::S=Si=S::
= are double bonds
: are single lone pairs
Theoretically SiO2 should look like CO2: ::O = C = O::
But since the Si-atom is much bigger than C, it is not energetically favorable to form double bonds towards the small oxygen atoms. The delocalized electrons (in the perpendicualar p-orbitals are too far away from the oxygen atoms to prefer this stretched state.
Instead SiO2 is the basic formula unit of a tetraedrical tertiary structure. Each Si-atom covalently binds four oxygen atoms with a single bond. A more accurate formula would be SiO4/2. Each oxygen binds two Si-atoms, so that a crystal structure is formed. This network is very strong wherefore the melting point is way higher than CO2. This is why SiO2(/4) produces sand while CO2 is rather hard to make solid. 不知道
Theoretically SiO2 should look like CO2: ::O = C = O::
But since the Si-atom is much bigger than C, it is not energetically favorable to form double bonds towards the small oxygen atoms. The delocalized electrons (in the perpendicualar p-orbitals are too far away from the oxygen atoms to prefer this stretched state.
Instead SiO2 is the basic formula unit of a tetraedrical tertiary structure. Each Si-atom covalently binds four oxygen atoms with a single bond. A more accurate formula would be SiO4/2. Each oxygen binds two Si-atoms, so that a crystal structure is formed. This network is very strong wherefore the melting point is way higher than CO2. This is why SiO2(/4) produces sand while CO2 is rather hard to make solid.
The dot structure for silicon dioxide begins with the S atom that has two double bonds branching from it, each attached to a single O atom. The two oxygen atoms then each have two double dots.
I cant add a picture here.I have drawn a Lewis structure of H2SiO3 on the following web. Visit it. It will be remove with in 10 days.
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http://members.optushome.com.au/scottsoftc/chapter04/section4.html If you're referring to quartz, it's in a crystal lattice structure.
Silicon is the central ion with four single bonds to each of the oxygen ions. Each oxygen ion also has 5 electrons around it.
The answer to your fantastic question is that it has 2 single bonds and one double bond
O::Si::O With two dots on top of each O and two on the bottom of them.
lewis structure of Cl2O7
Lewis structure was created in 1916.
What is Lewis Structure for the bicarbonate ion
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.
Potassium oxide (K2O) is an ionic compound, not a molecule, and does not have a Lewis structure.
lewis structure of Cl2O7
Lewis structure was created in 1916.
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.
Potassium oxide (K2O) is an ionic compound, not a molecule, and does not have a Lewis structure.
Resonance
The maximum number of electrons in a Lewis structure is eight, which is an octet of electrons.
CaCO3 does not have a lewis structure because this molecule is composed of ions. (Ca+2 and CO3-2). you have to draw the lewis structure of the ions separately, as shown in the parenthesis.
Lewis structure
chicken
Lewis structure, electron dot diagram, electron dot structure...