H-O-F-O
1. You write it out as shown above.
2. Calculate the valence electrons contributed by each atom:
H--> 1 electron
O--> 6 electrons
F--> 7 electrons
O--> 6 electrons
*Add them all up*
1+6+7+6= 20 electrons
3. Start adding the valence electrons to the atoms, make sure you do not violate any rules. Do not add any electrons to hydrogen. Start with adding electrons to the oxygen on the far right.
4. You should end up with H-O-F-O --> Three lone pairs on the oxygen & 1 single bond for a total of 8 electrons, 2 lone pairs on the Fluorine & 2 single bonds, 2 lone pairs on the second Oxygen & 2 single bonds, and finally no lone pairs on the hydrogen and one single bond connecting it to the oxygen, giving a total of 2 electrons.
Extra information:
Chlorine is the only halogen to form an isolable acid of formula HOXO with X is a halogen of oxidation level +3. Even HOClO is not very stable: disproportionating by auto-redox: 2 HClO2 → HClO + HClO3. Chlorites however are stable.
Fluorine resists oxidation above the 1+ level. So HOFOseems NOT to be stable enough to exist in reasonable amounts.
Neither bromous acid nor iodous acid have been isolated. A few salts of bromous acid, bromites, are known, but no iodites.
There are no double bonds
Resonance structure.
The Lewis dot structure for germanium (Ge) is: Ge: :Ge:
The Lewis structure of the compound CCLO is as follows: CCCl-O.
The formal charge of the NCO Lewis structure is zero.
No, not exactly. It is an ionic compound so it would not have a Lewis dot structure. However, the carbonate anion, CO3^2- does have a Lewis dot structure.
Resonance structure.
The Lewis dot structure for germanium (Ge) is: Ge: :Ge:
The Lewis structure of the compound CCLO is as follows: CCCl-O.
The formal charge of the NCO Lewis structure is zero.
No, not exactly. It is an ionic compound so it would not have a Lewis dot structure. However, the carbonate anion, CO3^2- does have a Lewis dot structure.
The molecular geometry of the BR3 Lewis structure is trigonal planar.
The Lewis structure was created by American chemist Gilbert N. Lewis in 1916. Lewis proposed using dots to represent the valence electrons of an atom in order to show how atoms bond together in molecules.
Sulfur can form a maximum of six bonds in a Lewis structure.
The bond angle in the CHCl3 Lewis structure is approximately 109.5 degrees.
The formal charge of sulfur in the SO2 Lewis structure is 0.
The SO2 molecule has a bent structure according to its Lewis diagram.
Yes, the Lewis structure for HOCl can be completed with the atoms arranged as shown.