
In which of the following compounds transition metal has zero oxidation state ?
A. $Cr{{O}_{5}}$
B. $N{{H}_{2}}.N{{H}_{2}}$
C. $NOCl{{O}_{4}}$
D. $[Fe{{(CO)}_{5}}]$
Answer
163.2k+ views
Hint: In order to solve this question we need to look for two things. First, we need an option in which there is a presence of transition metal and second we need to find the oxidation states and find the one compound with zero oxidation state.
Complete Step by Step Solution:
Transition metal describes the elements of the d-block. Between the s and p blocks are the components that make up the d-block. Between groups 2 and 13 of the periodic table is where this block is located. Fourth period onwards is when it begins.
Considering the definition of the transition metals we can see that in the question, only compounds of option A i.e. $Cr{{O}_{5}}$ and option D i.e. $[Fe{{(CO)}_{5}}]$has the presence of transition metal in it.
The hypothetical charge that an atom would hold if all of its links to other atoms were entirely ionic in nature is what is known as an atom's oxidation state.
So, in the case of $Cr{{O}_{5}}$we know that O carries a charge of -2. Let’s suppose the oxidation number of Cr is x. And this compound is an uncharged molecule, so the net charge on the compound is zero. Therefore, the oxidation number of Cr will be:
$x-2(5)=0$.
Solving it further,
$x-10=0\therefore x=10$ we know the oxidation state of +10 cannot exist so in this case the Cr will acquire the maximum stable oxidation state. For, Cr maximum stable oxidation state is +6. Therefore the oxidation state of Cr in $Cr{{O}_{5}}$ is +6.
Now, in the case of$[Fe{{(CO)}_{5}}]$ we know this is a coordination complex and CO is a ligand which carries a charge of 0. Let’s suppose the oxidation number of Fe is y. And this compound is an uncharged compound, so the net charge on the compound is zero.
Therefore, the oxidation number of Fe will be:
$y-5(0)=0$Solving it further,
$y=0$ Therefore the oxidation state of Fe in $[Fe{{(CO)}_{5}}]$ is 0.
Hence, the correct option is D. $[Fe{{(CO)}_{5}}]$
Note: In this question, first identify the option with the transition metal. After that, find the oxidation states with the appropriate method. If the oxidation state of any metal exceeds the maximum stable oxidation state then the oxidation state is that maximum stable state only.
Complete Step by Step Solution:
Transition metal describes the elements of the d-block. Between the s and p blocks are the components that make up the d-block. Between groups 2 and 13 of the periodic table is where this block is located. Fourth period onwards is when it begins.
Considering the definition of the transition metals we can see that in the question, only compounds of option A i.e. $Cr{{O}_{5}}$ and option D i.e. $[Fe{{(CO)}_{5}}]$has the presence of transition metal in it.
The hypothetical charge that an atom would hold if all of its links to other atoms were entirely ionic in nature is what is known as an atom's oxidation state.
So, in the case of $Cr{{O}_{5}}$we know that O carries a charge of -2. Let’s suppose the oxidation number of Cr is x. And this compound is an uncharged molecule, so the net charge on the compound is zero. Therefore, the oxidation number of Cr will be:
$x-2(5)=0$.
Solving it further,
$x-10=0\therefore x=10$ we know the oxidation state of +10 cannot exist so in this case the Cr will acquire the maximum stable oxidation state. For, Cr maximum stable oxidation state is +6. Therefore the oxidation state of Cr in $Cr{{O}_{5}}$ is +6.
Now, in the case of$[Fe{{(CO)}_{5}}]$ we know this is a coordination complex and CO is a ligand which carries a charge of 0. Let’s suppose the oxidation number of Fe is y. And this compound is an uncharged compound, so the net charge on the compound is zero.
Therefore, the oxidation number of Fe will be:
$y-5(0)=0$Solving it further,
$y=0$ Therefore the oxidation state of Fe in $[Fe{{(CO)}_{5}}]$ is 0.
Hence, the correct option is D. $[Fe{{(CO)}_{5}}]$
Note: In this question, first identify the option with the transition metal. After that, find the oxidation states with the appropriate method. If the oxidation state of any metal exceeds the maximum stable oxidation state then the oxidation state is that maximum stable state only.
Recently Updated Pages
JEE Main 2021 July 25 Shift 1 Question Paper with Answer Key

JEE Main 2021 July 22 Shift 2 Question Paper with Answer Key

JEE Main 2025 Session 2: Exam Date, Admit Card, Syllabus, & More

JEE Atomic Structure and Chemical Bonding important Concepts and Tips

JEE Amino Acids and Peptides Important Concepts and Tips for Exam Preparation

JEE Electricity and Magnetism Important Concepts and Tips for Exam Preparation

Trending doubts
Types of Solutions

Degree of Dissociation and Its Formula With Solved Example for JEE

Classification of Drugs

Instantaneous Velocity - Formula based Examples for JEE

JEE Main Chemistry Question Paper with Answer Keys and Solutions

JEE Main Chemistry Online Mock Test for Class 12

Other Pages
Haloalkanes and Haloarenes

Alcohol Phenol and Ether Class 12 Notes: CBSE Chemistry Chapter 7

Coordination Compounds Class 12 Notes: CBSE Chemistry Chapter 5

NCERT Solutions for Class 12 Chemistry In Hindi Chapter 10 Haloalkanes and Haloarenes In Hindi Mediem

Total MBBS Seats in India 2025: Government College Seat Matrix

NEET Total Marks 2025: Important Information and Key Updates
