Select the redox change in the following reaction

Oxidants are substances which

In which compound does Vanadium have an oxidation number of +4?

Which of the following is reduced in the following reaction?

Select the type of redox change in the following reaction:

Reductants are substances which

When KMnO₄ acts as an oxidising agent and ultimately forms then the number of electrons transferred in each case respectively is

Which of the following is a redox reaction?

Which of the following chemical reactions depict the oxidising behaviour of  ?

Arrange in increasing order of oxidation number of N:

Identify the oxidation number of V in  ions respectively.

Arrange the following in increasing order of oxidation number of Fe:

Determine the oxidation numbers of the following:

N atoms in  , Fe in and Cr in 

The correct order of the oxidation states of nitrogen in  and  is :

What is the oxidation number of Cr in ?

What is the oxidation number of Cr in ?

What is the oxidation number of Ba in  ?

Which of the following metal has more oxidation number in   ?

What is the oxidation number of Na in NaH?

Find the O.N. of Ca in ?

What is the O.N. of Cl in ?

What is the oxidation number of CI in CIF?

The oxidation number of potassium in respectively is :

Which of the following reactions is a redox reaction?

Identify the process in which change in the oxidation state is five :

In polythionic acid, $\mathrm{H}_2 \mathrm{~S}_x \mathrm{O}_6(x=3$ to 5$)$ the oxidation state(s) of sulphur is/are :

Consider the following reduction processes

$\begin{aligned} & \mathrm{Zn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}(\mathrm{s}) ; \mathrm{E}^{\mathrm{o}}=-0.76 \mathrm{~V} \\ & \mathrm{Ca}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Ca}(\mathrm{s}) ; \mathrm{E}^0=-2.87 \mathrm{~V} \\ & \mathrm{Mg}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mg}(\mathrm{s}) ; \mathrm{E}^0=-2.36 \mathrm{~V} \\ & \mathrm{Ni}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Ni}(\mathrm{s}) ; \mathrm{E}^0=-0.25 \mathrm{~V}\end{aligned}$

The reducing power of the metals increases in order:

In reaction with stronger oxidizing agents like KIO₄, hydrogen peroxide oxidizes with the evolution of O₂The oxidation number of I in KIO₄ changes to __________.

Experimentally it was found that a metal oxide has formula M_0.98O.Metal M, is present as M²⁺and  M³⁺ in its oxide. Fraction of the metal which exists as M³⁺  would be:

What is the oxidation number of P in P₄?

What is the sum of the oxidation numbers of all the atoms in  ?

Find the oxidation number of the  atom in ?

What is the oxidation state of Mo in $\left(\mathrm{NH}_4\right)_6 \mathrm{Mo}_7 \mathrm{O}_{24}$

Arrange the following species in decreasing order of oxidation numbers:

The possible oxidation state of oxygen is

In which of the following molecule nitrogen has highest oxidation state ? 

Oxidiation states of P in  and  are respectively

In Chromyl chloride, the oxidation state of chromium is (+) ______.

Which element undergoes oxidation as well as reduction in the following reaction?

The average oxidation states of sulphur in and  are:

Match the following:

Compound(atom)	Oxidation State of Atom
(I)	(A) +1
(II)	(B) -1
(III)	(C) +2
(IV)	(D) +7

The oxidation number of Mn in is :

Arrange the following compounds based on increasing oxidation state:

In the reaction , the species that is oxidised and the species that is reduced is:

Match the following:

compound	oxidation state
(I)	A) +6
(II)	B) +1
(III)	C) -2
(IV)	D) +4

Match the following:

compound	oxidation state
(I)	A) +2
(II)	B) +7
(III)	C) +6
(IV)	D) +4

For the reaction: 

What is the oxidation state changes of Sulphur?

What is the oxidation state of sulphur in Dithionic acid and sulfoxylic acid?

Which of the following is a self-indicator?

Eriochrome T is not used as an indicator for which of the following metals?

Which of the following species do not disproportionate?

What is the oxidation state of in and in ?

What are the two oxidation states present in ?

For the reaction: , what is the oxidation half reaction?
 

