key term - O2

Definition

O2, or dioxygen, is a diatomic molecule consisting of two oxygen atoms bonded together. This molecule is essential for life on Earth as it is a crucial component of cellular respiration, allowing organisms to produce energy. O2 also plays a significant role in various chemical processes, including combustion and oxidation reactions, making it a key substance in both biological and environmental systems.

5 Must Know Facts For Your Next Test

1. O2 has a double bond between its two oxygen atoms, which can be described using molecular orbital theory as a combination of two p-orbitals.
2. In molecular orbital theory, O2 has two unpaired electrons in its antibonding π* orbitals, making it paramagnetic and able to be attracted to magnetic fields.
3. The bond order of O2 is 2, indicating a stable bond between the oxygen atoms, which contributes to its relatively low reactivity compared to other diatomic molecules.
4. O2 is essential for aerobic respiration, as it serves as the final electron acceptor in the electron transport chain, leading to the production of ATP.
5. In addition to its role in respiration, O2 is involved in combustion reactions where it reacts with fuels to produce energy, carbon dioxide, and water.

Review Questions

• How does molecular orbital theory explain the magnetic properties of O2?
  • Molecular orbital theory explains the magnetic properties of O2 by showing that it has two unpaired electrons in its antibonding π* orbitals. This configuration results in O2 being paramagnetic, meaning it is attracted to magnetic fields. The presence of these unpaired electrons is significant because it distinguishes O2 from many other diatomic molecules that have all paired electrons and are therefore diamagnetic.
• Discuss how bond order impacts the stability of the O2 molecule.
  • The bond order of O2 is calculated as 2, indicating that there are two bonding pairs of electrons holding the two oxygen atoms together. A higher bond order typically correlates with greater stability, which means that O2 is more stable than other diatomic molecules with lower bond orders. The stability provided by this double bond allows O2 to exist in a gaseous state under standard conditions while still being reactive enough to participate in essential biological processes.
• Evaluate the importance of O2 in both biological systems and chemical reactions, providing specific examples.
  • O2 plays a vital role in biological systems by acting as the final electron acceptor in cellular respiration, enabling organisms to produce ATP for energy. Without O2, aerobic respiration would not occur efficiently, affecting all life forms dependent on it. In chemical reactions, O2 is crucial for combustion processes; for example, when hydrocarbons react with O2, they release energy used for heating or powering engines. These examples highlight how O2 connects life and energy production in both biological and chemical contexts.

Related terms

Molecular Orbital Theory:

A theory that describes the electronic structure of molecules by considering the combinations of atomic orbitals to form molecular orbitals.

Valence Electrons: Electrons located in the outermost shell of an atom that are involved in forming bonds with other atoms.

Bond Order: A concept that indicates the number of chemical bonds between a pair of atoms, calculated as half the difference between the number of bonding and antibonding electrons.