Question

How are the electron configurations of the elements in a given group similar? Illustrate this by writing shorthand configurations for the elements in Group 6A. Do not put spaces in your answer. For example you should enter [He]2(1) for Li. Elements in a given group generally have the same electron configuration except that the value for 1 ^ is different, and corresponds to the row in which the element is found.

Answer 1

Group 6A elements have similar electron configurations since they all have two electrons in the p subshell, with each element in the group increasing the principal quantum number in line with their row on the periodic table.

Step-by-step explanation:

The electron configurations of elements within the same group on the periodic table are similar because they have the same number of valence electrons in their outer shells. Taking Group 6A as an example, the elements have two electrons in their p subshell. Below are the shorthand electron configurations for Group 6A elements:

• Oxygen (O): [He]2s²2p´
• Sulfur (S): [Ne]3s²2p´
• Selenium (Se): [Ar]3d°104s²2p´
• Tellurium (Te): [Kr]4d°105s²2p´
• Polonium (Po): [Xe]4f°145d°106s²2p´

This progression follows the increase in principal quantum number (n) that corresponds to the row in which the element is found.