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Group 17 Elements
Chapter Name : The P- Block Elements
Sub Topic Code : 102_12_07_18_05
Topic Name : Group 17 Elements
Sub Topic Name : Electron Gain Enthalpy
Introduction

• Halogens have maximum negative electron gain enthalpy in the corresponding periods. • This is due to the fact that the atoms of these elements have only one electron less than stable noble gas configurations. • Electron gain enthalpy becomes less negative down the group. • However, the negative electron gain enthalpy of fluorine is less than that of chlorine. • It is due to small size of fluorine atom. • As a result, there are strong interelectronic repulsions in the relatively small 2p orbitals of fluorine and thus, the incoming electron does not experience much attraction.

Pre-Requisites:

Periodic table, elements, electron gain enthalpy

Activity:

See weeds have iodine in them.

Real Life Question:

Where does chlorine gas come from?

Key Words / FlashCards
Key Words Definitions (pref. in our own words)
group Group is the vertical column on the periodic table which contains elements having the similar properties.
Learning aids / Gadgets
Gadgets How it can be used
Chlorine disinfectant Chlorine is used as a disinfectant.
Places to visit :

Beach.

Practical examples around us
Examples Explainations
Sea weed, chlorine disinfectant Sea weed has iodine in it.
What you learn in Theory:

• Halogens have maximum negative electron gain enthalpy in the corresponding periods. • This is due to the fact that the atoms of these elements have only one electron less than stable noble gas configurations. • Electron gain enthalpy becomes less negative down the group. • However, the negative electron gain enthalpy of fluorine is less than that of chlorine. • It is due to small size of fluorine atom. • As a result, there are strong interelectronic repulsions in the relatively small 2p orbitals of fluorine and thus, the incoming electron does not experience much attraction.

What you learn in Practice:

• Halogens have maximum negative electron gain enthalpy in the corresponding periods. • This is due to the fact that the atoms of these elements have only one electron less than stable noble gas configurations. • Electron gain enthalpy becomes less negative down the group. • However, the negative electron gain enthalpy of fluorine is less than that of chlorine. • It is due to small size of fluorine atom. • As a result, there are strong interelectronic repulsions in the relatively small 2p orbitals of fluorine and thus, the incoming electron does not experience much attraction.

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