linear
Consider: Number of bonding domains on the central atom Number of non-bonding electron pairs (lone pairs) on the central atom
The electron geometry of thionyl chloride (SOCl₂) is tetrahedral. This is due to the presence of four regions of electron density around the central sulfur atom: two bonding pairs with chlorine atoms and one bonding pair with the oxygen atom, along with one lone pair. The arrangement of these electron pairs leads to a tetrahedral electron geometry, although the molecular geometry is bent or angular due to the presence of the lone pair.
Electron pair geometry considers both bonding and lone pairs of electrons around a central atom, while molecular geometry focuses solely on the arrangement of bonded atoms. This can lead to different geometries when there are lone pairs present; for example, in ammonia (NH₃), the electron pair geometry is tetrahedral due to one lone pair, but the molecular geometry is trigonal pyramidal. The presence of lone pairs affects bond angles and the overall shape of the molecule, resulting in distinct geometries.
check valence electron
The molecular geometry of NH4+ is tetrahedral. This is because NH4+ has four bonding regions (four hydrogen atoms bonding with the central nitrogen atom) and no lone pairs of electrons on the central nitrogen atom.
One can predict molecular geometry by considering the number of bonding and non-bonding electron pairs around the central atom, using VSEPR theory. The arrangement of these electron pairs determines the shape of the molecule.
Consider: Number of bonding domains on the central atom Number of non-bonding electron pairs (lone pairs) on the central atom
Check the link, it is a sheet describing the different types of electron and molecular geometry. It helped me a lot. ^^ electron pair geometry and molecular geometry won't be the same if there are lone pairs involved.
Octahedral is the edcc geometry and the molecular geometry is square pyramidal
electron pair geometry: octahedral molecular geometry: octahedral
The molecular geometry of SnCl5- is square pyramidal. This is because the central tin atom has five bonding pairs and no lone pairs, leading to a trigonal bipyramidal electron geometry. The lone pair occupies one of the equatorial positions, resulting in a square pyramidal molecular geometry.
Electron pair geometry considers both bonding and lone pairs of electrons around a central atom, while molecular geometry focuses solely on the arrangement of bonded atoms. This can lead to different geometries when there are lone pairs present; for example, in ammonia (NH₃), the electron pair geometry is tetrahedral due to one lone pair, but the molecular geometry is trigonal pyramidal. The presence of lone pairs affects bond angles and the overall shape of the molecule, resulting in distinct geometries.
a) ClF4- has a square planar geometry due to its five electron domains, with four bonding pairs and one lone pair. b) ClF4+ has a linear geometry with no lone pairs, resulting in a linear molecular shape. c) NO2- has a T-shaped geometry with three electron domains - one lone pair and two bonding pairs. d) BrF3 has a bent molecular geometry due to the presence of two lone pairs and two bonding pairs around the central atom. e) CO2 has a linear molecular geometry as it has two electron domains and no lone pairs around the central carbon atom.
check valence electron
Consider: Number of bonding domains on the central atom Number of non-bonding electron pairs (lone pairs) on the central atom
The molecular geometry of NH4+ is tetrahedral. This is because NH4+ has four bonding regions (four hydrogen atoms bonding with the central nitrogen atom) and no lone pairs of electrons on the central nitrogen atom.
Valence electron pairs will move as far apart from each other as possible. (Apex)