The Chemistry of Carbon-Carbon Double Bonds: Ethene and Beyond

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Welcome to a fascinating journey into the world of organic chemistry! In this video, we're diving deep into the chemistry of carbon-carbon double bonds, focusing on the iconic molecule, ethene. But we won't stop there; we'll explore the broader implications of double bonds in organic compounds.

Carbon is the ultimate building block of organic chemistry, and understanding its bonding properties is crucial. From single bonds in methane to the double bonds in ethene, we'll uncover the secrets behind the spatial distribution of bonds in three dimensions.

Join us as we unravel the mysteries of carbon-carbon double bonds, discussing bond lengths, bond angles, and the planar arrangement of atoms in ethene. We'll also touch on the VSEPR theory, a key concept in understanding molecular geometry.

Whether you're a chemistry enthusiast or a student looking to ace your organic chemistry class, this video will provide valuable insights into the chemistry of carbon compounds. Get ready to expand your knowledge and appreciation of the chemical world.

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In organic compounds carbon atoms almost always form four bonds. This suggests that the carbon atom’s four valence electrons are all involved in bonding. An examination of simple carbon-base molecules like methane (CH4) and carbon tetrachloride (CCl4) indicates that in these compounds the carbon atom forms four identical single covalent bonds and that the angles between the bonds are 109.5 degrees. It can be predicted from the valence shell electron pair is required to minimise the electrostatic repulsion between them.

The central role of carbon in organic chemistry depends on the fact carbon atoms can form chains of virtually unlimited length containing a succession of carbon-carbons bonds. The valence electrons not involved in forming carbon-carbon bonds are used in forming bonds with atoms of other elements such as hydrogen, oxygen, nitrogen and halogens. The properties of carbon that allow it to form a huge number and variety of compounds include:
• four outer shell valence electrons
• can form single, double and triple bonds
• can form chains and rings, which can be branched or unbranched
• can share electrons with other non-metals

Carbon atoms can bond to one another by single, double or triple covalent bonds.
Lewis electron-dot diagrams do not show the spatial distribution of bonds in three dimensions.

Carbon-carbon single bonds
Single covalent bonds around a carbon atom are arranged tetrahedrally (bond angle=109.28 ). Methane is a good example of this arrangement of carbon-hydrogen single bonds.
The two simplest molecules containing carbon-carbon single bonds are ethane (CH3CH3) and propane (CH 3CH2CH3). In these compounds each carbon atom forms four single bonds which again have a tetrahedral orientation. In the case of CH3CH3 three of the bonds formed by the carbon atoms are C-H bonds, while the other bond is a C-C bond. The length of the single C-C bond in these compounds has been found to be 0.154 nm.

Carbon-carbon double bonds
The compound ethene (CH2CH2) is the simplest carbon compound containing a C=C double bond. In this case only two of each carbon atom's four valence electrons are used in bonding with hydrogen atoms. Hence each carbon atom shares two pairs of electrons with another carbon atom. These two pairs of electrons constitute a double bond.

The presence of one double covalent bond forces the bonding electrons into a planar arrangement (bond angle=120 ), so the structure of ethane (ethylene) is planar.

An examination of compounds such as ethene (CH2CH2 ) indicates that the C=C bond length is 0.134 nm, the bond angles are 120°, and the geometric arrangement of the two carbon atoms and adjoining hydrogen atoms is planar. This again can be explained in terms of the VSEPR theory. In using the VSEPR theory the C=C double bond is viewed as a single region of charge. To minimise electron repulsion the three electron regions around each carbon atom adopt a planar orientation with bond angles of 120°.