A valence election in an atom of sulfur is excited by heating a sample. The electron jumps from the s orbital to the p orbital. What is the electron configuration of the excited sulfur atom, and what would the orbital diagram look like?
The lethal inhalation dose of sarin for a 200lb person has been determined to be 0.0015 mg. Determine the LD50 of sarin that researchers used to calculate this lethal inhalation dose.
To determine the electron configuration of an excited sulfur atom and the corresponding orbital diagram, we need to follow a few steps:
Step 1: Determine the electron configuration of the ground state sulfur atom.
The atomic number of sulfur is 16, so the ground state electron configuration would be: 1s2 2s2 2p6 3s2 3p4.
Step 2: Identify the valence electrons.
Valence electrons are the electrons in the outermost energy level of an atom. In this case, sulfur has six valence electrons in the 3s and 3p orbitals (2 from the 3s orbital and 4 from the 3p orbital).
Step 3: Determine the excited electron configuration.
When the electron in the 3s orbital of sulfur is excited, it jumps to the empty 3p orbital. This results in an excited state, where the electron configuration becomes: 1s2 2s2 2p6 3s1 3p5.
Step 4: Construct the orbital diagram.
The orbital diagram visually represents the distribution of electrons in different orbitals. For the excited sulfur atom, we can represent this as follows:
1s ↑↓
2s ↑↓
2p ↑↓ ↑↓ ↑↓
3s ↑
3p ↑↓ ↑↓ ↑↓ ↑↓
In the diagram, the arrows (↑ and ↓) represent the presence of electrons in each orbital, with the direction indicating their spin (either up or down).
So, the electron configuration of the excited sulfur atom is 1s2 2s2 2p6 3s1 3p5, and the corresponding orbital diagram shows how the electrons are distributed in the different orbitals.