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Question

Oxygen (at. no. 8) and sulphur (at. no. 16) belong to same group of the periodic table.

(a) State the electronic configuration of:

  1. Oxygen
  2. Sulphur

(b) Name the group in which these elements belong.


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Solution

(a) Electronic configuration: It is the distribution of electrons in the various shells around the nucleus of an atom.
(i) Atomic number of Oxygen (O)= 8

  • As atomic number= Number of protons and
  • Number of protons= Number of electrons for a neutral atom
  • Electronic configuration of Silicon= 2, 6 (K, L)

(ii) Atomic number of Sulphur (S)= 16

  • Electronic configuration of Sulphur= 2, 8, 6 (K, L, M)

(b) These elements occur in the group VI A or 16th group of the modern periodic table.

Group: A group is a vertical column in the periodic table. There are 18 groups in the periodic table.

  • The number of valence electrons present in the atom of an element indicate the group number.
  • Example: Oxygen and Sulphur both have same number of valence electrons i.e.; 6 valence electrons in their outermost shell i.e. L for Oxygen and M for Sulphur.
  • Therefore their group number is VI A. This group is numbered as 16 in the modern periodic table.
  • This can also be confirmed from the periodic table given below.

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