- Identify the four orbital types used in covalent bond formation
- Covalent bonds occur when electrons are shared between two atoms. A single covalent bond is when only one pair of electrons is shared between atoms.
- A sigma bond is the strongest type of covalent bond, in which the atomic orbitals directly overlap between the nuclei of two atoms.
- Sigma bonds can occur between any kind of atomic orbitals; the only requirement is that the atomic orbital overlap happens directly between the nuclei of atoms.
- atomic orbitalA region in space around the atom’s nucleus where there is a probability of finding an electron.
- covalent bondA type of chemical bond where two atoms are connected to each other by the sharing of two or more electrons.
- sigma bondA covalent bond whose electron density is concentrated in the region directly between the nuclei.
Hierarchical Structure of the Atom
There are four hierarchical levels that describe the position and energy of the electrons an atom has. Here they are listed along with some of the possible values (or letters) they can have:
- Principal energy levels (1, 2, 3, etc.)
- Sublevels (s, p, d, f)
Principal energy levels are made out of sublevels, which are in turn made out of orbitals, in which electrons are found.
An atomic orbital is defined as the probability of finding an electron in an area around an atom’s nucleus. Generally, orbital shapes are drawn to describe the region in space in which electrons are likely to be found. This is referred to as “electron density.”
Covalent bonding occurs when two atomic orbitals come together in close proximity and their electron densities overlap. The strongest type of covalent bonds are sigma bonds, which are formed by the direct overlap of orbitals from each of the two bonded atoms. Regardless of the atomic orbital type, sigma bonds can occur as long as the orbitals directly overlap between the nuclei of the atoms.
Single covalent bonds occur when one pair of electrons is shared between atoms as part of a molecule or compound. A single covalent bond can be represented by a single line between the two atoms. For instance, the diatomic hydrogen molecule, H2, can be written as H—H to indicate the single covalent bond between the two hydrogen atoms.
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