Advertisements
Advertisements
प्रश्न
Considering the parameters such as bond dissociation enthalpy, electron gain enthalpy and hydration enthalpy, compare the oxidising power of F2 and Cl2.
उत्तर
Fluorine is a much stronger oxidizing agent than chlorine. The oxidizing power depends on three factors.
1. Bond dissociation energy
2. Electron gain enthalpy
3. Hydration enthalpy
The electron gain enthalpy of chlorine is more negative than that of fluorine. However, the bond dissociation energy of fluorine is much lesser than that of chlorine. Also, because of its small size, the hydration energy of fluorine is much higher than that of chlorine. Therefore, the latter two factors more than compensate for the less negative electron gain enthalpy of fluorine. Thus, fluorine is a much stronger oxidizing agent than chlorine.
APPEARS IN
संबंधित प्रश्न
Account for the following:
N2 is less reactive at room temperature.
Give reasons for the following : (CH3)3 P = O exists but (CH3)3 N = O does not.
The group 15 element having inner electronic configuration as of argon is-
(a) Phosphorous (z = 15)
(b) Antimony (z =51)
(c) Arsenic (z = 33)
(d) Nitrogen (z = 7)
Among the hydrides of Group-15 elements, which have the lowest boiling point?
Among the hydrides of Group-15 elements, which have the highest bond angle?
Give reasons When Cl2 reacts with the excess of F2, ClF3 is formed and not FCl3.
Account for the following
Bi(V) is a stronger oxidizing agent than Sb(V).
Account for the following :
N − N single bond is weaker than P − P single bond.
What is the action of sodium on arsenic.
Explain the geometry of [Cu(NH3)4]2+ on the basis of hybridisation [ At. No. Cu = 29 ].
Give reasons for the following:
E⁰ value for (Mn3+|Mn2+) is highly positive than that for (Cr3+|Cr2+) couple.
In which of the following compound, nitrogen shows the oxidation state of +5?
Which of the following group 15 elements forms metallic bonds in an elemental state?
Which of the following orders are correct as per the properties mentioned against each?
| (i) | \[\ce{As2O3 < SiO2 < P2O3 < SO2}\] | Acid strength. |
| (ii) | \[\ce{AsH3 < PH3 < NH3}\] | Enthalpy of vapourisation. |
| (iii) | \[\ce{S < O < Cl < F}\] | More negative electron gain enthalpy. |
| (iv) | \[\ce{H2O > H2S > H2Se > H2Te}\] | Thermal stability. |
Account for the following:
Zinc is a comparatively a soft metal, iron and chromium are typically hard.
Which of the following pairs will have same chemical properties?
Given below are two statements, one is labelled as Assertion (A) and the other is labelled as Reason (R):
Assertion: Smaller the size of an atom greater is the electronegativity.
Reason: Electronegativity refers to the tendency of atom to share electrons with other atom.
The elements with zero electron affinity are
P4O10 is an anhydride of
