Question

1. identify the period and group numbers of the element with the electron - configuration: ne3s²3p⁴

Explanation:

Step1: Analyze the electron - shell number

The principal quantum number \(n\) of the out - most shell gives the period number. Here, the highest \(n\) value in the electron configuration \([Ne]3s^{2}3p^{4}\) is \(n = 3\), so the period number is 3.

Step2: Calculate the number of valence electrons

The electrons in the \(3s\) and \(3p\) orbitals are valence electrons. There are 2 electrons in \(3s\) and 4 electrons in \(3p\), so the total number of valence electrons is \(2 + 4=6\). For main - group elements, the group number is equal to the number of valence electrons (for groups 1 - 2 and 13 - 18). So the group number is 16.

Answer:

Period number: 3; Group number: 16