Muskan Shafi Education Content Expert
Education Content Expert
Electronic Configuration of an element is the arrangement of the electrons in the orbital shells and subshells. Electronic configuration determines the physical state of an element and its reactivity with other elements. Group 16 elements consist of Oxygen (O), Sulfur (S), Selenium (Se), Tellurium (Te), and Polonium (Po). They are also referred to as the oxygen family. The first four elements of Group 16 elements are nonmetals and are termed ‘the chalcogens’.
The electronic configuration of Group 16 elements is categorized by the presence of six electrons in their last shell or the valence shell. The general electronic configuration of Group 16 elements is ns2np4. Due to their electronic configuration, they can react with other elements and also exist in a combined state. Thus, Group 16 elements exist in free as well as in combined states.
Key Terms: Electronic Configuration, Group 16 Elements, Electrons, Valence Shell, Oxygen, Aufbau’s Principle, Periodic Table
What is Electronic Configuration?
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Electronic Configuration is defined as the distribution of electrons of an atom or molecule in atomic or molecular orbitals. The electronic configuration of an atom describes the precise distribution of electrons in an atom. Pauli’s Exclusion Principle, Hund’s Rule, and Aufbau’s Principle are the three principles that are considered during the arrangement of electrons or electronic configuration.
- According to Pauli’s Exclusion Principle, any two electrons in an atom cannot have the same four quantum numbers (n, l, m, s). The starting three quantum numbers can be the same but the fourth one can never be the same.
- According to Hund’s rule, when electrons are arranged in orbitals, then. the similar energy orbitals first occupy one electron in each of them, and after that, only the electrons can start pairing with other electrons in a half-filled orbital.
- According to Aufbau’s principle, the electron will fill the lowest energy level first and then proceed towards the higher energy levels.
Electronic Configuration
Electronic Configuration of Group 16 Elements
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The electronic configuration of Group 16 elements is characterized by the presence of six electrons in their last shell, which is also known as the valence shell. Group 16 elements consist of five elements namely:
- Oxygen (O)
- Sulfur (S)
- Selenium (Se)
- Tellurium (Te)
- Polonium (Po) (a radioactive element)
All Group 16 elements can exist in a free state in nature, however, due to their electronic configuration, they can react with other elements and can also exist in a combined state.
Read More: Electronic Configuration of First 30 Elements
Atomic Orbital Diagonal Rule
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Electronic configuration of an element is best determined using the three above-mentioned principles. For instance, the total number of electrons in an oxygen atom is 8. Going as per the principles, the first step is to fill the lowest energy shell 1s with two electrons. The remaining six electrons are then distributed in 2s and 2p orbitals. So, the 2s orbital will have two electrons, and 2p orbital will have four electrons.
Neil Bohr stated that all the members of the same group of the modern periodic table have a similar electronic configuration. Thus, the general electronic configuration of group 16 elements is ns2 np4.
| Atomic Number | Element | Electronic Configuration |
|---|---|---|
| 8 | O | [He]2s2 2p4 |
| 16 | S | [Ne]3s2 3p4 |
| 34 | Se | [Ar]3d10 4s2 4p4 |
| 52 | Te | [Kr]4d10 5s2 5p4 |
| 84 | Po | [Xe]4f14 5d10 6s2 6p4 |
Noble Gases are considered to have a complete electronic shell, thus, the electronic configuration of most elements is represented in terms of their nearest noble gas.
- One must note that the electronic configuration of any element determines its chemical properties.
- The electronic configuration of Group 16 elements indicates that they have six elements in their valence shell, and require two elements to complete the octet valency.
- As a result, all the elements of group 16 are negatively charged since they can receive two electrons from other elements.
- For instance, oxygen receives two electrons, one from each hydrogen atom to form water.
- Another example is Sulfur, which receives two electrons, one from each hydrogen atom to form hydrogen sulfide gas.
Things to Remember
- Electronic Configuration of an element shows how the electrons are distributed in its atomic orbitals.
- Group 16 has 5 elements namely Oxygen, Sulfur, Selenium, Tellurium, and Polonium.
- There are six electrons in the valence shell of Group 16 elements.
- The general electronic configuration of Group 16 elements is ns2np4.
- Group 16 elements require two elements to complete the octet valency.
- Group 16 elements exist in both free and combined states.
Previous Years’ Questions (PYQs)
- The first ionization energies of group 16 elements…
- Hydrides of group-16 elements show volatility in the order…
- Although the details of the structure of monoclinic sulphur…
- An element belonging to chalcogen group is… (COMEDK UGET 2015)
- If X is a member of the chalcogen family, the chemical highest stability…
- Which one of the following is not a Chalcogen… (Rajasthan PMT 2003)
- The electronic configuration of transition element… (KCET 2018)
- Which electronic configuration of an element has abnormally high… (NEET 1993)
- The electronic configuration of Eu (Atomic no 63)...
