{"id":5883,"date":"2024-02-03T22:12:09","date_gmt":"2024-02-03T16:12:09","guid":{"rendered":"https:\/\/valenceelectrons.com\/?p=5883"},"modified":"2024-02-03T22:12:12","modified_gmt":"2024-02-03T16:12:12","slug":"orbital-diagram-for-fluorine","status":"publish","type":"post","link":"https:\/\/valenceelectrons.com\/orbital-diagram-for-fluorine\/","title":{"rendered":"Orbital Notation and Diagram for Fluorine (F)"},"content":{"rendered":"\n

The fluorine orbital diagram is a graphical representation of the electron configuration of the fluorine<\/a> atom.<\/p>\n\n\n\n

This diagram shows how the electrons in the fluorine atom are arranged in different orbitals. Orbital is the region of space around the nucleus of an atom where electrons are found.<\/p>\n\n\n\n

To write an orbital diagram of fluorine, you first need to know the atomic orbitals and the orbital notation for the fluorine atom, and also you need to know Hund\u2019s principle.<\/p>\n\n\n

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\"Fluorine
Fluorine atom<\/figcaption><\/figure><\/div>\n\n\n

What is orbital?<\/h2>\n\n\n\n

The\u00a0electrons of the atom<\/a>\u00a0revolve around the nucleus in a certain circular path. These circular paths are called orbits (shell). Again, atomic energy shells are subdivided into sub-energy levels. These sub-energy levels are also called orbital.<\/p>\n\n\n\n

The most probable region of electron rotation around the nucleus is called the orbital. The sub-energy levels depend on the azimuthal quantum number. It is expressed by \u2018l\u2019.<\/p>\n\n\n\n

Orbit Number<\/strong><\/td>Value of \u2018l\u2019<\/strong><\/td>Number of subshells<\/strong><\/td>Number of orbital<\/strong><\/td>Subshell name<\/strong><\/td>Electrons holding capacity<\/strong><\/td>Electron Configuration<\/strong><\/td><\/tr>
1<\/td>0<\/td>1<\/td>1<\/td>1s<\/td>2<\/td>1s2<\/sup><\/td><\/tr>
2<\/td>0
1<\/td>		2<\/td>1
3<\/td>		2s
2p<\/td>		2
6<\/td>		2s2<\/sup> 2p6<\/sup><\/td><\/tr>
3<\/td>0
1
2<\/td>		3<\/td>1
3
5<\/td>		3s
3p
3d<\/td>		2
6
10<\/td>		3s2<\/sup> 3p6<\/sup> 3d10<\/sup><\/td><\/tr>
4<\/td>0
1
2
3<\/td>		4<\/td>1
3
5
7<\/td>		4s
4p
4d
4f<\/td>		2
6
10
14<\/td>		4s2<\/sup> 4p6<\/sup> 4d10<\/sup> 4f14<\/sup><\/td><\/tr><\/tbody><\/table>
Orbital number of the subshell<\/figcaption><\/figure>\n\n\n\n

The value of \u2018l\u2019 is from 0 to (n \u2013 1). The sub-energy levels are known as s, p, d, and f. The orbital number of the s-subshell is one, three in the p-subshell, five in the d-subshell, and seven in the f-subshell. Each orbital can have a maximum of two electrons.<\/p>\n\n\n\n

Sub-shell name<\/strong><\/td>Name source<\/strong><\/td>Value of \u2018l\u2019<\/strong><\/td>Value of \u2018m\u2019
(0 to \u00b1 l)<\/strong><\/td>		Number of orbital (2l+1)<\/strong><\/td>Electrons holding capacity
2(2l+1)<\/strong><\/td><\/tr>
s<\/td>Sharp<\/td>0<\/td>0<\/td>1<\/td>2<\/td><\/tr>
p<\/td>Principal<\/td>1<\/td>\u22121, 0, +1<\/td>3<\/td>6<\/td><\/tr>
d<\/td>Diffuse<\/td>2<\/td>\u22122, \u22121, 0, +1, +2<\/td>5<\/td>10<\/td><\/tr>
f<\/td>Fundamental<\/td>3<\/td>\u22123, \u22122, \u22121, 0, +1, +2, +3<\/td>7<\/td>14<\/td><\/tr><\/tbody><\/table>
Number of electrons in the orbital<\/figcaption><\/figure>\n\n\n\n

The sub-energy level \u2018s\u2019 can hold a maximum of two electrons, \u2018p\u2019 can hold a maximum of six electrons, \u2018d\u2019 can hold a maximum of ten electrons, and \u2018f\u2019 can hold a maximum of fourteen electrons.<\/p>\n\n\n\n

