University:
University of Alberta
Course:
CHEM 101 | Introductory University Chemistry I
Academic year:

2024
Views:

278

Pages:

4
Author:

Neena N.

Electronegativity Each non-metal has a slightly different ability to attract electrons in a covalent bond, which is called it's electronegativity. The electronegativity of the atoms in a covalent bond affects the sharing of electrons. When two atoms of unequal electronegativity form a covalent bond, the shared electron pair will spend more time around the atom with a greater electronegativity. This atom is assigned: 6- (Delta minus), and indicates that the shared electrons spend a relatively greater time around this atom giving it a partial negative charge. Conversely, the atom with lower electronegativity is assigned 6+ (Delta plus) and so the shared electrons spend relatively less time around this atom giving it a partial positive charge. Electronegativity of the elements tends to increase from left to right across a period in the periodic table. Electronegativity decreases down a group. These partial charges are important in other types of bonding and properties. Hybridisation In chemistry, hybridization refers to the mixing of atomic orbitals to form new hybrid orbitals that are used for bonding. Hybrid orbitals have different shapes and energies compared to the original atomic orbitals. They allow atoms to achieve a more stable configuration by maximizing the overlap of orbitals during bonding. Hybridization commonly occurs in organic compounds, such as hydrocarbons, and is used to explain molecular geometry and bond angles. The most common types of hybridization are sp, 2 3 sp, and sp hybridization. sp hybridization: In sp hybridization, one s orbital and one p orbital of the central atom combine to form two sp hybrid orbitals. These orbitals are linearly oriented at an angle of 180 degrees to each other. Examples of molecules with sp hybridization include linear molecules like acetylene (C2H2). sp2 hybridization: In sp2 hybridization, one s orbital and two p orbitals of the central atom combine to 2 form three sp hybrid orbitals. These orbitals are trigonally arranged in a plane with bond angles of approximately 120 degrees. This hybridization is commonly observed in molecules such as ethylene (C2H4) and benzene (C6H6). sp³ hybridization: In sp hybridization, one s orbital and three p orbitals of the central atom combine to 3 form four sp hybrid orbitals. These orbitals are tetrahedrally arranged with bond angles of approximately 109.5 degrees. Many molecules, including methane (CH4) and sp³ hybridization. ammonia (NH3), exhibit sp³ hybridization Unhybridized orbitals, on the other hand, refer to the atomic orbitals that are not involved in hybridization and remain in their original form. For example, in an sp³ hybridized carbon atom in methane (CH4), the remaining unhybridized p orbital is available for pi bonding with other atoms. It's important to note that hybridization is a concept used to describe the bonding and geometry in molecules. It is a simplified representation of molecular structure and does not necessarily reflect the true nature of electron distribution in molecules