Is it accidental that IA to VIIA main group elements during chemical reactions get eight electrons in the outermost shells of their ions, similar to noble gas atoms?

Except this all the noble gases have eight electrons in their outermost shell.

An element X has 3 electrons in the outer most shell of the atom. Write the symbol of its ion.

An atom of an element 'A' has three electrons in its outermost shell and that of 'B' has six electrons in the outrer most shell. The formula of the compound formed between these two elements is

Assertion (A): Helium is noble gas. Reason (R) : Any species (atoms or ion)with eight electrons in the valence shell is stable.

The equivalent weight of a species if acts as oxidant or reductant should be derived by: Eq. weight Mol.wt. of oxidant or reductant = ("Mol.w.t of oxidant or reductant")/("Number of electrons lost or gained by onemclecule of oxidant or reductant") . During chemical reactions, equal all equivalents of one species react with same number of equivalents of other species giving same number of equivalent of products. However this is not true for reactants if they react in terms of moles. Also Molarity can be converted to normality by multiplying the molarity with valence factor or .n. factor The equivalent weight of an element is 13.16. It forms an acidic oxide which with KOH forms a salt isomorphous with K_(2)SO_4 The atomic weight of element is :

The number of valence shell electrons that a group IA element loses to get octet configuration

Oxidation number is the charge which an atom of an element has in its ion or appears to have when present in the combined state. It is also called oxidation state. Oxidation number of any atom in the elementary state is zero. Oxidation number of a monoatomic ion is equal to the charge on it. In compounds of metals with non metals, metals have positive oxidation number while non metals have negative oxidation numbers. In compounds of two difference elements, the more electronegative element has negative oxidation number whereas the other has positive oxidation number. In complex ions, the sum of the oxidation number of all the atoms is equal to the charge on the ion. If a compound contains two or more atoms of the same element, they may have same or different oxidation states according as their chemical bonding is same or different. The oxidation state of the most electronegative element in the products of the reaction between BaO_(2) and H_(2)SO_(4) are

Passage-IV : Sulphur and rest of the elements of group 16 are less electronegative than oxygen. Therefore, their atoms cannot take up electrons easily. They can acquire ns^(2)np^(6) configuration by sharing two electrons with the atoms of other elements and thus, exhibit +2 oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the p and s-orbitals of the shell. As a result, they can show +4 and +6 oxidation states shell. The nature of the compounds of sulphur having +4 oxidation state is :

Passage-IV : Sulphur and rest of the elements of group 16 are less electronegative than oxygen. Therefore, their atoms cannot take up electrons easily. They can acquire ns^(2)np^(6) configuration by sharing two electrons with the atoms of other elements and thus, exhibit +2 oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the p and s-orbitals of the shell. As a result, they can show +4 and +6 oxidation states shell. Like sulphur, oxygen does not show +4 and +6 oxidation states. The reason is :