The molecular geometry of NF3 (nitrogen trifluoride) is trigonal pyramidal. This shape arises because the nitrogen atom has one lone pair of electrons and three bonded pairs of electrons with fluorine atoms. The lone pair occupies more space than the bonded pairs, causing the fluorine atoms to be pushed slightly downward, resulting in a pyramidal shape.
In a trigonal pyramidal geometry, the bond angles are slightly less than 109.5° due to the repulsion between the lone pair and the bonded pairs. This deviation from the ideal tetrahedral angle is a key characteristic of molecules with this geometry.
Understanding the molecular geometry of NF3 is important in predicting its physical and chemical properties, such as polarity and reactivity.