QQuestionChemistry
QuestionChemistry
What is the molecular orbital configuration of B^+ 2?
A. [core electrons] (σ2s)2(σ2s*)1
B. [core electrons] (σ2s)2(σ2s*)2(π2p)1
C. [core electrons] (σ2s)2(σ2s*)2(π2p)2
D. [core electrons] (σ2s)²(σ2s)²(π2p)²(σ2p)0 *
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Answer
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Step 1:: Determine the number of electrons in a B+ 2 ion
The atomic number of Boron (B) is 5, which means it has 5 electrons. Since we are considering B+ 2, we have to remove 2 electrons from a neutral Boron atom. So, B+ 2 has 3 electrons.
Step 2:: Write the core electrons configuration
Boron is in the 3rd period of the periodic table, so its core electrons configuration is [He] 2s² 2p⁰, where [He] represents the Helium noble gas core configuration (1s²).
Step 3:: Consider the promotion of an electron
To form molecular orbitals, we need to promote one of the 2s² electrons to the 2p orbital. The promotion energy is compensated by the stabilization of the molecule. The promoted configuration is [He] (σ2s)¹ (σ2s*)¹ (2p⁰).
Step 4:: Calculate the total number of electrons in molecular orbitals
Now, we have to add the remaining electrons from B+ 2 to the promoted configuration. Since B+ 2 has 3 electrons, and the promoted configuration has 2 electrons, the total number of electrons in molecular orbitals is 3 + 2 = 5 electrons.
Step 5:: Assign the electrons to the molecular orbitals
Final Answer
: Assign the electrons to the molecular orbitals
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