That would be Trigonal Pyramidal in shape and have an sp3 hybridization.
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∙ 12y agoTrigonal Pyramidal
No lone pairs
Tetrahedral. It is because in this molecular the central atom S have four bonds and no lone pairs. So the shape must and must be what I said.
There are no lone pairs and it's tetrahedral.
The lone pair electron region is the place around the central atom where electrons not bonding with another atom can be found. A lone pair of electrons are electrons that are not bonded with other atoms.
Trigonal Pyramidal
There are three single bonds total, one between each of the chlorine atoms and the central phosphorus atom. The phosphorus atom has an additional lone pair of electrons and is thus a has a tetrahedral geometry.
There are three single bonds total, one between each of the chlorine atoms and the central phosphorus atom. The phosphorus atom has an additional lone pair of electrons and is thus a has a tetrahedral geometry.
The question is not answerable. There is NO central atom in C2H2 (ethyn) and there's NO lone pair. All electrons are covalently shared in pairs: three pairs between C and C, one single pair in each C and H bond.
the geometric shape is trigonal bipyramidal since the central atom of As has 5 single bonds, and 0 lone pair electrons. the individual polarities between atoms cancel eachother out
"Central Cl atom, single bonded to 4 Oxygen atoms. Each oxygen has a formal charge -1 and 3 lone pairs. Cl has a formal charge of +3. bonded in tehrahedral"A better structure is central C atom, 3 double bonds to 3 O atoms with two lone pairs each and one single bond to one O atom with three lone pairs. Only the single bonded oxygen has a formal charge of -1, limiting formal change. This still has a tetrahedral shape.
In icl3 central atom is iodine and its valency is 7 out of 7 electrons 3 electrons are in chemical bonding so 2 lone pairs are there. Hybridization = number of sigma bonds + number of lone pairs = 3 sigma bonds + 2 lone pairs = 5 = sp3d ( 1 s + 3 P + 1 d = 5 ).
Because the central atom has two bonded regions (remember that single, double, and triple bonds all count as one charge cloud). In addition to the two bond regions, there is a lone pair of electrons on the central atom, which counts as the third charge cloud.
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.
GeF2 is a bent molecule with two single bonds and one lone pair on the central atom (Ge). The two fluorines have six electrons (dots) around them along with the single bond to germanium. The central atom's hybridization is SP2 and the AXE scheme is AX2E. The angle between the two fluorines is about 118o.
Lone pairs do not affect the shape of diatomic molecules, and Lone pairs are electrons that are not in bonds. Lone pairs do not affect the shape if they are not on the central atom.
Three. PBr3 is a molecular compound, there are three single bonds and a lone pair around the phosphorus atom, making up the octet.