Advertisements
Advertisements
प्रश्न
Calculate the oxidation number of the underlined atom.
Cr2O72−
Advertisements
उत्तर
Cr2O72−
Oxidation of O = –2
\[\ce{Cr2O^2-_7}\] is an ionic species.
∴ Sum of the oxidation numbers of all atoms = – 2
∴ 2 × (Oxidation number of Cr) + 7 × (Oxidation number of O) = – 2
∴ 2 × (Oxidation number of Cr) + 7 × (–2) = – 2
∴ 2 × (Oxidation number of Cr) – 14 = – 2
∴ 2 × (Oxidation number of Cr) = – 2 + 14
∴ Oxidation number of Cr = `+12/2`
∴ Oxidation number of Cr in \[\ce{Cr2O^2-_7}\] = +6
APPEARS IN
संबंधित प्रश्न
Choose the correct option.
Oxidation numbers of Cl atoms marked as Cla and Clb in CaOCl2 (bleaching powder) are
\[\begin{array}{cc} \ce{Cl^{{a}}}\phantom{.} \\/\phantom{...} \\ \ce{Ca}\phantom{......} \\ \backslash\phantom{..} \\\phantom{........} \ce{O-Cl^{{b}}}\phantom{.} \end{array}\]
Choose the correct option.
The coefficients p, q, r, s in the reaction \[\ce{{p}Cr2O7^{2Θ} + {q}Fe^{2⊕}->{r}Cr^{3⊕} + {s}Fe^{3⊕} + H2O}\] respectively are:
Choose the correct option.
Oxidation number of carbon in H2CO3 is
Calculate the oxidation number of the underlined atom.
H2SO4
Calculate the oxidation number of the underlined atom.
K2C2O4
Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.
\[\ce{HF_{(aq)} + {OH}^-_{ (aq)}->H2O_{(l)} + {F}^ -_{ (aq)}}\]
Identify the following pair of species is in its oxidized state?
Cl2/Cl−
Justify the following reaction as a redox reaction.
\[\ce{2Na_{(s)} + S_{(s)} -> Na2S_{(s)}}\]
Find out the oxidizing and reducing agents.
Provide the stock notation for the following compound:
FeO
Provide the stock notation for the following compound:
Fe2O3
Which of the following redox couple is a stronger oxidizing agent?
\[\ce{MnO^Θ_4}\](E0 = 1.51 V) and \[\ce{Cr2O^{2Θ}_7}\](E0 = 1.33 V)
Which of the following redox couple is a stronger reducing agent?
Li (E0 = - 3.05 V) and Mg (E0 = - 2.36 V)
The following statements are CORRECT, EXCEPT:
The oxidation number of oxygen in peroxides is ____________.
What is the oxidation number of As in H3AsO3?
What is the oxidation number of Mn in \[\ce{MnO^{2-}_4}\] ion?
In the reaction,
\[\ce{MnO^{-1}_4 (aq) + Br^{-1}(aq) -> MnO2(s) + BrO^{-1}_3(aq)}\]
the correct change in oxidation number of the species involved is ______.
In the following reaction, the oxidation number of Cr changes.
\[\ce{ClO^-_{( aq)} + Cr(OH)^-_{4(aq)} -> CrO^{2-}_{4(aq)} + Cl^-_{( aq)} (basic)}\]
Match the following.
| Compound | Oxidation no. of underlined element |
| i. \[\ce{\underline{C}_4H4O^{2-}_6}\] | a. +2.5 |
| ii. \[\ce{\underline{N}_3H}\] | b. +1.5 |
| iii. \[\ce{Mg2\underline{P}_2O7}\] | c. +5 |
| iv. \[\ce{Na2\underline{S}_4O6}\] | d. `-1//3` |
All of these are CORRECT for the complex K4[Mn(CN)6], EXCEPT:
Stock notations are used to specify the oxidation numbers of ____________.
The sum of oxidation number of all atoms in \[\ce{S2O^{2-}_3}\] ion is ______.
The oxidation state of phosphorous in Mg2P2O7 is ______.
The oxidation number of Cr in \[\ce{Cr(OH)^-_4}\] ion is ______.
Among group 16 elements, which one does not show −2 oxidation state?
Which of the following changes exhibit that nitrogen undergoes oxidation?
Find CORRECT statement for following reaction.
\[\ce{2Ag+ + Cu -> 2Ag + Cu^2+}\]
