Two atoms can share two electrons {covalent bond}|, which spend most time between the atomic nuclei and share a bonding orbital. Molecular electron orbitals fill with electrons using same rules as for filling atomic electron orbitals. Bonding orbitals fill before antibonding orbitals. Covalent bonding fills both atoms' outer shells.
antibonding
Shared electrons can spend most time outside the atomic nuclei on line between nuclei, in antibonding orbitals. Outside electrons pull nuclei apart and so oppose covalent chemical bonding. Net bond number equals (bonding electrons - antibonding electrons) / 2.
factor
Atoms with weak electric forces make covalent bonds. Atoms with weak electric forces can gain electrons to complete shell. Atoms with weak electric forces can lose electrons to empty shell.
Two different-electronegativity atoms can bind by sharing electrons, and one atom attracts shared electrons more {polar bond}| {polar covalent bonding}.
Covalent chemical bonds {sigma bond}| {sigma bonding orbital} can overlap atom s orbital and other-atom 1s or 2s orbital, 1p or 2p orbital, or s-p hybrid orbital, with constructive interference and electrons between nuclei. Sigma bonding orbitals are symmetric around line joining the atomic nuclei. Atom s orbital can overlap other-atom 1s or 2s orbital, 1p or 2p orbital, or s-p hybrid orbital {sigma antibonding orbital}, with destructive interference and electrons not between nuclei.
Covalent chemical bonds {pi bond}| {pi bonding orbital} can overlap atom 2p orbitals, so shared electrons are between nuclei but in two regions, one above and one below line between atomic nuclei. Atom 2p orbital can overlap other-atom 2p orbital {pi antibonding orbital}, with destructive interference and electrons not between nuclei.
5-Chemistry-Inorganic-Chemical Bond-Kinds
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Date Modified: 2022.0225