Respuesta :

The Oxidation state of an individual phosphorus atom in PO₃⁻³ is + 3

Further Explanation

Oxidation number  

  • Oxidation of an element refers to the charge that an atom would have if a compound was composed of ions.

Oxidation number neutral atoms and substances  

  • The oxidation number of neutral substances that contains only one element or atoms of the same element is zero.
  • This includes all neutral atoms such as potassium, Aluminium and molecular elements such as O2, S8, P4, etc.

Oxidation number of simple ions

  • Simple ions have an oxidation number equivalent to the charge on the ion.
  • For example the oxidation number of K+ ion is +1 while that of O^-2 is -2.

Oxidation number of Hydrogen  

  • Oxidation number of hydrogen is -1 when combined with metals. For example in NaH, CaH2, etc.
  • Oxidation number of hydrogen is +1 when it is combined with non-metals. For example in CH4, HCl, NH3, etc.

Oxidation number in compounds  

  • The sum of oxidation numbers in a neutral compound is zero. For example, the sum of oxidation number of hydrogen and oxygen in water is Zero.

Oxidation number in polyatomic ions

  • Oxidation number in polyatomic ions is equivalent to the charge on that ion.
  • For example; in SO4^-2, NO3^-1, etc.

In this case;

We are given PO3^-3 which is a polyatomic ion.

Therefore, the sum of oxidation number of oxygen and phosphorus will be -3

Oxidation number of Oxygen is -2  

Oxidation number of phosphorus is x  

Therefore;

(x) + (-2x3) = -3  

 x + -6 = -3  

 x = -3 + 6  

  x = + 3  

Therefore, the Oxidation number of Phosphorus in PO₃⁻³ is +3.

Keywords: Oxidation numbers, polyatomic ions  

Learn more about:  

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Level: High school  

Subject: Chemistry  

Topic: Oxidation numbers  

The oxidation state of phosphorus in [tex]{\text{PO}}_3^{3 - }[/tex] is [tex]\boxed{ + 3}[/tex] .

Further Explanation:

Redox reaction:

Redox is a term that is used collectively for the reduction-oxidation reaction. It is a type of chemical reaction in which the oxidation states of atoms are changed. In this reaction, both reduction and oxidation are carried out simultaneously. Such reactions are characterized by the transfer of electrons between the species involved in the reaction.

The process of gain of electrons or the decrease in the oxidation state of the atom is called reduction while that of loss of electrons or the increase in the oxidation number is known as oxidation. In redox reactions, one species lose electrons and the other species gain electrons. The species that lose electrons and itself gets oxidized is called as a reductant or reducing agent. The species that gains electrons and gets reduced is known as oxidant or oxidizing agent. The presence of redox pair or redox couple is a must for the redox reaction.

The general representation of a redox reaction is,

[tex]{\text{X}}+{\text{Y}}\to {{\text{X}}^ + }+{{\text{Y}}^ - }[/tex]

The oxidation half-reaction can be written as:

 [tex]{\text{X}}\to{{\text{X}}^ + }+{e^ - }[/tex]

The reduction half-reaction can be written as:

 [tex]{\text{Y}}+{e^ - }\to{{\text{Y}}^ - }[/tex]

Here, X is getting oxidized and its oxidation state changes from  to +1 whereas B is getting reduced and its oxidation state changes from 0 to -1. Hence, X acts as the reducing agent whereas Y is an oxidizing agent.

Rules to calculate the oxidation states of elements:

1. The oxidation state of a free element is always zero.

2. The oxidation state of oxygen is generally taken as -2, except for peroxides.

3. The oxidation state of hydrogen is normally taken as +1.

4. The sum of oxidation states of all the elements present in a neutral compound is zero.

5. The oxidation state of group 1 and group 2 elements are +1 and +2 respectively.

The oxidation state of O is -2.

The expression to calculate the oxidation number in [tex]{\text{PO}}_3^{3 - }[/tex] is:

[tex]\left[{\left({{\text{oxidation state of P}}}\right)+3\left({{\text{oxidation state of O}}} \right)} \right]=- 3[/tex]                            …… (1)

Rearrange equation (1) for the oxidation number of P

[tex]{\text{Oxidation number of P}}=\left[{\left({ - 3}\right) - 3\left({{\text{oxidation number of O}}}\right)}\right][/tex]                   …… (2)  

Substitute -2 for the oxidation state of O in equation (2).

 [tex]\begin{aligned}{\text{Oxidation state}}\;{\text{of P}}&=\left[{\left({ - 3} \right)-3\left({ - 2}\right)}\right]\\&=-3+6\\&=+3\\\end{aligned}[/tex]

So the oxidation state of P in [tex]{\mathbf{PO}}_{\mathbf{3}}^{{\mathbf{3 - }}}[/tex] is +3.

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Answer details:

Grade: High School

Subject: Chemistry

Chapter: Redox reactions

Keywords: oxidation state, +3, P, O, PO33-, free element, zero, neutral, redox reactions, reducing agent, oxidizing agent, reductant, oxidant, increase, decrease.

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