The resulting geometry of the molecule emerges from the geometry of the overlapping orbitals. atomic orbitals. The orbitals can be the standard s, p, d, and f orbitals or hybrid combinations of these.
The sp orbitals on the carbon atoms are linear with 180° between them, so the resulting geometry of the molecule is linear with 180° bond angles, in agreement with the experimentally measured geometry of HC‚CH, and also in agreement with the prediction of VSEPR theory.
According to this theory, the repulsion molecule (FIgure 10.1◀). The preferred geometry is the one in which the electron groups have the maximum separation (and therefore the minimum energy) possible. Consequently, of those electron groups are bonding groups and how many are lone pairs. We first look at
different repulsions—the resulting bond angles reflect these differences. paper. For molecules with four or more electron groups around the central atom, the geometries are three-dimensional and are therefore more difficult to imagine and to draw. We can understand these shapes by analogy to balloons tied together.