Electronic Configuration of first 30 Elements

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The number of electrons present in each subshell surrounding the nucleus of an atom is represented by its electronic configuration. The orbitals are denoted by the letters s, p, d, and f, and the maximum number of electrons present in these orbitals is 2, 6, 10, and 14. Aufbau’s principle, Pauli’s exclusion principle, and Hund’s rule are used to write the electronic configuration.

Aufbau’s Principle states that electrons are filled in shells in the following order of energy levels: 1s, 2s, 2p, 3s, 3p, 4s, 4p, 5s, 4d, 5p, 6s, 5d, 6p, 7s, 5f, 6d, 7p, and so on.

Pauli’s Exclusion Principle: 

According to Pauli’s exclusion principle, no two electrons in an atom can have the same four quantum numbers. Every orbital has the capacity to hold two electrons, and even those two electrons have different spins. This means that if one electron is spin-up, the other must be spin-down.

Hund’s Rule: 

Hund’s rule is an extension of Aufbau’s principle. In the case of Aufbau’s principle, electrons are filled in orbitals from lowest to highest energy levels. However, according to Hund’s rule, each orbital is partially filled before electron pairing. As a result, the singly filled electrons all have the same spin, ensuring the orbital stability.

Electronic Configuration Notation:

The number of electrons present in the subshell is represented by notation. It is written in superscript with the shell number, the name of the subshell, and the total number of electrons present in the subshell.

The electronic configuration of oxygen, for example, can be written as 1s2 2s2 2p4

The electronic configuration of the first 30 elements is shown in the table below.

Electronic Configuration

1. Hydrogen 1s1

2. Helium   1s2

3. Lithium     1s2 2s1

4. Beryllium    1s2 2s2

5. Boron     1s2 2s2 2p1

6. Carbon    1s2 2s2 2p2

7. Nitrogen      1s2 2s2 2p3

8. Oxygen     1s2 2s2 2p4

9. Fluorine   1s2 2s2 2p5

10. Neon    1s2 2s2 2p6

11. Sodium    1s2 2s2 2p6 3s1

12. Magnesium    1s2 2s2 2p6 3s2

13. Aluminum   1s2 2s2 2p6 3s2 3p1

14. Silicon    1s2 2s2 2p6 3s2 3p2

15. Phosphorus   1s2 2s2 2p6 3s2 3p3

16. Sulfur    1s2 2s2 2p6 3s2  3p4

17. Chlorine    1s2 2s2 2p6 3s2 3p5

18. Argon   1s2 2s2 2p6 3s2 3p6

19. Potassium 1s2 2s2 2p6 3s2 3p6 4s1

20. Calcium   1s2 2s2 2p6 3s2 3p6 4s2

21. Scandium 1s2 2s2 2p6 3s2 3p6 3d1 4s2

22. Titanium 1s2 2s2 2p6 3s2 3p6 3d2 4s2

23. Vanadium 1s2 2s2 2p6 3s2 3p6 3d3 4s2

24. Chromium 1s2 2s2 2p6 3s2 3p6 3d5 4s1

25. Manganese 1s2 2s2 2p6 3s2 3p6 3d5 4s2

26. Iron 1s2 2s2 2p6 3s2 3p6 3d6 4s2

27. Cobalt 1s2 2s2 2p6 3s2 3p6 3d7 4s2

28. Nickel 1s2 2s2 2p6 3s2 3p6 3d8 4s2

29. Copper 1s2 2s2 2p6 3s2 3p6 3d10 4s1

30. Zinc 1s2 2s2 2p6 3s2 3p6 3d10 4s2

How to write electronic configuration of elements?

So, before drawing an electronic configuration, we must first extract information from the periodic table such as the atomic number, number of electrons, shells, and so on. Let’s look at an example to better understand the writing method of an electronic configuration. The atomic number of potassium is 19. And it has 19 electrons that will be assigned to the s and p subshells.

The electronic configuration is as follows: 1s2 2s2 2p6 3s2 3p6 4s1. Its 19 electrons can be divided into shells in the following ways:

K shell (n=1) equals 2, L shell (n=2) equals 8, M shell (n=3) equals 8, and N shell (n=4) equals 1.

What is the significance of electronic configurations?

Electron configurations explain the chemical conduct of components by determining the valence electrons of an iota. It makes a difference to divide the components into distinct squares (such as the s-block components, the p-block components, the d-block components, and the f-block components). This makes it easier to consider the properties of the components as a whole.

It is important to note that, for components with higher nuclear numbers, a less difficult way of composing the electronic setup is with the assistance of respectable gases. Because respectable gases have filled the most distant shells, they can be used as a prefix to type in the electronic setup.

How Can I Tell What Electron Configuration I Have?

To determine the electron configurations of atoms, you must first determine the order in which the various sublevels are filled. Electrons enter available sublevels in descending order of increasing energy. Before proceeding to the next sublevel, a sublevel is filled or half-filled.

Because the s sublevel can only hold two electrons, the 1s is occupied at helium (1s2). The p sublevel has a capacity of six electrons, the d sublevel has a capacity of ten electrons, and the f sublevel has a capacity of fourteen electrons. Rather than writing out the entire configuration, the common shorthand notation is to refer to the noble gas core. Instead of writing out 1s2 2s2 2p6 3s2, the magnesium configuration could be written [Ne]3s2.

Conclusion

The number of electrons present in each subshell surrounding the nucleus of an atom is represented by its electronic configuration. The orbitals are denoted by the letters s, p, d, and f, and the maximum number of electrons present in these orbitals is 2, 6, 10, and 14. The number of electrons present in the subshell is represented by notation. It is written in superscript with the shell number, the name of the subshell, and the total number of electrons present in the subshell. The arrangement of electrons in energy levels around an atomic nucleus, also known as electronic configuration or electronic structure.