What kind of bond is 02

This is called a double bond. Each bond is a pair of electrons, one from each connected O atom. So the double bond, the two parallel lines, represents a total of 4 electrons. Each O is surrounded by four dots and two sticks or lines, representing another 4 electrons in the O 2 double bond.

So each O is surrounded by 8 total valence electrons, giving it an octet and making it stable. The nuclei contain the protons and neutrons, which are the solid parts of the molecule. Interestingly, the dots and lines represent electrons, which are not solid.

The diagram is drastically out of scale, as the relative size of the nucleus compared to the surrounding electrons is usually comparable to a pea in a stadium. The O 2 Lewis structure shows two oxygen atoms bonded in the same way to each other. If you have come straight to this page via a search engine follow this link before you go on.

A double covalent bond is where two pairs of electrons are shared between the atoms rather than just one pair. Two oxygen atoms can both achieve stable structures by sharing two pairs of electrons as in the diagram. The double bond is shown conventionally by two lines joining the atoms. Each line represents one pair of shared electrons. It is important to explore the bonding in ethene in more detail because it has a direct impact on its chemistry.

Unless you have some understanding of the true nature of the double bond, you can't really understand the way that ethene behaves. Ethene is built from hydrogen atoms 1s 1 and carbon atoms 1s 2 2s 2 2p x 1 2p y 1. The carbon atom doesn't have enough unpaired electrons to form the required number of bonds, so it needs to promote one of the 2s 2 pair into the empty 2p z orbital. This is exactly the same as happens whenever carbon forms bonds - whatever else it ends up joined to.

In the case of ethene, there is a difference from methane because each carbon is only joining to three other atoms rather than four. When the carbon atoms hybridise their outer orbitals before forming bonds, this time they only hybridise three of the orbitals rather than all four.

They use the 2s electron and two of the 2p electrons, but leave the other 2p electron unchanged. Note: You might wonder why it chooses to hybridise these three orbitals rather than just use the three p orbitals which already have the same energy.

It's because it uses the orbitals with the lowest energy first. The new orbitals formed are called sp 2 hybrids , because they are made by an s orbital and two p orbitals reorganising themselves.

The remaining p orbital is at right angles to them. The various atomic orbitals which are pointing towards each other now merge to give molecular orbitals, each containing a bonding pair of electrons.

Molecular orbitals made by end-to-end overlap of atomic orbitals are called sigma bonds. The p orbitals on each carbon aren't pointing towards each other, and so we'll leave those for a moment. In the diagram, the black dots represent the nuclei of the atoms. Each oxygen atom is two electrons short of a full outer shell, so each oxygen atom shares two of its electrons with the other atom, so both oxygen atoms have a full outer shell.

Lewis diagram of oxygen simplified 'dot and cross' electronic diagram for the covalently bonded oxygen molecule. Electronically , by sharing two electrons, both oxygen atoms attain a pseudo neon structure 2. On the left is the full 'dot and cross' electronic diagram for the covalent bonding in the oxygen molecule showing the inner non-valence electrons - omitted from the right diagram.

The colourless odourless gas that we can't live without!!! Website What next?