CHEM 6A Lecture Notes - Lecture 7: Atomic Radius, Formal Charge, Bond Order

• School: UCSD
• Department: Chemistry and Biochemistry
• Course: CHEM 6A
• Professor: Thomas Bussey

Document Summary

When two nonmetal atoms come close to one another, there are: Attractive forces between each nucleus and the other atoms" electrons. Covalent bonds result from a balance of these attractions and repulsions. Always result in greater electron density between the two nuclei. Bond order is the number of electron pairs shared between two nuclei involved in a covalent bond. Single covalent bond: two atoms share a pair of electrons between them (2 shared electrons equal 1 bond) Double covalent bond: two atoms share 2 pairs of electrons. Triple bonds: two atoms share 3 pairs of electrons. Bond length is the distance between two covalently bonded nuclei. Triple bonds are shorter than double, which are shorter than single. Bond strength is the energy required to separate 2 nuclei. Triple bonds are stronger than double, which are stronger than single. When comparing similar bonds, bond length and atomic radius becomes a factor.