Determine the oxidation number (oxidation state) of each element in the compound CuCO3. Cu: C: O: Determine the oxidation number of each element in CH4. C: H: Determine the oxidation number of each element in IF. I: F: Determine the oxidation number of each element in CH2Cl2. C: H: Cl:

Answer :

(a) The oxidation number of Cu, C and O is, (+2), (+4) and (-2)

(b) The oxidation number of C and H is, (-4) and (+1)

(c) The oxidation number of I and F is, (+1) and (-1)

(d) The oxidation number of C, H and Cl is, (0), (+1) and (-1)

Explanation :

Oxidation number : It is also called oxidation state. It is a number assigned to an element in a chemical compound that represent the number of electrons gained or lost by an element in a compound.

Rules for Oxidation Numbers :

The oxidation number of a free element is always zero.

The oxidation number of a monatomic ion equals the charge of the ion.

The oxidation number of  Hydrogen (H)  is +1, but it is -1 in when combined with less electronegative elements.

The oxidation number of  oxygen (O)  in compounds is usually -2, but it is -1 in peroxides.

The oxidation number of a Group 1 element in a compound is +1.

The oxidation number of a Group 2 element in a compound is +2.

The oxidation number of a Group 17 element in a binary compound is -1.

The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.

The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

(a) The given compound is,

Let the oxidation state of Cu be, 'x'

As, the oxidation number of carbon is (+4) and oxidation number of oxygen is (-2).

The oxidation state of Cu is, (+2)

(b) The given compound is,

Let the oxidation state of C be, 'x'

As, the oxidation number of hydrogen is (+1).

The oxidation state of C is, (-4)

(c) The given compound is,

Let the oxidation state of I be, 'x'

As, the oxidation number of a Group 17 element in a binary compound is -1. And iodine and fluorine belongs to 17 group.

The oxidation state of I is, (+1)

(d) The given compound is,

Let the oxidation state of C be, 'x'

As, the oxidation number of hydrogen is (+1) and oxidation number of a Group 17 element (Cl) in a binary compound is -1.

The oxidation state of C is, (0)

Different elements has different types of oxidation state or number.

The oxidation number of Copper is +2, Carbon is +4 and Oxygen is -2. The oxidation number of Carbon is -4 and Hydrogen is +1. The oxidation number of I is +1 and iron is -1. The oxidation number of Carbon is 0, Hydrogen is +1 and Chlorine is -1.

The oxidation state or oxidation number refers to the hypothetical charge occur on an atom if all of its bonds were fully ionic means complete transfer of electron. The oxidation state may be positive, negative or zero so different atoms formed different oxidation state.

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1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: