linear
Consider: Number of bonding domains on the central atom Number of non-bonding electron pairs (lone pairs) on the central atom
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.
The molecular geometry of a molecule can be determined using the VSEPR theory. VSEPR (Valence Shell Electron Pair Repulsion) Theory: The basic premise of this simple theory is that electron pairs (bonding and nonbonding) repel one another; so the electron pairs will adopt a geometry about an atom that minimizes these repulsions. Use the method below to determine the molecular geometry about an atom. Write the Lewis dot structure for the molecule. Count the number of things (atoms, groups of atoms, and lone pairs of electrons) that are directly attached to the central atom (the atom of interest) to determine the overall (electronic) geometry of the molecule. Now ignore the lone pairs of electrons to get the molecular geometry of the molecule. The molecular geometry describes the arrangement of the atoms only and not the lone pairs of electrons. If there are no lone pairs in the molecule, then the overall geometry and the molecular geometry are the same. If the overall geometry is tetrahedral, then there are three possibilities for the molecular geometry; if it is trigonal planar, there are two possibilities; and if it is linear, the molecular geometry must also be linear. The diagram below illustrates the relationship between overall (electronic) and molecular geometries. To view the geometry in greater detail, simply click on that geometry in the graphic below. Although there are many, many different geometries that molecules adopt, we are only concerned with the five shown below.
The electron-domain geometry of PF6 is Octahedral, since the central atom Phosphorus has an electron pair geometry which is octahedral
Consider: Number of bonding domains on the central atom Number of non-bonding electron pairs (lone pairs) on the central atom
electron pair geometry: octahedral molecular geometry: octahedral
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.
trigonal pyramidal
It should be sp3d. first draw the Lewis structure. then you can see the central S atom has 4 bonding pair and 1 lone pair. then draw molecular orbital. Distribute electron according the bonding and lone pair. the paired electron represent lone pair in Lewis structure. and the other unpaired electron distribute in the molecular orbital represent the number of bonding pair in Lewis structure
The molecular geometry of a molecule can be determined using the VSEPR theory. VSEPR (Valence Shell Electron Pair Repulsion) Theory: The basic premise of this simple theory is that electron pairs (bonding and nonbonding) repel one another; so the electron pairs will adopt a geometry about an atom that minimizes these repulsions. Use the method below to determine the molecular geometry about an atom. Write the Lewis dot structure for the molecule. Count the number of things (atoms, groups of atoms, and lone pairs of electrons) that are directly attached to the central atom (the atom of interest) to determine the overall (electronic) geometry of the molecule. Now ignore the lone pairs of electrons to get the molecular geometry of the molecule. The molecular geometry describes the arrangement of the atoms only and not the lone pairs of electrons. If there are no lone pairs in the molecule, then the overall geometry and the molecular geometry are the same. If the overall geometry is tetrahedral, then there are three possibilities for the molecular geometry; if it is trigonal planar, there are two possibilities; and if it is linear, the molecular geometry must also be linear. The diagram below illustrates the relationship between overall (electronic) and molecular geometries. To view the geometry in greater detail, simply click on that geometry in the graphic below. Although there are many, many different geometries that molecules adopt, we are only concerned with the five shown below.
The electron-domain geometry of PF6 is Octahedral, since the central atom Phosphorus has an electron pair geometry which is octahedral
The molecular geometry of the AsO2- ion is bent (because of the lone electron pair with the central arsenic atom, making the O-As-O bond angle very obtuse) but its electron domain geometry is trigonal planar because there are three domains, with a 120 deg. angle between them.
Silicon Tetrafluoride has a tetrahedral molecular geometry. That means there are 4 F atoms around the central atom Si.
three dimensional arrangement of atoms electron-group geometry