Diatomic molecules form what kind of bonds

The shape of the molecule formed is called linear. This can also be shown as H-H. Carbon atoms have four outer electrons so need four more for a full outer shell. The carbon forms four single bonds to the hydrogen atoms, so all the atoms now have a full outer shell of electrons.

The shape formed is called tetrahedral. Nitrogen atoms have five outer electrons so needs three more for a full outer shell.

Nitrogen forms three single covalent bonds to hydrogen atoms. The shape formed is called trigonal pyramidal. Oxygen atoms have six outer electrons so need two more for a full outer shell. The oxygen forms two single covalent bonds with the two hydrogen atoms.

The shape formed is called angular. This structure contains one shared pair of electrons, which was created by pairing the unpaired electrons on each c h l o r i n e atom. As this electron pair is located in between both c h l o r i n e electron dot structures, these electrons contribute to the overall electron configuration of both atoms. By correctly executing the pairing process, each c h l o r i n e atom is surrounded by a total of eight, fully-paired dots. This information is visually-highlighted in the structure shown below using a blue circle around one chlorine atom and a green box around the other chlorine atom.

As an octet configuration is the most stable electron arrangement that can be achieved by an atom, this structure represents the most stable bonding arrangement that can be achieved by combining two chlorine atoms. The structure shown above, which is a chemically-correct representation of a covalent compound, is the Lewis structure that represents the molecule that is formed when two chlorine atoms bond with one another.

Because this molecule only contains two atoms of the same element, it is classified as a homonuclear diatomic molecule. For a covalent molecule, the information represented in its chemical formula must be a direct reflection of its Lewis structure. Elemental symbols are incorporated into a chemical formula by counting the number of times that each symbol appears in the corresponding Lewis structure.

In order to ensure consistent formatting, the elemental symbol that appears fewer times is written first in a covalent chemical formula, and subscripts are used to indicate how many times each elemental symbol appears in the Lewis structure.

As indicated previously, values of "1" are usually implicitly-understood in chemistry and, therefore, should not be written in a chemical formula. The subscripts must not be reduced to the lowest-common ratio of whole numbers, even if it is mathematically-possible to do so , as dividing the subscripts would cause their values to be inconsistent with the number of times that each elemental symbol appears in the Lewis structure.

The chemical formula of a heteronuclear diatomic molecule can be determined using a modified version of the rules presented above. For example, consider the Lewis structure shown below, which represents the covalent molecule that is formed when hydrogen and iodine bond with one another.

This Lewis structure contains one hydrogen atom and one iodine atom. As stated above, the elemental symbol that appears fewer times is typically written first in a covalent chemical formula. However, in the current example, the elements are present in equal quantities.

As a result, the order in which the elemental symbols are written in the corresponding chemical formula must be determined using a secondary rule: The elemental symbol for the element that is farther away from fluorine on the periodic table is written first. Therefore, the elemental symbol for hydrogen , " H ," is written before iodine's elemental symbol, " I. The resultant chemical formula, H I , accurately summarizes the information in the Lewis structure shown above and, therefore, is the chemically-correct formula for this covalent molecule.

The chemical formula of a homonuclear diatomic molecule can be determined using a modified version of the rules presented above. For example, consider the Lewis structure shown below, which represents the covalent molecule that is formed when two chlorine atoms bond with one another.

As only one type of element is present in this Lewis structure, only one elemental symbol, " Cl ," is written in the corresponding chemical formula. Furthermore, because this Lewis structure contains two chlorine atoms, a subscript of " 2 " should be written on c h l o r i n e ' s elemental symbol. The resultant chemical formula, Cl 2 , accurately summarizes the information in the Lewis structure shown above and, therefore, is the chemically-correct formula for this covalent molecule.

For a covalent molecule, the information represented in its chemical name must also be a direct reflection of its Lewis structure. Therefore, the chemical name of a covalent molecule must contain information that indicates the identities of its constituent elements and usually reflects how many of each of those elements are present within the molecule. Note that, if written properly, the chemical formula for a covalent molecule also contains this information and, therefore, can be used as the basis for developing a chemical name.

Elemental names are incorporated into a covalent molecule's chemical name in the order in which their corresponding elemental symbols appear in the chemical formula. Oct 20, It would be a non-polar covalent bond.

Explanation: The difference in electronegativity determines the bond type between atoms. Related questions What is the Lennard-Jones potential? Why do elements share electrons? Can carbon form 4 bonds? Something went wrong. Try again? Cited by. Download options Please wait Supplementary information PDF K. Article type Paper. Submitted 05 Feb Accepted 10 May First published 31 May Download Citation. RSC Adv.