Want this question answered?
trigonal planar
tetrahedral due to the four area of electron density (two loan pair electrons and two bonded pairs).
Anything with six electron groups, keep in mind an electron group is a bonded atom or an electron pair, is an octahedral. Anything in an octahedral and a lone pair is the square pyramidal geometry. So all angles between the atoms are a little less than 90 degrees and the angle of the electron pair is greater than 90.
3
electron-group geometry Apex!
trigonal planar
The molecular geometry for a molecule with two electron groups and only bonded pairs is linear.
This is a linear molecule.
The electron domain geometry of XeF2 is linear. This is because the central atom Xe has two bonded atoms (F) and no lone pairs of electrons, resulting in a linear molecular geometry.
The molecular geometry of CS2 is linear. This molecule consists of a central carbon atom bonded to two sulfur atoms, and there are no lone pairs on the central atom. The bonds and atoms are arranged in a straight line, giving it a linear molecular geometry.
Electron pairs
In molecular geometry, bond length refers to the distance separating nuclei of bonded atoms in a single molecule.
tetrahedral due to the four area of electron density (two loan pair electrons and two bonded pairs).
The molecular geometry characterized by 109.5 degree bond angles is tetrahedral. This geometry occurs when a central atom is bonded to four surrounding atoms with no lone pairs on the central atom. An example of a molecule with this geometry is methane (CH4).
The molecular geometry of SF2 is bent or V-shape. This is because the sulfur atom has two bonded fluorine atoms and one lone pair of electrons, causing the molecule to take on a bent shape.
The electron domain geometry of NO2 is bent or V-shaped, with an angle of approximately 134 degrees. This is because NO2 has two electron domains around the nitrogen atom, resulting in a bent molecular geometry.
In a molecule with 4 electron domains, the molecular geometry can be tetrahedral if all domains are bonded pairs or trigonal pyramidal if one domain is a lone pair. This arrangement follows the VSEPR theory, which predicts the shape of molecules based on the number of electron domains around the central atom.