- The outermost electronic configuration of the most electronegative… (JEE Advanced 1988)
Sample Questions
Ques. What is the electronic configuration of Group 16 elements? Give an example to explain the same. (3 Marks)
Ans. Group 16 elements have six electrons in their last shell valence shell. Thus, the general electronic configuration of Group 16 elements is ns2np4. Consider an example of Oxygen which is a group 16 element with the atomic number 8. As per the principles for electronic configuration, the lowest energy shell 1s is first filled with two electrons. Then, the remaining six electrons are distributed in 2s and 2p orbitals. Thus, the 2s orbital will have two electrons, and the 2p orbital will have four electrons.
Ques. Explain the general characteristics of Group 16 elements. (3 Marks)
Ans. Group 16 elements include oxygen, sulfur, selenium, tellurium, and polonium. The initial four elements of Group 16 are together termed chalcogens or ore-forming elements. They are called ore-forming elements because an extensive number of metal ores are found in the earth’s crust in the form of sulfides or oxides. Oxygen, a Group 16 element, is the most abundantly found element that is accessible in nature. It is generally found as silicates and different compounds like carbonates, oxides, and sulfates.
Ques. List the electronic configuration of all Group 16 elements. (3 Marks)
Ans. The electronic configuration of all Group 16 elements is as follows:
- Oxygen: [He]2s2 2p4
- Sulphur: [Ne]3s2 3p4
- Selenium: [Ar]3d10 4s2 4p4
- Tellurium: [Kr]4d10 5s2 5p4
- Polonium :[Xe]4f14 5d10 6s2 6p4
Ques. What is the oxidation state of Group 16 elements? (3 Marks)
Ans. Group 16 elements have an electronic configuration of ns2 np4 in their valance shell. Thus, all the elements in Group 16 accomplish noble gas configuration either by the gain of two electrons, framing M-2 or by sharing two electrons, in this manner shaping two covalent bonds.
Therefore, it indicates both negative and positive oxidation states of group 16 elements. The general oxidation states shown by the Group 16 elements are -2, +2, +4 and + 6.
Ques. What is Aufbau Principle? (3 Marks)
Ans. Aufbau Principle is a very crucial principle that has to be followed while determining the electronic configuration of an element. One can write the electronic configuration of an element just by understanding the Aufbau principle. According to the Aufbau Principle, in the ground state, the electrons occupy the atomic orbitals in their order of increasing energies, which is given by n+l rule. The higher the value of n+l for the orbital, the higher would be the energy. In case the two orbitals have the same value for n+l, the orbital with the lower value of n will have the lower energy. Thus, the electrons will occupy that first.
Ques. Name the Group 16 elements and list their nature. (3 Marks)
Ans. Group 16 of the periodic table includes the following elements:
- Oxygen (O)
- Sulfur (S)
- Selenium (Se)
- Tellurium (Te)
- Polonium (Po)
Oxygen and Sulfur are non-metals, whereas Selenium and Tellurium are metalloids. Polonium is metal under typical conditions and is a radioactive element.
Ques. Explain the electron gain enthalpy in Group 16 elements. (3 Marks)
Ans. The electron gain enthalpy decreases when there is an increase in the size of the central atom moving down the group in the periodic table. In group 16 elements, the Oxygen molecule has a less negative electron gain enthalpy than sulfur. The basis for this is that Oxygen, due to its compressed nature encounters more repulsion between the electrons effectively present and the approaching electron.
Ques. Explain the following properties and trends for Group 16 elements:
(A) Ionization Enthalpy
(B) Electronegativity
(C) Atomic and Ionic Radii (3 Marks)
Ans. (A) The ionization enthalpy decreases with an increase in the size of the central atom, thus, it decreases as one moves down group 16 from Oxygen to Polonium since the size of the atom increases as we move down.
(B) Electronegativity decreases as we move down the group, thus, it decreases as we move from oxygen to polonium due to an increase in nuclear size.
(C) The atomic and ionic radius increases as we move from Oxygen to Polonium in Group 16.
Ques. What is the importance of electronic configuration? (3 Marks)
Ans. Electric Configuration is useful as:
- It helps in determining the valency of an element.
- It predicts the properties of a group of elements. Elements with similar electron configurations exhibit similar properties.
- It also helps to interpret atomic spectra.
Ques. What are shells and subshells? (2 Marks)
Ans. Shells, also known as energy levels, are defined as the definite pathway of electrons around the nucleus of the atom. Subshells are the pathway of electron movement within the shell.
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