Fluorine Electron Configuration and Atomic Orbital Diagram

Fluorine is the ninth element in the periodic table and the symbol is ‘F’. The atomic number of fluorine is 9, which means that its atom has nine electrons around its nucleus. To write the electron configuration for fluorine, the first two electrons enter the 1s orbital. Since the 1s orbital can hold only two electrons the next two electrons enter the 2s orbital. The remaining five electrons enter the 2p subshell. Hence, the electron configuration of fluorine will be 1s² 2s² 2p⁵.

The electron configuration of fluorine refers to the arrangement of electrons in the fluorine atom’s orbitals. It describes how electrons are distributed among the various atomic orbitals and energy levels, and provides a detailed map of where each electron is likely to be found.

To understand the mechanism of fluorine electron configuration, you need to understand two basic things. These are orbits and orbitals. Also, you can arrange electrons in those two ways. In this article, I have discussed all the necessary points to understand the mechanism of fluorine electron configuration. I hope this will be helpful in your study.

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Electron arrangement for Fluorine through orbit

The atomic number is the number of electrons in that element. The atomic number of fluorine is 9. That is, the number of electrons in fluorine is 9. Therefore, a fluorine atom will have two electrons in the first shell and seven in the 2nd shell. Hence, the order of the number of electrons in each shell of the fluorine atom is 2, 7. Electrons can be arranged correctly through orbits from elements 1 to 18.

Electron configuration of fluorine through orbital

Atomic energy shells are subdivided into sub-energy levels. These sub-energy levels are also called orbital. 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 ‘l’. The value of ‘l’ is from 0 to (n – 1). The sub-energy levels are known as s, p, d, and f.

Orbit Number	Value of ‘l’	Number of subshells	Number of orbitals	Subshell name	Electrons holding capacity	Electron configuration
1	0	1	1	1s	2	1s2
2	0 1	2	1 3	2s 2p	2 6	2s2 2p6
3	0 1 2	3	1 3 5	3s 3p 3d	2 6 10	3s2 3p6 3d10
4	0 1 2 3	4	1 3 5 7	4s 4p 4d 4f	2 6 10 14	4s2 4p6 4d10 4f14

Explanation:

• If n = 1,
  (n – 1) = (1–1) = 0
  Therefore, the value of ‘l’ is 0. So, the sub-energy level is 1s.
• If n = 2,
  (n – 1) = (2–1) = 1.
  Therefore, the value of ‘l’ is 0, 1. So, the sub-energy levels are 2s, and 2p.
• If n = 3,
  (n – 1) = (3–1) = 2.
  Therefore, the value of ‘l’ is 0, 1, 2. So, the sub-energy levels are 3s, 3p, and 3d.
• If n = 4,
  (n – 1) = (4–1) = 3
  Therefore, the value of ‘l’ is 0, 1, 2, 3. So, the sub-energy levels are 4s, 4p, 4d, and 4f.
• If n = 5,
  (n – 1) = (n – 5) = 4.

Therefore, l = 0,1,2,3,4. The number of sub-shells will be 5 but 4s, 4p, 4d, and 4f in these four subshells it is possible to arrange the electrons of all the elements of the periodic table.

Sub-shell name	Name source	Value of ‘l’	Value of ‘m’ (0 to ± l)	Number of orbital (2l+1)	Electrons holding capacity 2(2l+1)
s	Sharp	0	0	1	2
p	Principal	1	−1, 0, +1	3	6
d	Diffuse	2	−2, −1, 0, +1, +2	5	10
f	Fundamental	3	−3, −2, −1, 0, +1, +2, +3	7	14

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.

The sub-energy level ‘s’ can hold a maximum of two electrons, ‘p’ can hold a maximum of six electrons, ‘d’ can hold a maximum of ten electrons, and ‘f’ can hold a maximum of fourteen electrons.

Aufbau is a German word, which means building up. The main proponents of this principle are scientists Niels Bohr and Pauli. The Aufbau method is to do electron configuration through the sub-energy level.

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.

The energy of an orbital is calculated from the value of the principal quantum number ‘n’ and the azimuthal quantum number ‘l’. The orbital for which the value of (n + l) is lower is the low energy orbital and the electron will enter that orbital first.

Orbital	Orbit (n)	Azimuthal quantum number (l)	Orbital energy (n + l)
3d	3	2	5
4s	4	0	4

Here, the energy of 4s orbital is less than that of 3d. So, the electron will enter the 4s orbital first and enter the 3d orbital when the 4s orbital is full. Following the Aufbau principle, the sequence of entry of electrons into orbitals is 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p.