Which of the following compounds exhibit a oxidation state for oxygen?

What is the oxidation State of nitrogen in ?

Match the following with the oxidation state of chlorine:

Compound	Oxidation state
I)	A)
II)	B)
III)	C)
IV)	D)

What are the two oxidation states in thiosulfurous acid?

What is the oxidation state of nitrogen in peroxynitrous acid?

Metaboric acid dehydrates to form pyroboric acid. What is the change in oxidation state change?

Hypophosphate salts on standing in air convert into pyrophosphates. What is the change in oxidation state?

How many of these oxoacids have sulphur in  oxidation state?

Which of the following sulfur oxoacids has sulfur in 0 oxidation state?

Metaperiodic acid reacts with hot water to give

Match the following:

Compound	Oxidation State
I)	A)
II)	B)
III)	C)
IV)	D)

Which of the following oxoacids have phosphorus in oxidation state?

 

What is the oxidation state of in Ruthenic acid?

Arrange the following oxoacids based on increasing oxidation state:

$\mathrm{Br}_2+\underset{\text { hot }+ \text { conc. }}{\mathrm{NaOH}} \longrightarrow \mathrm{NaBr}+X+\mathrm{H}_2 \mathrm{O}$

Sum of stoichiometric coefficients of $\mathrm{Br}_2\: \: \&\: \: \mathrm{NaOH}$ in balanced equation is.

From the given list, the number of compounds with +4 oxidation state of Sulphur is _________ .

$\mathrm{SO}_3, \mathrm{H}_2 \mathrm{SO}_3, \mathrm{SOCl}_2, \mathrm{SF}_4, \mathrm{BaSO}_4, \mathrm{H}_2 \mathrm{~S}_2 \mathrm{O}_7$

Which of the following cannot function as an oxidising agent?

In chromyl chloride test for confirmation of $\mathrm{Cl}^{-}$ion, a yellow solution is obtained. Acidification of the solution and addition of amyl alcohol and $10 \% \mathrm{H}_2 \mathrm{O}_2$ turns organic layer blue indicating formation of chromium pentoxide. The oxidation state of chromium in that is :

The oxidation number of iron in the compound formed during brown ring test for $\mathrm{NO}_3^{-}$ion is_________.

Reduction potential of ions are given below:

$\begin{array}{ccc}\mathrm{ClO}_4^{-} & \mathrm{IO}_4^{-} & \mathrm{BrO}_4^{-} \\ \mathrm{E}^{\circ}=1.19 \mathrm{~V} & \mathrm{E}^{\circ}=1.65 \mathrm{~V} & \mathrm{E}^{\circ}=1.74 \mathrm{~V}\end{array}$

The correct order of their oxidizing power is.

In the reaction of potassium dichromate, potassium chloride and sulfuric acid (conc.), the oxidation state of the chromium in the product is (+) ________ .

In acidic medium, $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ shows oxidizing action as represented in the half reaction. $\mathrm{Cr}_2 \mathrm{O}_7^{2-}+\mathrm{XH}^{+}+\mathrm{Ye}^{-} \rightarrow 2 \mathrm{~A}+\mathrm{ZH}_2 \mathrm{O}$
$\mathrm{X}, \mathrm{Y}, \mathrm{Z}$ and $\mathrm{A}$ respectively are :

Which of the following is not a redox reaction?

Which of the following statements regarding sulphur is incorrect ?

Oxidation number of Carbon in $\mathrm{C}_3 \mathrm{O}_2, \mathrm{Mg}_2 \mathrm{C}_3$ are respectively

Oxidation involves:-

Oxidation is a process in which

Oxidation number of N in $\mathrm{HNO}_3$ is

Oxidation number of lodine $\mathrm{IO}_3^{-}$is

Oxidation number of Sulphur in $S_8$

Oxidation states of P in $\mathrm{H}_4 \mathrm{P}_2 \mathrm{O}_5, \mathrm{H}_4 \mathrm{P}_2 \mathrm{O}_5, \mathrm{H}_4 \mathrm{P}_2 \mathrm{O}_7$, respectively are

