If you maximize the unshared electrons in the boron atom, the electron configuration is?

i know the electron configuration at ground state is 1S2 2S2 2P1

but when it maximizes unshared electrons i don't understand how it affects the configuration

I think the question means that B will have 1s2 2s1 2p2 and that's how you get BF3, BH3, etc but I must confess the wording is confusing.

When we talk about maximizing unshared electrons in the boron atom, we are referring to its ability to form compounds by sharing its valence electrons with other atoms. The valence electrons are the electrons in the outermost energy level, which for boron is the 2nd energy level.

In the ground state electron configuration of boron, we have 2 electrons in the 1s orbital and 2 electrons in the 2s orbital, leaving 1 unpaired electron in the 2p orbital. The ground state electron configuration is typically represented as 1s² 2s² 2p¹.

Now, to maximize the unshared electrons, boron can form compounds by promoting one of its 2s electrons to the 2p orbital. This would result in a partially filled p sublevel, which is more stable due to electron-electron repulsion. The electron configuration would now be 1s² 2s¹ 2p², with two unpaired electrons in the 2p orbital.

So, when we maximize the unshared electrons in the boron atom, the electron configuration becomes 1s² 2s¹ 2p².

To determine the electron configuration, it's useful to understand the Aufbau principle, which states that electrons occupy the lowest energy orbitals available. The Pauli exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers, and the Hund's rule states that, when orbitals of equal energy are available, electrons will occupy them singly before pairing up. By following these principles, we can determine the electron configuration of an atom.