Use the rules (in order) to assign oxidation numbers to each of
the elements in the compounds below.
hydroxylamine
H
N
O
NH2OH
___-7-6-5-4-3-2-10+1+2+3+4+5+6+7
___-7-6-5-4-3-2-10+1+2+3+4+5+6+7
___-7-6-5-4-3-2-10+1+2+3+4+5+6+7
magnesium bromide
Br
Mg
MgBr2
___-7-6-5-4-3-2-10+1+2+3+4+5+6+7
___-7-6-5-4-3-2-10+1+2+3+4+5+6+7
boric acid
H
B
O
H3BO3
For each of the following:
• Assign Oxidation States (Numbers) to each atom in reactants
and products
• Identify the species being reduced and the species being
oxidized
• Balance each redox reaction using the Half-Reaction method
O2 + ClO-2 -->
H2O + ClO2
Al + MnO-4 --> MnO2 +
Al(OH)-4
NO2- + Al --> NH3 +
AlO2
Also could you please explain how you get the oxidation numbers,
i am having trouble with that as well as to how...
Give an example of a balanced reaction with oxidation numbers for
the following elements.
a) selenium
b.) tellurium
c.) polonium
Reaction with anything. Just need an example of what that might
look like.
Assign the oxidation numbers to each species as a reactant and
as a product.
Balance equation _2_KCLO3(s)-->__2_KCl(s) + __3__
O2
K in KCLO3(S)
K in KCL(s)
Cl in KCLO3(S)
Cl in KCL (s)
O in KCLO3 (S)
O in O2
In this reaction __________ is oxidized and __________ is
reduced
1. Assign oxidation numbers to the Iron atoms of Magnetite.
Recall Magnetite's chemical formula Fe3O4 is better written as
FeOFe2O3.
2. Sketch electron filling of the d-orbitals for the Fe3+, Fe2+,
Gd3+ and Y3+ ions. Rank them according to increasing
paramagnetism.
3. Hessonite (Cinnamon Stone) is a variety of Grossular which is
a Calcium-Aluminum rich garnet gemstone with a formula of
Ca3Al2(SiO4)3.Would you expect this garnet to be magnetic?
Explain.
Determine the oxidation number of iodine in each of the
following compounds. Be sure to enter your answer as X+ or X-
(a)NaI
(b)I2
(c)IO2
(d)I2O7
(e)KIO4
(f)Ca(IO)2
In each of the following balanced oxidation-reduction equations,
identify those elements that undergo changes in oxidation number
and indicate the magnitude of the change in each case
Part A
2MnO4−(aq)+3S2−(aq)+4H2O(l)→3S(s)+2MnO2(s)+8OH−(aq)
Enter your answers as chemical symbols separated by a comma.
Part C
4H2O2(aq)+Cl2O7(g)+2OH−(aq)→2ClO2−(aq)+5H2O(l)+4O2(g)
Enter your answers as chemical symbols separated by a comma
Ba2+(aq)+2OH−(aq)+H2O2(aq)+2ClO2(aq)→Ba(ClO2)2(s)+2H2O(l)+O2(g)
Enter your answers as chemical symbols separated by a comma
In each of the following balanced oxidation-reduction equations,
identify those elements that undergo changes in oxidation number
and indicate the magnitude of the change in each case.
2MnO4−(aq)+3S2−(aq)+4H2O(l)→3S(s)+2MnO2(s)+8OH−(aq)
4H2O2(aq)+Cl2O7(g)+2OH−(aq)→2ClO2−(aq)+5H2O(l)+4O2(g)
Ba2+(aq)+2OH−(aq)+H2O2(aq)+2ClO2(aq)→Ba(ClO2)2(s)+2H2O(l)+O2(g)
Determine the oxidation state for each of the elements
below.
The oxidation state of
...
iodine
...
in
...
diiodine pentoxide
I2O5
...
is
...
___ .
The oxidation state of
sulfur
in
sulfur trioxide
SO3
is
__
The oxidation state of
bromine
in
bromine trifluoride
BrF3
is
___.