In chemistry, sigma bonds (σ bonds) are the strongest type of covalent chemical bond. They are formed by head-on overlapping between atomic orbitals. Sigma bonding is most simply defined for diatomic molecules using the language and tools of symmetry groups.
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Electron geometry: tetrahedral, sp3 hybridized.
Since four atoms of hydrogen are surrounding the germanium in this case, a sp3 hybrization is making up the sigma bons for this molecular compound. The germanium atom can use its singly occupied p-type orbitals, to form two covalent bonds with two hydrogen atoms, and use the s and the other p to form the other two covalent bonds with the remaining hydrogens.
(a) Hybridization of orbitals
See the Lewis structure of propyne in the first diagram below.
C1 is directly bonded to two other atoms (H and C2) so it is sp hybridized.
C2 is directly bonded to two other atoms (C1 and C3) so it is sp hybridized.
C3 is directly bonded to four other atoms (C2 and 3 H) so it is sp³ hybridized.
(b) C2-C3 Sigma Bond
See the atomic and molecular orbitals in the second picture below.
C3 is using its hybrid atomic orbitals to form sigma molecular bonds. The C2-C3 sigma bond is formed by the overlap of the C2 sp atomic orbital with the C3 sp³ atomic orbital to make a σ(sp-sp³) molecular orbital.
(c) Bond angles
C1 and C2 are sp hybridized. Since the angle between sp orbitals is 180°, all atoms directly attached the C1 and C2 must be in a straight line. The C-C-C bond angle is 180°.
the answer is 0.8m.