Therefore, the complete electron configuration for fluorine should be written as 1s² 2s² 2p⁵.

Note: The unabbreviated electron configuration of fluorine is [He] 2s² 2p⁵. When writing an electron configuration, you have to write serially.

How to write the orbital diagram for fluorine?

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.

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. To draw the orbital diagram of fluorine, you have to write the orbital notation of fluorine. Which has been discussed in detail above.

1s is the closest and lowest energy orbital to the nucleus. Therefore, the electrons will first enter the 1s orbital. According to Hund’s 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.

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. 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.

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Electron configuration of fluorine in the excited state

Atoms can jump from one orbital to another orbital in the excited state. This is called a quantum jump. The ground-state electron configuration of fluorine is 1s² 2s² 2p⁵. We already know that the p-subshell has three orbitals. The orbitals are p_x, p_y, and p_z and each orbital can have a maximum of two electrons.

In the fluorine ground-state electron configuration, the five electrons of the 3p orbital are located in the p_x, p_y, and p_z orbitals. Then correct electron configuration of fluorine in the ground state will be 1s² 2s² 2p_x² 2p_y² 2p_z¹. This electron configuration shows that the last shell of the fluorine atom has an unpaired electron(2p_z¹). So the valency of fluorine is 1.

When fluorine atoms are excited, then fluorine atoms absorb energy. As a result, an electron in the 2p_y orbital jumps to the 3s orbital. Therefore, the electron configuration of fluorine(F*) in an excited state will be 1s² 2s² 2p_x² 2p_y¹ 2p_z¹ 3s¹.

Fluoride ion(F^–) electron configuration

After arranging the electrons, it is seen that the last shell of the fluorine atom has seven electrons. In this case, the valence electrons of fluorine are seven. The elements that have 5, 6, or 7 electrons in the last shell receive the electrons in the last shell during bond formation. The element that receives electrons and forms a bond is called anion.

During the formation of a bond, the last shell of fluorine receives an electron and turns into a fluoride ion(F^–). That is, fluorine is an anion element.

F + e^–  → F^–

The electron configuration of fluoride ion(F^–) is 1s² 2s² 2p⁶. This electron configuration shows that the fluoride ion(F^–) has acquired the electron configuration of neon and it achieves a stable electron configuration.

How to determine the group and period of fluorine through the electron configuration?

The last orbit of an element is the period of that element. The electron configuration of the fluorine atom shows that the last orbit of the fluorine atom is 2. So, the period of fluorine is 2.

On the other hand, the number of electrons present in the last orbit of an element is the number of groups in that element. But in the case of p-block elements, group diagnosis is different.

To determine the group of p-block elements, the group has to be determined by adding 10 to the total number of electrons in the last orbit. The total number of electrons in the last orbit of the fluorine atom is seven. That is, the group number of fluorine is 7 + 10 = 17. Therefore, we can say that the period of the fluorine element is 2 and the group is 17.

How to determine the block of fluorine through the electron configuration?

The elements in the periodic table are divided into four blocks based on the electron configuration of the element. The block of elements is determined based on the electron configuration of the element.

If the last electron enters the p-orbital after the electron configuration of the element, then that element is called the p-block element. The electron configuration of fluorine(F) shows that the last electron of fluorine enters the p-orbital. Therefore, fluorine is the p-block element.

Why fluorine is a halogen element?

The elements in group 17 of the periodic table are called halogen elements. One of the elements in group 17 of the periodic table is fluorine and the first element in group 17 is fluorine. Therefore, fluorine is a halogen element.

Bond formation of fluorine atom

Fluorine atoms form covalent bonds. Fluorine and hydrogen atoms form hydrogen fluoride(FH) compounds through covalent bonds by sharing electrons.

The electron configuration of hydrogen shows that the hydrogen atom has an electron. The hydrogen atom wants to complete its first orbit by receiving one more electron.

Again, the electron configuration of the fluorine atom shows that the last orbit of the fluorine atom has seven electrons. The fluorine atom wants to fill the octave by taking an electron in its last orbit.

Therefore, hydrogen and fluorine atoms share their electrons and fill the last orbit. Hydrogen and fluorine share electrons to form covalent bonds and produce hydrogen fluoride(HF) compounds.

The interhalogen reaction of chlorine

The compound formed by the reaction of two halogen elements at the required heat and pressure is called an interhalogen compound. The fluorine atom is a heavy halogen.

Fluorine atoms react with bromine(Br), chlorine(Cl), iodine(I) to form compounds BrF, ClF, ClF₃, BrF₃, BrF₅, IF₃, IF₅, IF₇. Of the halogen atoms, fluorine forms the most interhalogen compound.

