MCQ
The largest oxidation number exhibited by an element depends on its outer electronic configuration. With which of the following outer electronic configurations the element will exhibit largest oxidation number?
- A3d14s 2
- B
- C3d54s1
- D3d54s2
✓
Answer
- 3d54s2
Explanation:
Highest O.N. of any transition element = (n – 1)d electrons +ns electrons. Therefore, larger the number of electrons in the 3d orbitals, higher is the maximum O.N.
- 3d14s2 = 3
- 3d2 4s2 = 3 + 2 = 5
- 3d54s1 = 5 + 1 = 6
- 3d54s2 = 5 + 2 = 7
Need a full question paper?
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
Explore more
Similar questions
First three ionisation energies (in $kJ/mol$) of three representative elements are given below
→| Element | $IE_1$ | $IE_2$ | $IE_3$ |
| $P$ | $495.8$ | $4562$ | $6910$ |
| $Q$ | $737.7$ | $1451$ | $7733$ |
| $R$ | $577.5$ | $1817$ | $2745$ |
Then incorrect option is
For a gaseous reaction $pA + qB \rightleftharpoons qC + pD$ , Which of the following relationship is true
→$\Delta {H^o}$ combustion of $C_4H_{10}(g)$ is $-2650\, kJ\, mol^{-1}$ the amount of heat evolve at constant pressure that can be obtained by burning $5.8\, kg$ of $C_4H_{10}$ is approx
→The number of electrons involved in the bond formation of ${N_2}$ molecule
→$K_1 , K_2$ and $K_3$ are the equilibrium constants of the following reactions $(I), (II)$ and $(III)$ respectively
→$(I)\,\,\,\,{N_2} + 2{O_2} \rightleftharpoons 2N{O_2}$
$(II)\,\,\,\,2N{O_2} \rightleftharpoons {N_2} + 2{O_2}$
$(III)\,\,\,\,N{O_2} \rightleftharpoons \frac{1}{2}{N_2} + 2{O_2}$
The correct relation from the following is
Which of the following atoms has minimum covalent radius
Product $(A)$ of the reaction is
→The enolic form of acetone contains
The single Bond covalent radius $(SBCR)$ of $P$ is $0.11\,nm.$ The single Bond covalent radius of $Cl$ is : ( $P =$ phosphorus)
→In which of the following equilibrium reactions, the equilibrium would shift to the right, if total pressure is increased