2012年6月5日 · $\ce{C2}$ and its isoelectronic molecules $\ce{CN+}$, BN and $\ce{CB-}$ (each having eight valence electrons) are bound by a quadruple bond. The bonding comprises not only one σ- and two π-bonds, but also one weak ‘inverted’ bond, which can be characterized by the interaction of electrons in two outwardly pointing sp hybrid orbitals.

2015年8月13日 · s orbitals have spherical symmetry, and p orbitals have a dumb-bell shape. When these orbitals overlap, then they form the bonding orbitals (and corresponding antibonding orbitals). The p-orbitals are aligned along Cartesian (xyz) axes. If all three p-orbitals overlap, then the s-orbitals can't get 'close enough' to overlap and form a fourth bond.

2018年6月24日 · I calculated that the bond orders of $\ce{C_2}^+$, $\ce{C_2}$, and $\ce{C_2}^-$ are 1.5, 2, and 2.5, respectively. Why doesn't $\ce{C_2}^-$ have a higher ionization than the other two molecules? Shouldn't the molecule with the larger bond order have the larger ionization energy, because it would be more difficult to remove an electron from the ...

This is in contrast to the center resonance structure, which has two aromatic rings and is more stable, thus giving the bonds between carbons 1-2; 3-4; 5-6; 7-8; and 9-10 more double bond character than the other bonds and making them shorter.

2020年2月11日 · I have seen some books indicated sigma bond has C2 symmetry. I understand pi and delta bond change their signs about C2 and C4 rotation about bond axis, but I don't understand why sigma bond has C2 symmetry not C∞ about its bond axis. The example of the sigma bond came from two 1s orbitals.

2017年3月20日 · Due to a number of constraints that you will learn about soon enough™, a carbon–carbon triple bond $\ce{C#C}$ will consist of one σ bond and two π bonds as shown in the image below. Figure 1: $\ce{H-C#C-H}$ showing the σ and π orbitals required to make the respective bonds. Image taken from jahschem.wikispaces.org.

2015年12月6日 · C2+ or C2- bond strength Post by Anne Cam 3A » Sat Dec 05, 2015 3:24 am Question 4, part A of the 2010 final asks whether C 2 + or C 2 - has the stronger bond, and I determined C 2 + to be stronger since it has the higher bond order.

2017年11月12日 · We do indeed have a calcium cation $\ce{Ca^2+}$. The counterion is a diatomic anion, the ethynediide anion $\ce{C2^2-}$. It consists of two carbon atoms connected by a triple bond with each carbon atom carrying an additional lone pair and thus formal negative charge for an overall charge of $2-$. The bond between the two carbon atoms is covalent.

2018年12月4日 · I was looking at an old final and saw a question about the C2+ bond and the C2- bond. What would the lewis structures of C2+ and C2- look like? and which has a stronger bond?

2015年12月22日 · You can draw hyperconjugation structures to compare bond length. The more α-hydrogens the alkene has, the more hyperconjugation structures it has, and the higher is the degree of delocalization of the π-bond and therefore the longer is the bond. When double bond character decreases, bond length increases. Therefore the answer should be (d).