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).
S [Ne] 3s2 3p4
ns2np4
ns2np1
s2 p4
6
It is alternatively called the Carbon family.
Beacause of electronic configuration (M.O.T)
Because it has same number of valence electrons in the same energy level.
Oxygen needs 2 electrons to fill it's valence shell which is why it forms a 2- ion.
2The answer is 1 or two but:-Copper has an electronic configuration of [Ar] 3d10 4s1Copper is a transition metal and the simple concept of valence electrons is difficult to apply to these. You could say 1, expecting the 4s electron to be lost, which does happen to form Cu+ , cuprous, compounds. However copper readily forms Cu2+ in cupric compounds, e.g. in copper sulfate. In these one of the d electrons is also lost to give a d9 configuration.Other oxidation states such as copper (III) and copper(IV) are known.
S [Ne] 3s2 3p4
The Group 6A elements are oxygen, sulfur, selenium, tellurium and polonium. The number of valence electrons in Group 6A is 6.
Sulfur is part of column 16 or group 6A because, all elements in group 6A have 6 valence electrons. Sulfur has 6 valence electrons.
It is alternatively called the Carbon family.
oxygen has 6 valence electrons as indicated by the 6A above the group oxygen is in
Beacause of electronic configuration (M.O.T)
they are in the same group "6a" because they have the same number of Valence electrons
Because it has same number of valence electrons in the same energy level.
Oxygen needs 2 electrons to fill it's valence shell which is why it forms a 2- ion.
Sulfur is in group XVI (or 6A) and so has 6 valence electrons. The electron dot diagram for S would thus have to show (b) six dots.
group 6A
2The answer is 1 or two but:-Copper has an electronic configuration of [Ar] 3d10 4s1Copper is a transition metal and the simple concept of valence electrons is difficult to apply to these. You could say 1, expecting the 4s electron to be lost, which does happen to form Cu+ , cuprous, compounds. However copper readily forms Cu2+ in cupric compounds, e.g. in copper sulfate. In these one of the d electrons is also lost to give a d9 configuration.Other oxidation states such as copper (III) and copper(IV) are known.