactions
- Match the e-
- Add together
- simplify by getting rid of spectators
Oxidation half, where are e-?
products
LOSING e-
Reduction half, where are e-?
reactants
GAINING e-
