Table of Contents
Explanation of Group 16 Elements Electronic Configuration
Group 16 elements have an electronic configuration of ns2np3. The ns2np3 configuration is the result of the 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6. Electronic Configuration of Group 16 Elements | Atomic Orbital Diagonal Rule.
The electronic configuration of group 16 elements is ns2np4. In this configuration, the s orbital is filled with two electrons, and the p orbital is filled with four electrons.
The diagonal rule is a simple way to predict the shape of an atomic orbital. The rule states that the shape of an atomic orbital is a simplex with the number of vertices equal to the number of atomic orbitals in the atom. The shape of the atomic orbital is determined by the distance between the nucleus and the electron. The closer the electron is to the nucleus, the more spherical the orbital will be. The further the electron is from the nucleus, the more linear the orbital will be.
Group 16 of the periodic table consists of the elements oxygen, sulfur, selenium, tellurium, and polonium. These elements have six electrons in their outermost shells. The electronic configuration of group 16 elements is [He]2s2p4.
Atomic Orbital Diagonal Rule
The atomic orbital diagonal rule states that the total electron density of an atom is the sum of the electron densities of the individual atomic orbitals. This rule is often used to predict the shapes of molecules.
About Electronic Configuration
Electronic configuration is the distribution of electrons in an atom. The electronic configuration of an atom is determined by the number of protons in the nucleus and the number of electrons in the outer shell. Electrons in the outer shell are called valence electrons. The electronic configuration of an atom can be represented by a notation called the orbital diagram. Electronic Configuration of Group 16 Elements | Atomic Orbital Diagonal Rule.