Question

Based on VSEPR theory and your observations from the molecular geometry lab, what is the predicted hybridization at an atom which is surrounded by two double bonds?

1) sp
2) sp2
3) sp3
4) sp3d

Answer 1

When an atom is surrounded by two double bonds, it is predicted to have sp hybridization.

Step-by-step explanation:

Based on VSEPR theory and observations from the molecular geometry lab, an atom surrounded by two double bonds would have sp hybridization. Carbon atoms 2 and 3 in the lab observation have linear geometries and would be classified as sp hybrids, while carbon atoms 1 and 4 have tetrahedral geometries with sp³ hybridization.

The concept is often used to explain the geometry and bonding in molecules.

Here are some key points about hybridization:

Atomic Orbitals: In an atom, electrons are arranged in orbitals around the nucleus. These orbitals include s, p, d, and f orbitals. Hybridization involves the combination of these atomic orbitals to form new, hybrid orbitals.

Types of Hybridization: The most common types of hybridization involve the combination of s and p orbitals. The resulting hybrid orbitals are labeled based on the number of atomic orbitals involved. Common hybridization states include sp, sp², sp³, dsp³, and d²sp³.

Hybrid Orbitals and Bonding: Hybrid orbitals are used for bonding in molecules. For example, in methane (CH₄), carbon undergoes sp³ hybridization, forming four sp³ hybrid orbitals that overlap with the 1s orbitals of four hydrogen atoms to create four sigma bonds.

Geometry of Molecules: The hybridization of orbitals influences the geometry of molecules. For instance, molecules with sp³ hybridization often exhibit tetrahedral geometry, while those with sp² hybridization often have trigonal planar or trigonal pyramidal geometry.

Pi Bonds and Unhybridized Orbitals: In addition to sigma bonds formed by hybrid orbitals, molecules can have pi (π) bonds formed by the overlap of unhybridized p orbitals. This is common in molecules with double or triple bonds.

Hybridization in Organic Chemistry: Hybridization is frequently used to explain the bonding in organic compounds. For example, in the organic molecule ethene (C₂H₄), carbon atoms undergo sp² hybridization, resulting in a double bond between the carbon atoms.

Understanding hybridization is crucial for predicting molecular shapes, bond angles, and the nature of chemical bonds in molecules. It provides a theoretical framework for explaining the observed properties of compounds in organic and inorganic chemistry.

Answer 2

The atom with two double bonds is predicted to have sp hybridization, indicated by VSEPR theory and laboratory observations.

Step-by-step explanation:

Based on VSEPR theory and observations from the molecular geometry lab, the predicted hybridization at an atom which is surrounded by two double bonds is sp hybridization. This is due to the fact that a central atom with two regions of electron density, such as in a molecule like carbon dioxide (CO₂) which has two double bonds, will have its s orbital and one p orbital combine to form two sp hybrid orbitals. These hybrid orbitals are arranged in a linear geometry, 180° apart. An example can be seen in the molecular geometry of BeCl₂, where the beryllium atom adopts sp hybridization to form two identical sigma bonds with chlorine atoms.