what is the electron configuration for an excited state of boron?
The Correct Answer and Explanation is:
In its ground state, boron (B) has an atomic number of 5, meaning it has 5 electrons. The electron configuration for the ground state of boron is:
B: 1s22s22p1\text{B: } 1s^2 2s^2 2p^1B: 1s22s22p1
This configuration shows that two electrons occupy the 1s orbital, two occupy the 2s orbital, and one occupies the 2p orbital.
For an excited state, one or more electrons in the atom absorb energy and move to higher orbitals. In this excited state, the electron configuration will differ from the ground state, as an electron from a lower-energy orbital may jump to a higher-energy orbital.
For example, one possible excited state of boron could involve the electron in the 2p orbital absorbing energy and moving to the 3s orbital. The excited state electron configuration would then be:
B (excited state): 1s22s22p03s1\text{B (excited state): } 1s^2 2s^2 2p^0 3s^1B (excited state): 1s22s22p03s1
Here, the electron configuration indicates that:
- The 1s orbital still holds two electrons.
- The 2s orbital still holds two electrons.
- The 2p orbital is empty (as one electron has been promoted).
- The 3s orbital now holds one electron (which was promoted from the 2p orbital).
There are many possible excited states, depending on how the energy is absorbed. In other variations, the electron might be excited to the 3p orbital or higher.
Explanation:
The electron configuration of an atom reflects the distribution of electrons among its orbitals. Electrons in lower orbitals have less energy, while those in higher orbitals have more energy. When an atom is in an excited state, energy is absorbed, and one or more electrons move to higher orbitals.
In this example, boron absorbs energy, causing an electron to jump from the 2p orbital to the 3s orbital, resulting in a different electron configuration. The excited state is unstable and will eventually return to the ground state by emitting energy, typically in the form of light (photon).
