We can't draw structures on this board.
Ca:^2+
+
..^-
:F:
..
About the best I can do.
Ca:^2+
+
..^-
:F:
..
About the best I can do.
So, Ca donates two electrons to F, forming the positively charged Ca2+ ion with the electron configuration of [Ar]. Meanwhile, F accepts Ca's two electrons, becoming the negatively charged F- ion with the electron configuration of [Ne].
Now let's draw their Lewis structures. Remember, Ca has 20 electrons and F has 9 electrons.
The Lewis structure for Ca2+ will have 18 electrons, since it lost two. It will be represented as Ca2+:
Ca
:
On the other hand, F- gained one electron, so its Lewis structure will have 10 electrons. It will be represented as F-:
F
:
And that's how Ca and F atoms bond and form ions. It's like a romantic exchange of electrons. Quite electrifying!
The electron configurations and Lewis structures of the resultant ions are as follows:
1. Ca2+ Ion:
- Calcium (Ca) has atomic number 20, so its neutral atom has 20 electrons: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2.
- When Ca loses 2 electrons, it forms the Ca2+ ion.
- The electron configuration of Ca2+ ion is: 1s^2 2s^2 2p^6 3s^2 3p^6.
Lewis Structure of Ca2+ ion:
- Since Ca loses 2 electrons, it loses the outermost 4s^2 electrons.
- There will be no dots or lines around the Ca2+ symbol in the Lewis structure since it does not have any valence electrons left after losing 2 electrons.
2. F- Ion:
- Fluorine (F) has atomic number 9, so its neutral atom has 9 electrons: 1s^2 2s^2 2p^5.
- When F gains 1 electron, it forms the F- ion.
- The electron configuration of F- ion is: 1s^2 2s^2 2p^6.
Lewis Structure of F- ion:
- Since F gains 1 electron, it adds 1 dot to its Lewis structure.
- F- ion will have 8 electrons (an octet) around the symbol (F) in the Lewis structure, represented by 4 pairs of dots.
Note: The actual electron configurations and Lewis structures may differ slightly due to variations in electron pairing and distribution.
1. Electron Configurations:
- Calcium (Ca) atom: The atomic number of calcium is 20, indicating that it has 20 electrons. The electron configuration of Ca is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s².
- Fluorine (F) atom: The atomic number of fluorine is 9, indicating that it has 9 electrons. The electron configuration of F is 1s² 2s² 2p⁵.
2. Formation of Ions:
When Ca and F atoms react, they tend to achieve stable electron configurations by transferring or sharing electrons. Calcium has 2 valence electrons in its 4s² orbital, and fluorine requires 1 additional electron to fill its 2p⁶ orbital. Therefore, calcium easily loses 2 electrons, while fluorine easily gains 1 electron to form stable ions.
- Calcium ion (Ca²⁺): By losing 2 electrons, calcium forms a positive ion with a net charge of +2. The resulting electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ (equivalent to the noble gas configuration of argon, Ar).
- Fluoride ion (F⁻): By gaining 1 electron, fluorine forms a negative ion with a net charge of -1. The resulting electron configuration is 1s² 2s² 2p⁶ (equivalent to the noble gas configuration of neon, Ne).
3. Lewis Structures:
- Calcium ion (Ca²⁺): Since calcium loses 2 electrons, it becomes Ca²⁺. In Lewis structure, Ca²⁺ is represented by Ca with a positive charge (+2) and no dots around it, as it lost its 2 valence electrons.
- Fluoride ion (F⁻): Since fluorine gains 1 electron, it becomes F⁻. In Lewis structure, F⁻ is represented by F with a negative charge (-1), and it will have 8 valence electrons by sharing additional electron(s) with calcium.
Therefore, the Lewis structures of the resultant ions are:
- Ca²⁺: Ca²⁺
- F⁻: F⁻
I hope this explanation helps you understand how to determine the electron configurations and Lewis structures of ions resulting from the reaction of Ca and F atoms. Let me know if you have any further questions!