The Lewis structure is a diagram that represents the bonding between atoms in a molecule and the lone pairs of electrons that may exist. Let’s explore the Lewis structures and 3D representations for the molecules BH3, NH3, and FCl3.
1. BH3 (Boron Trifluoride)
The Lewis structure for BH3 has boron (B) in the center with three fluorine (F) atoms attached to it, each sharing one pair of electrons with boron. Boron has only six electrons in its valence shell, leading to an electron-deficient molecule.
In its 3D representation, BH3 has a trigonal planar shape, with bond angles of approximately 120 degrees between the fluorine atoms.
2. NH3 (Ammonia)
For NH3, nitrogen (N) is the central atom with three hydrogen (H) atoms bonded to it. The Lewis structure shows nitrogen sharing its three valence electrons with each hydrogen, along with one lone pair of electrons on nitrogen.
In 3D, ammonia has a trigonal pyramidal shape due to the presence of the lone pair, causing the hydrogen atoms to be pushed down, resulting in bond angles of about 107 degrees.
3. FCl3 (Chlorine Trifluoride)
The Lewis structure of FCl3 features chlorine (Cl) at the center with three fluorine (F) atoms attached. Chlorine has one lone pair of electrons. Each bond between Cl and F involves sharing one pair of electrons.
In its 3D form, FCl3 adopts a T-shaped geometry because of the lone pair, with bond angles of approximately 90 degrees.
These structures provide insight into the arrangement and bonding of atoms within each molecule, showcasing the diversity in molecular shapes and electron arrangements.