Examples of electron configuration

The electronic configuration is one that indicates how electrons are structured and how they communicate within an atom.

The configuration indicates the location of the electrons at the different orbital levels of the energy levels of a chemical element.

Types of electron configuration

• Condensed configuration: levels that appear full in the standard configuration that can be presented with a noble gas .
• Developed configuration: represent all the electrons in an atom using arrows that simulate the rotation of each one.
• Semi-developed configuration: it is a combination of the two previous configurations.

The levels are 1, 2, 3, 4, 5, 6 and 7 and the energy sublevels are represented by “s”, “p”, “d” and “f”, for example: 1s, 2s, 2p, 3s , 3p, 4s, 3d, 4p . These levels indicate the order of filling with the electrons.

For filling, the Möller diagram is usually used , which has a diagonal shape. From level 1s an arrow is followed until reaching the last level in that scheme . You cannot skip a level until you complete the previous one. Electrons occupy the lowest energy sublevels first.

To know how electrons are distributed in a chemical element, its atomic number must be known.

Examples of electron configuration

In the following representation, Z is the atomic number of each element.

• Hydrogen (Z = 1) = 1s ¹
• Lithium (Z = 3) = 1s ² , 2s ¹
• Sodium (Z = 11) = 1s ² , 2s ² , 2p ⁶ , 3s ¹
• Potassium (Z = 19) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ¹
• Xenon (Z = 54) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ² , 3d ¹⁰ , 4p ⁶ , 5s ² , 4d ¹⁰ , 5p ⁶
• Osmium (Z = 76) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ² , 3d ¹⁰ , 4p ⁶ , 5s ² , 4d ¹⁰ , 5p ⁶ , 6s ² , 4f ¹⁴ , 5d ⁶
• Lead (Z = 82) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ² , 3d ¹⁰ , 4p ⁶ , 5s ² , 4d ¹⁰ , 5p ⁶ , 6s ² , 4f ¹⁴ , 5d ¹⁰ , 6p ^two
• Cesium (Z = 55) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ² , 3d ¹⁰ , 4p ⁶ , 5s ² , 4d ¹⁰ , 5p ⁶ , 6s ¹
• Helium (Z = 2) = 1s ²
• Beryllium (Z = 4) = 1s ² , 2s ²
• Boron (Z = 5) = 1s ² , 2s ² , 2p ¹
• Carbon (Z = 6) = 1s ² , 2s ² , 2p ²
• Nitrogen (Z = 7) = 1s ² , 2s ² , 2p ³
• Oxygen (Z = 8) = 1s ² , 2s ² , 2p ⁴
• Fluorine (Z = 9) = 1s ² , 2s ² , 2p ⁵
• Neon (Z = 10) = 1s ² , 2s ² , 2p ⁶
• Magnesium (Z = 12) = 1s ² , 2s ² , 2p ⁶ , 3s ²
• Aluminum (Z = 13) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ¹
• Silicon (Z = 14) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ²
• Phosphorus (Z = 15) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ³
• Sulfur (Z = 16) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁴
• Chlorine (Z = 17) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁵
• Argon (Z = 18) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶
• Calcium (Z = 20) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ²
• Strontium (Z = 38) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ² , 3d ¹⁰ , 4p ⁶ , 5s ²
• Iridium (Z = 72 ) = 1s2, 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ² , 3d ¹⁰ , 4p ⁶ , 5s ² , 4d ¹⁰ , 5p ⁶ , 6s ² , 4f ¹⁴ , 5d ⁷
• Antimony (Z = 51) =  1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ² , 3d ¹⁰ , 4p ⁶ , 5s ² , 4d ¹⁰ , 5p ³
• Mercury (Z = 80) =  1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ² , 3d ¹⁰ , 4p ⁶ , 5s ² , 4d ¹⁰ , 5p ⁶ , 6s ² , 4f ¹⁴ , 5d ¹⁰
• Franci (Z = 87) =  1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ² , 3d ¹⁰ , 4p ⁶ , 5s ² , 4d ¹⁰ , 5p ⁶ , 6s ² , 4f ¹⁴ , 5d ¹⁰ , 6p6 , 7s1
• Iron (Z = 26) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ² , 3d ⁶
• Cobalt (Z = 27) = 1s ² , 2s ² , 2p ⁶ , 3s ² , 3p ⁶ , 4s ² , 3d ⁷