the combination of carbon and oxygen would result in what type of bond
covalent
title: Carbon–oxygen bond text: Carbon–oxygen bond A carbon–oxygen bond is a polar covalent bond between carbon and oxygen. Oxygen has 6 valence electrons and prefers to either share two electrons in bonding with carbon, leaving the 4 nonbonding electrons in 2 lone pairs :O: or to share two pairs of electrons to form the carbonyl functional group. =O: Simple representatives of these two bond types are the OH in alcohols such as the ethanol in beverages and fuels and the C=O in ketones (as well as many other related carbonyl compounds). The C–O bond is strongly polarized towards oxygen (electronegativity of C "vs" O, title: Carbon–oxygen bond text: have a very high bond energy, even higher than N–N triple bonds. Oxygen can also be trivalent, for example in triethyloxonium tetrafluoroborate. Carbon–oxygen bond forming reactions are the Williamson ether synthesis, nucleophilic acyl substitutions and electrophilic addition to alkenes. The Paternò–Büchi reaction involves carbonyl compounds. Carbon–oxygen bonds are present in these functional groups: Carbon–oxygen bond A carbon–oxygen bond is a polar covalent bond between carbon and oxygen. Oxygen has 6 valence electrons and prefers to either share two electrons in bonding with carbon, leaving the 4 nonbonding electrons in 2 lone pairs :O: or to share two pairs of electrons title: Carbon–oxygen bond text: 2.55 "vs" 3.44). Bond lengths for paraffinic C–O bonds are in the range of 143 pm – less than those of C–N or C–C bonds. Shortened single bonds are found with carboxylic acids (136 pm) due to partial double bond character and elongated bonds are found in epoxides (147 pm). The C–O bond strength is also larger than C–N or C–C. For example, bond strengths are /mol (at 298 K) in methanol, /mol in methylamine, and /mol in ethane. Carbon and oxygen form terminal double bonds in functional groups collectively known as carbonyl compounds to which belong such compounds as title: Double bond text: double bonds plumbenes and stannenes are similar in strength to hydrogen bonds. The Carter-Goddard-Malrieu-Trinquier model can be used to predict the nature of the bonding. Double bond A double bond in chemistry is a chemical bond between two chemical elements involving four bonding electrons instead of the usual two. The most common double bond, that is between two carbon atoms, can be found in alkenes. Many types of double bonds exist between two different elements. For example, in a carbonyl group with a carbon atom and an oxygen atom. Other common double bonds are found in azo compounds (N=N), imines title: Chemical bond text: two or more atoms share valence electrons more or less equally. The simplest and most common type is a single bond in which two atoms share two electrons. Other types include the double bond, the triple bond, one- and three-electron bonds, the three-center two-electron bond and three-center four-electron bond. In nonpolar covalent bonds, the electronegativity difference between the bonded atoms is small, typically 0 to 0.3. Bonds within most organic compounds are described as covalent. The figure shows methane (CH), in which each hydrogen forms a covalent bond with the carbon. See sigma bonds and pi bonds for LCAO-description of