Conversion of $\mathrm{PbSO}_4$ to PBS is

What volume of 3 molar $\mathrm{HNO}_3$ is needed to oxidise of 8 g of $\mathrm{Fe}^{2+}$ to $\mathrm{Fe}^{3+}$ ? $\mathrm{HNO}_3$ get converted to NO :

When $\mathrm{KMnO}_4$  act as an oxidising agent ultimately forms $\mathrm{MnO}_4^{2-}, \mathrm{MnO}_2, \mathrm{Mn}_2 \mathrm{O}_3$ and $\mathrm{Mn}^{2+}$ then the number of electrons transferred in each case are:

Which act as a reducing agent?

Which of the following arrangements represent increasing oxidation number of the central atom?

 Sum of oxidation state (magnitude) and coordination number of cobalt in $\mathrm{Na}\left[\mathrm{Co}(\right.$ bpy $\left.) \mathrm{Cl}_4\right]$ is _________.

If potassium iodide (KI) acts as oxidizing agent, change occurs from, indicates presence of :-

In which of the following compounds an element exhibits two different oxidation states ?

In which of the following compounds iron has an oxidation number of +3.

What is the oxidation number of Cr in Cr₂ O₇^2-

Which of the following arrangements represents increasing oxidation number of central atom ?

Which substance can act only as a reducing agent ?

The oxidation number of nitrogen atoms in NH₄NO₃ are

A weak acid is titrated with a weak base. Consider the following statements regarding the pH of the solution at the equivalence point:

(i) pH depends on the concentration of acid and base

(ii) pH is independent of the concentration of acid and base

(iii) pH depends on the $p K_a$ of acid and $p K_b$ of base
(iv) pH is independent of the $p K_a$ of acid and $p K_b$ of base

The correct statements are:

(A) Only (i) and (iii)

(B) Only (i) and (iv)

(C) Only (ii) and (iii)

(D) Only (ii) and (iv)

The metal with the highest oxidation present in $\mathrm{K}_2 \mathrm{CrO}_4, \mathrm{NbCl}_5$ and $\mathrm{MnO}_2$ is

The oxidising ability of the given anions follows the order

The reaction, $\begin{aligned} & \mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7+m \mathrm{meSO}_4+n \mathrm{H}_2 \mathrm{SO}_4 \rightarrow \mathrm{Cr}_2\left(\mathrm{SO}_4\right)_3+\mathrm{PFe}_2\left(\mathrm{SO}_4\right)_3+\mathrm{K}_2 \mathrm{SO}_4+ \\ & q \mathrm{H}_2 \mathrm{O}\end{aligned}$ when balanced, m.n, p and q are, respectively

In the reaction $\mathrm{SO}_2+2 \mathrm{H}_2 \mathrm{~S} \rightarrow 3 \mathrm{~S}+2 \mathrm{H}_2 \mathrm{O}$ the substance that is oxidized is

The formal oxidation numbers of Cr and Cl in the ions $\mathrm{Cr}_2 \mathrm{O}_7^{2-}$ and $\mathrm{ClO}_3^{-}$, respectively, are:

The oxidation number of sulphur is $+4$  in 

The oxidation states of P atom in POCl₃, H₂PO₃ and H₄P₂O₆ , respectively, are

The incorrect statements among the following is

Which of the following oxidation reactions are carried out by both $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ and $\mathrm{KMnO}_4$ in acidic medium?
A. $\mathrm{I}^- \rightarrow \mathrm{I}_2$
B. $\mathrm{S}^{2-} \rightarrow \mathrm{~S}$
C. $\mathrm{Fe}^{2+} \rightarrow \mathrm{Fe}^{3+}$
D. ${I }^{-} \rightarrow \mathrm{IO}_3^{-}$
E. $\mathrm{S}_2 \mathrm{O}_3{ }^{2-} \rightarrow \mathrm{SO}_4{ }^{2-}$

Choose the correct answer from the options given below :

The compound that can work both as an oxidising and reducing agent is

Given below are two statements :

Statement (I) : The oxidation state of an element in a particular compound is the charge acquired by its atom on the basis of electron gain enthalpy consideration from other atoms in the molecule.

