The molecular geometry of CHF3 (trifluoromethane) is tetrahedral. This shape arises because the central carbon atom is bonded to three fluorine atoms and one hydrogen atom. The four bonding pairs of electrons repel each other and arrange themselves in such a way as to minimize repulsion, leading to a tetrahedral configuration.
Regarding polarity, CHF3 is considered polar. Although the molecule has a symmetrical tetrahedral shape, the presence of three highly electronegative fluorine atoms creates an uneven distribution of electron density. The fluorine atoms pull the electron density toward themselves, leading to a dipole moment. The carbon-hydrogen bond is much less polar compared to the carbon-fluorine bonds, so the overall effect is that the molecule has a net dipole moment directed towards the fluorine atoms. Thus, the molecule is polar.