Advertisements
Advertisements
Question
Identify the following pair of species is in its oxidized state?
\[\ce{O2/O^2-}\]
Advertisements
Solution
\[\ce{O2/O^2-}\]
Here, each O gains two electrons to form \[\ce{O^2-}\] ion.
\[\ce{O2_{(g)} + 2e- ->2O^2-_{ (aq)}}\]
Hence, \[\ce{O2/O^2-}\] is in a reduced state.
APPEARS IN
RELATED QUESTIONS
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.
Which of the following halogens does always show oxidation state -1?
Calculate the oxidation number of the underlined atom.
HNO3
Calculate the oxidation number of the underlined atom.
H2S4O6
Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.
\[\ce{I2_{(aq)} + 2S2O^{2-}_{3(aq)}->S4O^{2-}_{6(aq)} + 2I^-_{ (aq)}}\]
What is oxidation?
Identify the following pair of species is in its oxidized state?
Cu/Cu2+
Provide the stock notation for the following compound:
HAuCl4
Provide the stock notation for the following compound:
Tl2O
Which of the following redox couple is a stronger oxidizing agent?
Cl2 (E0 = 1.36 V) and Br2 (E0 = 1.09 V)
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?
Zn (E0 = - 0.76 V) and Fe (E0 = - 0.44 V)
Complete the following table:
Assign oxidation number to the underlined species and write Stock notation of compound
| Compound | Oxidation number | Stock notation |
| AuCl3 | ||
| SnCl2 | ||
| \[\ce{\underline{{V}}_2O^{4-}_{7}}\] | ||
| \[\ce{\underline{{Pt}}Cl^2-_6}\] | ||
| H3AsO3 |
The following statements are CORRECT, EXCEPT:
Oxidation state of Xe in XeOF4 is ____________.
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 which among the following compounds, oxidation number of nitrogen is + 5?
The sum of oxidation states of all atoms in \[\ce{SnO^{2-}_2}\] and CO2 are ____________ respectively.
What is the oxidation number of Carbon in K2C2O4?
The oxidation state of phosphorous in Mg2P2O7 is ______.
Which among the following pair of elements show highest oxidation state +7 in their different compounds?
The brown ring complex is formulated as [Fe(H2O)5NO]SO4. The oxidation number of iron is ______.
Which of the following changes exhibit that nitrogen undergoes oxidation?
Which of the following statements are INCORRECT?
- All the transition metals except scandium form MO oxides which are ionic.
- The highest oxidation number corresponding to the group number in transition metals oxides is attained in Sc2B5 to Mn2B7.
- Basic character increases from V2B5 to V2B4 to V2B5.
- V2B4 dissolves in acids to give VO43– salts.
- CrO is basic but Cr2B5 is atmospheric.
Choose the correct answer from the options given below:
