Explanation of Group 16 Elements Electronic Configuration
The electronic configuration of any element is defined as the arrangement of the electrons around the nucleus. The electronic configuration of any element determines its physical state and reactivity with other elements. When one looks at the Group 16 elements, the electronic configuration of all the elements in that group is categorized by the presence of six electrons in their last shell or the valence shell.
The elements present in group 16 consist of oxygen (0), sulfur (S), selenium (Se), tellurium (Te), and polonium (Po). Of all the elements, only Polonium is radioactive. All these elements can exist in a free state in nature. However, due to its electronic configuration, it can react with other elements and also exists in a combined state.
As stated earlier, electronic configuration refers to the arrangement of electrons on its orbital shells and subshells. All elements in group 16 have six electrons in its last shell; for example, the total number of electrons for oxygen is 8, which is distributed in two shells as 2 and 8. To understand the electronic distribution for other members of group 16, it is important to learn some basic principles to do so.
The first rule is to fill the lower energy shells with electrons first before moving to the higher shells. Hund’s rule, Pauli’s exclusion principle, and Aufbau’s rule are needed to be followed while distributing the electrons. According to Pauli’s exclusion principle, no two electrons in the same atom can not have the same quantum numbers (n,l,m, and s); the first three might have the same quantum number, but it will differ from the fourth value.
According to Hund’s rule, similar energy orbitals accommodate one electron, and then other electrons can pair with them in half-filled orbitals. According to Aufbau’s principle, electrons first occupy the lowest energy levels. All these three principles can be followed while determining the electronic configuration of an atom.
Atomic Orbital Diagonal Rule
Considering all the three above mentioned principles is the best approach for deciphering the electronic configuration of any element. For example, the total number of electrons in an oxygen atom is 8. The first step is to fill the lowest energy shell 1s with two electrons. The remaining six electrons are distributed in 2s and 2p orbitals. 2s orbital will have two electrons, and 2p orbital will have four electrons.
According to Neil Bohr, all the members of the same group of the Periodic table have a similar electronic configuration. Therefore, it also stands true for all the members of group 16, and the electronic configuration of oxygen follows the pattern of the general electronic configuration of group 16 elements, which is ns2 np4.
Since the noble gas is considered to have a complete electronic shell, the electronic configuration of most elements is represented in terms of its nearest noble gas.
It is important to note that the electronic configuration of any element determines its chemical properties. Group 16 electron configuration indicates that its members of Group 16 have six elements in its valence shell, and therefore require two elements to complete the octet valency. Therefore all the elements of group 16 are negatively charged since it can receive two electrons from other elements.
These anions can interact with positively charged cations that can donate electrons so that their octet is also completed along with these anions. For example, oxygen receives two electrons, one from each hydrogen atom to form water. Sulfur receives two electrons, one from each hydrogen atom to form hydrogen sulfide gas.
About Electronic Configuration
Students have been introduced to the atomic structure of elements in the previous classes. We all know that Atoms consist of electrons, protons and neutrons. In this class, we will get to learn about the arrangement of these subatomic particles inside the atoms of any particular element.
The rules and principles used for determining the position of all electrons are studied under the Physical Chemistry of Class 11 NCERT textbooks. It also mentions the story of various scientists working to understand and identify the difference between various types of materials available on Earth and their properties. It is the story of the gradual development of chemistry as a subject of study.
The electrons are the freely moving subatomic particles revolving around a nucleus centre consisting of protons and neutrons. The degree of freedom of electrons varies according to the orbit they choose for their position. Several protons present in the atoms of an element are known as the 'Atomic Number' of the element.
This Atomic number also gives us information about the number of electrons present in the atom which are equal in number to balance the net positive charge of protons. The Periodic Table arranges the elements in the increasing order of their atomic number and categorizes all elements into different groups. Neil Bohr suggested that the elements of the same group have similar electronic configurations.
For example, the atoms Hydrogen and Helium with single and double electrons respectively occupy the lowest valency positions. The rule and principle to arrange the electrons by assigning different orbits around the nucleus are known as the Electronic configuration of atoms. As the chemical properties of the elements depend on the number of outermost free electrons. We all know that the properties of the elements under the same group are the same so the number of electrons in the outermost cell is equal. The Elements of group 16 such as Oxygen, Sulfur, Selenium, Tellurium, Polonium and all have 6 electrons on the outermost cell. The 's' valence shells always contain 2 electrons, The 'p' valence shell contains 4 electrons.
To know the significance of the electronic configuration of the Group 16 elements, log into Vedantu and seek deeper insights from the expert mentors. Study and understand the concepts of this topic to answer critical questions easily.
FAQs on Electronic Configuration of Group 16 Elements
1. When is the right time to learn about the Electronic Configuration of Atoms?
Chemistry as a subject is quite vast. Students learn about elements and compounds and their basic physical and chemical properties in high school classes. The presence of sub-atomic particles that govern these properties is studied in higher classes. The Central Board of Secondary Education (CBSE) has structured its curriculum with the introduction of the electronic configuration of atoms in Class 11. The NCERT textbook also mentions the earlier developments before the concept. Students, who are willing to choose the science stream as their career, will need to study this fundamental topic right from the beginning at the basic level. It is then they can proceed to learn advanced concepts in the higher classes easily.
2. What is the electronic configuration of the other group elements?
The other group of elements also follow the same principle of filling up the free electrons in their valence shells but differ in the number of electrons present on the outer shell of the atom. As the Hydrogen group elements Lithium, Sodium, Potassium, Rubidium, Cesium, and Fluorine also have one free electron in their outermost shells.
The Group 2 elements such as Beryllium, Magnesium, Calcium, and Strontium have 2 free electrons in the outermost shells. Likewise, you can easily find out about all the groups of the elements and their electronic configuration by studying their positions in the Periodic Table.
3. Why does the difference in the number of free electrons on outermost Valence shells of atoms impart different properties to the elements?
The properties of elements such as metal, non-metal, or its state such as solid, liquid, or gas, and others depend on the interaction of atoms of the same element or other elements. This interaction in turn is controlled by the number of electrons that can be released or accepted easily by all atoms of the element. So, we can conclude that the number of electrons present on the outermost valence shells determines the movement of electrons. So it is quite clearly understood that the number of electrons is responsible for the properties of the elements.
4. What are noble gases?
The natural properties of elements are reactive. They cannot exist in the free state and are present in the form of combined with other elements. But some elements are capable of existing in a free and pure state. Examples are Neon, Argon, Krypton, Xenon, etc.
These are unreactive and are present as trace gases in the atmosphere. so they are termed Noble gases. According to the electronic configuration theory the atoms of these gases hold the maximum amount of electrons that can be present. And these gases are in no need of any exchange of electrons with any other elements.
6. What is the General Electronic Configuration of Group 16 Elements?
The general electronic configuration of group 16 elements is ns2 np4.
7. What is the Number of Electrons Present in the Valence Shell of Group 16 Elements?
Six electrons are present in the valence shell of group 16 elements.
8. What are the Principles Followed to Define Electronic Configuration?
Pauli’s exclusion principle, Hund’s rule, and Aufbau’s principles are followed to determine the electronic configuration of any elements.
9. What is the Radioactive Element in Group 16?
Polonium is a radioactive element in group 16.
10. Why are Elements of Group 16 Negatively Charged?
Since all the elements of group 16 have six electrons in their valence shell, they can accept two electrons to complete the octet valency. Therefore, these elements are negatively charged.
