Single bond - wikipedia Single bond This article has multiple issues. Please help improve it or discuss these issues on the talk page. ( Learn how and when to remove these template messages ) This article needs additional citations for verification. Please help improve this article by adding citations to reliable sources. Unsourced material may be challenged and removed. ( August 2012 ) This article is incomplete. Please help to improve it, or discuss the issue on the talk page. ( July 2012 ) Lewis structure for molecular hydrogen. Note depiction of the single bond. Lewis structure for methane. Note depiction of the four single bonds between the carbon and hydrogen atoms. Lewis structure for an alkane. Note that all the bonds are single covalent bonds. In chemistry, a single bond is a chemical bond between two atoms involving two valence electrons. That is, the atoms share one pair of electrons where the bond forms. Therefore, a single bond is a type of covalent bond. When shared, each of the two electrons involved is no longer in the sole possession of the orbital in which it originated. Rather, both of the two electrons spend time in either of the orbitals which overlap in the bonding process. As a Lewis structure, a single bond is denoted as AːA or A-A, for which A represents an element ( Moore, Stanitski, and Jurs 329 ). In the first rendition, each dot represents a shared electron, and in the second rendition, the bar represents both of the electrons shared in the single bond. A covalent bond can also be a double bond or a triple bond. A single bond is weaker than either a double bond or a triple bond. This difference in strength can be explained by examining the component bonds of which each of these types of covalent bonds consists ( Moore, Stanitski, and Jurs 393 ). Usually, a single bond is a sigma bond. An exception is the bond in diboron, which is a pi bond. In contrast, the double bond consists of one sigma bond and one pi bond, and a triple bond consists of one sigma bond and two pi bonds ( Moore, Stanitski, and Jurs 396 ). The number of component bonds is what determines the strength disparity. It stands to reason that the single bond is the weakest of the three because it consists of only a sigma bond, and the double bond or triple bond consist not only of this type of component bond but also at least one additional bond. The single bond has the capacity for rotation, a property not possessed by the double bond or the triple bond. The structure of pi bonds does not allow for rotation ( at least not at 298 K ), so the double bond and the triple bond which contain pi bonds are held due to this property. The sigma bond is not so restrictive, and the single bond is able to rotate using the sigma bond as the axis of rotation ( Moore, Stanitski, and Jurs 396 - 397 ). Another property comparison can be made in bond length. Single bonds are the longest of the three types of covalent bonds as interatomic attraction is greater in the two other types, double and triple. The increase in component bonds is the reason for this attraction increase as more electrons are shared between the bonded atoms ( Moore, Stanitski, and Jurs 343 ). Single bonds are often seen in diatomic molecules. Examples of this use of single bonds include H, F, and HCl. Single bonds are also seen in molecules made up of more than two atoms. Examples of this use of single bonds include : Both bonds in H O All 4 bonds in CH Single bonding even appears in molecules as complex as hydrocarbons larger than methane. The type of covalent bonding in hydrocarbons is extremely important in the nomenclature of these molecules. Hydrocarbons containing only single bonds are referred to as alkanes ( Moore, Stanitski, and Jurs 334 ). The names of specific molecules which belong to this group end with the suffix -- ane ' Examples include ethane, 2 - methylbutane, and cyclopentane ( Moore, Stanitski, and Jurs 335 ). References Jump up ^ `` covalent bonding - single bonds ''. Chemguide.co.uk. Retrieved 2012 - 08 - 12. Moore, John W., Conrad L. Stanitski, and Peter C. Jurs. Chemistry : The Molecular Science, Indiana University. Australia : Cengage Learning, 2012. Print. See also Bond order Chemical bonds Intramolecular ( strong ) Covalent By symmetry Sigma ( σ ) Pi ( π ) Delta ( δ ) Phi ( φ ) By multiplicity 1 ( single ) 2 ( double ) 3 ( triple ) 4 ( quadruple ) 5 ( quintuple ) 6 ( sextuple ) Miscellaneous Agostic Bent Coordinate ( dipolar ) Pi backbond Charge - shift Hapticity Conjugation Hyperconjugation Antibonding Resonant Electron deficiency 3c -- 2e 4c -- 2e Hypercoordination 3c -- 4e Aromaticity möbius super sigma homo spiro σ - bishomo spherical Y - Metallic Metal aromaticity Ionic Intermolecular ( weak ) van der Waals forces London dispersion Hydrogen Low - barrier Resonance - assisted Symmetric Dihydrogen bonds C -- H O interaction Noncovalent other Mechanical Halogen Aurophilicity Intercalation Stacking Cation -- pi Anion -- pi Salt bridge Retrieved from `` https://en.wikipedia.org/w/index.php?title=Single_bond&oldid=806434193 '' Categories : Chemical bonding Hidden categories : Articles needing additional references from August 2012 All articles needing additional references Articles to be expanded from July 2012 Talk About Wikipedia Bosanski Čeština Deutsch فارسی 한국어 Italiano Nederlands 日本 語 Српски / srpski Srpskohrvatski / српскохрватски தமிழ் 粵語 中文 Edit links This page was last edited on 22 October 2017, at 00 : 45. 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Question: which type of bond represents a single weak chemical bond
Answer: sigma bond