Complete the electron dot structure below to show how beryllium flouride (BeF2) is formed.
F F
Be+ -> Be
F F
To complete the electron dot structure for beryllium fluoride (BeF2), we need to show the arrangement of the valence electrons around each atom. Let's go step by step:
Step 1: Determine the number of valence electrons.
Beryllium (Be) is in group 2 of the periodic table, so it has 2 valence electrons.
Fluorine (F) is in group 17, so it has 7 valence electrons each.
Step 2: Place the atoms.
Beryllium (Be) is the central atom because it is the least electronegative. Place the Be atom in the center of the structure.
Step 3: Connect the atoms with single bonds.
Beryllium forms a single bond with each fluorine atom. Connect each fluorine (F) atom to the beryllium (Be) atom with a single bond.
Step 4: Distribute the remaining electrons.
Start by placing an electron pair on each atom's side, including the central atom (Be). Then, add the remaining electrons in pairs, making sure to satisfy the octet rule for each atom. Since beryllium only needs 4 electrons to satisfy the octet rule, it will not have any lone pairs.
The completed electron dot structure for beryllium fluoride (BeF2) is as follows:
F F
Be - F or F
F F
Note: The dash between the Be and F atoms represents a single bond.