if Ca and F atoms are allowed to react what will be the electron configurations and lewis structures of the resultant ions?
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To determine the electron configurations and Lewis structures of the resultant ions when Ca and F atoms react, we first need to consider the electron configurations of the individual atoms.
The atomic number of calcium (Ca) is 20, which means it has 20 electrons. The electron configuration of Ca can be represented as: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s².
The atomic number of fluorine (F) is 9, and it has 9 electrons. The electron configuration of F can be represented as: 1s² 2s² 2p⁵.
Now, let's consider the reaction between Ca and F. Calcium has two valence electrons in its outermost shell (4s orbital), while fluorine has seven valence electrons in its outermost shell (one in the 2s orbital and six in the 2p orbital). Since they can achieve a stable electron configuration by gaining or losing electrons, it is likely that calcium will lose two electrons and fluorine will gain one electron.
When calcium loses two electrons, it forms Ca²⁺ ion. Its electron configuration becomes: 1s² 2s² 2p⁶ 3s² 3p⁶.
When fluorine gains one electron, it forms F⁻ ion. Its electron configuration becomes: 1s² 2s² 2p⁶ 3s² 3p⁶.
Now, let's depict the Lewis structures of these ions.
- Ca²⁺ ion: It loses the two valence electrons from the 4s orbital. Hence, it has no dots or lines in the Lewis structure, as it has completely lost its valence electrons.
- F⁻ ion: It gains an electron in its outermost 2p orbital, which already had three unpaired electrons. Therefore, in the Lewis structure of F⁻, there will be six dots around the fluorine atom, representing the lone pairs.
So, the resultant ions are Ca²⁺ (calcium cation) and F⁻ (fluoride anion), with their respective electron configurations and Lewis structures as described above.