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Electron gain enthalpy with negative sign of fluorine is less than that of chlorine due to :
Electron gain enthalpy with negative sign of fluorine is less than that of chlorine due to :
Updated On: Jun 23, 2024
- High ionization enthalpy of fluorine
- Smaller size of chlorine atom
- Smaller size of fluorine atom
- Bigger size of $2p$ orbital of fluorine
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The Correct Option is C
Solution and Explanation
The electron gain enthalpy order for halogens is
$CI > F > Br > I$
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.
$CI > F > Br > I$
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.
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Concepts Used:
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- P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
- P block elements are shiny and usually a good conductor of electricity and heat as they have a tendency to lose an electron. You will find some amazing properties of elements in a P-block element like gallium. It’s a metal that can melt in the palm of your hand. Silicon is also one of the most important metalloids of the p-block group as it is an important component of glass.
P block elements consist of:
- Group 13 Elements: Boron family
- Group 14 Elements: Carbon family
- Group 15 Elements: Nitrogen family
- Group 16 Elements: Oxygen family
- Group 17 Elements: Fluorine family
- Group 18 Elements: Neon family
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