Valence electron configuration in group 1A:
ns1
in which n=1, 2, 3, 4, 5, ... etc.
Starting with Hydrogen, H, electron configuration:
1s1
followed by Lithium, Li, electron configuration:
(1s2), 2s1
(non valence electrons in () brackets)
They all have a single valence electron in the s orbital of the respective energy level.
these elements have 5 electron in the valence shells and have configuration of ns np5
Valence electron configuration in group 7A (halogens): ns2, np5 in which n=2, 3, 4, 5, ... etc. Starting with fluorine, F, electron configuration: (1s2), 2s2 2p5 (non valence electrons in () brackets)
Elements that have configuration of ns2np5 are members of the Halogen group(Group VIIA). They are, Fluorine, Bromine, Iodine and Astatine.
The elements in group 6a (16) have six valence electrons. The valence electron configuration is Xs2Xp4 , where X is the main energy level (period number).
the valence electron configuration of the representative elements are corresponding to the group in which they are found
these elements have 5 electron in the valence shells and have configuration of ns np5
Valence electron configuration in group 7A (halogens): ns2, np5 in which n=2, 3, 4, 5, ... etc. Starting with fluorine, F, electron configuration: (1s2), 2s2 2p5 (non valence electrons in () brackets)
valence electrons and electronic configuration.
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Elements that have configuration of ns2np5 are members of the Halogen group(Group VIIA). They are, Fluorine, Bromine, Iodine and Astatine.
All elements in group 1 have 1 valence electron.
Atoms of elements in Groups 13-18 have 10 fewer valence electrons than their groups numbers.However , helium atoms have only 2 valence electrons.
The elements in group 6a (16) have six valence electrons. The valence electron configuration is Xs2Xp4 , where X is the main energy level (period number).
the valence electron configuration of the representative elements are corresponding to the group in which they are found
There are 2 valence electrons (electrons in the outer shell) of group 2 elements in the ground (un-ionised or standard) state. This causes them to form +2 ions.
All elements in group 16 share similar properties because their valence shells all contain the s2p4 electron configuration.
All elements in group 16 share similar properties because their valence shells all contain the s2p4 electron configuration.