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Lewis Structure of Strontium Fluoride SrF2 Ionic Compound
Published on March 15, 2026
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Determine the Lewis structure for the ionic compound strontium fluoride (SrF2) by identifying the stable cation (Sr2+) and anions (F-) formed via electron transfer.
Question
SrF2 what is the lewis structure of (strontium fluoride) ?
Answer
The user is asking for the Lewis structure of strontium fluoride (
Here is the step-by-step process to determine the Lewis structure for strontium fluoride:
1. Determine the Type of Compound
Strontium (
2. Determine the Ions Formed
In ionic compounds, atoms achieve a stable noble gas configuration by transferring electrons.
- Strontium (
): Strontium is in Group 2. It loses 2 valence electrons to achieve the configuration of Krypton ( ). - Fluorine (
): Fluorine is in Group 17. It gains 1 electron to achieve the configuration of Neon ( ).
Since strontium loses 2 electrons, it requires two fluoride ions to balance the charge:
3. Draw the Lewis Structure for Ionic Compounds
For ionic compounds, the Lewis structure represents the stable ions that result from the electron transfer, not shared bonds.
- Cation (
): Strontium loses its 2 valence electrons. It is represented by its symbol with a charge and no valence electrons shown. - Anion (
): Fluorine gains 1 electron to complete its octet (8 valence electrons). It is represented by its symbol, a charge, and 8 valence electrons (represented by dots).
Since there are two fluoride ions for every one strontium ion, the structure must show both anions surrounding the cation.
Final Lewis Structure Representation
The Lewis structure for strontium fluoride shows the strontium cation surrounded by two fluoride anions:
Or, more formally:
The final structure consists of the strontium ion with a