Draw the Lewis Structure, Indicate the Molecular Structure and Indicate the Bond Angles for BF₃

The Lewis structure for boron trifluoride (BF₃) shows that boron (B) is the central atom surrounded by three fluorine (F) atoms. Each fluorine atom forms a single bond with the boron atom.

To draw the Lewis structure, follow these steps:

1. Count the total valence electrons: Boron has 3 valence electrons, and each fluorine has 7 valence electrons, giving us a total of 3 + (3 × 7) = 24 valence electrons.
2. Place boron in the center and connect each fluorine atom to boron with a single bond (which uses 2 electrons for each bond).
3. Distribute the remaining electrons to satisfy the octet rule for fluorine, ensuring each fluorine has 8 electrons around it while boron has just 6 electrons.

The Lewis structure can be represented as:

    F
    |
F - B - F

In this configuration, boron does not have a complete octet, which is common for boron compounds.

BF₃ has a trigonal planar molecular geometry, as the three fluorine atoms are positioned around the boron atom in a plane, making angles of approximately 120 degrees between the bonds. This arrangement minimizes the repulsion between the electron pairs and leads to a stable structure.

In summary, the bond angles in BF₃ are approximately 120 degrees, reflecting its trigonal planar shape, which is a key characteristic of molecules with three bonding pairs and no lone pairs on the central atom.