What is the lewis dot structure for Fluoride, F1- and Mg2???
for fluorine [F]1-
the lewis dot structure would have it having a full octet thus 8 electrons since fluorine usually has 7 electrons
I'll try to draw it.
  ..
:F: -1
  ..
Mg2+
Mg atom would be Mg: but it has lost those two electrons when it becomes the 2+ ion.
To draw the Lewis dot structure for Fluoride (F), F1-, and Mg2+, we need to determine the number of valence electrons for each element.
1. Fluoride (F):
- Fluorine is in Group 7A or 17 of the periodic table.
- It has 7 valence electrons.
2. Fluoride ion (F1-):
- The negative charge indicates that an extra electron has been gained.
- Adding this one additional electron gives a total of 8 valence electrons for F1-.
3. Magnesium ion (Mg2+):
- Magnesium is in Group 2A or 2 of the periodic table.
- It has 2 valence electrons.
- In the ion form, Mg2+ has lost two electrons, resulting in 0 valence electrons.
Now we can draw the Lewis dot structures:
1. Fluoride (F):
- Place one dot around the symbol of fluorine, representing its valence electron.
F: •
2. Fluoride ion (F1-):
- Since there is an extra electron, place brackets around the symbol and include a negative charge (-) outside the brackets.
- The extra electron pairs with one of the existing dots.
[F]1-
3. Magnesium ion (Mg2+):
- Since magnesium has lost two electrons, we remove both dots.
Mg2+: no dots
Keep in mind that Lewis dot structures show the valence electrons. For a complete electron configuration, you would need to include inner electrons as well.
To determine the Lewis dot structure for molecules or ions, we need to follow a few steps:
1. Determine the number of valence electrons for each atom. For main group elements, the number of valence electrons can be determined by the group number (excluding the "A" portion) on the periodic table. In the case of Fluoride (F), it is in group 7, so it has 7 valence electrons. Similarly, Magnesium (Mg) is in group 2, so it has 2 valence electrons.
2. For ions, we need to adjust the number of valence electrons based on the ionic charge. In the case of F^1-, which has a charge of -1, we add one extra electron. So the total number of valence electrons for F^1- is 7 + 1 = 8. Conversely, for Mg^2+, which has a charge of +2, we remove two valence electrons. So the total number of valence electrons for Mg^2+ is 2 - 2 = 0.
3. Decide which atom will be the central atom. In general, the less electronegative atom is the central atom. Fluoride only has one atom, so it is the central atom. For Mg^2+, the central atom is Mg.
4. Connect the atoms using single bonds. Since Fluoride (F) has only one atom, there are no bonds to draw for it. For Mg^2+, we connect the central Mg atom to two additional F atoms using single bonds.
5. Distribute the remaining valence electrons around the atoms, ensuring each atom satisfies the octet rule (except for hydrogen). Start by placing electrons as lone pairs on each atom, followed by pairing them up if necessary.
Now, let's break this down for each compound:
1. Fluoride (F):
- F has 7 valence electrons.
- Since F does not form any bonds, we place all 7 valence electrons as lone pairs around the F atom.
2. Fluoride Ion (F^-):
- F has 7 valence electrons.
- We add one extra electron to account for the -1 charge, totaling 8 valence electrons.
- Since F does not form any bonds, we place all 8 valence electrons as lone pairs around the F atom.
3. Magnesium Ion (Mg^2+):
- Mg has 2 valence electrons.
- We remove 2 valence electrons to account for the +2 charge, totaling 0 valence electrons.
- Since Mg forms two bonds with F, we draw two lines (each line represents a bond) extending from Mg to F on either side.
- Since Mg has no valence electrons remaining, there are no lone pairs around the Mg atom.
- Each F atom contributes one valence electron to the shared bonds with Mg, thus satisfying their octet rule.
Note: The Lewis dot structures are often represented using dots or crosses to represent electrons, but I have described them using lines for simplicity.