Here, we are required to determine how many electrons are typically involved in bonding for group 1, group 2 and group 3 elements and How many electrons are typically involved in bonding for group 6, 7 and 8 elements.
For group 1: Only one electron.
For group 2: Only two electrons
For group 3: Only 3 electrons
For group 6: Only 2 electrons
Fir group 7: Only 1 electron
For group 8: No electron
<em>The Valence electrons are the electrons which are available for bonding and chemical reactions in elements.</em>
<em>The Valence electrons are the electrons which are available for bonding and chemical reactions in elements.However, not all Valence electrons are actively involved in bonding. This is evident in the group 7(halogens) elements, although they have 7 Valence electrons, only one is actively involved in bonding.</em>
For group 1 elements: They have only one Valence electron and it is actively involved in bonding (ionic bonding)
For group 2 elements: They have only two Valence electron and both are actively involved in bonding (ionic bonding)
For group 3 elements: They have only three Valence electrons and all three are typically used for bonding.
For group 6 elements: They have 6 Valence electrons and are electronegative. As such, they only need to receive 2 electrons from an electropositive element and consequently, they only contribute two electrons into the bonding. As such, only 2 electrons are typically used for bonding.
For group 7: They have 7 Valence electrons and are highly electronegative. As such, they only need to receive 1 electrons from an electropositive element and consequently, they only contribute 1 electrons into the bonding. As such, only 1 electrons are typically used for bonding.
For group 8: They have a full octet configuration and are unreactive. Therefore, no electron is typically used for bonding.
S-S Overlapping. In this kind of overlapping, one 's' orbital from each participating atom undergoes head-on overlapping along the internuclear axis. ...
Electron affinity for fluorine is than chlorine most likely , due to the electron repulsion that occur between the electron where n= 2 . the elements in the second period have such small electron clouds that electron repulsion is greater than that of the rest of the family.
