Advertisements
Advertisements
Question
Calculate the oxidation number of the underlined atom.
H2S4O6
Advertisements
Solution
H2S4O6
Oxidation number of H = +1
Oxidation number of O = –2
H2S4O6 is a neutral molecule.
∴ Sum of the oxidation numbers of all atoms = 0
∴ 2 × (Oxidation number of H) + 4 × (Oxidation number of S) + 6 × (Oxidation number of O) = 0
∴ 2 × (+1) + 4 × (Oxidation number of S) + 6 × (–2) = 0
∴ 4 × (Oxidation number of S) + 2 – 12 = 0
∴ 4 × (Oxidation number of S) = + 10
∴ Oxidation number of S =`+10/4`
∴ Oxidation number of S in H2S4O6 = +2.5
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.
A compound contains atoms of three elements A, B, and C. If the oxidation state of A is +2, B is +5 and that of C is -2, the compound is possibly represented by
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 is the correct stock notation for manganese dioxide?
Choose the correct option.
Oxidation number of oxygen in superoxide is
Choose the correct option.
Which of the following halogens does always show oxidation state -1?
Calculate the oxidation number of the underlined atom.
H3PO3
Calculate the oxidation number of the underlined atom.
K2C2O4
Calculate the oxidation number of the underlined atom.
NaH2PO4
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:
Tl2O
Provide the stock notation for the following compound:
FeO
Provide the stock notation for the following compound:
MnO
Assign oxidation number atom in the following species.
\[\ce{Cr(OH)^Θ_4}\]
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:
Oxidation state of Xe in XeOF4 is ____________.
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 ______.
Identify the strongest oxidising agent.
\[\ce{Na^+ + e^- -> Na}\]; E0 = −2.714 V
\[\ce{Pt^{2+} + 2e^- -> Pt}\]; E0 = +1.200 V
\[\ce{I2 + 2e^- -> 2I^-}\]; E0 = + 0.535 V
\[\ce{Co^{2+} + 2e^- -> Co}\]; 0 = −0.280 V
In which among the following compounds, oxidation number of nitrogen is + 5?
When methane undergoes combustion in air, the oxidation number of C ____________.
What is the oxidation number of Carbon in K2C2O4?
The oxidation state of phosphorous in Mg2P2O7 is ______.
The oxidation number of Cr in \[\ce{Cr(OH)^-_4}\] ion is ______.
What is the oxidation state of chlorine atom in perchloric acid?
The oxidation number of oxygen in oxygen difluoride (OF2) and dioxygen difluoride (O2F2) respectively is ______.
