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myrzilka [38]
3 years ago
14

Use the changes in oxidation numbers to identify which atoms are oxidized and which are reduced in each reaction.

Chemistry
1 answer:
krok68 [10]3 years ago
5 0
You didn't include much information as to what you were referring too, however I answered a similar question recently to a friend so I'm hoping this is the same question in complete as to yours, if not I apologize.

a.) 2Na(s) + Cl2(g) -----> 2NaCl(s) 
Na --> Na+1 is oxidized 
Cl2 --> Cl- is reduced 

b.) 2HNO3(aq) + 6HI(aq) ----> 2NO(g) + 3I2(s) + 4H2O(l) 
N+5 --> N+2 is reduced 
I-1 --> I2 is oxidized 
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Draw the best Lewis structure for NH3 by filling in the bonds, lone pairs, and formal charges. (Assign bonds, lone pairs, radica
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Answer :  The Lewis-dot structure of NH_3 is shown below.

Explanation :

Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.

In the Lewis-dot structure the valance electrons are shown by 'dot'.

The given molecule is, NH_3

As we know that hydrogen has '1' valence electron and nitrogen has '5' valence electrons.

Therefore, the total number of valence electrons in NH_3 = 5 + 3(1) = 8

According to Lewis-dot structure, there are 6 number of bonding electrons and 2 number of non-bonding electrons.

Now we have to determine the formal charge for each atom.

Formula for formal charge :

\text{Formal charge}=\text{Valence electrons}-\text{Non-bonding electrons}-\frac{\text{Bonding electrons}}{2}

\text{Formal charge on N}=5-2-\frac{6}{2}=0

\text{Formal charge on }H_1=1-0-\frac{2}{2}=0

\text{Formal charge on }H_2=1-0-\frac{2}{2}=0

\text{Formal charge on }H_3=1-0-\frac{2}{2}=0

Hence, the Lewis-dot structure of NH_3 is shown below.

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How many valence electrons configuration of oxygen?
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