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Double bonds have more electrons that are strongly attracted to the nuclei of the atoms that are bonding, so they pull the atoms closer, which means that the length of the bond between the two atoms is shorter. In single bonds, fewer electrons are shared between two atoms, so there is less attraction to the nuclei of the bonding atoms, and the atoms are not pulled as closely together.
Double bonds (4 e) have more electrons than single bonds (2 e), and have a stronger negative charge, atrracting the nuclei of the bonding atoms that are charged positively. The attraction is stronger, thus the half distance between centers of the bonding atoms is shorter.
Double bonds have a higher number of electrons than single bonds, therefore being pulled closer to the nucleus of the atom. The nucleus of the atom is positively charged while the electrons are negative, opposites attract :)
Double bonds are shorter than single bonds because they contain more electrons. When an anion contains a large amount of electrons, that means that it can be more easily pulled into a cation. When the two are easily pulled into each other, that results in a shorter bond length.
It's because single bonds share fewer electrons between two atoms so the attraction between the electrons and the nucleus is less than a double or triple bond because they have more electrons, thereby making the bond length shorter.
Due to the weaker connection of having 2 electrons in a single compared compared to a double bond with 4 electrons, the double bond is shorter because there are more protons in the double bond compared to the single bond.
I think this is a good idea to think about. So the difference between the double bond and single bonds is the number of electrons in the bond. 2 for single and 4 for double bonds. Therefore, with more electrons, there is a greater force of attraction to the atom center. Hence, the length of the bond forces them to come to be pulled in making a bond with a shorter length.
Double bonds have a greater interaction between electrons than single bonds. If you think about it in the electron cloud model, more of the electron clouds would have to overlap in odder to form a double bond when compared to a single bond. This increased overlap can be seen as the nuclei getting closer and the bond length decreasing.
Double bonds are shorter considering that they are stronger bonds since the distance between the nuclei of two atoms is smaller. Single bonds are weaker than double bonds, considering the distance between their nuclei is larger. It takes more energy to break apart double bonds compared to single bonds.
Double bonds are shorter than single bonds because double bonds are stronger and have 2 pairs of electrons that pull the positive nucleus closer together and result in a shorter bond length. On the other hand, single bonds only share 1 pair of electrons that do not pull the positive nucleus as close together, which is why they have a longer bond length.
Bethany Yang 2D wrote:Can someone explain in simple terms why double bonds are shorter than single bonds?
Double bonds are shorter than single bonds because together, they are stronger and can pull the two atoms closer together. Because the atoms are closer together resulting in the increased strength of the double bond vs the single bond, the distance (ie. bond length) between the two atoms will shorter.
Hope this helps!
Double bonds are shorter than single bonds because they are stronger. They are able to pull in electrons from the other atom better, which shrinks the size of the bond that holds the two atoms together.
There are more electrons shared between atoms in a double bond. Therefore, the attractive forces between atoms with double bonds are stronger, thus pulling them in closer. Atoms that share a single bond have smaller attractive forces in comparison, and are usually longer.
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