Molecule atoms have stable electrical attractions {bonding, molecule}| {chemical bond}.
electrons
Only outermost electrons participate in chemical bonds, because they can contact another atom.
electrons: stability
Atoms have potential energy. Bonding lowers potential energy. Because radius is less, filled outer-electron shells have lower potential energy than unfilled.
electrons: types
Bonding types result from competition between weak bonds with low activation energy and strong bonds with large activation energy. Single covalent bond overlaps sigma orbitals. Double covalent bond overlaps sigma orbitals and pi orbitals. Triple covalent bond overlaps sigma orbitals and two pi orbitals.
electrons: bond order
Bonding order is 1sigma bonding, 1sigma antibonding, 2sigma bonding, 2sigma antibonding, 2sigma bonding, 2pi bonding, 2pi antibonding, 2sigma antibonding, 3sigma bonding, 3sigma antibonding, 3sigma bonding, 3sigma antibonding, 3pi bonding, 3pi antibonding, and so on.
bond length
Bonded atom pairs always have same average distance between nuclei. Bond length has lowest potential energy.
bond strength
Non-polar covalent bonds are stronger than polar, ionic, or metallic bonds, because atoms share electrons more equally and attractive force between electrons and nuclei is higher, making bond length less. Multiple bonds have shorter bond lengths, because nucleus shielding is more.
Ionic bonds are stronger if ions have more charges and larger sizes.
Metal alloys make stronger metallic bonds, because rapid electron transfer maximizes shell filling.
bond angle
Average angle between two bonds is always the same.
Physical Sciences>Chemistry>Inorganic>Chemical Bond
5-Chemistry-Inorganic-Chemical Bond
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Date Modified: 2022.0224