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 in group 7A have 7 valence electrons. Elements in group 1A have one valence electron, elements in group 2A have 2 valence electrons, etc. Noble gases have a full outer shell of 8 valence electrons.
There are 7 valence electrons in group 7A.
There are 7 valence electrons in group 7A.
these elements have 5 electron in the valence shells and have configuration of ns np5
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)
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 electrons and electronic configuration.
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)
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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.