Electronic configuration VIP questions'24

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What is meant by the electronic configuration of an element ?

An element’s electronic configuration is a symbolic representation illustrating how its atoms’ electrons are distributed across various atomic orbitals. When documenting electron configurations, a standardized format is employed: first noting the energy level and type of orbital, then expressing the number of electrons in that orbital as a superscript.

The electronic configuration of 30 elements given below:

(In the order of Atomic number, Name of element, Electronic configuration)

1.Hydrogen :1s¹

2.Helium: 1s²

3.Lithium: 1s² 2s¹

4.Beryllium: 1s² 2s²

5.Boron: 1s² 2s²2p¹

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 2s²2p⁶ 3s² 3^s1

13.Aluminum 1s² 2s² 2p⁶ 3s² 3p¹

14. Silicon 1s² 2s² 2p⁶ 3s² 3p²

15. Phosphorus 1s² 2s² 2p⁶ 3s² 3p³

16. Sulphur 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 2s²2p⁶ 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 3p⁶3d⁷ 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

A pictorial Representation

What are the three rules that must be followed while writing the electronic configuration of elements?

The three rules that dictate the manner in which electrons are filled in atomic orbitals are:

The Aufbau principle: electrons must completely fill the atomic orbitals of a given energy level before occupying an orbital associated with a higher energy level. Electrons occupy orbitals in the increasing order of orbital energy level.

Pauli’s exclusion principle: states that no two electrons can have equal values for all four quantum numbers. Consequently, each subshell of an orbital can accommodate a maximum of 2 electrons and both these electrons must have opposite spins.

Hund’s rule of maximum multiplicity: All the subshells in an orbital must be singly occupied before any subshell is doubly occupied. Furthermore, the spin of all the electrons in the singly occupied subshells must be the same (in order to maximize the overall spin).

Why are electronic configurations important?

Electron configurations offer valuable insights into the chemical behavior of elements by by helping determine the valence electrons of an atom. It also helps classify elements into different blocks (such as the s-block elements, the p-block elements, the d-block elements, and the f-block elements).

How to determine the electronic configurationof an atom

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 1s²2s² 2p6 3s2, the magnesium configuration could be written [Ne]3s²

write down electronic configurations of noble gases.

Helium (He) – 1s²

Neon (Ne) – [He] 2s² 2p⁶

Argon (Ar) – [Ne] 3s² 3p⁶

Krypton (Kr) – [Ar] 3d¹⁰ 4s² 4p⁶

Xenon (Xe) – [Kr] 4d¹⁰5s²5p⁶

Radon (Rn) –[Xe] 4f¹⁴5d¹⁰6s²6p⁶

What is the speciality of electronic configuration of copper?

The electronic configuration of copper is [Ar] 3d¹⁰4s¹This configuration disobeys the aufbau principle due to the relatively small energy gap between the 3d and the 4s orbitals. The completely filled d-orbital offers more stability than the partially filled configuration.

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