Fluorine Atomic Number



Element Fluorine - F

Comprehensive data on the chemical element Fluorine is provided on this page; including scores of properties, element names in many languages, most known nuclides of Fluorine. Common chemical compounds are also provided for many elements. In addition technical terms are linked to their definitions and the menu contains links to related articles that are a great aid in one's studies.

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Overview of Fluorine

Fluorine atoms have 9 electrons and the shell structure is 2.7. The ground state electron configuration of ground state gaseous neutral fluorine is He. 2p5 and the term symbol is 2P3/2. Click to see full answer Regarding this, what are the quantum numbers for fluorine? Name: Fluorine Symbol: F Atomic Number: 9 Atomic Mass: 18.998404 amu Melting Point:-219.62 °C (53.530006 K, -363.31598 °F) Boiling Point:-188.14 °C (85.01 K, -306.652 °F) Number of Protons/Electrons: 9 Number of Neutrons: 10 Classification: Halogen Crystal Structure: Cubic Density @ 293 K: 1.696 g/cm 3 Color: Greenish Atomic Structure.

  • Atomic Number: 9
  • Group: 17
  • Period: 2
  • Series: Halogens

Fluorine's Name in Other Languages

  • Latin: Fluorum
  • Czech: Fluor
  • Croatian: Fluor
  • French: Fluor
  • German: Fluor - r
  • Italian: Fluoro
  • Norwegian: Fluor
  • Portuguese: Flúor
  • Russian: Фтор
  • Spanish: Flúor
  • Swedish: Fluor

Atomic Structure of Fluorine

  • Atomic Radius: 0.57Å
  • Atomic Volume: 17.1cm3/mol
  • Covalent Radius: 0.72Å
  • Cross Section (Thermal Neutron Capture)σa/barns: 0.0096
  • Crystal Structure: Cubic
  • Electron Configuration:
    1s2 2s2p5
  • Electrons per Energy Level: 2,7
    Shell Model
  • Ionic Radius: 1.33Å
  • Filling Orbital: 2p5
  • Number of Electrons (with no charge): 9
  • Number of Neutrons (most common/stable nuclide): 10
  • Number of Protons: 9
  • Oxidation States: -1
  • Valence Electrons: 2s2p5
    Electron Dot Model

Chemical Properties of Fluorine

  • Electrochemical Equivalent: 0.70883g/amp-hr
  • Electron Work Function:
  • Electronegativity: 3.98 (Pauling); 4.1 (Allrod Rochow)
  • Heat of Fusion: 0.2552kJ/mol
  • Incompatibilities:
    Water, nitric acid, oxidizers, organic compounds
  • Ionization Potential
    • First: 17.422
    • Second: 34.97
    • Third: 62.707
  • Valence Electron Potential (-eV): -10.1

Physical Properties of Fluorine

  • Atomic Mass Average: 18.9984
  • Boiling Point: 85.1K -188.05°C -306.49°F
  • Coefficient of lineal thermal expansion/K-1: N/A
  • Conductivity
    Electrical:
    Thermal: 0.000279 W/cmK
  • Density: 1.696g/L @ 273K & 1atm
  • Description:
    Greenish-yellow gas of the Halogen family
  • Enthalpy of Atomization: 79.08 kJ/mole @ 25°C
  • Enthalpy of Fusion: 0.26 kJ/mole
  • Enthalpy of Vaporization: 3.31 kJ/mole
  • Flammablity Class: Non-flammable gas (extreme oxidizer)
  • Freezing Point:see melting point
  • Heat of Vaporization: 3.2698kJ/mol
  • Melting Point: 53.63K -219.52°C -363.14°F
  • Molar Volume: 17.1 cm3/mole
  • Optical Refractive Index: 1.000195
  • Physical State (at 20°C & 1atm): Gas
  • Realitive Gas Density (Air=1) = 1.31
  • Specific Heat: 0.82J/gK

Regulatory / Health

  • CAS Number
    • 7782-41-4 cryogenic liquid
  • UN/NA ID and ERG Guide Number
    • 1045 / 124 compressed
    • 9192 / 167 cryogenic liquid
  • RTECS: LM6475000
  • NFPA 704
    • Health:
    • Fire:
    • Reactivity:
    • Special Hazard: OxidizerOSHAPermissible Exposure Limit (PEL)
      • 1 ppm = 1.55mg/m3 @ 25°C & 1 atm
      • TWA: 0.1 ppm
    • OSHA PEL Vacated 1989
      • TWA: 0.1 ppm
    • NIOSHRecommended Exposure Limit (REL)
      • TWA: 0.1 ppm
      • IDLH: 25 ppm
    • Routes of Exposure: Inhalation; Skin and/or eye contact
    • Target Organs: Eyes, skin, respiratory system, liver, kidneys
    • Levels In Humans:
      Note: this data represents naturally occuring levels of elements in the typical human, it DOES NOT represent recommended daily allowances.
      • Blood/mg dm-3: 0.5
      • Bone/p.p.m: 2000-12,000
      • Liver/p.p.m: 0.22-7
      • Muscle/p.p.m: 0.05
      • Daily Dietary Intake: 0.3-0.5 mg
      • Total Mass In Avg. 70kg human: 2.6 g

