Search results
Results From The WOW.Com Content Network
No description. Template parameters Parameter Description Type Status title title no description Unknown optional mark mark no description Unknown optional caption caption no description Unknown optional float float no description Unknown optional style style no description Unknown optional form form no description Unknown optional number number no description Unknown optional See also ...
Main page; Contents; Current events; Random article; About Wikipedia; Contact us; Donate; Help; Learn to edit; Community portal; Recent changes; Upload file
This is a documentation subpage for Template:Periodic table. It may contain usage information, categories and other content that is not part of the original template page. This periodic table is the prime form presented at this English wikipedia.
Fluorine is a chemical element; it has symbol F and atomic number 9. It is the lightest halogen [note 1] and exists at standard conditions as pale yellow diatomic gas. Fluorine is extremely reactive as it reacts with all other elements except for the light inert gases. It is highly toxic.
See {{Element-symbol-to-oxidation-state-data/doc}} for an overview. This list pulls data from {{Element-symbol-to-oxidation-state-data}} for each element then formats the result with {{Element-symbol-to-oxidation-state-row}}
Periodic table of the chemical elements showing the most or more commonly named sets of elements (in periodic tables), and a traditional dividing line between metals and nonmetals. The f-block actually fits between groups 2 and 3; it is usually shown at the foot of the table to save horizontal space.
Like the periodic table, the list below organizes the elements by the number of protons in their atoms; it can also be organized by other properties, such as atomic weight, density, and electronegativity. For more detailed information about the origins of element names, see List of chemical element name etymologies.
The fluorine–fluorine bond of the difluorine molecule is relatively weak when compared to the bonds of heavier dihalogen molecules. The bond energy is significantly weaker than those of Cl 2 or Br 2 molecules and similar to the easily cleaved oxygen–oxygen bonds of peroxides or nitrogen–nitrogen bonds of hydrazines. [8]