• Cl₂ + F₂ (250°C) → 2ClF
• Cl₂ + 3F₂ (250°C) → 2ClF₃
• I₂ + 5F₂ → 2IF₅
• IF₅ + F₂ (270°C) → IF₇
• Br₂ + F₂ → 2BrF

Formation of the fluorine compound

Fluorine is a highly active and electrically negative element. It is a powerful oxidation element. Fluorine combines with various elements to form compounds.

Reaction of fluorine atom with group-1 element

Fluorine atoms react with hydrogen to form fluoride compounds.
H₂ + F₂ → 2HF
Here, HF is water soluble. In contact with water, the H – F bond is broken down into H⁺ ions. Which combines with water to produce H₃O⁺ ions.
HF + H₂O → H₃O⁺ + F^–

Again, fluorine atoms react with group-1 elements to form halide compounds. Group-1 elements are Lithium(Li), Sodium(Na), Potassium(K), Rubidium(Rb), Cesium(Cs).

• 2Li + F₂ → 2LiF
• 2Na + F₂ → 2NaF
• 2K + F₂ → 2KF
• 2Rb + F₂ → 2RbF
• 2Cs + F₂ → 2CsF

The reaction of the fluorine atom with the element of group 2

Group-2 elements are Beryllium(Be), Magnesium(Mg), Calcium(Ca), Strontium(Sr), Barium(Ba). Fluorine atoms react with group-2 elements to form compounds.

• Be + F₂ → BeF₂
• Mg + F₂ → MgF₂
• Ca + F₂ → CaF₂
• Sr + F₂ → SrF₂
• Ba + F₂ → BaF₂

The reaction of fluorine atom with the element of group-13

Fluorine forms halide compounds at high temperatures with 13-group elements. Group-13 elements are boron(B), aluminum(Al), gallium(Ga), indium(In), thallium(Tl).

• 2B + 3F₂ → 2BF₃
• 2Al + 3F₂ → 2AlF₃
• 2Ga + 3F₂ → 2GaF₃

Reaction of Fluorine Atoms with Group-15 Elements

Group-15 elements are nitrogen(N), phosphorus(P), arsenic(As), antimony(Sb), bismuth(Bi), and moscovium(Mc). Fluorine atoms react with Group-15 elements to form tetrachloride and pentachloride compounds.

• N₂ + 3F₂ → 2NF₃
• P₄ + F₂ → 4PF₃
• P₄ + 10F₂ → 4PF₅

The nitrogen atom alone does not form the Penta halide compound. Because nitrogen atoms do not have d-orbitals.

Reaction of fluorine atom with inert gas xenon(Xe )

In the presence of nickel, xenon, and fluorine in a 1:2 volume ratio are heated to 400 °C to produce xenon difluoride after a long time.
Xe + F₂ (Ni) → XeF₂

Again, xenon and fluorine gas are mixed in a 1: 2 volume ratio to produce xenon tetrafluoride at certain pressures and temperatures.
Xe + 2F → XeF₄

Properties of fluorine atom

• The atomic number of fluorine atoms is 9. The atomic number of an element is the number of electrons and protons in that element. That is, the number of electrons and protons in the fluorine atom is nine.
• The active atomic mass of the fluorine atom is 18.9984.
• Fluorine is a halogen element.
• The valency(valence) of a Fluorine atom is 1 and the valence electrons of a fluorine atom are seven.
• Fluorine atoms are the 2nd period of the periodic table and an element of the 17-group.
• Fluorine is an anion element.
• Fluorine atoms form covalent bonds.
• The electron configuration of fluorine ends in a p-orbital. Therefore, it is a p-block element.
• The melting point of a fluorine atom is 53.48 K ​(−219.67 °C, ​−363.41 °F) and the boiling point is 85.03 K ​(−188.11 °C, ​−306.60 °F).
• The value electronegativity of fluorine atoms is 3.98 (Pauling scale).
• The oxidation state of fluorine is –1.
• The atomic radius of a fluorine atom is 42pm.
• Fluorine atom van der Waals radius is 135 pm.
• The ionic radius of the fluorine atom is 136pm.
• Ionization energies of fluorine atoms are 1st: 1681 kJ/mol, 2nd: 3374 kJ/mol, 3rd: 6147 kJ/mol.
• The electron addiction of fluorine atoms is –329kj/mol.
• The covalent radius of the fluorine atom is 64 pm.
• Fluorine is thermally conductive and electricity is slightly conductive.
• Fluorine is a very active and electrically negative element.
• Fluorine is a p-block element. Therefore, the ionization energy is greater than the ionization energy of the s-block element.