    Who / Where / When / How

    • Discoverer: Henri Moissan
    • Discovery Location: Paris France
    • Discovery Year: 1886
    • Name Origin:
      Latin: fluo (flow).
    • Abundance of Fluorine:
      • Earth's Crust/p.p.m.: 950
      • Seawater/p.p.m.:
        • Atlantic Suface: 0.0001
        • Atlantic Deep: 0.000096
        • Pacific Surface: 0.0001
        • Pacific Deep: 0.00004
      • Atmosphere/p.p.m.: N/A
      • Sun (Relative to H=1E12): 0.000363
    • Sources of Fluorine:
      Found in the minerals fluorite (CaF2) and cryolite (Na2AlF6). Around 2,400 tons of fluorine gas and 4,700,000 tons of fluorite are produced each year. Primary mining areas are Canada, USA, UK, Russia, Mexico and Italy.
    • Uses of Fluorine:
      Combines more readily than any other element. Used in refrigerants and other chloro fluorocarbons. Also in toothpaste as sodium fluoride (NaF) and stannous fluoride (SnF2); also in Teflon.
    • Additional Notes:
      Fluorine gas is highly toxic and corrosive. Even exposure to low concentrations causes lung and eye irritation. Metal fluorides are also very toxic while organic fluorides are often quite harmless.

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    References

    A list of reference sources used to compile the data provided on our periodic table of elements can be found on the main periodic table page.

    Related Resources

    • Anatomy of the Atom
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    • Molarity, Molality and Normality
      Introduces stoichiometry and explains the differences between molarity, molality and normality.
    • Molar Mass Calculations and Javascript Calculator
      Molar mass calculations are explained and there is a JavaScript calculator to aid calculations.
    • Chemical Database
      This database focuses on the most common chemical compounds used in the home and industry.

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Fluorine (F) is the first element in the Halogen group (group 17) in the periodic table. Its atomic number is 9 and its atomic weight is 19, and it's a gas at room temperature. It is the most electronegative element, given that it is the top element in the Halogen Group, and therefore is very reactive. It is a nonmetal, and is one of the few elements that can form diatomic molecules (F2). It has 5 valence electrons in the 2p level. Its electron configuration is 1s22s22p5. It will usually form the anion F- since it is extremely electronegative and a strong oxidizing agent. Fluorine is a Lewis acid in weak acid, which means that it accepts electrons when reacting. Fluorine has many isotopes, but the only stable one found in nature is F-19.

Quick Reference Table

SymbolF
Atomic Number9
Group17 (Halogens)
Electron Configuration1s22s22p5
Atomic Weight18.998 g
Density1.7 g/L
Melting Point-219.62oC
Boiling Point-188.12oC
Critical Point144.13K, 5.172 MPa
Oxidation States-1
Electronegativity3.98
Stable IsotopesF-19

Brief History

In the late 1600's minerals which we now know contain fluorine were used in etching glass. The discovery of the element was prompted by the search for the chemical substance which was able to attack glass (it is HF, a weak acid). The early history of the isolation and work with fluorine and hydrogen fluoride is filled with accidents since both are extremely dangerous. Eventually, electrolysis of a mixture of KF and HF (carefully ensuring that the resulting hydrogen and fluorine would not come in contact) in a platinum apparatus yielded the element.

Fluorine was discovered in 1530 by Georgius Agricola. He originally found it in the compound Fluorspar, which was used to promote the fusion of metals. It was under this application until 1670, when Schwanhard discovered its usefulness in etching glass. Pure fluorine (from the Latin fluere, for 'flow') was was not isolated until 1886 by Henri Moissan, burning and even killing many scientists along the way. It has many uses today, a particular one being used in the Manhattan project to help create the first nuclear bomb.

Electronegativity of Fluorine

Fluorine is the most electronegative element on the periodic table, which means that it is a very strong oxidizing agent and accepts other elements' electrons. Fluorine's atomic electron configuration is 1s22s22p5. (see Figure 2)

Fluorine is the most electronegative element because it has 5 electrons in it's 2P shell. The optimal electron configuration of the 2P orbital contains 6 electrons, so since Fluorine is so close to ideal electron configuration, the electrons are held very tightly to the nucleus. The high electronegativity of fluorine explains its small radius because the positive protons have a very strong attraction to the negative electrons, holding them closer to the nucleus than the bigger and less electronegative elements.