What is the orbital notation for fluorine?<\/h2>\n\n\n\n

The fluorine orbital notation is a shorthand system designed to represent the exact positions of the electrons in the fluorine atom. This is similar to electron configuration<\/a>, but numbers are used instead of boxes to represent the positions of the electrons.<\/p>\n\n\n\n

This orbital notation system always follows the Aufbau principle. The Aufbau principle is that the electrons present in the atom will first complete the lowest energy orbital and then gradually continue to complete the higher energy orbital.<\/p>\n\n\n\n

\"Electron
Electron configuration via Aufbau principal<\/figcaption><\/figure>\n\n\n\n

The atomic number of fluorine<\/a> is 9, which means it has 9 electrons. Now it is possible to find the orbital notation of fluorine very easily through electron configuration. That is, the orbital notation of fluorine is 1s2<\/sup> 2s2<\/sup> 2p5<\/sup>.<\/p>\n\n\n\n

What is Hund\u2019s principle?<\/h2>\n\n\n\n

Hund\u2019s principle is a rule that helps to determine how electrons are distributed in orbitals when multiple orbitals of the same energy level are available.<\/p>\n\n\n\n

Hund\u2019s principle is that electrons in different orbitals with the same energy would be positioned in such a way that they could be in the unpaired state of maximum number and the spin of the unpaired electrons would be one-way.<\/p>\n\n\n\n

For example, we already know that the p-subshell has three orbitals. The orbitals are px<\/sub>, py<\/sub>, and pz<\/sub> and each orbital can have a maximum of two electrons.<\/p>\n\n\n\n

When electrons want to enter the p-subshell, then the first electron will enter the px<\/sub> orbital in the clockwise direction.<\/p>\n\n\n

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\"p-sub
p-sub shell with three electrons<\/figcaption><\/figure><\/div>\n\n\n

The second electron will also enter the py<\/sub> orbital in the clockwise direction and the third electron will also enter the pz<\/sub> orbital in the clockwise direction.<\/p>\n\n\n\n

Now, when the fourth electron wants to enter the p-subshell, then it will enter the px<\/sub> orbital in the anti-clockwise direction.<\/p>\n\n\n\n

The fifth electron will also enter the py<\/sub> orbital in the anti-clockwise direction and the sixth electron will also enter the pz<\/sub> orbital in the anti-clockwise direction.<\/p>\n\n\n

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\"p-sub
p-sub shell with six electrons<\/figcaption><\/figure><\/div>\n\n\n

Here, the clockwise direction is expressed by the upper sign (\u2191) and the anti-clockwise direction by the lower sign (\u2193). Basically, these two symbols (\u2191\u2193) indicate the direction of electron spin.<\/p>\n\n\n\n

How to write the orbital diagram for fluorine?<\/h2>\n\n\n\n

Orbital diagrams are usually represented by boxes. Each box represents an orbital and the arrows within the box represent the position of the electron. The boxes are arranged in order of energy of the orbitals.<\/p>\n\n\n\n

The lowest energy orbitals are closest to the nucleus and the higher energy orbitals are progressively further away from the nucleus in order of their energy levels.<\/p>\n\n\n\n

To draw the orbital diagram of fluorine, you have to write the orbital notation of fluorine. Which has been discussed in detail above.<\/p>\n\n\n

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\"Fluorine
Fluorine (F) orbital diagram<\/figcaption><\/figure><\/div>\n\n\n

1s is the closest and lowest energy orbital to the nucleus. Therefore, the electrons will first enter the 1s orbital.<\/p>\n\n\n\n

According to Hund\u2019s principle, the first electron will enter the 1s orbital in the clockwise direction and the remaining one electron will enter the 1s orbital in the anti-clockwise direction.<\/p>\n\n\n\n

The 1s orbital is now filled with two electrons. Then the next two electrons will enter the 2s orbital just like the 1s orbital. The 2s orbital is now full.<\/p>\n\n\n\n

So, the next three electrons will enter the 2p orbital in the clockwise direction and the remaining two electrons will enter the 2p orbital in the anti-clockwise direction. This is clearly shown in the figure of the orbital diagram of fluorine.<\/p>\n\n\n\n

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\"Orbital<\/a><\/figure><\/div>\n\n\n
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Try the Orbital Diagram Calculator and get instant results for any element.<\/a><\/p>\n<\/blockquote>\n<\/div><\/div>\n\n\n\n

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