The central atom in a Lewis structure is usually the least electronegative atom.
EDIT:
If an atom occurs only once, this atom is most likely to be the central atom (exception is hydrogen, as it can make only 1 bond [1 electron necessary to reach a noble gas electron configuration]). The atom that can form the greatest number of bonds (has the least number of valence electrons) or is the least electronegative (least likely to attract atoms).
It is usually the the one with the highest valence, the one with the lowest electronegativity, or, for organic molecules, the carbon atom.
It is where all the pairs of electrons are centered around.
The least-electronegative atom is central (except for hydrogen, which is never central).
Usually some nonmetal, but if a compound of oxygen with another nonmetalit will be the other nonmetal, not oxygen.
In a Lewis structure the least electronegative atom is usually the central atom
why do you even care
nitrogen
Every pair of electrons on the central atom (S) of the Lewis structure of SF6 is shared by an F atom, so therefore there are no lone pairs on the central atom.
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The central atom of this ion is the C atom and it has 8 valence electrons.
There is none because there are no bonds in an atom.
nitrogen
D. least electronegative atom
Every pair of electrons on the central atom (S) of the Lewis structure of SF6 is shared by an F atom, so therefore there are no lone pairs on the central atom.
+1
The central atom of this ion is the C atom and it has 8 valence electrons.
There is none because there are no bonds in an atom.
I is the central atom single bonded to the 4 Br atoms. I also has 2 lone pairs of electrons. It may also be written without showing the lone pairs on any of the electrons, but with a negative charge on the I atom instead (that's how it was on my homework).
To be the central atom in a compound, the atom must be able to simultaneously bond to at least two other atoms. He, F, and H cannot serve as central atoms in a Lewis structure
The Lewis structure of an atom gives a clear illustration of the valence electrons.
It should be sp3d. first draw the Lewis structure. then you can see the central S atom has 4 bonding pair and 1 lone pair. then draw molecular orbital. Distribute electron according the bonding and lone pair. the paired electron represent lone pair in Lewis structure. and the other unpaired electron distribute in the molecular orbital represent the number of bonding pair in Lewis structure
The Lewis dot structure for CH3OH starts with a central C atom. Three H atoms are single bonded to the carbon atom, and an OH group is also bonded to the C atom with a single C-O bond.
The correct Lewis Structure for the oxygen atom will be an 'O' with two dots above and below, with one dot on the left and on the right sides.