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प्रश्न
Although fluorine is more electronegative than oxygen, but the ability of oxygen to stabilise higher oxidation states exceeds that of fluorine. Why?
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उत्तर
The electronic configuration of fluorine is \[\ce{1s^2 2s^2 2p^5}\]. Thus it can form only one bond as it has only one unpaired electron. Electronic configuration of oxygen is \[\ce{1s^2 2s^2 2p^6 3s^2 3p^6}\].
It may be mentioned that oxygen also has vacant d-orbitals along with two 3p orbitals containing single electron. Thus, oxygen has greater bond formation capacity. In other words, it has greater ability to stabilize higher oxidation states.
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संबंधित प्रश्न
|
`E_((M^(2+)/M)` |
Cr | Mn | Fe | Co | Ni | Cu |
| -0.91 | -1.18 | -0.44 | -0.28 | -0.25 | -0.34 |
From the given data of E0 values, answer the following questions :
(1) Why is `E_(((Cu^(2+))/(Cu)))` value exceptionally positive
(2) Why is `E_(((Mn^(2+))/(Mn)))` value is highly negative as compared to other elements
(3) Which is the stronger reducing agents Cr2+ or Fe2+ ? Give Reason.
To what extent do the electronic configurations decide the stability of oxidation states in the first series of the transition elements? Illustrate your answer with examples.
Which one of the following ions is coloured?
NF3 is possible, but NF5 is not. Why?
Why do transition metals exhibit higher enthalpy of atomization?
Give reasons for the following:
The transition metals generally form coloured compounds.
Maximum oxidation state is shown by ____________.
In lake test for Al3+ ions, there is the formation of coloured ‘floating lake’. It is due to ______.
A complex in which dsp2 hybridisation takes place is ______.
Why are all copper halides known except that copper iodide?
Give reasons for the following statement:
Transition metals and most of their compounds show paramagnetic behaviour.
Consider the following standard electrode potentials (E° in volts) in aqueous solution:
| Element | M3+/M | M+/M |
| Al | - 1.66 | +0.55 |
| Tl | + 1.26 | -0.34 |
Based on these data, which of the following statements is correct?
The disproportionation of \[\ce{MnO^{2-}_4}\] in acidic medium resulted in the formation of two manganese compounds A and B. If the oxidation state of Mn in B is smaller than that of A, then the spin-only magnetic moment (µ) value of B in BM is ______. (Nearest integer)
The oxidation state of Fe in [Fe(CO)5] is ______.
Account for the following:
Ce4+ is a strong oxidising agent.
The second ionization enthalpies of chromium and manganese are 1592 and 1509 kJ/mol respectively. Explain the lower value of Mn.
Write the ionic equation for reaction of KI with acidified KMnO4.
Explain the magnetic properties of d-block (or transition) elements.
Compare the general characteristics of the first series of the transition metals with those of the second and third series metals in the respective vertical columns. Give special emphasis on the following point:
Ionisation enthalpies
