Chemistry, 03.07.2019 11:10 tallen21

Determine the oxidation state of nitrogen in lino3.

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Answer from: monaldossari

Answer : The oxidation state of nitrogen in LiNO_3 is, (+5)

Explanation :

Rules for the oxidation numbers :

The oxidation number of a free element is always be zero. The oxidation number of a monatomic ion equal to the charge of the ion. The oxidation number of Hydrogen (H) is +1.The oxidation number of oxygen (O) in compounds is usually -2, but it is -1 in the 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.

The given compound is, LiNO_3

Let the oxidation state of 'N' be, 'x'

$(+1)+x+3(-2)=0\\\\x=+5$

Hence, the oxidation state of N is, (+5)

Answer from: oportela23

The oxidation state of N in ${\text{LiN}}{{\text{O}}_3}$ is $\boxed{ + 5}$

Further Explanation:

Redox 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 at the same time. 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 an oxidant or oxidizing agent. The presence of a redox pair or redox couple is a must for the redox reaction.

The general representation of a redox reaction is,

${\text{X}}+{\text{Y}}\to{{\text{X}}^+}+{{\text{Y}}^-}$

The oxidation half-reaction can be written as:

${\text{X}}\to{{\text{X}}^+}+{e^-}$

The reduction half-reaction can be written as:

${\text{Y}}+{e^-}\to{{\text{Y}}^-}$

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 number of a free element is always zero.

2. The oxidation number 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 numbers of all the elements present in a neutral compound is zero.

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

The oxidation state of O is -2 and the oxidation state of Li is +1.

The expression to calculate the oxidation state in ${\text{LiN}}{{\text{O}}_3}$ is:

$\left[ {1\left( {{\text{oxidation state of Li}}} \right) + 1\left( {{\text{oxidation state of N}}} \right) + 3\left( {{\text{oxidation state of O}}} \right)} \right] = 0$ …… (1)

Rearrange equation (1) for the oxidation state of N.

${\text{Oxidation state of N}} = \left[ { - 1\left( {{\text{oxidation state of Li}}} \right) - 3\left( {{\text{oxidation state of O}}} \right)} \right]$ …… (2)

Substitute -2 for the oxidation ${\text{state}}$ of O and +1 for the oxidation state of Li in equation (2).

$\begin{aligned}{\text{Oxidation state}}\;{\text{of N}}&=\left[{-1\left({{\text{+1}}}\right)-3\left({-{\text{2}}}\right)}\right]\\&=\left[{-1+6}\right]\\&=+5\\\end{aligned}$

Therefore the oxidation state of N in ${\mathbf{LiN}}{{\mathbf{O}}_{\mathbf{3}}}$ is +5.

Learn more:

1. What is the oxidation state of phosphorus in ${\text{PO}}_3^{3-}$ ion?

2. Determine the oxidation state of Cl in ${\text{NaCl}}{{\text{O}}_{\text{3}}}$ :

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Redox reactions

Keywords: redox reaction, N, LiNO3, oxidation, reduction, reductant, oxidant, reducing agent, oxidizing agent, electrons, redox pair, redox couple, oxidation state, oxidized, reduced, simultaneously, +5, -2, +1, Li, O.

Answer from: Quest

hydrocarbons are organic compounds that contain only hydrogens and carbons. they can be saturated (those which contain only carbon-carbon single bonds) or unsaturated (those which contain carbon-carbon double or triple bonds) in nature. hydrocarbons can undergo several reactions like substitution, elimination etc.

on substituting one or more hydrogen atoms in hydrocarbon it results in the formation of haloalkane. as the halogen atoms are large compared to the carbon and hydrogen atoms, due to which the molecular weight increases and the bond become polar because of presence electronegative halogen atom and results in the increase in boiling point of the haloalkane.

thus, the correct option is (b) that is the boiling point of the new compound increases on substituting a hydrogen atom with a halogen in a hydrocarbon.

Answer from: Quest

you need to have a picture of the atom that way we can answer it

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