Electron gain enthalpy with negative sign of fluorine is less than that of chlorine due to :
(a) High ionization enthalpy of fluorine
(b) Smaller size of chlorine atom
(c) Smaller size of fluorine atom
(d) Bigger size of 2p orbital of fluorine
(c) The electron gain enthalpy order for halogens is Cl > F > Br > I Due to small size of fluorine the extra electron to be added feels more electron-electron repulsion. Therefore fluorine has less value for electron affinity than chlorine.
Ionization enthalpy is the energy required to remove an electron from an isolated gaseous atom in its ground state. Although the atoms are widely separated in the gaseous state, there...
[Hint : Due to small size of F atom and compact 2p orbitals there are strong interelectronic repulsions in the relatively smaller 2p orbitals of fluorine. So the incoming electron...
(i) This is due to smaller size of oxygen the electron cloud is distributed over a small region of space, making electron density high which repels the incoming electrons.
(ii) Because...
Second electron affinity of O is largely +ve because of repulsion between negatively charged ions and second electron to be added. Energy required to overcome repulsion is more than the...
The electron gain enthalpy for halogens is highly negative because they can acquire the nearest stable noble gas configuration by accepting an extra electron.