How many electrons are there in the outermost shell of a group 16 element?

6

The correct answer is option (4) 6.

Group 16 elements, also known as the oxygen family or chalcogens, have six electrons in their outermost shell. The outermost shell is referred to as the valence shell, and the electrons in this shell are called valence electrons. Group 16 of the periodic table includes elements such as oxygen (O), sulfur (S), selenium (Se), tellurium (Te), and polonium (Po). These elements share similar chemical properties and have six valence electrons. The electron configuration of group 16 elements is typically written as \(ns^2 np^4\), where \(n\) represents the principal quantum number of the outermost shell. Oxygen, for instance, is in the 2nd period of the periodic table. Its electron configuration is \(1s^2 2s^2 2p^4\). In this case, the 2nd shell (valence shell) has 6 electrons (\(2s^2\) and \(2p^4\)). As you move across a period (horizontal row) in the periodic table, the number of valence electrons increases by one from left to right. Group 16 elements are in the 2nd period, and they have 6 valence electrons. The number of valence electrons determines the chemical properties of an element. Group 16 elements tend to form compounds with other elements, including gaining two electrons to achieve a stable \(ns^2 np^6\) electron configuration. In summary, a group 16 element has 6 electrons in its outermost shell, and this characteristic defines its chemical behavior and reactivity.