Ok
Um, I do know the Answer,
There are no Lone Pairs of Electrons in the Valence Shell of The Central Atom of SiCl4, because:
Si has the Number Configuration of: 2,8,4 The '4' is the number of dots, it has surrounding Si, one above Si, one under Si, one on the right side of Si, one on the left side of Si.
Cl has the Number Configuration of: 2,8,7 The '7' is the number of dots, it has surrounding Cl, you can have it in any order, i.e. one above Cl, two under Cl, two on the right side of Cl, two on the left side of Cl. But when you join SiCl4 together, and make it into a Lewis Structure, then the Central Atom is Si,
Then Si will have one Cl bonding above Si, one Cl bonding under Si, one Cl bonding on the right side of Si, one Cl bonding on the left side of Si, and now all you can see, is that Si has Four Cl, attaching, bonding to Si, and now Si doesnt have any Lone Pairs
1: Both the lone pairs asa well as the bond pairs participate in determining the geometery of the molecules 2: The electron pairs are arranged around the central polyvalent atom so as to remain at a miximum distance apart to avoid repulsions 3: The electron pairs of lone pairs occupy more space then the bond pairs from ncert:- 1)The shape of a molecule depends upon the number of valence shell electron pairs (bonded or nonbonded) around the central atom. 2)Pairs of electrons in the valence shell repel one another since their electron clouds are negatively charged. 3)These pairs of electrons tend to occupy such positions in space that minimise repulsion and thus maximise distance between them. 3)The valence shell is taken as a sphere with the electron pairs localising on the spherical surface at maximum distance from one another. 4)A multiple bond is treated as if it is a single electron pair and the two or three electron pairs of a multiple bond are treated as a single super pair. 5) Where two or more resonance structures can represent a molecule, the VSEPR model is applicable
The repulsion is between valence electrons.
4
Two lone pair on the central selenium and three lone pairs on each chlorine. So total of eight lone pairs.
In NF3, the Nitrogen atom has 5 valence electrons and each Fluorine atom shares 1 more electron with Nitrogen. That makes 8 electrons (4 pairs of electrons) around Nitrogen. Betweent the four electron pairs, 3 pairs are bonded with Fluorine and the other one is a lone pair. Therefore around the central atom Nitrogen, there are three Fluorine atoms and a lone electron pair.
None
4 pairs
3 pairs
The answer is not 6 as said here before! The number of valence electrons in O2 (oxygen molecule) is: 12 valence electrons. 6 of them from each oxygen (O) atom. 4 valence electrons make up the double bond between the two oxygen atoms, and the remaining 8 valence electrons form lone pairs (non-bonding pairs) on the oxygen atoms, 2 lone pairs on each. I hope there is some help in this.
If an atom has five valence electrons, it will have one lone pair of electrons.
12
1
lone pairs
ow many valence electrons in methyl fluoride/
These pairs of electrons are referred to as lone pairs.
Valence shell electron pair repulsion theory, otherwise known as VSEPR theory, is used to predict the geometry of molecules. This is based on the number of electron pairs surrounding their central atoms. This is based on the idea that valence electron pairs surrounding and Adam generally repel each other, so their arrangement is based on the minimizing of said repulsion.
According to VSEPR theory, molecules adjust their geometry to keep the electrons in valence shells as far apart from each other as possible.