Draw the electron configuration for neutral atom of carbon _ energy
The Correct Answer and Explanation is:
To draw the electron configuration of a neutral carbon atom, begin by noting that carbon has an atomic number of 6, meaning it contains 6 electrons in its neutral state.
Correct Box Diagram:
Electrons fill atomic orbitals in order of increasing energy, following Aufbau Principle, Pauli Exclusion Principle, and Hund’s Rule.
- 1s orbital: 2 electrons
- 2s orbital: 2 electrons
- 2p orbital: 2 electrons (placed in separate orbitals due to Hund’s Rule)
Thus, the orbital diagram appears as follows:
CopyEdit1s ↑↓
2s ↑↓
2p ↑ ↑
In the box diagram:
- Each box represents an orbital.
- Arrows represent electrons.
- Arrows pointing up and down indicate opposite spins.
Explanation (≈300 words):
The electron configuration of carbon provides insight into the arrangement of electrons within its atomic orbitals. Carbon has six electrons, and these occupy energy levels in a specific sequence based on fundamental quantum principles.
The first two electrons enter the 1s orbital, the lowest energy level. This orbital is spherically symmetrical and can hold a maximum of two electrons, which must have opposite spins. This requirement arises from the Pauli Exclusion Principle, which states that no two electrons in an atom can have the same set of quantum numbers.
The next two electrons occupy the 2s orbital, which also holds a maximum of two electrons. Like the 1s orbital, this one is spherical and lies at a higher energy level than the 1s.
The final two electrons go into the 2p orbitals. The p sublevel has three orbitals (2px, 2py, 2pz), each capable of holding two electrons. According to Hund’s Rule, electrons fill these degenerate orbitals singly first, with parallel spins, to minimize repulsion and maintain the lowest energy configuration.
As a result, the carbon atom has two electrons in the 1s, two in the 2s, and one each in two of the three 2p orbitals. The 2p orbital diagram shows two half-filled orbitals, which is typical for carbon and essential for its bonding behavior in forming four covalent bonds in organic compounds.
This specific arrangement allows carbon to hybridize and form various chemical bonds, contributing to its role as the backbone of organic chemistry.
