(c) Calculate the bond order in H2-.

검증된 단계별 안내

Identify the molecular orbitals involved in the bonding of the hydrogen molecule ion \( \text{H}_2^- \).

Determine the total number of electrons in \( \text{H}_2^- \). Since each hydrogen atom contributes one electron and there is an additional electron due to the negative charge, there are 3 electrons in total.

Fill the molecular orbitals with the electrons, starting with the lowest energy level. The order is: \( \sigma_{1s} \) and \( \sigma^*_{1s} \).

Calculate the bond order using the formula: \( \text{Bond Order} = \frac{1}{2} (\text{Number of bonding electrons} - \text{Number of antibonding electrons}) \).

Determine the number of electrons in bonding and antibonding orbitals, and apply them to the bond order formula to find the bond order of \( \text{H}_2^- \).

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Bond Order

Bond order is a measure of the number of chemical bonds between a pair of atoms. It is calculated as the difference between the number of bonding electrons and the number of antibonding electrons, divided by two. A higher bond order indicates a stronger bond and greater stability of the molecule.

Molecular Orbital Theory

Molecular Orbital Theory describes the behavior of electrons in molecules using molecular orbitals, which are formed by the combination of atomic orbitals. In this theory, electrons occupy these orbitals, which can be bonding or antibonding. Understanding how these orbitals are filled is crucial for determining bond order and the stability of the molecule.

Electron Configuration of H2-

H2- is a molecular ion consisting of two hydrogen atoms and an extra electron, resulting in a total of three electrons. The electron configuration for H2- involves filling the bonding molecular orbital (σ1s) with two electrons and the antibonding molecular orbital (σ*1s) with one electron. This configuration is essential for calculating the bond order and understanding the stability of the ion.