Which molecular geometry is characteristic of a central atom with four bonds and no lone pairs?

The molecular geometry of a central atom with four bonds and no lone pairs is characterized as tetrahedral. In this arrangement, the four bonds are spaced out as far apart as possible to minimize electron pair repulsion, according to VSEPR (Valence Shell Electron Pair Repulsion) theory. This gives rise to bond angles of approximately 109.5 degrees between each of the bonds.

In a tetrahedral geometry, the central atom is positioned at the center of a tetrahedron with the surrounding atoms located at the vertices. This geometry is common in molecules such as methane (CH₄), where carbon is the central atom bonded to four hydrogen atoms with no lone pairs affecting the shape.

Other geometries mentioned do not apply to the situation described. Linear geometry involves two bonds and is typically observed with central atoms having no lone pairs and two bonded atoms, resulting in a straight-line arrangement. Trigonal planar geometry arises when there are three bonds and no lone pairs, leading to a flat triangular configuration with bond angles of 120 degrees. Octahedral geometry is seen when there are six bonds and no lone pairs, resulting in an octahedral shape with bond angles of 90 degrees.

Thus, the correct characterization for a central atom with four bonds