Drawing perspective representations of a trigonal bipyramid valence=5 and of an octahedron with valence=6?

Question

Also what would be the angles

thanks.

Answer 1

Structures of Molecules. Valence Electrons of Atoms. We have seen that an atom of an element has a characteristic number of electrons, equal to its atomic number Z. These electrons are arranged in shells about the nucleus, some being close to the nucleus, others far away. It is the electrons in the outermost shell, furthest from the nucleus, and therefore least tightly held, that are involved in chemical bonding. These are the valence electrons. The electrons close to the nucleus, called inner or core electrons, are much too tightly held to be lost to or shared with another atom. As we have seen, the number of valence electrons that an atom has is equal to the last digit of its group number. Thus Na, in group 1, has one valence electron; Al in group 13 has three valence electrons; Br in group 17 has seven valence electrons; and Fe in group 8 has eight valence electrons. The Lewis symbol for an element shows the valence electrons as dots arranged about the symbol for the element, as illustrated in Figure 3-1a for Na, Al, and Br. Dots are placed as if the symbol of the element were surrounded by an invisible square. (There is no physical significance to the square; it simply aids us in orderly thinking.) The first dot can be placed on any of the 4 sides, but the second, third, and fourth dots are then placed singly on the remaining 3 sides of the square; electrons are not placed in pairs (i.e., 2 dots on the same side of the square) until 4 have been placed singly. Dots that singly occupy the side of a square are referred to as unpaired electrons.

G.N. Lewis developed this approach to representing the valence electrons of an element before the quantum view of the atom discussed in Chapter 2 was complete. It is of interest from our perspective, though, to examine the correspondence between the Lewis symbol for an element and its valence electron configuration. In particular, we might expect the number of unpaired electrons in the Lewis symbol to correspond with the number of electrons that singly occupy valence orbitals of the atom. The Lewis symbols and valence orbital occupations of the atoms of period 2 are shown here. What we see is interesting and a bit puzzling. First, most of the atoms show the intuitively expected correspondence. Thus Li, N, O, F, and Ne exhibit the same number of unpaired electrons in the Lewis symbol and in the quantum orbital occupation diagram. Further, the numbers of unpaired electrons for these elements correspond with their usual valences; i.e., with the number of bonds that they form. However, for Be, B, and C in groups 2, 13, and 14, the numbers of unpaired electrons in the Lewis symbols do not correspond with the orbital occupation diagrams. Thus the Lewis symbol for carbon leads us to expect 4 unpaired electrons; the orbital occupation diagram predicts 2. The observed valence for carbon is (almost) invariably 4, in accord with the Lewis symbol. Similarly, the valences of Be and B are as expected from the Lewis symbols, but in conflict with the orbital occupation diagrams. Yet the success of the quantum theory of the atom has been so profound that we believe completely that the orbital occupation diagrams are correct. How are we to explain the bonding properties of elements in groups 2, 13, and 14 in terms of the orbital occupation diagrams? The orbital diagrams can be brought into correspondence with the observed valences by a simple expedient: the downspin electron of the pair in the s orbital is placed in an empty p orbital, with its spin parallel to those of the other electrons. When this is done for Be, B, and C, the numbers of unpaired electrons correspond with the predictions of the Lewis symbol, and with the observed valences

Answer 2

When I was about 9 or 10 I did

Answer 3

Three of the positions in a trigonal bipyramid are labeled equatorial because they lie along the equator of the molecule. The other two are axial because they lie along an axis perpendicular to the equatorial plane. The angle between the three equatorial positions is 120o, while the angle between an axial and an equatorial position is 90o. example is PCl5.The term octahedron literally means "eight sides," but it is the six corners, or vertices, that interest us. To imagine the geometry of an SF6 molecule, locate fluorine atoms on opposite sides of the sulfur atom along the X, Y, and Z axes of an XYZ coordinate system.
drawing is getting difficult for me as symbols are not activated




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