The hybridization state of carbon in: a CO3 2− C in CO3 2− is sp2-hybridized and is bound to three oxygen atoms.
A carbon atom is sp2 hybridized when bonding occurs between 1 s orbital and two p orbitals. Two single bonds and one double bond form between three atoms. The hybrid orbitals are arranged in a triangular array with 120° angles between the bonds. Example: hybridization of graphite. 3.
(c) Graphite? C in CO2–3 is sp2 hybridized and bound to three oxygen atoms. Each carbon atom in diamond is sp3 hybridized and bonded to four other carbon atoms. Each carbon atom in graphite is sp2 hybridized and bonded to three other carbon atoms.
Carbon sp2 hybridization. A carbon atom bonded to three atoms (two single bonds, one double bond) is sp2 hybridized, forming a flat trigonal or triangular arrangement with 120° angles between the bonds. Note that acetic acid contains one sp2 carbon atom and one sp3 carbon atom.
Sp3 hybridization. In sp3 hybridization, the carbon atom is bonded to four other atoms. In this case, 1 s orbital and 3 p orbitals combine in the same shell of an atom to form four new equivalent orbitals. The arrangement of the orbitals is tetrahedral with a bond angle of 109.5°.
3 that the molecular geometry of CO is 3 2− trigonal planar with bond angles of 120° .< /p>
Lewis structure of CO32– (carbonate) ion
In the carbonate ion there is < b> two oxygen atoms, each carrying -1 charge. One of these oxygen atoms accepts a proton (H+ ion) and forms an -OH group.
CCl4 has a tetrahedral arrangement of electron pairs around the carbon atom, which requires sp3 hybridization.