Geometry electron

The electron configuration expected for Ni2+ is [Ar]3unpaired electrons it would have to be (c) square planar in its electronic geometry, as both the octahedral and tetrahedral geometries require a species to have two unpaired electrons. Square planar does not. 

The molecular or ionic geometry is identical to its electronic geometry when there are no lone pairs on the central atom. 

The Lewis formula predicts 2 electron groups around the central Be atom and a linear electronic geometry. There are no lone pairs on the Cd atom, so the molecular geometry is the same as the electronic geometry linear (Section 8-5). 

The Lewis formula for the molecule (type AB4) predicts 4 electron groups around the central Sn atom and a tetrahedral electronic geometry. Since there are no lone pairs on Sn, the molecular geometry is also tetrahedral (Section 8-7). 

This polyatomic ion (type AB6), like (c), does not obey the octet rule without modification since 12 electrons must be shared to form 6 Sb-F bonds. Sb is a 5 A element, but the charge on the ion gives an extra electron which participates in bonding. The Lewis formula predicts 6 electron groups around the central Sb atom and an octahedral electronic geometry. There are no lone pairs on the Sb atom, so the ionic geometry is the same as the electronic geometry (Section 8-12). 

BrF3 The ideal bond angles would be those for a trigonal bipyramidal electronic geometry (type... 

The Lewis formula for the ion (type AB3U) predicts 4 electron groups around O including 1 lone pair of electrons. The electronic geometry is tetrahedral and the ionic geometry is trigonal pyramidal (Section 8-8). 

The Lewis formula shows 6 electron groups around the central P atom. The electronic geometry and the ionic geometry are both octahedral because there are no lone pairs of electrons on P (Section 8-12). 

The Lewis formula shows 5 electron groups around the central P atom and its electronic geometry is trigonal bipyramidal. The ionic geometry is a seesaw due to the presence of 1 lone pair of electrons on the central P atom (Section 8-11). 

The Lewis formula predicts 5 electron groups around the central I atom and a trigonal bipyramidal electronic geometry. This ionic geometry is linear. 

This molecule (type AB3) has a trigonal planar electronic geometry and trigonal planar molecular geometry. The B-Cl bonds are polar, but since the molecule is symmetrical, the bond dipoles cancel to give a nonpolar molecule (Section 8-6). 

This molecule (type AB3U) has a tetrahedral electronic geometry and a pyramidal molecular geometry. Cl (EN = 3.0) is more electronegative than As (EN = 2.1). The polar As-Cl bond dipoles oppose the effect of the lone pair. The molecule is only slightly polar (Section 8-8). 

This molecule (type AB2U2) has a tetrahedral electronic geometry and an angular molecular geometry. Oxygen (EN = 3.5) is less electronegative than F (EN = 4.0). The O-F bond dipole opposes the effect of the two lone pairs of electrons and so, OF2 is polar (Section 8-9). 

BF3 and CF4 are nonpolar molecules. CF4, NF3, OF2 and HF have tetrahedral electronic geometries, but have different molecular geometries since they have 0, 1,2, and 3 lone pairs of electrons around the center atom, respectively. 

Molecule or Ion Electronic Geometry Molecular Geometry Hybridization of S Atom... 

The Lewis dot formula predicts 4 regions of high electron density around the central N atom, a tetrahedral electronic geometry and a pyramidal molecular geometry. The N atom has sp3 hybridization (Sections 8-8 and 28-14). The three-dimensional structure is shown below. 

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