Tetrahedral geometry molecular

Molecular Geometry Tetrahedral with four atoms bonded. Trigonal pyramidal with three atoms bonded. Bent with two atoms bonded. Trigonal planar with three atoms bonded. Linear with two atoms bonded. 

The answer is D. If you draw the electron-dot structure of the CCl molecule, you can see that there are four electron pairs around the central carbon atom. All these electrons form four carbon-chlorine bonds which make the molecular geometry - tetrahedral. 

Electron-domain geometry tetrahedral, molecular geometry tetrahedral... 

Four electron pairs, all bonding, yield the same electron-pair and molecular geometries tetrahedral (Line 4). The tetrahedral methane molecule, CH4, looks like a tall pyramid with a triangular base (Fig. 13.5[a]). Each bond angle is 109.5°—the tetrahedral angle. 

In cases where the bonds are di.stributed symmetrically around the central atom, the nature of the atoms surrounding the central atom determines whether the molecule is polar ovCTall. For example, CCI4 and CHCI3 have the same molecular geometry (tetrahedral), but CCI4 is nonpolar because the bond dipoles... 

Tetrahedral molecular geometry, with 109.5° bond angles, minimizes repulsion among the bonding electron pairs of methane. ... 

The effect of molecular geometry can often be evaluated in a straightforward manner. Consider the tetrahedral CH4 molecule, which will be shown as having one C-H bond pointing "up" and the other three forming a tripod-like base ... 

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 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 AB4) has a tetrahedral electronic geometry and tetrahedral molecular geometry. The C-F bonds are polar, but since the molecule is symmetrical, the bond dipoles cancel to give a nonpolar molecule (Section 8-7). 

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. 

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. 

The Lewis structure of NC13 has three Cl atoms bonded to N and one lone pair attached N. These four electron groups around N produce a tetrahedral electron-group geometry. The fact that one of the electron groups is a lone pair means that the molecular geometry trigonal pyramidal. 

B The Lewis structure of POCl3 has three single P-Cl bonds and one P-0 bond. These four electron groups around P produce a tetrahedral electron-group geometry. No lone pairs are attached to P and thus the molecular geometry is tetrahedral. 

The VSEPR notation for the Cl2F+ ion is AX2E3. According to Table 11.1, molecules of this type exhibit an angular molecular geometry. Our next task is to select a hybridization scheme that is consistent with the predicted shape. It turns out that the only way we can end up with a tetrahedral array of electron groups is if the central chlorine atom is sp3 hybridized. In this scheme, two of the sp3 hybrid orbitals are filled, while the remaining two are half occupied. 

If we examine the other central atom, the oxygen with the attached hydrogen, we observe the presence of two lone pairs and two bonds. The presence of these pairs and bonds, which total four, means that the electron-group geometry is tetrahedral. This arrangement has sp3 4 5 6 hybridization. Since there are two lone pairs, the molecular geometry is bent. 

The molecular geometry of methane and of methyl fluoride is tetrahedral. In the case of methane, this symmetrical arrangement of polar covalent carbon-hydrogen bonds leads to a canceling of the bond polarities resulting in a nonpolar molecule. As a nonpolar molecule, the strongest intermolecular force in methane is a London force. In methyl fluoride, a fluorine atom replaces one of the hydrogen... 

Values of umn, umx and uM for synunetrical tetrahedral (MZ3), trigonal bipyramidal (MZ4), and octahedral (MZ5) groups can be obtained from Eq. 17 using the rv values calculated from Eq. 1-3 and 6-10. Values of rV mn, rv,mi and rV-ax for symmetrical bicycloalkyl and heterobicycloalkyl groups can be calculated from molecular geometry. The appropriate values are then obtainable from Eq. 17. 

In any molecule in which there are no nonbonding pairs around the central atom, the molecular shape is the same as the molecular geometry. Thus, to use the examples from Table 6.2, all three two-substituent molecules have both a linear geometry and a linear shape. Both BH3 and H2CO have a triangular planar shape, CH4 has a tetrahedral shape, PF5 a triangular bipyramidal shape, and SF6 a square bipyramidal shape. 

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