BeH2 AXE Electron geometry: otation: Molecular geometry: Lewis structure VSEPR structure Polar/Nonpolar: Electron configuration of center atom: For the center atom: Atomic orbital diagram Hybridized orbital diagram Hybridized structure
The Correct Answer and Explanation is:
For Beryllium Hydride (BeH2), we can analyze it using the VSEPR theory, which gives us a comprehensive view of its molecular geometry, hybridization, and electron configuration.
1. Lewis Structure:
- BeH2 consists of a central beryllium (Be) atom bonded to two hydrogen (H) atoms.
- Beryllium is in group 2, so it has two valence electrons, while hydrogen, being a group 1 element, has one valence electron.
- To form bonds, beryllium shares its two electrons with two hydrogen atoms. This results in Be having two single bonds to the two H atoms, and no lone pairs on Be.
The Lewis structure of BeH2:
nginxCopyEditH — Be — H
2. VSEPR Structure:
- The central Be atom has two regions of electron density (from the two Be-H bonds).
- Since there are no lone pairs on Be, the electron pairs will repel each other and arrange themselves as far apart as possible, which results in a linear structure.
- Therefore, the electron geometry is linear with a bond angle of 180°.
3. Molecular Geometry:
- Since the electron geometry is linear and there are no lone pairs, the molecular geometry is also linear.
4. Polar/Nonpolar:
- BeH2 is nonpolar. The linear geometry and the fact that the Be-H bonds are symmetrical lead to no net dipole moment across the molecule.
5. Electron Configuration of Center Atom (Be):
- The electron configuration of Beryllium (Be) is: 1s22s21s^2 2s^21s22s2
- In its ground state, Be has two electrons in the 2s orbital.
6. For the Center Atom: Atomic Orbital Diagram:
- The atomic orbital diagram for Be will show two 2s electrons and two 2p orbitals that are empty.
- When bonding, the 2s and 2p orbitals mix and hybridize.
7. Hybridized Orbital Diagram:
- Since Be forms two bonds with hydrogen, it undergoes sp hybridization. This is because sp hybridization is needed to form two equivalent bonds that are 180° apart (linear geometry).
- The sp hybrid orbitals form the bonds with the hydrogen atoms, while the leftover p orbital remains empty.
8. Hybridized Structure:
- The hybridized structure involves one sp hybrid orbital forming a bond with each hydrogen atom. The remaining p orbital does not participate in bonding.
Summary:
- Electron Geometry: Linear
- Molecular Geometry: Linear
- Lewis Structure: BeH2 with two single bonds
- VSEPR Structure: Linear
- Polar/Nonpolar: Nonpolar
- Electron Configuration of Be: 1s² 2s²
- Hybridization of Be: sp
- Hybridized Structure: Two sp orbitals form bonds with hydrogen, leaving a lone p orbital.
This explanation highlights all the structural and electronic details of BeH2.
