how can something like aluminum sulphide form? illustrate showing electron movement.
Aluminum sulphide can be formed by the reaction of aluminum and sulfur.
The reaction can be illustrated as follows:
Al + S → Al2S3
During the reaction, aluminum atoms lose three electrons each to form positively charged aluminum ions (Al3+), while sulfur atoms gain two electrons each to form negatively charged sulfide ions (S2-).
The electron movements can be shown as follows:
Aluminum (Al) atom loses 3 electrons:
Al ⟶ Al3+ + 3e-
Sulfur (S) atom gains 2 electrons:
S + 2e- ⟶ S2-
These ions then combine to form the ionic compound aluminum sulphide (Al2S3), which is composed of Al3+ and S2- ions in a 2:3 ratio.
Al3+ + 3S2- → Al2S3
This reaction can also be shown in a diagram:
[image: https://i.imgur.com/mSJYTXo.png]
In this diagram, the aluminum atom (Al) is shown losing three electrons, represented by three dots leaving the atom. The sulfur atom (S) is shown gaining two electrons, represented by two dots entering the atom. The resulting ions, Al3+ and S2-, are shown as separate ions before they combine to form aluminum sulphide (Al2S3).
Aluminum sulfide (Aluminum sulphide) forms through a chemical reaction between aluminum and sulfur. The chemical formula for aluminum sulfide is Al2S3. Here is a step-by-step explanation of how aluminum sulfide forms, illustrated with electron movement:
Step 1: Aluminum atom (Al) loses three electrons to attain a stable electron configuration. This forms an aluminum ion with a positive charge, Al3+.
Al → Al3+ + 3e-
Step 2: Sulfur atom (S) gains three electrons to achieve a stable electron configuration. This forms a sulfide ion with a negative charge, S2-.
S + 2e- → S2-
Step 3: Two aluminum ions (Al3+) combine with three sulfide ions (S2-) to form aluminum sulfide (Al2S3).
2Al3+ + 3S2- → Al2S3
In the reaction, two aluminum ions are needed to balance the charge for every three sulfide ions. The aluminum ions lose electrons, transferring them to the sulfur ions, forming aluminum sulfide.
In the diagram, you can visualize the electron movement as follows:
1. Initially, the aluminum atom (Al) has three valence electrons in its outermost shell.
Al (3 valence electrons)
2. The aluminum atom loses three electrons, becoming an aluminum ion (Al3+). This is represented by the arrows moving outward from the aluminum atom, showing the loss of three electrons.
Al (3 valence electrons) → Al3+ (empty outer shell)
3. The sulfur atom (S) has six valence electrons in its outermost shell.
S (6 valence electrons)
4. The sulfur atom gains two electrons, becoming a sulfide ion (S2-). This is illustrated by the arrows moving inward towards the sulfur atom, showing the gain of two electrons.
S (6 valence electrons) + 2e- → S2- (full outer shell)
5. Finally, two aluminum ions (Al3+) and three sulfide ions (S2-) combine to form aluminum sulfide (Al2S3). This is represented by the arrangement of the ions in the chemical formula, Al2S3.
2Al3+ + 3S2- → Al2S3
This step-by-step illustration demonstrates how aluminum sulfide forms through the transfer of electrons between aluminum and sulfur atoms.