Reactions of Fluorine

Because of its reactivity, elemental fluorine is never found in nature and no other chemical element can displace fluorine from its compounds. Fluorine bonds with almost any element, both metals and nonmetals, because it is a very strong oxidizing agent. It is very unstable and reactive since it is so close to its ideal electron configuration. It forms covalent bonds with nonmetals, and since it is the most electronegative element, is always going to be the element that is reduced. It can also form a diatomic element with itself ((F_2)), or covalent bonds where it oxidizes other halogens ((ClF), (ClF_3), (ClF_5)). It will react explosively with many elements and compounds such as Hydrogen and water. Elemental Fluorine is slightly basic, which means that when it reacts with water it forms (OH^-).

[3F_2+2H_2O rightarrow O_2+4HF tag{1}]

When combined with Hydrogen, Fluorine forms Hydrofluoric acid ((HF)), which is a weak acid. This acid is very dangerous and when dissociated can cause severe damage to the body because while it may not be painful initially, it passes through tissues quickly and can cause deep burns that interfere with nerve function.

[HF+H_2O rightarrow H_3O^++F^- tag{2}]

There are also some organic compounds made of Fluorine, ranging from nontoxic to highly toxic. Fluorine forms covalent bonds with Carbon, which sometimes form into stable aromatic rings. When Carbon reacts with Fluorine the reaction is complex and forms a mixture of (CF_4), (C_2F_6), an (C_5F_{12}).

[C_{(s)} + F_{2(g)} rightarrow CF_{4(g)} + C_2F_6 + C_5F_{12} tag{3}]

Fluorine reacts with Oxygen to form (OF_2) because Fluorine is more electronegative than Oxygen. The reaction goes:

[2F_2 + O_2 rightarrow 2OF_2 tag{4}]

Fluorine is so electronegative that sometimes it will even form molecules with noble gases like Xenon, such as the the molecule Xenon Difluoride, (XeF_2).

[Xe + F_2 rightarrow XeF_2 tag{5}]

Fluorine also forms strong ionic compounds with metals. Some common ionic reactions of Fluorine are:

[F_2 + 2NaOH rightarrow O_2 + 2NaF +H_2 tag{6}]

[4F_2 + HCl + H_2O rightarrow 3HF + OF_2 + ClF_3 tag{7}]

[F_2 + 2HNO_3 rightarrow 2NO_3F + H_2 tag{8}]

Fluorine atomic number

Applications of Fluorine

Compounds of fluorine are present in fluoridated toothpaste and in many municipal water systems where they help to prevent tooth decay. And, of course, fluorocarbons such as Teflon have made a major impact on life in the 20th century. There are many applications of fluorine:

  • Rocket fuels
  • Polymer and plastics production
  • teflon and tefzel production
  • When combined with Oxygen, used as a refrigerator cooler
  • Hydrofluoric acid used for glass etching
  • Purify public water supplies
  • Uranium production
  • Air conditioning

Sources

Fluorine can either be found in nature or produced in a lab. To make it in a lab, compounds like Potassium Fluoride are put through electrolysis with Hydrofluoric acid to create pure Fluorine and other compounds. It can be carried out with a variety of compounds, usually ionic ones involving Fluorine and a metal. Fluorine can also be found in nature in various minerals and compounds. The two main compounds it can be found in are Fluorspar ((CaF_2)) and Cryolite ((Na_3AlF_6)).

References

  1. Newth, G. S. Inorganic Chemistry. Longmans, Green, and Co.:New York, 1903.
  2. Latimer, Wendell M., Hildebrand, Joel H. Reference Book of Inorganic Chemistry. The Macmillan Company: New York, 1938.

Fluorine On Periodic Table

Problems

(Highlight to view answers)

1. Q. What is the electron configuration of Fluorine? of F-?

A. 1s22s22p5

1s22s22p6

2. Q. Is Fluorine usually oxidized or reduced? explain.

A. Fluorine is usually reduced because it accepts an electron from other elements since it is so electronegative.

3. Q. What are some common uses of Fluorine?

A. Toothpaste, plastics, rocket fuels, glass etching, etc.

4. Q. Does Fluorine form compounds with nonmetals? if so, give two examples, one of them being of an oxide.

A. OF2, ClF

5. Q. What group is Fluorine in? (include name of group and number)

Fluorine Atomic Number 19

A. 17, Halogens

Contributors and Attributions

  • Rachel Feldman (University of California, Davis)

  • Stephen R. Marsden