Statement (II) : $\mathrm{p} \pi-\mathrm{p} \pi$ bond formation is more prevalent in second period elements over other periods.

In the light of the above statements, choose the most appropriate answer from the options given below :

In which of the following compounds, an element exhibits two different oxidation states.

The exhibition of various oxidation states by an element is also related to the outer orbital electronic configuration of its atom. Atom(s) having which of the following outermost electronic configurations will exhibit more than one oxidation state in its compounds.

$\begin{aligned} & \text { (i) } 3 s^1 \\ & \text { (ii) } 3 d^1 4 s^2 \\ & \text { (iii) } 3 d^2 4 s^2 \\ & \text { (iv) } 3 s^2 3 p^3\end{aligned}$

The most commonly used reducing agent is

The oxidation number of an element in a compound is evaluated on the basis of certain rules. Which of the following rules is not correct in this respect?

Thiosulphate reacts differently with iodine and bromine in the reactions given below:

$$
\begin{aligned}
& 2 \mathrm{~S}_2 \mathrm{O}_3^{2-}+\mathrm{I}_2 \rightarrow \mathrm{~S}_4 \mathrm{O}_6^{2-}+2 \mathrm{I}^{-} \\
& \mathrm{S}_2 \mathrm{O}_3^{2-}+2 \mathrm{Br}_2+5 \mathrm{H}_2 \mathrm{O} \rightarrow 2 \mathrm{SO}_4^{2-}+2 \mathrm{Br}^{-}+10 \mathrm{H}^{+}
\end{aligned}
$$

Which of the following statements justifies the above dual behaviour of thiosulphate?

For the given cell, $M g\left|M g^{2+}\right|\left|C u^{2+}\right| C u$
(i) $M g$ is cathode
(ii) Cu is cathode
(iii) The cell reaction is $\mathrm{Mg}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Mg}^{2+}+\mathrm{Cu}$
(iv) Cu is the oxidising agent

Only $2 \mathrm{~mL}$ of $\mathrm{KMnO}_4$ solution of unknown molarity is required to reach the end point of a titration of $20 \mathrm{~mL}$ of oxalic acid ( $2 \mathrm{M})$ in acidic medium. The molarity of $\mathrm{KMnO}_4$ solution should be _________ M.

Oxidation Number of S in $\mathrm{H}_2 \mathrm{SO}_5$ is

Oxidation states of sulphur atoms in $S_4 O_6{ }^{-2}$ from left to right respectively are

The basicity of thiosulphuric acid is

The number of neutrons present in the more abundant isotope of boron is ' $\mathrm{x}$ '. Amorphous boron upon heating with air forms a product, in which the oxidation state of boron is ' $y$ '. The value of $x+y$ is ...

The oxidation number of phosphurus in hypophosphoric acid is  -

The oxidation state of S in $\mathrm{H}_2 \mathrm{SO}_4$ is 

The oxidation states of iron atoms in compounds (A), (B) and (C), respectively,  are x, y and z. The sum of x, y and z is______.

$\begin{array}{ccc}\mathrm{Na}_4\left[\mathrm{Fe}(\mathrm{CN})_5(\mathrm{NOS})\right] & \mathrm{Na}_4\left[\mathrm{FeO}_4\right] & {\left[\mathrm{Fe}_2(\mathrm{CO})_9\right]} \\ (\mathrm{B}) & (\mathrm{C})\end{array}$

The pair in which phosphorous atoms have a formal oxidation state of +3 is :

The redox reaction among the following is:

The total change in the oxidation state of manganese involved in the reaction of $\mathrm{KMnO}_4$ and potassium iodide in the acidic medium is __________ .

The oxidation state of cobalt in the following molecules is

Consider a titration of potassium dichromate solution with acidified Mohr’s salt solution using diphenylamine as an indicator. The number of moles of Mohr’s salt required per mole of dichromate is

(Response should be only in integer like 67 or 8).

Among the following , identify the species with an atom in +6 oxidation state :