Sketch, on paper, the Lewis structure of F2, remembering to:Step 1: Arrange the atomsStep 2: Count the number of valence electrons.Step 3: Allocate two electrons between each pair of atoms which are assumed to be covalently bound.Step 4: Use the remaining valence electrons to form lone pairs, and/or double and triple bonds.What is the total number of valence electrons in F2?What type of bond exists between the two fluorine atoms?How many lone pairs are there on each fluorine atom?
Question
Sketch, on paper, the Lewis structure of F2, remembering to:Step 1: Arrange the atomsStep 2: Count the number of valence electrons.Step 3: Allocate two electrons between each pair of atoms which are assumed to be covalently bound.Step 4: Use the remaining valence electrons to form lone pairs, and/or double and triple bonds.What is the total number of valence electrons in F2?What type of bond exists between the two fluorine atoms?How many lone pairs are there on each fluorine atom?
Solution
Step 1: Arrange the atoms Since there are only two fluorine atoms in F2, you can simply put them side by side.
Step 2: Count the number of valence electrons. Fluorine is in group 17 of the periodic table, so it has 7 valence electrons. Since there are two fluorine atoms, the total number of valence electrons in F2 is 7*2 = 14.
Step 3: Allocate two electrons between each pair of atoms which are assumed to be covalently bound. You can draw a single line (representing a pair of electrons) between the two fluorine atoms to indicate a covalent bond. This uses up 2 of the 14 valence electrons, leaving 12.
Step 4: Use the remaining valence electrons to form lone pairs, and/or double and triple bonds. The remaining 12 electrons can be distributed as lone pairs around the two fluorine atoms. Each fluorine atom gets three lone pairs (6 electrons), using up all 12 remaining electrons.
So, the total number of valence electrons in F2 is 14.
The bond between the two fluorine atoms is a single covalent bond.
Each fluorine atom has three lone pairs.
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