Draw the electron configuration for a neutral atom of boron. energy
The Correct Answer and Explanation is:
Electron Configuration of a Neutral Boron Atom:
The electron configuration of a neutral atom of boron is:
1s² 2s² 2p¹
Explanation
Boron is the fifth element in the periodic table. A neutral boron atom contains five protons in its nucleus and therefore has five electrons to maintain electrical neutrality.
Electrons in an atom occupy energy levels or shells, and within those shells, they fill sublevels or orbitals in a specific order based on energy. This order is governed by the Aufbau principle, the Pauli exclusion principle, and Hund’s rule.
The first shell has only one sublevel—the 1s orbital—which can hold a maximum of two electrons. In boron, the first two electrons fill this orbital: 1s².
Next, the second shell begins to fill. The second shell contains two sublevels—the 2s and 2p orbitals. The 2s orbital can also hold up to two electrons, and the next two electrons in boron go here: 2s².
That accounts for four electrons. The fifth electron enters the 2p orbital. The 2p sublevel has three orbitals, each of which can hold two electrons, for a total of six electrons. But since boron has only one remaining electron, it will occupy just one of the three 2p orbitals. This is written as 2p¹.
Putting it all together, the complete electron configuration for boron is:
1s² 2s² 2p¹
This configuration shows how electrons are distributed among the atom’s orbitals in order of increasing energy. It also explains why boron is in Group 13 of the periodic table—it has three valence electrons in the second energy level (two in the 2s and one in the 2p). These valence electrons play a crucial role in chemical bonding and reactivity.
Understanding electron configuration helps predict how an element will interact with others in forming molecules and compounds.
