That would be Trigonal Pyramidal in shape and have an sp3 hybridization.
Trigonal 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
To determine the hybridization of the central atom in a molecule, you can use the formula: hybridization number of sigma bonds number of lone pairs on the central atom. Count the number of sigma bonds and lone pairs around the central atom, then use this formula to find the hybridization.
To determine the hybridization of the central atom in a molecule, you can use the formula: hybridization number of sigma bonds number of lone pairs on the central atom. Count the number of sigma bonds and lone pairs around the central atom, then use this formula to find the hybridization.
To determine the hybridization of a central atom in a molecule, you can use the formula: hybridization number of sigma bonds number of lone pairs on the central atom. Count the sigma bonds and lone pairs, then use this formula to find the hybridization.
SF6 has no lone pairs on the central atom sulfur. It forms six bonds with fluorine atoms which gives it an octahedral geometry.
To determine the sp hybridization of a molecule, you can look at the number of sigma bonds and lone pairs around the central atom. If there are two sigma bonds and no lone pairs, the central atom is sp hybridized.
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.
In methane (CH4), the central carbon atom does not have any lone pairs of electrons. Instead, it forms four single covalent bonds with the four hydrogen atoms around it.
There are no lone pairs on the central atom in BCl3 because boron (B) is in group 13 (or 3A) and can have only 3 bonds around it.
The central atom in BrO2- has sp3 hybridization. There are two sigma bonds and two lone pairs around the central bromine atom, leading to a tetrahedral geometry and sp3 hybridization.
"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.
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.