S has 6 valence electrons
0 has 6 valence electrons: total 18 for 3 Oxygen
O(formal charge): 6(valence electrons)-4(Non bonding Valence Electrons)-4(bonding electrons)/2=0
ormal charge): 6(valence electrons)-0(N0nbonding Valence Electrons)-12(bonding electrons)/2=0
The molecular geometry of SO3 is trigonal planar
Type of Hybrid orbita:SP2
Angle between bonded atoms: 120o
Sulfur would be the central atom. 3 oxygens branch out. 2 of the oxygens have single bonds; 1 oxygen has a double bond. total of 24 electrons used. The central sulfur has a formal charge of +2, while the two oxygens which are single bonded to the sulfur each have formal charges of -1.
[This answer is wrong. Sulfur is the central atom and the three oxygen do branch from it, but each oxygen is double bonded to the sulfur. Your formal charge calculations were correct but you did not fully minimize it. The reason sulfur can be an "octet rule violator" in this case (having 12 electrons being shared) is because it is in the third period and has access to what are called d sub-shell energy levels].
The first answer is correct, but in reality the sulfur is bonded by the strength of 4/3 of a bond. The Lewis structure is denoted by three bracketed drawing, showing a double bond with each oxygen separately.
Sulfur would be the central atom. 3 oxygens branch out. 2 of the oxygens have single bonds; 1 oxygen has a double bond. total of 24 electrons used. The central sulfur has a formal charge of +2, while the two oxygens which are single bonded to the sulfur each have formal charges of -1.
[This answer is wrong. Sulfur is the central atom and the three oxygen do branch from it, but each oxygen is double bonded to the sulfur. Your formal charge calculations were correct but you did not fully minimize it. The reason sulfur can be an "octet rule violator" in this case (having 12 electrons being shared) is because it is in the third period and has access to what are called d sub-shell energy levels].
The first answer is correct, but in reality the sulfur is bonded by the strength of 4/3 of a bond. The Lewis structure is denoted by three bracketed drawing, showing a double bond with each oxygen separately.
It's trigonal planar, and it exhibits resonance.
SO3's simplified Lewis structure looks something like this:
O
|
S=O
|
O
the ion (SO3 2-) is pyramidal:
.. 2-
0--S--O
|
O
the molecule (SO3) is triangular with resonance:
O=S--O
|
O
This is the Lewis structure for SO2 - O:S:O
Note is is bent planar
Ask prof. Valverde or Valdez.
:o=o=s=o:
h2so3
I think it is acid, because there is a question that asks the acid site of SO3.
Ax3e3
For SO3, two equivalent resonance structures are sufficient to describe the bonding.
lewis structure of Cl2O7
Lewis structure was created in 1916.
I think it is acid, because there is a question that asks the acid site of SO3.
apex users its defenatley 3
Ax3e3
o o Oo
For SO3, two equivalent resonance structures are sufficient to describe the bonding.
three
lewis structure of Cl2O7
Lewis structure was created in 1916.
The compound SO3 is a type of covalent bond. It is a covalent bond because both sulfur and oxygen are nonmetals that are bonded.
What is Lewis Structure for the bicarbonate ion
Yes, XeF4, or xenon tetrafluoride, has a Lewis structure.
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.